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www.chemactive.com GCSE CHEMISTRY ACIDS, BASES & SALTS High Demand Questions QUESTIONSHEET 1 A food scientist checked the quality of a bottle of vinegar. He took 50 cm 3 of the vinegar and found out how much sodium hydroxide was needed to neutralise it. (a) (i) Explain what is meant by ‘neutralise’. ......................................................................................................................................................................... [1] (ii) What apparatus could the scientist have used to measure the amount of sodium hydroxide needed? ......................................................................................................................................................................... [1] He also tested some ethanoic acid solution. Ethanoic acid is the acid which is found in vinegar. His results are shown below. vinegar ethanoic acid volume used/cm 3 50 10 volume of NaOH needed to neutralise/cm 3 30 10 The ethanoic acid solution contained 10 g of acid in every 100 cm 3 of solution. (b) (i) How many grams of ethanoic acid are there in 10 cm 3 of solution? ......................................................................................................................................................................... [1] (ii) Work out how many grams of ethanoic acid are in 50 cm 3 of the vinegar. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What must you assume is kept constant to allow you to work out the answer to (ii) ? ......................................................................................................................................................................... [1] A label on the bottle of vinegar states that it contains 8 g of ethanoic acid in 100 cm 3 of vinegar. (c) Using your answer to (b)(ii) work out whether the answer on the bottle is correct. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 8

GCSE/IGCSE Chemistry Question Bank with Answers

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A comprehensive 347 page question - answer guide with hundreds of questions based on the newest GCSE/IGCSE Syllabus. These questions are also useful for O Level or other such syllabus.Note - There is a watermark which is to ensure that no one else takes right to this work (which does not belong to me too).

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Page 1: GCSE/IGCSE Chemistry Question Bank with Answers

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GCSE CHEMISTRY ACIDS, BASES & SALTS

High Demand Questions QUESTIONSHEET 1 A food scientist checked the quality of a bottle of vinegar. He took 50 cm3 of the vinegar and found out how much sodium hydroxide was needed to neutralise it. (a) (i) Explain what is meant by ‘neutralise’. ......................................................................................................................................................................... [1] (ii) What apparatus could the scientist have used to measure the amount of sodium hydroxide needed? ......................................................................................................................................................................... [1] He also tested some ethanoic acid solution. Ethanoic acid is the acid which is found in vinegar. His results are shown below.

vinegar ethanoic acid volume used/cm3 50 10 volume of NaOH needed to neutralise/cm3 30 10

The ethanoic acid solution contained 10 g of acid in every 100 cm3 of solution. (b) (i) How many grams of ethanoic acid are there in 10 cm3 of solution? ......................................................................................................................................................................... [1] (ii) Work out how many grams of ethanoic acid are in 50 cm3 of the vinegar. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What must you assume is kept constant to allow you to work out the answer to (ii) ? ......................................................................................................................................................................... [1] A label on the bottle of vinegar states that it contains 8 g of ethanoic acid in 100 cm3 of vinegar. (c) Using your answer to (b)(ii) work out whether the answer on the bottle is correct. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

Page 2: GCSE/IGCSE Chemistry Question Bank with Answers

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GCSE CHEMISTRY ACIDS, BASES & SALTS High Demand Questions QUESTIONSHEET 2 Small pieces of the metals copper, magnesium, nickel and zinc were placed in test tubes containing small quantities of hydrochloric acid. The following results were observed.

copper magnesium nickel zinc (a) Use the observations from above to complete the following reactivity series. 1. ........................................................................................................................................................ most reactive 2. .............................................................................................................................................................................. 3. .............................................................................................................................................................................. 4. ......................................................................................................................................................... least reactive

[2] (b) (i) What is the name of the gas produced in the above reactions? ......................................................................................................................................................................... [1] (ii) Describe the test and result you would use to identify this gas. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) The reaction between the metals and the hydrochloric acid also produces a chemical compound known as a salt. (i) What is the name of the salt formed in the reaction between magnesium and hydrochloric acid? ......................................................................................................................................................................... [1] (ii) What type of bonding is present in this salt? ......................................................................................................................................................................... [1] (iii) This salt is a solid at room temperature. Explain why a salt has a high melting and boiling point. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS

High Demand Questions QUESTIONSHEET 3 (a) The metal sodium burns in limited oxygen with a bright yellow flame to form sodium oxide. (i) Write a word equation for the reaction between sodium and oxygen. ......................................................................................................................................................................... [1] (ii) What is the formula of sodium oxide? (A sodium ion is Na+

and an oxide ion is O2-

) ......................................................................................................................................................................... [1] (iii) Predict whether sodium oxide is a solid, liquid or gas at room temperature. ......................................................................................................................................................................... [1] (iv) Sodium oxide dissolves readily in water. What colour would the resulting solution turn pH paper? ......................................................................................................................................................................... [1] (b) Sulphur dioxide is produced when coal is burnt and is responsible for the formation of acid rain. (i) Complete the following equation and put in the missing state symbol. S (s) + ____ (g) → SO2 ____ [2] (ii) Acid rain is a weak acid. Predict what pH it would have if it was tested with pH paper. ......................................................................................................................................................................... [1] (iii) Write down two problems which acid rain can cause. 1. .......................................................................................................................................................................... 2............................................................................................................................................................................ [2]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS High Demand Questions QUESTIONSHEET 4 The following experiment was carried out using concentrated ammonia solution and concentrated hydrochloric acid.

(a) Ammonia contains the elements hydrogen and nitrogen and has the chemical formula NH3. (i) Name the type of bonding that exists in ammonia ......................................................................................................................................................................... [1] (ii) Use the Periodic Table to draw a 'dot and cross' diagram to show the bonding in a molecule of

ammonia. You need only show the electrons in the outer energy level.

[2] (iii) Explain why ammonia has a low boiling point. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) The ammonia and hydrogen chloride gases meet and react to form the ring of white smoke which is

shown in the diagram. (i) Explain, in terms of the particles of the gases, why the gases meet. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Explain why the ring of white smoke forms nearer to the concentrated hydrochloric acid. ......................................................................................................................................................................... [1] (iii) What is the name of the chemical formed when ammonia and hydrogen chloride react? ......................................................................................................................................................................... [1]

TOTAL / 9

cotton wool soaked in concentrated ammonia solution

cotton wool soaked in concentrated hydrochloric acid

white smoke forms here

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GCSE CHEMISTRY ACIDS, BASES & SALTS

High Demand Questions QUESTIONSHEET 5 The diagram below shows an experiment to measure the rate of reaction between calcium carbonate and sulphuric acid.

calcium carbonate

sulphuric acid

gas syringe

(a) The reaction between calcium carbonate and sulphuric acid produces a chemical compound called a salt, a gas and water.

(i) The gas produced can be identified using limewater. Name the gas and the result of this test.

Name of gas ............................................................................................................................................... Result of test ......................................................................................................................................... [2]

(ii) What is the name of the salt produced? ......................................................................................................................................................................... [1]

(b) The experiment was repeated with exactly the same volume of sulphuric acid and the same mass of calcium carbonate. This time the calcium carbonate used was a powder.

(i) What happens to the rate of the reaction? ......................................................................................................................................................................... [1]

(ii) Use the idea of particles to explain your answer to (b) (i). .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(c) The experiment was repeated but with magnesium metal instead of calcium carbonate and a different salt and a different gas were produced.

(i) What gas is produced in the reaction between magnesium and sulphuric acid? ......................................................................................................................................................................... [1]

(ii) Describe the test you would use to identify this gas and the result that you would obtain. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Write down one use in industry of this gas. ......................................................................................................................................................................... [1]

TOTAL / 10

Calcium carbonate

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GCSE CHEMISTRY ACIDS, BASES & SALTS High Demand Questions QUESTIONSHEET 6 The table below shows the colours of various indicators at different pH values.

indicator colour 1 pH colour 2 pH bromophenol blue yellow 3 blue 4.5 phenolphthalein colourless 8 pink 10 methyl orange red 3 yellow 4.5 thymol blue yellow 6 blue 7.5

Hydrochloric acid has a pH of 1.0 and ethanoic acid has a pH of 5.0 Ammonia solution has a pH of 10.0 and sodium hydroxide has a pH of 12.5 (a) Complete the table below to show colours of the indicators in the solutions.

indicator solution colour bromophenol blue hydrochloric acid phenolphthalein ethanoic acid methyl orange ammonia solution thymol blue sodium hydroxide

[4] (b) (i) Name one indicator which turns the same colour in both ethanoic acid and sodium hydroxide ......................................................................................................................................................................... [1] (ii) Which two indicators turn the same colour in hydrochloric acid? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS

High Demand Questions QUESTIONSHEET 7 Slaked lime is used raise the pH of soil. (a) What is the chemical name for slaked lime? ......................................................................................................................................................................... [1] (b) The recommended amount to use is 125 g per square metre of soil. How much slaked lime would you need to apply to a rectangular garden which measured 10 metres by 8 metres? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Less calcium oxide than slaked lime is needed to treat the same garden. Why would the gardener prefer to use slaked lime? ......................................................................................................................................................................... [1] (d) (i) Write an equation for the reaction of slaked lime with nitric acid. ......................................................................................................................................................................... [2] (ii) How much slaked lime is needed to neutralise 63 g of nitric acid? (Ar: H=1; N=14; O=16 Ca=40) .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS High Demand Questions QUESTIONSHEET 8 Sulphur dioxide reacts with chlorine, in the presence of water, to produce a mixture of hydrochloric and sulphuric acids. (a) Complete the equation for the reaction. SO2 + Cl2 + __H2O ______ + _______ [2] (b) This reaction can be used to reduce the amount of chlorine in water. If a bottle of tap water contained 2 mg of chlorine, how much sulphur dioxide must be added to reduce this to 1 mg? (Ar: O=16; S=32; Cl=35.5) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] The concentration of a solution can be expressed in grams per cubic decimetre (g/dm3). To calculate this you must divide the amount of substance dissolved (g) by the volume of the solution (dm3). (c) Which of the following has the greater concentration? Show your working. A 10 g of potassium hydroxide in 2 dm3 of solution. B 50 g of potassium hydroxide in 5 dm3 of solution .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Medium Demand Questions QUESTIONSHEET 9 The pH of chemicals found around the home may be tested using pH paper. Some typical results are shown below.

pH 1 2 3 4 5 6 7 8 9 10 11 12 13 14 ↓ ↓ ↓ lemon juice orange juice washing-up liquid oven cleaner (a) Answer the following questions using the above information. (i) What is the pH of oven cleaner? ......................................................................................................................................................................... [1] (ii) Which is the most acidic solution? ......................................................................................................................................................................... [1] (iii) What would be the pH of a neutral solution? ......................................................................................................................................................................... [1] (b) Vinegar was also tested using pH paper and found to have a pH of 4.1. What colour did the pH paper become? ......................................................................................................................................................................... [1] (c) When a wasp stings someone its injects a liquid in the person's skin. An old fashioned remedy for wasp stings is to rub vinegar on them. (i) Suggest the pH of the liquid which wasps inject into the skin. ......................................................................................................................................................................... [1] (ii) What name is given to the reaction which happens between this liquid and the vinegar? ......................................................................................................................................................................... [1] (iii) Name the colourless, tasteless liquid that is produced in this reaction. ......................................................................................................................................................................... [1]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS Medium Demand Questions QUESTIONSHEET 10 Some people suffer from acid indigestion when their stomach produces excess stomach acid. The label on a household brand of indigestion tablets says that it contains magnesium carbonate. (a) Magnesium carbonate is insoluble in water. When mixed with water, what colour would it turn pH paper? ......................................................................................................................................................................... [1] (b) The instructions on the packet suggest that 1 or 2 tablets are chewed as required. (i) What name is given to the reaction which happens between the excess acid and the indigestion tablet? ......................................................................................................................................................................... [1] (ii) Explain why the instructions suggest that the tablets are chewed when taken. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) The acid present in the stomach is called hydrochloric acid. Hydrochloric acid, HCl, reacts with magnesium carbonate, MgCO3, to produce magnesium chloride, carbon dioxide and water. (i) Complete and balance the equation for this reaction. ___HCl (aq) + MgCO3(s) → MgCl2 (aq) + ___ (g) + H2O (l) [2] (ii) Limewater can be used to test for carbon dioxide. What is the result of this test? ......................................................................................................................................................................... [1] (iii) Use these relative atomic masses: C = 12; O = 16; Mg = 24 to calculate the relative formula mass of magnesium carbonate. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Medium Demand Questions QUESTIONSHEET 11

(a) In an experiment ammonia solution, an alkali, was added to nitric acid.

nitric acid

ammonium hydroxide

apparatus A

(i) What is the name of apparatus A? ......................................................................................................................................................................... [1]

(ii) What is the name of the reaction when the acid reacts with the alkali? ......................................................................................................................................................................... [1]

(iii) What is the pH when just enough ammonia solution is added to react with all the nitric acid? ......................................................................................................................................................................... [1]

(b) (i) What is the ion which is present in any solution of acid? ......................................................................................................................................................................... [1]

(ii) What is the ion which is present in any solution of alkali? ......................................................................................................................................................................... [1]

(iii) Write the simplest ionic equation which represents the above reaction. ......................................................................................................................................................................... [1]

(c) The following label is found on the bottle containing the nitric acid.

(i) What does the label tell you about the nitric acid? ......................................................................................................................................................................... [1]

(ii) Suggest two precautions which should be taken when using the nitric acid in the experiment. 1. ..................................................................................................................................................................... [1] 2. ..................................................................................................................................................................... [1]

TOTAL / 9

ammonia solution

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GCSE CHEMISTRY ACIDS, BASES & SALTS Medium Demand Questions QUESTIONSHEET 12 (a) Below are the chemical formulae of four acids. HCl H2SO4 HNO3 CH3COOH (i) What colour would they all turn a solution of litmus? ......................................................................................................................................................................... [1] (ii) Write down the name of the ion present in solutions of all the acids. ......................................................................................................................................................................... [1] (b) Below are the chemical formulae of four alkalis. NaOH KOH Mg(OH)2 NH4OH (i) What colour would they all turn a solution of litmus? ......................................................................................................................................................................... [1] (ii) Write down the name of the ion present in solutions of all the alkalis. ......................................................................................................................................................................... [1] (c) A solution of sulphuric acid can be used to neutralise a solution of sodium hydroxide. (i) What is the pH of the solution when it is exactly neutral? ......................................................................................................................................................................... [1] (ii) What is the name of the salt formed in the neutralisation reaction? ......................................................................................................................................................................... [1] (iii) Balance the following symbol equation for the reaction. H2SO4 (aq) + ____ NaOH (aq) → Na2SO4 (aq) + ____ H2O (l) [2] (d) When nitric acid neutralises ammonium hydroxide the salt formed is called ammonium nitrate. Give one important use of ammonium nitrate. ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Medium Demand Questions QUESTIONSHEET 13 (a) Many power stations in the UK burn coal to produce electricity. Coal is a fossil fuel. Describe how the coal is formed. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) Fossil fuels, such as coal, contain sulphur as an impurity. When the coal is burnt the sulphur is oxidised. (i) Explain what is meant by the term 'oxidised'. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) What is the name of the gas formed when the sulphur is oxidised? ......................................................................................................................................................................... [1] (c) Write a symbol equation for what happens when this gas reacts with rain water. ......................................................................................................................................................................... [2] (d) Explain why acid rain can erode limestone. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS Medium Demand Questions QUESTIONSHEET 14 Below is information about six chemicals.

chemical state at 20 °C pH in water reaction with acid A gas 1 none B liquid 7 none C solid 4 none D solid 8 forms a salt, carbon dioxide and water E solid 14 forms a salt and water F solid no reaction fizzes

Use the table to write the letter of the chemical substance which: (a) forms the most strongly acidic solution. ......................................................................................................................................................................... [1] (b) forms a neutral solution. ......................................................................................................................................................................... [1] (c) forms a solution which turns pH paper orange. ......................................................................................................................................................................... [1] (d) is a metal . ......................................................................................................................................................................... [1] (e) is a carbonate. ......................................................................................................................................................................... [1] (f) is water. ......................................................................................................................................................................... [1] (g) is sulphur dioxide. ......................................................................................................................................................................... [1]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Medium Demand Questions QUESTIONSHEET 15 Antacid tablets are used to treat indigestion, which is caused by excess acid in the stomach. Details of four solids, which are used to neutralise stomach acid, are shown in the table below.

Name of solid Formula Reaction with acid Cost per gram magnesium carbonate fizzes 16.0 p CaCO3 11.0 p magnesium hydroxide Mg(OH) 2 does not fizz 7.5 p aluminium hydroxide Al(OH) 3 does not fizz 22.0 p

(a) Complete the table. [3] (b) Complete the equation for the reaction of magnesium hydroxide with hydrochloric acid. Mg(OH) 2 + 2HCl + H2O [1] (c) An experiment was carried out to find out how much acid was needed to neutralise one gram of

each of the solids. The solid was put into a flask with water and an indicator, then acid was added. (i) Describe how you would find out the exact amount of acid needed. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Why is it important to use the same concentration of acid each time? ......................................................................................................................................................................... [1] (d) Another way to compare the solids is to find out how much solid is needed to neutralise 20 cm3 of acid. The results are shown below.

Solid Mass of solid to neutralise 20 cm3 of acid

Magnesium carbonate 0.7 g CaCO3 1.2 g

Magnesium hydroxide 0.6 g Aluminium hydroxide 0.4 g

(i) Calculate the costs of each solid used. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4]

(Continued...)

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GCSE CHEMISTRY ACIDS, BASES & SALTS QUESTIONSHEET 15 CONTINUED (ii) Use all the information given to choose the best antacid. Give a reason for your answer .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 14

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Medium Demand Questions QUESTIONSHEET 16 James spilt some acid on the floor. He looked at the possibility of treating it with one of four chemicals. Their properties are summarised in the table.

substance pH reaction with acid A 13.0 produces a salt and water B 8.5 produces a salt, water and carbon dioxide C 8.0 produces a salt and water D 1.0 no reaction

(a) (i) Why would substance D be useless for the purpose? ......................................................................................................................................................................... [1] (ii) Which other substance would you advise him to avoid? (Give a reason) .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What type of substance is B? ......................................................................................................................................................................... [1] (b) Sodium chloride is probably the best known salt. It is used in the food industry, spread on roads in

winter and used to make a range of other chemicals. (i) State two uses of sodium chloride in the food industry. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Name two other chemicals made from sodium chloride. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Why is sodium chloride spread on winter roads? ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS Low Demand Questions QUESTIONSHEET 17 Nettles, bees and ants sting by injecting acid into your skin. Wasp stings are alkaline. (a) How could you test to prove that the liquid from an ant is acid? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Vinegar is used to treat a wasp sting and ammonia to treat a bee sting. Explain why this works and what it tells you about vinegar and ammonia. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) Car batteries contain strong sulphuric acid. To treat a spillage from a car battery, you must first add lots of water then put washing soda on it. Explain this treatment. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Low Demand Questions QUESTIONSHEET 18 The pH of soil is very important in deciding which crops grow best. The table below shows the pH ranges which are best for some plants.

Plant pH range beans 6.0 to 7.5 potato 5.0 to 6.5 onion 6.0 to 7.0 leek 6.0 to 8.0

The soil in three fields was tested. The results are shown below.

field pH of soil A 6.6 B 7.3 C 5.5

(a) In which field is the soil most acidic? ......................................................................................................................................................................... [1] (b) For each field list the crops which would grow best in it. Field A ................................................................................................................................................. [3] Field B .................................................................................................................................................. [2] Field C .................................................................................................................................................. [1] (c) Lime can be added to raise the pH of the soil. Which field would need lime before you could grow leeks in it? ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY ACIDS, BASES & SALTS Low Demand Questions QUESTIONSHEET 19

Epsom salts was a favourite medicine of our grandparents. Its chemical name is magnesium sulphate. (a) Write down the formula of magnesium sulphate. ......................................................................................................................................................................... [1] Salts can be made in a number of ways. I adding a metal to an acid II adding a carbonate to an acid III adding a hydroxide to an acid (b) For each of the methods above, give the correct chemical name of two substances which could be mixed

to make magnesium sulphate. method I ............................................................................................................................................... [2] method II ............................................................................................................................................... [2] method III ............................................................................................................................................. [2] (c) In each case the magnesium sulphate is formed as a solution in water. What would you need to do to produce solid magnesium sulphate? ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY ACIDS, BASES & SALTS

Low Demand Questions QUESTIONSHEET 20 Complete the following sentences about acids, bases and salts. (i) Acids have a pH below ________. [1] (ii) When acids are mixed with alkalis they become ________. [1] (iii) All acids contain ________. [1] (iv) Acids react with carbonates to produce ________ ________ gas. [1] (v) The acid found in vinegar is called ________ ________. [1] (vi) Acids are also found in __________. [1] (vii) An example of an alkali is _________. [1] (viii) Safety spectacles must be used when handling acids or alkalis, because they are ________. [1]

TOTAL / 8

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

High Demand Questions QUESTIONSHEET 1 (a) Oxygen and sulphur are in the same group of the periodic table. Complete the table below to show the arrangement of electrons in oxygen and sulphur atoms.

Atom shell 1 shell 2 shell 3 oxygen sulphur

[2] (b) (i) Draw a diagram of an oxygen atom. [2] (ii) Use your diagram to describe two ways in which oxygen can achieve a full outside shell of electrons. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Some of the oxygen in the atmosphere is in the form of ozone, O3. Scientists believe that chlorine

radicals are destroying ozone. (i) What is the difference between a chlorine radical and a chlorine molecule? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) What substances are thought to be main sources of chlorine radicals in the atmosphere? ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING High Demand Questions QUESTIONSHEET 2 (a) There are eleven electrons in a sodium atom. The amounts of energy required to remove each one have been measured and the results shown on a sketch graph. (i) Why is the first electron in sodium the easiest to remove? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Why do the energies for electrons 2 to 9 go up by relatively small amounts? ......................................................................................................................................................................... [1] (iii) Why are the last two energies very high? ......................................................................................................................................................................... [1] (b) Draw a sketch graph to show the energies needed to remove the first four electrons in aluminium. Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 7

Number of electrons

1 2 4 3 5 6 7 8 9 10 11 0

20000

40000

60000

100000

80000

120000

140000

160000

180000

Energy /kJmol-1

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

High Demand Questions QUESTIONSHEET 3

(a) (i) Explain what is meant by the numbers in the symbol Ca4020 .

.............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Use the numbers to state the number of protons, neutrons and electrons found in Ca40

20 protons neutrons electrons

[3] (b) Complete the table below to show the numbers of protons, neutrons and electrons found in the ions

shown.

ion protons neutrons electrons +H1

1

+294 Be

+35626 Fe

−I12753

−27934 Se

[8]

TOTAL / 13

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING High Demand Questions QUESTIONSHEET 4

Neon has two main isotopes, Ne2010 and Ne22

10 (a) Draw diagrams of the atoms of each of the neon isotopes. [3] (b) Neon gas is made up of 90% of neon-20 and 10% of neon-22. Calculate the exact relative atomic mass of neon. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) How do the chemical properties of each isotope of neon compare with each other? Explain your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

High Demand Questions QUESTIONSHEET 5 The diagram below shows the electronic arrangement of an unknown substance. (a) (i) How many protons would there be if the unknown substance was a neutral atom? ......................................................................................................................................................................... [1] (ii) What would the diagram represent if it was a neutral atom? ......................................................................................................................................................................... [1] (b)(i) How many protons would there be if the substance was a 2+ ion? ......................................................................................................................................................................... [1] (ii) What would the diagram represent if it was a 2+ ion? ......................................................................................................................................................................... [1] (c) (i) In what group of the periodic table would the unknown substance be if the represented a 1+ ion? ......................................................................................................................................................................... [1] (ii) How many neutrons would the 1+ ion have if its relative atomic mass was 39? ......................................................................................................................................................................... [1] (d) (i) In what group of the periodic table would the unknown substance be if it represented a 1- ion? ......................................................................................................................................................................... [1] (ii) What would the relative atomic mass of the 1- ion be if it had 20 neutrons? ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING High Demand Questions QUESTIONSHEET 6 An unknown element is found to exist as the following two isotopes: X24

13 X2813

(a) Complete the following table:

number of protons number of neutrons number of electrons

X2413

13

X2813

13 15

[2] (b) Describe what is meant by the term ‘isotopes’. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) In experiments, both isotopes were found to show the same chemical behaviour. Use the information in the table to explain why the chemical behaviour of both isotopes is the same. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) A naturally occurring sample was found to contain 25% of X-24 and 75% of X-28. Calculate the relative atomic mass of the element X. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (e) Use your periodic table to identify X. ......................................................................................................................................................................... [1]

TOTAL / 9 High Demand Questions QUESTIONSHEET 7

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

The diagrams below represent the electronic arrangement of different atoms and ions. (a) Which letter represents an atom of a Group I metal? ......................................................................................................................................................................... [1] (b) Which letter represents an atom of a Group VII non-metal? ......................................................................................................................................................................... [1] (c) Which letter represents an atom of a noble or inert gas? ......................................................................................................................................................................... [1] (d) Which letter represents an atom which is not in the second period of the Periodic Table? ......................................................................................................................................................................... [1] (e) Which letter represents an ion of a Group I metal? ......................................................................................................................................................................... [1] (f) Which two letters represent atoms which form an ionic compound with a formula similar to Na2S? ......................................................................................................................................................................... [1] (g) Which two letters represent atoms which form a molecule with a formula similar to SiCl4? ......................................................................................................................................................................... [1] TOTAL / 7 High Demand Questions QUESTIONSHEET 8

A B C

D E F

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING (a) Use the Periodic Table to write down the electronic arrangement of: (i) calcium ......................................................................................................................................................................... [1] (ii) chlorine ......................................................................................................................................................................... [1] (b) If calcium is heated and put into a gas jar of chlorine a violent reaction takes place and solid calcium

chloride is formed. The reaction proceeds due to the transfer of electrons. (i) Use the electron arrangements and the idea of electron transfer to explain how the reaction between

atoms of calcium and chlorine takes place. (You may include a diagram in your answer) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4] (ii) Write down the formulae of the ions that calcium and chlorine form during the reaction. ......................................................................................................................................................................... [2] (iii) Write down the formula of calcium chloride. ......................................................................................................................................................................... [1] (c) Calcium chloride is a solid at room temperature and has a high melting point. Explain why calcium chloride has a high melting point. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11 Medium Demand Questions QUESTIONSHEET 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Carbon is known to exist as two different allotropes. The allotropes are known as diamond and graphite. Both diamond and graphite consist of carbon atoms bonded together in three-dimensional structures. (a) What is the name given the type of bond in which electrons are shared? ......................................................................................................................................................................... [1] (b) (i) Diamond is one of the hardest substances known to man and is used on the edges of glass cutting tools. Explain why the structure of diamond makes it so hard. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Graphite is soft and slippery and is used to lubricate surfaces. Explain why the structure of graphite makes it soft and slippery. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Diamond is an electrical insulator, but graphite conducts electricity. Explain why graphite conducts electricity. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7 Medium Demand Questions QUESTIONSHEET 10

Carbon atoms

Carbon atoms

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING Various parts of the helicopter below are made out of metal, because metals are strong and malleable.

(a) Describe, with the aid of a diagram, the metallic bonding present in metals.

[4] (b) Use your knowledge of the structure of metals to explain why: (i) they are strong .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) they are malleable .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) As the blades of the helicopter rotate, heat produced in the joints is conducted away along the blades. Explain how metals conduct heat. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) The properties of some of the metals used in the helicopter have been altered by mixing them with other

metals. What name is given to this type of mixture? ......................................................................................................................................................................... [1] TOTAL / 10 Medium Demand Questions QUESTIONSHEET 11

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Sodium chloride is often called common salt. It can be made by reacting a small piece of hot sodium with chlorine gas. (a) Write the electronic arrangement for an atom of: (i) sodium ......................................................................................................................................................................... [1] (ii) chlorine ......................................................................................................................................................................... [1] (b) Write down the formulae of the ions formed by: (i) sodium ......................................................................................................................................................................... [1] (ii) chlorine ......................................................................................................................................................................... [1] (c) Write down the formula of sodium chloride. ......................................................................................................................................................................... [1] (d) Solid sodium chloride will not conduct electricity, but when dissolved in water it will. (i) Explain why an aqueous solution of sodium chloride conducts electricity. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) In what other way could you alter the state of sodium chloride so that it will conduct electricity? ......................................................................................................................................................................... [1] (e) A hot piece of sodium was placed in a jar of helium. No reaction took place. (i) Write the name of the group of the periodic table to which helium belongs. ......................................................................................................................................................................... [1] (ii) Explain why helium is unreactive. ......................................................................................................................................................................... [1]

TOTAL / 9 Medium Demand Questions QUESTIONSHEET 12

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING The following table shows some of the ions found in natural waters.

ion Mg2+ Na+ SO42- NO3

- Ca2+ C1- K+

name magnesium sodium sulphate nitrate calcium chloride potassium

(a) Use the list of ions to work out the formulae of the following compounds: (Explain your answers) (i) sodium sulphate .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) potassium nitrate .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) calcium chloride .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) magnesium nitrate .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (v) potassium chloride .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) (i) What type of bonding occurs in all of these compounds? ......................................................................................................................................................................... [1] (ii) Explain how this type of bonding occurs. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

QUESTIONSHEET 12 CONTINUED (c) (i) Iodine is in the same group of the Periodic Table as chlorine. What is the formula of an iodide ion? ......................................................................................................................................................................... [1] (ii) Strontium, Sr, is in the same group of the Periodic Table as magnesium. What is the formula of the strontium ion? ......................................................................................................................................................................... [1] (iii) What is the formula of strontium iodide? ......................................................................................................................................................................... [1] TOTAL / 16

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING Medium Demand Questions QUESTIONSHEET 13 The flow chart below can be used to decide on the type of bonding found in different substances. Use the chart to identify the structure of the following substances: (a) (i) Decane boils at –30oC. It does not conduct electricity under any circumstances. ......................................................................................................................................................................... [1] (ii) Boron melts at 2027oC. Molten boron does not conduct electricity. ......................................................................................................................................................................... [1] (iii) Glucose melts at 146oC, but the molten solid does not conduct electricity. ......................................................................................................................................................................... [1] (iv) Solid cobalt conducts electricity. It melts at 1495oC. ......................................................................................................................................................................... [1] (v) A solution of calcium nitrate in water conducts electricity. Solid calcium nitrate melts at 561oC. ......................................................................................................................................................................... [1]

(Continued...)

Is the substance a solid?

Does it melt at a low temperature?

Does it conduct electricity when

molten or dissolved in

water?

simple molecular

Does it melt at a low temperature?

Does it conduct electricity when

solid?

giant atomic

giant metallic

giant ionic

no

yes

yes

yes

no

no

no

yes

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

QUESTIONSHEET 13 CONTINUED (b) Carbon dioxide has a simple molecular structure. What does this tell you about its melting point and boiling point? ......................................................................................................................................................................... [1] (c) Draw a diagram to show the structure of cobalt.

[2]

TOTAL / 8

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING Medium Demand Questions QUESTIONSHEET 14 The table below shows the electronic arrangements of six atoms, A to F.

atom A B C D E F

electronic arrangement 2, 8, 6 2, 8, 8 2, 8, 3 2 2, 8, 8, 6 2, 5

Use the letters representing the atoms to select the following: (a) Two atoms from the same group of the periodic table .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) The ion K+ ......................................................................................................................................................................... [1] (c) Two noble gases. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) An atom which has 3 electrons in its outside shell. ......................................................................................................................................................................... [1] (e) An atom which has 5 electrons in its outside shell. ......................................................................................................................................................................... [1] (f) An atom with the atomic number 24. ......................................................................................................................................................................... [1] (g) An atom with 7 protons. ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Medium Demand Questions QUESTIONSHEET 15 The diagrams below show the structures of ethanol, mica and diamond. (a) How many bonds does each carbon have in: (i) ethanol? ......................................................................................................................................................................... [1] (ii) diamond? ......................................................................................................................................................................... [1] (b) How many bonds does each hydrogen have in ethanol? ......................................................................................................................................................................... [1] (c) (i) How many bonds does each silicon have in mica? ......................................................................................................................................................................... [1] (ii) How many bonds does each oxygen have in mica? ......................................................................................................................................................................... [1] (d) (i) Which of the elements, carbon, hydrogen, oxygen and silicon would you expect to find in the same group of the Period Table? ......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

H

H H

C C O

H H

H O

O Si

O

O

O

O Si

O

O

O Si

O

O

O Si O

O

O Si

O

O Si

Mica Ethanol Diamond

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Medium Demand Questions QUESTIONSHEET 16 (a) The diagram below shows an atom of magnesium. (i) What is the name of part A? ......................................................................................................................................................................... [1] (ii) What two types of particle does part A contain? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What is the charge on part A? ......................................................................................................................................................................... [1] (b)(i) How many electrons are in one atom of magnesium? ......................................................................................................................................................................... [1] (ii) Write the electron arrangement for an atom of magnesium. ......................................................................................................................................................................... [1] (c) Use the diagram and your answer to part (b) to answer the following questions. (i) In what group of the Periodic Table is magnesium? ......................................................................................................................................................................... [1] Explain your answer. ......................................................................................................................................................................... [1] (ii) In what period of the Periodic Table is magnesium? ......................................................................................................................................................................... [1] Explain your answer. ......................................................................................................................................................................... [1]

TOTAL / 10

electron

PART A

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Low Demand Questions QUESTIONSHEET 17 Oxygen is able to form two bonds with other elements. Potassium can form one bond, magnesium two and aluminium three. (a) Work out the formulae of the following compounds. (i) potassium oxide ......................................................................................................................................................................... [1] (ii) magnesium oxide ......................................................................................................................................................................... [1] (iii) aluminium oxide ......................................................................................................................................................................... [1] (b) Iron sometimes forms two bonds and sometimes three. (i) Work out the formulae of the two oxides of iron. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) How are the two oxides of iron distinguished in their names? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 6

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING Low Demand Questions QUESTIONSHEET 18 Here are the formulae of three compounds containing sodium. (i) NaCl (ii) Na2SO4 (iii) NaHCO3 (a) Give the name of each compound. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) (i) Which compound is made up of the most atoms? ......................................................................................................................................................................... [1] (ii) How many atoms does it contain? ......................................................................................................................................................................... [1] (c)(i) Which compound has the most different types of atoms? ......................................................................................................................................................................... [1] (ii) List the types of atom in this compound. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING

Low Demand Questions QUESTIONSHEET 19 Complete the following paragraphs about atoms. Atoms are the ________ particles of matter that can exist on their own. They are made up of particles called protons, ________ and electrons. Protons have a ________ charge and electrons have a _________ charge. The protons are found in the _______ of the atom. In a neutral atom, the number of protons must _________ the number of electrons. If they do not, the particle will be called an _______. The number of protons in an atom is called its ________ ________. The total number of particles in the nucleus gives the ________ ________ of the element. The atoms of different elements are _________. They must contain different numbers of ________ and ________, although they may have the same number of ________.

TOTAL / 13

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING Low Demand Questions QUESTIONSHEET 20 Complete the following table

Name of element neon sodium carbon

symbol Mg N

mass number 20 24 14

atomic number 10 11 7 6

number of neutrons 12 12 7 6

[9]

TOTAL / 10

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GCSE CHEMISTRY ENERGETICS

High Demand Questions QUESTIONSHEET 1 A gas barbecue uses butane (C4H10) as a fuel. The butane is stored as a liquid in a container. When the burner is turned on, the liquid turns to a gas and is lit by pushing a button to create a small spark. (a) Suggest one advantage and one disadvantage of using butane compared to charcoal as a source of heat. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Describe the arrangement and movement of molecules in butane when it is: (i) a liquid .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) a gas .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) What term is used to describe the change of state from liquid to gas? ......................................................................................................................................................................... [1] (d)(i) Draw a diagram to show the structural arrangement of the atoms in a molecule of butane.

[2] (ii) How does the structure of butane explain why it has a low boiling point? ......................................................................................................................................................................... [1] (e) Explain why a spark is needed to start the butane burning. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 12

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GCSE CHEMISTRY ENERGETICS High Demand Questions QUESTIONSHEET 2 Fuel cells are often taken into space to supply energy. They turn the energy of a fuel directly into electricity. (a) (i) Why are porous electrodes needed in a fuel cell? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Why is nickel included in the electrodes? ......................................................................................................................................................................... [1] (b) What is the main way in which fuel cells differ from other electrochemical cells? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) Write an equation for the overall reaction taking place in a fuel cell. ......................................................................................................................................................................... [2] (d) Give two reasons why fuel cells are more suitable than dry cells for use in spacecrafts. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) What other type of cell could be used in a spacecraft? ......................................................................................................................................................................... [1]

TOTAL / 8

steam

oxygen hydrogen

hot potassium hydroxide solution

porous carbon containing

nickel

FUEL CELL

+ -

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GCSE CHEMISTRY ENERGETICS

High Demand Questions QUESTIONSHEET 3 A bomb calorimeter is used to burn small, weighed samples of fuels in an atmosphere of oxygen. The energy produced is transferred to the surrounding water. The fuels are electrically ignited. A bomb calorimeter is often used to find the energy values of foods. (a) (i) What is the advantage of burning the fuel in oxygen rather than in air? ......................................................................................................................................................................... [1] (ii) What is the advantage of surrounding the bomb calorimeter with water? ......................................................................................................................................................................... [1] (b) A bomb calorimeter was used to measure the energy value of glucose. When 2 g of glucose was burned, 31 200 J of energy were released. (i) Complete the equation for the combustion of glucose. C6H12O6 + 6O2 ∏ + [2] (ii) Calculate the energy value of glucose in kJ per 100 g. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 6

thermometer

water

fuel oxygen

stirrer

BOMB CALORIMETER

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GCSE CHEMISTRY ENERGETICS High Demand Questions QUESTIONSHEET 4 (a) Cold packs are used to treat sports injuries. A pack contains water and ammonium nitrate crystals. When mixed, rapid cooling takes place. (i) Draw an energy level diagram to show the process occurring in the cold pack. Explain your diagram. [3] (ii) Explain in terms of bonding why this process takes in heat. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) A company has recently invented ‘cook-in-the-box’ meals. To start the cooking process a tab is pulled which lights a match. The match starts a reaction which continues without further heating.

A reaction which could be used is that between aluminium and iron(III) oxide, to produce aluminium oxide and iron.

(i) Write a symbol equation for the reaction between aluminium and iron(III) oxide. ......................................................................................................................................................................... [2] (ii) Explain why the match is needed to start the reaction, but once started it continues without further

heating. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY ENERGETICS

High Demand Questions QUESTIONSHEET 5 A Sumo wrestler eats more than 7 kg of steak every day, together with fresh vegetables. An Olympic rower’s lunch would be something like 350 g steak, vegetables, treacle pudding and unsweetened lemon juice. (a) Why does the rower eat treacle pudding, but the sumo wrestler does not? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) In view of your answer to (a), why is the rower’s lemon juice unsweetened? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 4

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GCSE CHEMISTRY ENERGETICS High Demand Questions QUESTIONSHEET 6 When hydrogen reacts with iodine, we can show the reaction as follows: H – H + I – I 2 (H – I) (a) Given the following bond energies, calculate the heat of reaction. (H – H = 436 kJ, I – I = 151 kJ, H – I = 298kJ) .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) Is the reaction exothermic or endothermic? ......................................................................................................................................................................... [1] (c) Draw an energy level diagram for the reaction. [3]

TOTAL / 7

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GCSE CHEMISTRY ENERGETICS

High Demand Questions QUESTIONSHEET 7 When 10 cm3 of 0.1M hydrochloric acid reacts with 10 cm3 of 0.1M sodium hydroxide solution, the temperature rises from 20°C to 35°C. (a) Use the formula

heat energy = 4.2 5 temperature change 5 mass of reactants (in grams) to calculate the energy in kilojoules from the reaction. The density of both dilute hydrochloric acid and sodium hydroxide is 1g/cm3.

.............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) How many moles of 0.1M hydrochloric acid are in 10 cm3 of 0.1 M solution? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Write a symbol equation for the reaction between hydrochloric acid and sodium hydroxide. ......................................................................................................................................................................... [1] (d) How much energy would you get by reacting 1 mole of hydrochloric acid? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY ENERGETICS High Demand Questions QUESTIONSHEET 8 The reactions between bromine (Br2) and hydrogen (H2) to make hydrogen bromine (HBr) can be represented by the following equation: Br-Br + H-H ∏ H-Br +H-Br (a) Use the following bond energies to answer questions (i), (ii) and (iii). Br-Br: 193 kJ/mol; H-H: 436 kJ/mol; H-Br: 366 kJ/mol (i) Calculate the total energy required to break bonds in this reaction.

.............................................................................................................................................................................. .............................................................................................................................................................................. Answer ............................................................................................................................................ kJ/mol

[2]

(ii) Calculate the total energy released when bonds are formed in this reaction.

.............................................................................................................................................................................. .............................................................................................................................................................................. Answer ............................................................................................................................................ kJ/mol

[2]

(iii) Calculate the overall energy change for this reaction.

.............................................................................................................................................................................. ..............................................................................................................................................................................

Answer ............................................................................................................................................ kJ/mol

[2] (b) Explain what the sign of the answer you calculated in (a) part (iii) tells you about the reaction. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) Below is the energy level diagram for the reaction between hydrogen and bromine.

Write down the letter which represents the activation energy ......................................................................................................................................................................... [1]

TOTAL / 8

a b

c

d

reaction path

energy

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 9 Lucy was trying to compare the amount of energy released when three different alcohols were burned. She used the apparatus shown below. (a) Lucy weighed the burner before and after burning the alcohols. She stirred the water throughout. (i) Explain why she weighed the burner before and after. ......................................................................................................................................................................... [1]

(ii) Why did Lucy stir the water? ......................................................................................................................................................................... [1] (iii) What else would Lucy need to measure before and after burning the alcohol? ......................................................................................................................................................................... [1] (iv) What two things would Lucy need to keep the same if she was to make a fair comparison between the alcohols? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Lucy calculated the temperature rise for each gram of alcohol which was burned.

alcohol temperature rise

mass burned

temperature rise per gram burned

methanol 16oC 2 g 8oC/g

ethanol 33oC 3 g 11oC/g

propanol 48oC 4 g

(i) Complete the table. [1] (ii) Which alcohol releases the most energy per gram? Suggest an explanation. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

beaker

water

alcohol burner

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 10 When a small piece of calcium is added to water in a beaker a reaction occurs. (a) What would you observe? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) 50 cm3 of water was heated from 20°C to 25°C in the reaction. (heat energy = 4.2 × temperature change × mass of water in grams) (i) Calculate the energy given off. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Is the reaction exothermic or endothermic? ......................................................................................................................................................................... [1] (c) Write the equation (symbols) for the reaction between calcium and water. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 11 (a) When the fuel methane is burnt in a Bunsen burner heat energy is released to the surroundings. The amount of heat given out from the Bunsen burner is controlled by the position of the air hole. (i) Is the flame of a Bunsen burner hottest when the air hole is closed or open? ......................................................................................................................................................................... [1] (ii) Explain your answer to part (i). ......................................................................................................................................................................... [1] (b) Methane is a part of a group of chemicals called hydrocarbons. (i) Which two elements do hydrocarbons contain? 1. ................................................................................................................................................................ 2. ................................................................................................................................................................

[2] (ii) When any hydrocarbon burns which two chemical compounds are formed? 1. ................................................................................................................................................................ 2. ................................................................................................................................................................

[2] (c) The methane does not burn until it is lit by a naked flame. The energy supplied by the flame is called

activation energy. (i) Explain what is meant by the term ‘activation energy’. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) The rate of some chemical reactions can be increased by using a catalyst. Use the idea of activation energy to explain how a catalyst works. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 12 The following experiment was used to compare how much heat energy three different fuels gave out when they were burnt. (a) Here are the results when 1.0 g of each fuel was burnt.

fuel temperature of water at start temperature of water at end ethanol 19oC 36oC paraffin 20oC 47oC

white spirit 18oC 41oC (i) Are the reactions exothermic or endothermic? .............................................................................................................................................................................. Explain your answer. ......................................................................................................................................................................... [2] (ii) What was the temperature change when 1.0 g of ethanol was burnt? ......................................................................................................................................................................... [1] (iii) Which fuel released the most energy when it was burnt? ......................................................................................................................................................................... [1] (iv) Why it is important to burn 1.0 g of each fuel in each experiment? ......................................................................................................................................................................... [1] (b) When fuels burn they react with a gas in the air. Write down the name of this gas. ......................................................................................................................................................................... [1] (c) When ethanol burns in excess air, carbon dioxide is released into the atmosphere. Describe one problem that this may cause in the environment. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) When ethanol burns in a shortage of air another gas is formed which is highly toxic. Write down the name of this toxic gas. ......................................................................................................................................................................... [1]

TOTAL / 9

thermometer

spirit burner 100 g water

metal can

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 13 Look at the diagram. It shows the apparatus used to calculate the energy released when fuel is burnt.

The table below shows the results when 1.0 g of each fuel is burnt.

fuel temperature of water at start temperature of water at end ethanol 20oC 40oC paraffin 19oC 58oC petrol 21oC 42oC

(a) Which fuel released the least amount of heat energy? .............................................................................................................................................................................. Explain your answer ......................................................................................................................................................................... [2] (b) Why is it important for there to be 100 g of water in the metal can for each reaction? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Calculate the energy transferred when 2.0 g of paraffin burns. (The specific heat capacity of water is 4.2 J g-1 K-1) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 7

thermometer

spirit burner 100 g water

metal can

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GCSE CHEMISTRY ENERGETICS Medium Demand Questions QUESTIONSHEET 14 The following diagram represents the energy level diagram for the reaction between magnesium (Mg) and oxygen (O2) to form magnesium oxide (MgO).

(a) On the energy level diagram write the words reactants and products in the correct places. [1] (b) Indicate on the energy level diagram the activation energy. [1] (c) The reaction between magnesium and oxygen may be represented by the following symbol equation: 2Mg + O2 → 2MgO (i) Calculate the mass of magnesium required to produce 100 g of magnesium oxide. (Relative atomic masses: O = 16, Mg = 24) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) It is known that 32 g of oxygen takes up 24 dm3 of space at 25oC. Calculate the volume of oxygen that is needed to react completely with 12 g of magnesium. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 8

energy

reaction path

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 15 (a) In the laboratory a Bunsen burner is used as a heat source. The gas which is burnt in a Bunsen burner is called methane. (i) When methane is burnt heat energy is released into the surroundings. What name is given to this type of

reaction? ......................................................................................................................................................................... [1] (ii) Methane is called a non-renewable fuel. Explain what is meant by a non-renewable fuel. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Name two fuels which are renewable. 1. ........................................................................................................................................................... [1] 2. ........................................................................................................................................................... [1] (b) The reaction between methane (CH4) and oxygen (O2) which takes place during burning produces carbon dioxide (CO2) and water (H2O). It may be represented using the following display formulae. O=O H-O-H + O=C=O + O=O H-O-H (i) Name two different bonds which are broken during the reaction. 1. ........................................................................................................................................................... [1] 2. ........................................................................................................................................................... [1] (ii) Which two bonds are made during the reaction? 1. ........................................................................................................................................................... [1] 2............................................................................................................................................................. [1] (iii) Calculate the overall energy change for the reaction between methane and oxygen. The bond energies are C-H: 435 kJ, O=O: 497 kJ, C=O: 803 kJ, H-O: 464 kJ) .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4]

TOTAL / 13

H

H

H

H

C

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GCSE CHEMISTRY ENERGETICS

Medium Demand Questions QUESTIONSHEET 16 The equipment below was used to measure the temperature change when the metal zinc was placed into sulphuric acid. During the reaction heat energy is transferred to the surroundings. (a) What would you see happen to the reading on the thermometer during the experiment? ......................................................................................................................................................................... [1] (b) The experiment was repeated but this time a catalyst was also added. (i) Explain what a catalyst is. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) What would you see happen to the reading on the thermometer during this second experiment? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 5

thermometer

glass beaker

sulphuric acid zinc

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GCSE CHEMISTRY ENERGETICS

Low Demand Questions QUESTIONSHEET 17 The temperatures of reactions of zinc, magnesium and nickel with hydrochloric acid were measured. The results are shown in the table.

metal Temp at start oC Highest temp reached oC

Temp change oC

nickel 19 24 5 magnesium 19 57

zinc 19 30 11 (a)(i) What piece of equipment would you use to measure the temperature? ......................................................................................................................................................................... [1] (ii) Calculate the temperature change for the magnesium reaction. ......................................................................................................................................................................... [1] (iii) Calcium is more reactive than zinc. Predict the temperature change for a reaction between calcium and hydrochloric acid. ......................................................................................................................................................................... [1] (b) What name is given to reactions which give out heat? ......................................................................................................................................................................... [1] (c) (i) Suggest another reaction which would give out heat. ......................................................................................................................................................................... [1] (ii) Why are reactions which give out heat useful? ......................................................................................................................................................................... [1] (iii) Why are reactions which take in heat useful? ......................................................................................................................................................................... [1]

TOTAL / 7

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GCSE CHEMISTRY ENERGETICS

Low Demand Questions QUESTIONSHEET 18 A person’s daily energy requirements depend on a number of things. These include the person’s sex and size. (a) Name two more things which could affect your energy requirements. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) For breakfast a man eats the following bowl of cereal 325 J bacon 1430 J egg 660 J tea (with sugar) 200 J How much energy in total does he get from his breakfast? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) An Indian farmer consumes 7200 J per day. The man described above consumes 20 000 J per day. (i) How would you expect the man and the farmer to differ in appearance? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Why is the farmer often very tired? ......................................................................................................................................................................... [1] (iii) Suggest two things that the man could do to lose weight. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY ENERGETICS

Low Demand Questions QUESTIONSHEET 19 A modern power station uses powdered coal. A blast of air is passed up through the burning coal. This is more efficient and produces less harmful gases than large pieces of coal. (a) Why does powdered coal burn more efficiently? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Sometimes the powdered coal is blown into a flame. Why is this better? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Using oxygen instead of air speeds up the burning process. Explain the reason for this. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Name two gases which may form when coal is burned. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY ENERGETICS

Low Demand Questions QUESTIONSHEET 20 (a) List three characteristics of an ideal fuel. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b)(i) Describe an experiment to compare paraffin and alcohol as fuels. Mention all the measurements you would make. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4] (ii) Why would it be difficult to compare coal using the same method? ......................................................................................................................................................................... [1] (iii) Why is it difficult to compare methane gas using the same method? ......................................................................................................................................................................... [1] (c) George compared two fuels and came up with the following results. Fuel A produces 1500 kJ Fuel B produces 790 kJ Why are these results of very little use? ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 1 Since 1900 it has been known that substances containing nitrogen increase the yield of crops. European countries imported large quantities of sodium nitrate (NaNO3) from Chile. This nitrate was a non-renewable resource. (a) Name the group of chemicals that plants make from nitrate fertilisers. ......................................................................................................................................................................... [1] (b) What is meant by the term ‘non-renewable’. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c)(i) Calculate the relative molecular mass of sodium nitrate. The relative atomic masses of N = 14, O = 16, and Na = 23. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Calculate the percentage of nitrogen in sodium nitrate. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Today nitrate fertilisers are made by first making ammonia gas from nitrogen and hydrogen. (i) Name the raw material used as a source of nitrogen. ......................................................................................................................................................................... [1] (ii) Name a raw material used as a source of hydrogen. ......................................................................................................................................................................... [1] (e) Ammonia is made by passing a mixture of nitrogen and hydrogen over finely divided iron metal. (i) What is the purpose of the iron? ......................................................................................................................................................................... [1] (ii) Explain why the iron used is finely divided. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 1 CONTINUED (f) A solid fertiliser is made by dissolving ammonia gas in water. Ammonia solution is then reacted with an acid. Name the acid you would react with ammonia to make ammonium sulphate. ......................................................................................................................................................................... [1] (g) Overuse of nitrate fertilisers can be harmful. They can cause eutrophication in lakes and rivers. Explain what happens in the eutrophication process. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4]

TOTAL / 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 2 National Quicklime is a company that is involved in the quarrying of limestone. They propose to open a new limestone quarry in the Peak District National Park. The proposed site is well known as an area of outstanding natural beauty. (a) Give three reasons in favour of opening the quarry. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) Give three reasons against the opening of the quarry. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) The limestone (calcium carbonate) will be used to make quicklime (calcium oxide). The equation for the reaction is given below: CaCO3(s) → CaO(s) + CO2 (g) (i) What do the symbols (s) and (g) mean? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Calculate the relative molecular masses of calcium carbonate, calcium oxide, and carbon dioxide. (relative atomic masses C=12, O=16, Ca= 40) .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

(Continued...)

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 2 CONTINUED (d) The company wants to produce 1,680 tonnes of quicklime per week. (i) Calculate the minimum mass of limestone needed to produce 1,680 tonnes of quicklime. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Suggest a reason why more than the minimum mass you have calculated would have to be heated to obtain 1,680 tonnes of quicklime. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) Give another use of limestone. ......................................................................................................................................................................... [1]

TOTAL / 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 3 Chlorine is manufactured by the electrolysis of sodium chloride solution. A simple electrolysis cell that can be used in the laboratory is shown below. (a) Label the anode on the diagram. [1] (b) How would you prove that the gas collected was chlorine? Test ......................................................................................................................................................................... [1] Result ......................................................................................................................................................................... [1] (c) Give one important use of chlorine. ......................................................................................................................................................................... [1] (d) Complete the ionic equation showing the formation of chlorine gas. ___ Cl − → ______ + ______ [1] (e) Name the other gas formed in the electrolysis of salt solution. ......................................................................................................................................................................... [1] (f) After running the cell for several minutes, some Universal Indicator was added to the cell. The indicator turned blue. (i) What does this test show? ......................................................................................................................................................................... [1] (ii) Give the chemical name of the substance formed that turns the indicator blue. ......................................................................................................................................................................... [1]

(Continued...)

sodium chloride solution

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 3 CONTINUED (g) Some students decided to investigate how changing some of the factors in the experiment would affect the amount of chlorine produced. John made the following prediction: 'more chlorine will be produced if the concentration of sodium chloride solution is increased.' Describe how the students could use this apparatus to test their prediction. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [5] (h) Suggest two other changes that John could investigate to see if they affected the amount of chlorine produced. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 4 Aluminium is obtained from bauxite. Bauxite is purified to form aluminium oxide. (a) Write down the formulae of the ions present in aluminium oxide. aluminium ion _______________ oxide ion _________________ [2] (b) Aluminium oxide is mixed with cryolite before being placed in the cell. What is the function of the cryolite? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) Explain why the electrolyte has to be molten in order to conduct electricity. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) A typical cell is shown below. (i) Aluminium ions are attracted to the cathode. Write an equation to show how aluminium ions are changed into atoms. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Explain what happens to the oxide ions. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

(Continued...)

+ -

cathode

carbon anode

Electrolyte - mixture of

aluminium oxide and cryolite

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 4 CONTINUED (e) Extraction of aluminium from its ore uses electricity. Iron can be extracted from its ore by heating with carbon. Gold is found occuring naturally. Explain why these three metals have such different ways of extracting them. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) The graph below shows the production of bauxite ore, purified aluminium oxide and aluminium metal from three different countries. (i) Which country has no deposits of bauxite? ......................................................................................................................................................................... [1] (ii) Suggest two reasons why Jamaica produces little aluminium metal, despite mining large quantities of bauxite. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 14

bauxite ore purified aluminium oxide

aluminium metal

5

10

15

20

Australia Jamaica United Kingdom

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 5 Many power stations burn coal as their source of energy. Coal mainly consists of the element carbon. (a) Write a symbol equation for the burning of carbon in a good supply of air. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) Coal also contains small amounts of sulphur. The sulphur burns to form sulphur dioxide gas. Explain how sulphur dioxide causes pollution and how this harms trees. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) One method of preventing this pollution is to remove sulphur dioxide gas before it escapes into the air.

This can be done by reacting the gas with calcium oxide in the power station chimney. The equation for the reaction is shown below: CaO + SO2 CaSO3 (i) Give the name used to describe this type of reaction. ......................................................................................................................................................................... [1] (ii) Calculate the relative molecular masses of: CaO [1] SO2 [1] (Relative atomic masses: O = 16, S = 32, Ca = 40) (iii) A power station produces 32 tonnes of sulphur dioxide in one day. Calculate the minimum mass of calcium oxide needed to absorb 32 tonnes of sulphur dioxide. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 5 CONTINUED (iv) Give two reasons why a greater mass of calcium oxide would be needed in practice. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Another method is to remove the sulphur from coal before it is burnt. The sulphur may be used in the contact process. Sulphur dioxide reacts with oxygen as shown in the equation below: 2SO2 + O2 � 2SO3 (i) What does the symbol � mean? ......................................................................................................................................................................... [1] (ii) Name the product formed in this reaction. ......................................................................................................................................................................... [1] (iii) Name the major chemical formed in the contact process. ......................................................................................................................................................................... [1]

TOTAL / 14

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

High Demand Questions QUESTIONSHEET 6 (a) Sulphuric acid is made from sulphur by the contact process. Sulphur is burned to form sulphur dioxide. This is then changed to sulphur trioxide by reacting it with more oxygen. A catalyst is used in this stage of the process. 2SO2 + O2 2SO3 energy released = -189 kJ The reverse reaction is 2SO3 2SO2 + O2 What is the energy change for this reaction? ......................................................................................................................................................................... [1] (b) A catalyst is used because it lowers the activation energy. (i) What is meant by activation energy? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Label the activation energy on the energy level diagram for the formation of sulphur trioxide. [1] (iii) What effect does a catalyst have by lowering the activation energy? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

2SO3

2SO2 + O2

Time

Energy

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 6 CONTINUED (c) The percentage conversion of sulphur dioxide varies with the temperature. This is shown in the graph below: (i) Use the graph to find the percentage of sulphur trioxide produced at a temperature of 575oC. ......................................................................................................................................................................... [1] (ii) Calculate the amount of sulphur dioxide converted when 300 tonnes of sulphur dioxide ar reacted with oxygen at 575oC. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Running the process at 300 oC has the advantage of 100% conversion. Suggest one disadvantage of operating at this temperature. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

% conversion

of SO2 to SO3

300 400 500 600 700 800 0

20

40

60

80

100

Temperature / oC

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QUESTIONSHEET 6 CONTINUED

(d) Sulphur trioxide is mixed with concentrated sulphuric acid to form oleum, H2S2O7. The oleum is diluted to produce more sulphuric acid. (i) Give the symbol equation for this reaction. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Explain why the oleum is not added directly to water to form sulphuric acid. ......................................................................................................................................................................... [1] (e) The catalyst used contains vanadium. (i) Name the block of the Periodic Table to which vanadium belongs. ......................................................................................................................................................................... [1] (ii) Vanadium is a very expensive metal. Explain why, despite the high cost, it can be used in this process. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 13

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High Demand Questions QUESTIONSHEET 7 The world produces close to 10 million tonnes of copper each year. Copper pyrites is one of the main ores of copper. The ore contains the elements copper and sulphur. To extract the copper the ore is crushed and concentrated. The concentrated ore is roasted in air to separate the copper from the sulphur. The sulphur reacts with air to form sulphur dioxide gas. (a) Explain why the ore needs to be concentrated. ......................................................................................................................................................................... [1] (b) Explain why it is important that the sulphur dioxide gas is not allowed to escape into the atmosphere. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Sulphur dioxide may be used to make sulphuric acid. Outline the major stages in this industrial process. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (d) The copper formed is called blister copper and is impure. Copper is purified by electrolysis. A diagram of the process is shown below.

(Continued...)

+- ANODE CATHODE

copper

copper sulphate solution

blister copper

‘anode slime’

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

QUESTIONSHEET 7 CONTINUED (i) Use the diagram to explain how the impure copper is purified. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) Complete the symbol equation for the reaction at the cathode. Cu2+ + ______ → Cu [1] (iii) The reaction at the cathode is an example of 'reduction'. Explain this term by using this reaction as an example. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) What is the importance of the 'anode slime' in paying for this expensive process. ......................................................................................................................................................................... [1] (e) In the periodic table copper is a transition element. It is used in wiring as it is a good conductor of electricity. Give two other properties of transition elements. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 15

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High Demand Questions QUESTIONSHEET 8 (a) The table below shows the percentage and the boiling point of the three main elements in liquid air.

Element Percentage Boiling point (oC) argon -186

nitrogen 78.04 % -196 oxygen 20.93% -183

(i) Complete the table. [1] (ii) Name the gas with the highest boiling point ............................................................................... [1] (b) The following diagram shows the fractionating column for separating liquid air into argon, nitrogen and oxygen. (i) Name this method of separation .............................................................................................................. [1] (ii) Name A. ................................................................................................................................................... [1] (iii) Name B. ................................................................................................................................................... [1] (c) Name two gases which are present in the atmosphere but not in liquid air. ........................................................... and ........................................................ [2] (d) Give one use of (i) argon ......................................................................................................................................................................... [1] (ii) nitrogen ......................................................................................................................................................................... [1] (e) Explain how oxygen is used in the steel industry. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11

A

B

nitrogen

liquid air at 200 oC

well insulated fractionating

column

perforated shelves

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 9 The diagram below shows part of the process in which nitric acid is formed from ammonia. (a) Which raw material is used to obtain oxygen? ......................................................................................................................................................................... [1] (b) Write down the formulas for the following substances: (i) nitrogen monoxide ________________ (ii) oxygen ________________ (iii) nitrogen dioxide ________________ [3] (c) Name the catalyst used in this process. ......................................................................................................................................................................... [1] (d) What information given in the diagram suggests that nitrogen monoxide is insoluble in water? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) Explain how nitrogen dioxide is converted into nitric acid. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) The nitric acid formed may be used to make ammonium nitrate fertiliser. (i) What substance is added to nitric acid to form ammonium nitrate? ......................................................................................................................................................................... [1] (ii) What type of reaction takes place when ammonium nitrate is formed? ......................................................................................................................................................................... [1]

(Continued...)

nitrogen monoxide + oxygen

nitrogen dioxide

oxygen

ammonia hot platinum

gauze gases cooled using water

∧ ∧

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 9 CONTINUED (iii) Explain why nitrate fertilisers are used. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) A bag of garden fertiliser has the label 'N:P:K 10:0:5’ Explain what this information means. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 10 The Haber process is used to manufacture ammonia. Nitrogen gas and hydrogen gas react with each other in the presence of a catalyst. (a) Name the catalyst used in the Haber process. ......................................................................................................................................................................... [1] (b) Balance the following equation for the reaction N2 + ____ H2 � ____ NH3 [2] (c) This is a reversible reaction. Explain what is meant by the term ‘reversible reaction’. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (d) The graph below shows the percentage yield of ammonia at different temperatures and pressures.

(Continued...)

100 200 300 400 500

20

40

60

80

100

pressure/atmosphere

% yield of

ammonia

300o C

500o C

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 10 CONTINUED (i) Use the graph to complete the following sentences: The percentage of ammonia __________ as the pressure increases. The percentage of ammonia __________ as the temperature increases. [2] (ii) Use the graph to find the conditions required to give a yield of 60% ammonia. temperature __________oC pressure __________ atmospheres [1] (iii) On the graph draw the line you would expect showing the percentage yield of ammonia for a temperature of 350oC. [1] (e) Pressures greater than 500 atmospheres increase the yield of ammonia. Suggest two reasons why very high pressures of above 500 atm are not used. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) Temperatures lower than 300oC often give a yield of 100% of ammonia. Suggest a reason why very low temperatures of less than 300oC are not used. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (g) After reacting the gases with the catalyst a mixture of unreacted nitrogen, unreacted hydrogen and ammonia is formed. The boiling points of these three gases are given in the table below.

gas boiling point (oC) ammonia -33 hydrogen -252 nitrogen -196

Use the information to suggest a method for extracting the ammonia. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (h) What happens to the nitrogen and hydrogen that leave the process unreacted? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 14

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 11 Iron is extracted from its ore in a blast furnace. The raw materials are iron ore, limestone, carbon, and hot air. (a) Name one ore of iron. ......................................................................................................................................................................... [1] (b) The iron ore is reduced using carbon monoxide. (i) Explain how carbon monoxide is formed in the blast furnace. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) What is meant by the term 'reduced'? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) The limestone (CaCO3) is heated to a high temperature and it decomposes. (i) Write a symbol equation for the decomposition of limestone. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Explain the reason for adding limestone to the furnace. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (d) Name the two liquids that are tapped off from the furnace. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) The furnace runs for 24 hours a day. Suggest one problem caused by these operating conditions. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 11 CONTINUED (f) Discuss the factors that would influence the choice of a site for a new blast furnace. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (g) The iron formed is used to make alloys. Name and give a use of an alloy containing iron. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 12 Aluminium metal is extracted from its ore, bauxite. Impurities such as iron(III) oxide and silicon oxide have to be removed. The purified bauxite is mainly aluminium oxide. Aluminium oxide solid is added to the electrolysis cell. bauxite aluminium oxide aluminium (4 tonnes) (2 tonnes) (1 tonne) The cell requires a current of 100,000 amps and reaches a temperature of 1000oC. In Scotland, aluminium is made near to hydroelectric power plants. (a) Suggest two reasons why the extraction of aluminium is an expensive process. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Describe three environmental problems which could be caused by an increase in the demand for products made from aluminium. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) A typical electrolysis cell is shown below: (i) Label the following on the diagram: anode, cathode, electrolyte, aluminium metal [3]

(Continued...)

+ -

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 12 CONTINUED (ii) Explain why the carbon anodes have to be replaced. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) The following reactions take place at the electrodes: Al3+ + 3e- Al 2O2- O2 + 4e-

(i) Which reaction takes place at the cathode? ......................................................................................................................................................................... [1] (ii) In a day 320 tonnes of oxygen gas are formed. How much aluminium metal will be formed in this time? (relative atomic masses: O = 16, Al = 27) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 14

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 13 Sulphuric acid, H2SO4 is made by a method called the contact process. A flow diagram for that process is shown in the following diagram. (i) Name gas G. ......................................................................................................................................................................... [1] (ii) Name catalyst C. ......................................................................................................................................................................... [1] (iii) Name liquid L. ......................................................................................................................................................................... [1] (iv) Complete the symbol equation for the sulphur burning in air.

S (....) + .......(g) ς SO2 (......) [2] (v) Explain the importance of not allowing any of the sulphur dioxide to escape into the atmosphere. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (vi) Name all the elements present in oleum, H2S2O7. ......................................................................................................................................................................... [1]

(Continued...)

gas G

sulphur sulphur dioxide

sulphur trioxide

oleum H2S2O7

concentrated sulphuric

acid

400-500oC catalyst C

burnt in

air

dissolved in concentrated

sulphuric acid

dissolved in concentrated

sulphuric acid

add liquid L

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GCSE CHEMISTRY INDUSTRIAL PROCESSES QUESTIONSHEET 13 CONTINUED (vii) Sulphur dioxide reacts with water to form sulphuric acid:

SO3 + H2O ς H2SO4

Explain why this is never done in the contact process. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (viii) Give one industrial use of sulphuric acid. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

TOTAL / 9 Medium Demand Questions QUESTIONSHEET 14 Ammonia is manufactured by the Haber process where nitrogen is reacted with hydrogen by passing the mixture over iron at certain conditions. (a) (i) Complete and balance the equation

......(g) + .......H2(g) � ...... NH3 (g) [2] (ii) Explain why the mixture is passed over iron.

.............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iii) State how heat affects the speed of the reaction between the two reactants - nitrogen and hydrogen. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) The graph below shows the effect of temperature and pressure on the yield of ammonia produced during its manufacture (i) State what happens to the yield of ammonia when: the pressure increases. ......................................................................................................................................................................... [1] the temperature increases. ......................................................................................................................................................................... [1] (ii) The graph shows the highest yield of ammonia can be obtained by using a pressure of 500 atmospheres. Give one reason why this condition is not normally used in industry. ......................................................................................................................................................................... [1]

0 100 200 300 400 500 0

10

20

30

40

50

60

70

80

350oC

450oC

550oC

Percentages yield of ammonia

Pressure (in atmospheres)

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

(Continued...) QUESTIONSHEET 14 CONTINUED (c) One of the main uses of ammonia is to manufacture nitrogenous fertilisers such as ammonium sulphate. Name the substance that is used to neutralise ammonia to make this fertiliser. ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

Medium Demand Questions QUESTIONSHEET 15 The diagram below shows a blast furnace which is used for the extraction of iron from iron ore. (a) (i) One of the raw materials fed in at the top of the blast furnace is iron ore , which is mainly iron(III) oxide. Name the other two raw materials. 1. ................................................................ II. ................................................................ [2] (ii) Name the substance which is formed at A. ......................................................................................................................................................................... [1] (b) One of the main reactions taking place inside the blast furnace is Fe2O3 + 3CO → 2Fe + 3CO2

(i) Name the reducing agent in this equation. ......................................................................................................................................................................... [1] (ii) Calculate the relative molecular mass (Mr) of iron(III) oxide, Fe2O3. Ar (Fe) =56 Ar (O) = 16 .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

raw materials

waste gases

hot air

molten iron

hot air

A

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GCSE CHEMISTRY INDUSTRIAL PROCESSES

(Continued...)

QUESTIONSHEET 15 CONTINUED (iii) Use the given equation to calculate the mass of iron formed from 320 tonnes of iron(lIl) oxide.

.............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

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TOTAL / 8

Medium Demand Questions QUESTIONSHEET 16 Aluminium is extracted by the electrolysis of molten aluminium oxide (dissolved in molten cryolite). It is an expensive metal to produce. (a) (i) Give one reason why aluminium is expensive to make. ......................................................................................................................................................................... [1] (ii) State what is meant by the term electrolysis. ......................................................................................................................................................................... [1] (iii) Explain the reason why aluminium oxide is dissolved in molten cryolite. ......................................................................................................................................................................... [1] (iv) Explain why the aluminium oxide needs to in the molten state. ......................................................................................................................................................................... [1] (v) During electrolysis the aluminium ion (Al3+) is attracted towards the negative electrode. Give both the name and symbol of the ion attracted towards the positive electrode. Name. .................................................... Symbol. ....................................................... [1] (b) (i) State and explain one important factor that needs to be considered when an aluminium extraction plant site is chosen. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Aluminium is a metal that is encouraged to be recycled. Explain why we should recycle as much aluminium as possible. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) Aluminium has many different uses. Give one reason why aluminium is chosen to make each of the following items: (i) cooking foil ......................................................................................................................................................................... [1] (ii) electric cables ......................................................................................................................................................................... [1] (iii) window frames ......................................................................................................................................................................... [1]

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TOTAL / 11 Low Demand Questions QUESTIONSHEET 17 This question is about the extraction of metals. (a) (i) Match the metals to their methods of extraction.

Metal Method of extraction Sodium Heat sulphide with oxygen Zinc Electrolysis Copper Reduction with coke

[3] (ii) Explain how you matched the metals to the methods. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What is the main element in coke? ......................................................................................................................................................................... [1] (b) Titanium (Ti) can be extracted from titanium chloride by heating with sodium. TiCl4 + 4Na 4NaCl + Ti (i) What type of reaction is this? ......................................................................................................................................................................... [1] (ii) What does the reaction tell you about titanium compared to sodium? ......................................................................................................................................................................... [1]

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TOTAL / 8

Low Demand Questions QUESTIONSHEET 18 The diagram below shows the outline of a Blast Furnace. (a) Select letters which show: (i) the place where the air blast goes in ______ [1] (ii) the place where the ore and coke go in ______ [1] (iii) the place where the hot gases come out ______ [1] (iv) the place where the iron comes out ______ [1] (b) (i) What use is made of the hot waste gases? ......................................................................................................................................................................... [1] (ii) Name two of the waste gases. ......................................................................................................................................................................... [2] (c) The iron formed in the blast furnace is brittle. What element in the iron causes this? ......................................................................................................................................................................... [1]

A

B

C

D

E

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TOTAL / 8 Low Demand Questions QUESTIONSHEET 19 Ammonia is made from nitrogen and hydrogen. (a) Why is it difficult to react nitrogen with hydrogen? ......................................................................................................................................................................... [1] (b) The reaction is described as reversible. What does this mean? ......................................................................................................................................................................... [1] (c) The reaction is quite slow. What is added to speed it up? ......................................................................................................................................................................... [1] (d) Only about 15% of the nitrogen and hydrogen are converted to ammonia. What happens to the remaining 85%? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) Ammonia is very soluble in water. In what two ways can you recognise a solution of ammonia? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) Ammonia reacts with nitric acid to make a salt which can be used as a fertiliser. (i) Name the salt. ......................................................................................................................................................................... [1] (ii) Why is it a good fertiliser? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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Low Demand Questions QUESTIONSHEET 20 (a) A lot of chemicals can be made from common salt. (i) What is the chemical name for common salt? ......................................................................................................................................................................... [1] (ii) Give two other uses for common salt. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Sodium hydroxide is made from salt. (i) Circle a description in the list below that applies to sodium hydroxide. Strong acid strong alkali neutral weak acid weak alkali [1] (ii) Name two things made using sodium hydroxide. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Chlorine can be extracted from salt. (i) Circle two descriptions in the list below that apply to chlorine. Solid liquid gas bleach reducing agent [2] (ii) Give two uses of chlorine. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 1 Some students made a simple cell. Two pieces of metal foil were dipped into a beaker containing salt solution as shown in the diagram below. The voltage was measured. (a) Name the piece of apparatus that was used to measure the voltage. ......................................................................................................................................................................... [1] The results are given in the table below:

EXPERIMENT METAL A METAL B VOLTAGE OBTAINED/volts 1 2 3 4

magnesium zinc iron

copper

copper copper copper copper

1.6 0.6 0.3 0.0

(b) What is the pattern between the reactivity of the metal and the voltage obtained? .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) Predict the voltage obtained if aluminium was used as metal A and copper was used as metal B. ......................................................................................................................................................................... [1] (d) Predict the voltage obtained if metals A and B were swapped over in experiment 1. ......................................................................................................................................................................... [1] (e) When silver was used as metal A voltage of 0.05 volts was obtained. Explain this result. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (f) Give one disadvantage of making electrical cells using this method. ......................................................................................................................................................................... [1]

TOTAL / 8

metal A

metal B

salt solution

meter

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES High Demand Questions QUESTIONSHEET 2 Small pieces of four different metals were placed in identical amounts of hydrochloric acid. The results are shown below. (a) Place the metals on order of reactivity, starting with the most reactive. [2] (b) The four metals used in the experiment were calcium, magnesium, iron and platinum. Use your knowledge of these four metals to identify the metals A, B, C & D. [3] Metal A ..................................................................................................................................................... Metal B ...................................................................................................................................................... Metal C ...................................................................................................................................................... Metal D ...................................................................................................................................................... (c) When magnesium meets with hydrochloric acid, it forms magnesium chloride and hydrogen. (i) Balance the following equation Mg(s) + ___HCl(aq) MgCl2(aq) + H2(g) [1] (ii) When magnesium reacts with sulphuric acid it forms magnesium sulphate. If a chloride ion is Cl- and a sulphate ion is SO4

2-, what is the formula of magnesium sulphate? Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What salt is formed when magnesium reacts with nitric acid? ......................................................................................................................................................................... [1]

TOTAL / 9

Metal A Metal B Metal C Metal D

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 3 Below is a section of the reactivity series for metals. potassium calcium magnesium zinc increasing reactivity lead copper Use this reactivity series to answer the following questions. (a) Predict if there will be a reaction when the following chemicals are added together. If you predict a react, write a word equation for it. (i) zinc and copper sulphate solution [2] prediction .............................................................................................................................................................................. equation .............................................................................................................................................................................. (ii) Calcium and potassium sulphate solution [1] prediction .............................................................................................................................................................................. equation .............................................................................................................................................................................. (iii) Magnesium and zinc sulphate solution [2] prediction .............................................................................................................................................................................. equation .............................................................................................................................................................................. (b) In a displacement reaction, two metals of different reactivity ‘compete’ for oxygen. In such a reaction, oxidation and reduction occur simultaneously. (i) What is meant by reduction? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES QUESTIONSHEET 3 CONTINUED (ii) Write a word equation for the reaction between magnesium and copper(II) oxide. ......................................................................................................................................................................... [1] (iii) In the equation, circle the reducing agent. [1] (iv) The reaction between magnesium and copper(II) oxide needs to be heated. The heat supplies the

activation energy. What is meant by the term ‘activation energy’? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) In a series of experiments it was found that carbon would react with zinc oxide, but not with magnesium oxide. (i) Write down the name of another metal oxide, which would react with carbon. ......................................................................................................................................................................... [1] (ii) Write the name of another metal oxide, which would not react with carbon. ......................................................................................................................................................................... [1]

TOTAL / 12

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 4 A student investigated the different reactivities of a set of metals by placing pieces of each metal in metal nitrate solutions. The table below shows some of the results.

solution aluminium barium lithium magnesium aluminium nitrate barium nitrate lithium nitrate magnesium nitrate

= reaction observed = no reaction (a) Use the results given to put the metals in order of reactivity starting with the most reactive. [2] (b) Use the reactivity series in (a) to complete the table. [3] (c) It is known that aluminium is more reactive than silver. However, when a piece of aluminium is put in a solution of silver nitrate, no reaction is observed. Explain this result. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 8

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 5 Below is a section of the reactivity series of metals. The non-metal, carbon is also included. magnesium aluminium carbon zinc increasing reactivity iron lead Both aluminium and iron are found in nature as their oxides. The methods of extracting the pure metals depend on their reactivity. (a) Aluminium is extracted by electrolysis from its oxide. (i) What is the name of an aluminium ore consisting of aluminium oxide? ......................................................................................................................................................................... [1] (ii) During electrolysis, cryolite is added to molten aluminium oxide. Explain why. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Write balanced ionic equations for the reactions occurring at the electrodes during the electrolysis. anode ......................................................................................................................................................................... [1] cathode ......................................................................................................................................................................... [1] (b) Iron is extracted from its oxide by reduction in a blast furnace. (i) What is the name of the iron ore consisting of iron(III) oxide? ......................................................................................................................................................................... [1] (ii) Explain what is meant by ‘reduction’. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

QUESTIONSHEET 5 CONTINUED (iii) The main reducing agent in the blast furnace is carbon monoxide, which reacts with iron(III) oxide to produce pure iron. Balance the equation for this reaction. ___CO + Fe2O3 ___CO2 + ___Fe [2] (iv) A waste product of the blast furnace is called slag. Give one use for slag. ......................................................................................................................................................................... [1] (c) Explain why aluminium is extracted by electrolysis, rather than in a blast furnace. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 12

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES High Demand Questions QUESTIONSHEET 6 A new metal has been discovered. It has the name mancunium with the symbol M. Mancunium reacts violently with water to form a colourless gas and an alkaline solution. The alkaline solution is mancunium hydroxide with formula MOH. Mancunium also forms a chloride salt with formula MCl. (a) Describe a test to show that the solution formed with water was alkaline. TEST ......................................................................................................................................................................... [1] RESULT ......................................................................................................................................................................... [1] (b) Use the information to predict the formula of mancunium oxide. ......................................................................................................................................................................... [1] (c) In which group of the Periodic Table would you place mancunium. Give a reason for your answer. GROUP ......................................................................................................................................................................... [1] REASON ......................................................................................................................................................................... [1] (d) Part of the reactivity series for metals is shown below. CALCIUM ZINC IRON COPPER Rewrite this reactivity series and include the metal mancunium. Give a reason for your position. REACTIVITY SERIES REASON .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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QUESTIONSHEET 6 CONTINUED (e) Mancunium was found to react with copper sulphate solution. Give the names of the products of the reaction. ......................................................................................................................................................................... [1] (f) Mancunium hydroxide reacts with sulphuric acid to form a salt and water. (i) Complete the word equation by naming the salt formed in this reaction. mancunium hydroxide + sulphuric acid → _____________________ + water [1] (ii) Complete the symbol equation for this reaction. ______ MOH + H2SO4 → ________________________________ [2]

TOTAL / 11

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 7 Reactions that give out a large amount of heat have many uses. A company has invented 'cook-in-the-can' meals. A ring is pulled which ignites the chemicals surrounding the can. The chemicals react and produce heat, which cooks the food in the can. One of the reactions used is a mixture of aluminium powder and iron(III) oxide. The aluminium used is finely powdered. (a)(i) Complete the word equation below for this reaction: aluminium + iron(III) oxide → ______________ + ___________ [1] (ii) Balance the symbol equation for this reaction. ___ Al + Fe2O3 → Al2O3 + ___ Fe [1] (b) Use your ideas of the reactivity series of metals to explain why these substances react. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Suggest a reason why the aluminium used is powdered. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d)(i) John tried out some reactions in the laboratory that may produce heat. He used a mixture of powdered copper metal and iron(III) oxide. Give a reason why John was unsuccessful. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) John found a copy of the reactivity series in a chemistry textbook. It is shown below: magnesium zinc iron silver gold Use this information to name another metal that John could use that would react with iron(III) oxide. ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

High Demand Questions QUESTIONSHEET 8 Some students were investigating the reaction between zinc metal and copper sulphate solution. They set up the apparatus as shown in the diagram below. (a) Name a piece of apparatus that could be used to measure out 50 cm3 of copper sulphate solution. ......................................................................................................................................................................... [1] (b) Name a piece of apparatus that could be used to measure 5 g of zinc metal. ......................................................................................................................................................................... [1] (c) The reaction is exothermic. Describe what the students would see. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (d) Complete the equation for the reaction Zn + CuSO4 → _________ + __________ [1] (e) Zinc metal was present 'in excess' in this experiment. Explain what is meant by 'in excess'. ......................................................................................................................................................................... [1] (f) The students repeated the experiment but added zinc to magnesium sulphate solution. (i) What would the students see? ......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

Thermometer

50 cm3 copper sulphate solution

5 g zinc metal

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES Medium Demand Questions QUESTIONSHEET 9 Reactions were carried out using four different metals - A, B, C and D. The table below shows the results of reacting these metals with air and then with water.

metal reaction with air reaction with water

A B C D

changes colour on heating burns in air to form a white solid

no reaction changes colour when placed in air

no reaction bubbles of gas on surface

no reaction fizzes vigorously

(a) From the reactions in the table, give one example of a chemical change. [1] Give a reason for your choice. METAL .............................................................................................................................................................................. REACTION WITH .............................................................................................................................................................................. REASON .............................................................................................................................................................................. (b) Use the information in the table to place the four metals in order of reactivity. [2] MOST REACTIVE ____________________ ____________________ ____________________ LEAST REACTIVE ____________________ (c) Which of the four metals is most likely to be an alkali metal? Give a reason for your choice. The group I metal is likely to be _____________ REASON ......................................................................................................................................................................... [2] (d) Which of the four metals would be found 'native'? ......................................................................................................................................................................... [1] (e) Metal A was found to be copper. Write a word equation for the reaction of copper in air. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) A student wished to try the reaction between metal D and hydrochloric acid. Explain why you should not carry out this reaction. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 10 The following questions are all about the reactivity of the metals copper, iron, magnesium and potassium. (a) Match up each of the metals with its reaction with water. (The first one has been done for you) [3] (b) When metals react with water, they form a metal hydroxide or a metal oxide, depending on their

reactivity. From the metals above name a metal which forms: (i) a metal hydroxide ......................................................................................................................................................................... [1] (ii) a metal oxide ......................................................................................................................................................................... [1] (c) When metals react with water they always release a gas. (i) Name the gas released when metals react with water. ......................................................................................................................................................................... [1] (ii) Describe a test to prove the identity of the gas Test ......................................................................................................................................................................... [1] .............................................................................................................................................................................. Result .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 8

copper

iron

magnesium

potassium

reacts with steam

vigorous reaction in cold water

no reaction with steam or water

reacts reversibly with steam

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 11 In a series of experiments a small piece of metal was placed in a solution of a metal salt. Here is a list of reactions which take place. 1 aluminium + zinc sulphate solution 2 iron + lead nitrate solution 3 zinc + iron(II) sulphate solution (a) Use the information above to place the metals in order of reactivity, starting with the most reactive. [2] (b) In another reaction, magnesium was placed in copper(II) sulphate solution. (i) Write a balanced equation for the reaction between magnesium and copper(II) sulphate. ......................................................................................................................................................................... [2] (ii) What would you observe in this reaction? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Where in the series you have written would you place copper and magnesium? copper ......................................................................................................................................................................... [1] magnesium ......................................................................................................................................................................... [1] (c) Use your reactivity series to predict whether there will be a reaction between these metals and solutions.

Write word equations for any reactions you predict. (i) iron and zinc sulphate .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) aluminium and iron(II) sulphate .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 12 A student placed a small piece of lithium in a trough. Below is a diagram of what the student observed. (a) The experiment was repeated with a piece of sodium. (i) What other observations would be made? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Write a balanced symbol equation for the reaction of sodium with water. ......................................................................................................................................................................... [1] (iii) If universal indicator is added to the trough, what colour would it turn? What pH does this represent? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) The experiment was repeated again, with a small piece of potassium. What new observations would be made? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) The metals lithium, sodium and potassium are all in Group I of the periodic table. (i) By what other name is Group I known? ......................................................................................................................................................................... [1]

(Continued...)

trough of water

lithium

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES QUESTIONSHEET 12 CONTINUED (ii) Why do all metals in Group I react in a similar way? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iii) Describe and explain how the reactivity of Group I metals changes on descending the group. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4]

TOTAL / 13

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 13 Blackpool pier is made from an iron framework. The iron legs stand in the sea. Salt in sea water tends to speed up rusting. The pier is protected from rusting by connecting blocks of scrap zinc metal to the iron legs of the pier. (a) Name the two substances required for iron to rust. ......................................................................................................................................................................... [1] (b) How does the zinc prevent the iron from rusting? ......................................................................................................................................................................... [1] (c) Explain why zinc is suitable for this purpose. ......................................................................................................................................................................... [1] (d) Why will the zinc only work when the tide is in and the blocks are covered in sea water? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) Mark on the diagram the direction in which the electrons flow in the wire. [1]

(Continued...)

PIER

sea water

block of scrap zinc

iron leg of the pier

wire

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES QUESTIONSHEET 13 CONTINUED (f) Predict what would happen if the zinc was replaced with copper metal. Give a reason for your prediction. PREDICTION ......................................................................................................................................................................... [1] REASON ......................................................................................................................................................................... [1] (g) Salt water appears to make iron rust more quickly than water containing no salt. Describe how you could carry out an experiment in test tubes with some iron nails to investigate this. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 14 The table shows the dates of discovery of some metals.

metal date of discovery potassium 1807 sodium 1807 magnesium 1755 zinc 1746 copper known since ancient times

(a) What is the pattern between the reactivity of a metal and its date of discovery? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) A large piece of zinc metal was placed into blue copper sulphate solution. (i) Describe what you would see in this reaction. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Complete the word equation for this reaction. zinc + copper sulphate → ___________________ + ___________________ [1] (c) The temperature of the copper sulphate solution was recorded before the zinc was added and then several minutes later. The results were: Temperature at start = 18oC Temperature after reaction = 31oC (i) Calculate the rise in temperature in this reaction. ......................................................................................................................................................................... [1] (ii) What word is used to describe reactions that give out energy? ......................................................................................................................................................................... [1] (iii) Give two ways in which the reaction could be changed to produce a higher temperature rise. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES Medium Demand Questions QUESTIONSHEET 15 A part of a reactivity series of metals is shown below: SODIUM MAGNESIUM ALUMINIUM CARBON ZINC IRON HYDROGEN COPPER

Use this information to explain as fully as you can the following reactions. (a) A brown solid is formed when a piece of magnesium metal is placed in copper sulphate solution.

.............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(b) Nothing happens when a piece of copper metal is placed in zinc sulphate solution. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(c) Iron can be extracted from its oxide using carbon. Aluminium cannot be extracted from its oxide using carbon.

.............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (d) Zinc metal reacts with hydrochloric acid to form hydrogen gas. Copper metal does not react with hydrochloric acid.

.............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

(e) Zinc carbonate decomposes on heating but sodium carbonate does not. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 12

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Medium Demand Questions QUESTIONSHEET 16 A group of students were investigating the effects of 'acid rain'. They decided to look at the effect of acid on metals used as building materials. Lead and copper are used for roofing and iron and aluminium can be used for window frames. Their chemistry book listed these metals in order of their reactivity as follows: ALUMINIUM IRON LEAD COPPER The students tested the metals by adding dilute sulphuric acid to pieces of each of them. Only the iron seemed to give a reaction. (a) What would you see when iron reacted with the acid? ......................................................................................................................................................................... [1] (b) Explain why the aluminium did not react with the acid, even when the book said it was more reactive. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Suggest why sulphuric acid was used in this test and not any other acid. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) The reaction with acid did not prove that lead was more reactive than copper. The students had available: 1. small pieces of copper and lead 2. solutions of copper nitrate and lead nitrate. (i) From these four substances choose two that the students should mix to show that lead is more reactive than copper. 1____________________________ [1] 2____________________________ [1] (ii) What would you see when the substances were mixed? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES QUESTIONSHEET 16 CONTINUED (iii) Write a word equation for the reaction. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iv) Explain how this reaction proves that lead is more reactive than copper. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Low Demand Questions QUESTIONSHEET 17 The reactivity series shows the relative reactivities of different metals. Below is a reactivity series for eight metals. sodium calcium magnesium zinc iron increasing reactivity lead copper mercury silver Use the series above to answer the following questions. (a) Name the metal which is found uncombined in the Earth’s crust. ......................................................................................................................................................................... [1] (b) Which metal is stored under oil? ......................................................................................................................................................................... [1] (c) Which metal is a liquid at room temperature? ......................................................................................................................................................................... [1] (d) Which metal is shiny when cut, but tarnishes in a few seconds? ......................................................................................................................................................................... [1] (e) Which metal burns with a bright, white flame? ......................................................................................................................................................................... [1] (f) Which metal is extracted from its ore in a blast furnace? ......................................................................................................................................................................... [1] (g) Which metal is used to galvanise iron to prevent rusting? ......................................................................................................................................................................... [1] (h) Which metal reacts vigorously with cold water? ......................................................................................................................................................................... [1] (i) Which metal burns with a brick red flame? ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Low Demand Questions QUESTIONSHEET 18 The 'thermit' reaction is used to weld railway lines together. The reaction mixture contains aluminium metal and iron oxide. The substances are mixed in powder form in a clay pot. The mixture is lit with a magnesium fuse. (a) Complete the word equation for this reaction: aluminium + iron oxide → _________________ + _____________________ [2] (b) The magnesium ribbon burns at 700oC yet the iron will only melt at 1500oC. Explain why this reaction forms molten iron. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Suggest a reason why the aluminium and iron oxide are in powder form. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Suggest why a tap is needed at the bottom of the clay pot. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

railway lines

tap

reaction mixture

clay pot

magnesium fuse

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

QUESTIONSHEET 18 CONTINUED (e) Suggest a reason for using a clay pot to hold the mixture. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (f) If copper powder is mixed with iron oxide there is no reaction. Explain why this reaction works with aluminium metal but not copper metal. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 11

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES Low Demand Questions QUESTIONSHEET 19 In an experiment different metals were heated in a Bunsen burner flame for 30 seconds and then removed. The observations are given below.

metal observation copper turned black - did not burn

magnesium burned with white flame silver no obvious change

(a) Place the metals in order of reactivity, starting with the most reactive. [1] (b) When metals burn in air, an oxidation reaction takes place. (i) What is meant by ‘oxidation’? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Write a word equation for an oxidation reaction which happened in the experiment. ......................................................................................................................................................................... [1] (c) In another experiment, a piece of polished copper was placed in a solution of silver nitrate. (i) What was observed? ......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) In another experiment a piece of polished copper was placed in a solution of magnesium sulphate. (i) What was observed? ......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES

Low Demand Questions QUESTIONSHEET 20 Magnesium reacts very slowly with water. A piece of magnesium is kept under water for a week in the apparatus shown. (a)(i) What gas is collected in the test tube? ......................................................................................................................................................................... [1] (ii) A white solid forms on the surface of the magnesium. What is this solid? ......................................................................................................................................................................... [1] (b) magnesium will react much faster with steam. (i) Name the gas collected in the test tube. ......................................................................................................................................................................... [1] (ii) Suggest two other metals which will react with steam in the same way as magnesium. ......................................................................................................................................................................... [2] (iii) Name a metal that will not react in this way. ......................................................................................................................................................................... [1]

(Continued...)

gas

water

magnesium

gas magnesium

steam

heat

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES QUESTIONSHEET 20 CONTINUED (c) Explain why many items of jewellery are made from gold or silver and not from iron. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY NON-METALS

High Demand Questions QUESTIONSHEET 1 The table below gives some information about the halogens:

Element Atomic number Molecular formula Bond length/nm Bond energy/ kJ per mole

Chlorine 17 C12 0.20 240 Bromine 35 Br2 0.23 195 Iodine 53 I2 0.26 150

Astatine 85 At2 0.29 Note: Bond length = distance between atoms in a molecule nm = nanometres (10-9 metres) Bond energy = energy needed to break the bond in the molecule (a) As the atomic number in the halogens increases, what happens to the (i) bond length? ......................................................................................................................................................................... [1] (ii) bond energy? ......................................................................................................................................................................... [1] (b) What do you think is the bond energy in astatine? ......................................................................................................................................................................... [1] (c) Describe the relationship between bond length and bond energy as the halogen series is descended. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] The solubility of the halogens in water may be summarised as follows: chlorine dissolves fairly readily bromine dissolves slightly iodine almost insoluble Chemical reactions occur when the halogens dissolve in water. (d) What is likely to be the reaction of astatine with water? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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GCSE CHEMISTRY NON-METALS QUESTIONSHEET 1 CONTINUED (e) List the four elements in order of reactivity, placing the most reactive first. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) Does your order of reactivity seem to fit with the bond energies? ......................................................................................................................................................................... [1] Give a reason for your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 12

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High Demand Questions QUESTIONSHEET 2 When sulphur is heated in air, a colourless, poisonous gas with an unpleasant, choking smell is formed. If this gas is collected, dried, then cooled to below –10oC, it forms a colourless liquid. Dry pH paper dipped into this liquid does not change colour, but damp pH paper dipped into the liquid shows a pH of less than 7. (a) What is the name of the colourless gas? ......................................................................................................................................................................... [1] (b) What is the boiling point of the colourless liquid? ......................................................................................................................................................................... [1] (c) Why does the colourless liquid not affect the dry pH paper? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) When damp pH paper is used, the colourless liquid becomes acidic. How do you know this? ......................................................................................................................................................................... [1] If the colourless gas from above is reacted with oxygen at 450oC and in the presence of vanadium pentoxide, sulphur trioxide forms as a colourless gas, which then cools to colourless crystals. If water is added to the crystals, a fiercely exothermic reaction takes place and sulphuric acid forms. (e) Write a balanced chemical equation for the reaction between the colourless gas named in part (a) with oxygen. ......................................................................................................................................................................... [2] (f) The vanadium pentoxide is recovered after the above reaction. What is its purpose in the reaction? ......................................................................................................................................................................... [1] (g) What is meant by an ‘exothermic reaction’? ......................................................................................................................................................................... [1] (h) Write a balanced chemical equation for the reaction of sulphur trioxide with water. ......................................................................................................................................................................... [2] (i) In fact, this reaction is much too exothermic to carry out safely. It would spray sulphuric acid all around the room. In practice, the sulphur trioxide is added to 98% sulphuric acid, where it reacts with the 2% water present to form more sulphuric acid. Why is the reaction much safer when carried out like this? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 13

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High Demand Questions QUESTIONSHEET 3 The diagram below shows an apparatus that can be used to react chlorine with iron.

(a) (i) Describe the appearance of the Group VII element chlorine. ......................................................................................................................................................................... [1] (ii) What compound is formed during the reaction that takes place? ......................................................................................................................................................................... [1] (iii) Complete and balance the following symbol equation for the chemical change that takes place. ..... Fe (s) + ............ (g) ς ..... FeCl

3(s) [2]

(iv) Give one reason why this reaction must be carried out in a fume cupboard. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) The element iodine is below chlorine in Group VII of the Periodic Table. If iodine was allowed to react with iron wire, state whether you would expect this reaction to be more vigorous, less vigorous or about the same as the reaction between chlorine and iron wire. ......................................................................................................................................................................... [1] (c) Group I elements also react with Group VII elements. (i) Complete and balance the symbol equation for the reaction between sodium and bromine. ..... Na (....) + Br

2(....) ς .....NaBr (s) [2]

(ii) If the following pairs of elements were allowed to react together, choose the pair that would be most reactive and give an explanation for your choice.

lithium and fluorine

sodium and chlorine

potassium and chlorine

potassium and fluorine

(Continued...)

excess chlorine dry chlorine

product

iron wire

HEAT

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QUESTIONSHEET 3 CONTINUED The most reactive pair is: ............................................................. [1] Give an explanation for your choice. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11

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GCSE CHEMISTRY NON-METALS High Demand Questions QUESTIONSHEET 4 For each of the following pairs of substances describe how you would distinguish between them by giving one chemical test in each case. Describe your observation on both substances. (i) Nitrogen and oxygen. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Hydrogen and chlorine. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Carbon dioxide and sulphur dioxide. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (iv) Water and ammonia solution. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 10

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High Demand Questions QUESTIONSHEET 5 Sulphuric acid is manufactured industrially by the contact process. During the early part of the process, sulphur is reacted with oxygen to give an oxide A. This substance is then converted into sulphur trioxide by reacting A with the element B. (a) (i) Calculate the simplest formula of the oxide of sulphur A from the following information. 3.2 g of sulphur gave 6.4 g of the oxide A. Please show how you worked out your answer. Ar(S) = 32; Ar(O) = 16. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) Name the element B. ......................................[1] (b) The reaction between A and B to give the gas sulphur trioxide is reversible. Explain the term ‘reversible’ and complete and balance the chemical equation. (i) A reversible reaction is .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Complete and balance the equation; .............. + ............ ....... SO3 [2] (c) Both oxygen and sulphur are in the same group of the Periodic Table. One method for both to react is to become an ion X2-. Explain in terms of their electronic structures why oxygen is more reactive towards this change than sulphur. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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High Demand Questions QUESTIONSHEET 6 Plants need many substances for healthy growth and for the chemical reactions which occur within them. Most of these substances are absorbed in solution in water through the roots. The three main essential elements which plants need are nitrogen, phosphorus and potassium. These elements may be supplied naturally by the soil, but often we need to add one or more of them in the form of fertilisers. A fertiliser is sold in a bag labelled with its name followed by three numbers which indicate, respectively, the percentages of nitrogen, phosphorus and potassium present. e.g. Regular 20 – 10 – 12 means that the fertiliser is called regular and contains 20% nitrogen, 10% phosphorus and 12% potassium. Such fertilisers are known as NPK fertilisers. Here is a list of some common fertilisers. Universal 15 – 15 – 15 Extra grass 29 – 5 – 5 Double season PK for fertile soils 0 – 20 – 20 Maincrop potato 10 – 10 – 15 + 4.5 Mg Concentrated maincrop potato 15 – 15 – 19 Granphos 2 – 40 – 0 Barley for high potash clay soils 29 – 13 – 0 Winter wheat 9 – 23 – 18 (a) Why are these fertilisers known as NPK fertilisers? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Name the essential element which: (i) is already present in fertile soil and so does not need adding. ......................................................................................................................................................................... [1] (ii) favours green growth (e.g. grass). ......................................................................................................................................................................... [1] (iii) potatoes need in extra high concentration. ......................................................................................................................................................................... [1] (c) Name an element, other than nitrogen, phosphorus or potassium, which potatoes need. ......................................................................................................................................................................... [1] (d) What percentage of nitrogen would be supplied by a fertiliser of pure ammonium nitrate NH4 NO3? (Relative atomic masses: H = 1, N = 14, O = 16). .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

(Continued...)

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QUESTIONSHEET 6 CONTINUED (e) A farmer was offered a choice of potassium nitrate or urea as a fertiliser. Although much more expensive per gram of nitrogen, he chose potassium nitrate. Give one reason which may have influenced his choice.

.............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 10

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High Demand Questions QUESTIONSHEET 7 Phosphorus (P) is directly below nitrogen in the periodic table. (a) Write down the electronic configuration of phosphorus. ......................................................................................................................................................................... [1] (b) Write down the formula of the compound you would expect phosphorus to form with hydrogen, and use a dot and cross diagram to show how it is formed. Formula .................................................................................................................................................. [3] (c) (i) Would you expect this compound to be a solid, a liquid or a gas at room temperature? ......................................................................................................................................................................... [1] (ii) Explain your reasons. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Give one use for phosphorus-containing compounds ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY NON-METALS

High Demand Questions QUESTIONSHEET 8 (a) Solid sulphur consists of rings of eight atoms. Fill in the gaps in the table below to show the changes in appearance and structure of sulphur when it is heated.

appearance structure Yellow solid Rings of 8 atoms

Melts to form a _____ _____ liquid

Boils Separated sulphur atoms and groups of atoms [4]

(b) Sulphur exists in two crystalline forms. What are different crystalline forms of the same element known as? ......................................................................................................................................................................... [1] (c) When molten sulphur is cooled slowly, needle-like crystals form under the surface. Why do some rocks contain crystals when they are split open? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) These crystals change slowly to another form with rhombic-shaped crystals as they cool. (i) What changes are seen as the needle-like crystals cool? ......................................................................................................................................................................... [1] (ii) What changes would be seen in the rhombic crystals as they cool? ......................................................................................................................................................................... [1]

TOTAL / 9

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GCSE CHEMISTRY NON-METALS Medium Demand Questions QUESTIONSHEET 9 Tooth decay in the UK is a serious problem. About 7000 sets of dentures are supplied each year to school children alone. This is a waste of healthy teeth and money. It has been suggested that the presence of fluoride ions, F -, in drinking water helps to prevent tooth decay. The data in the following table come from six different areas of the country, where fluoride ions occur naturally in the water supply.

DMF teeth per 100 children fluoride concentration/ppm 430 0.5 350 0.9 240 2.6 720 0.1 250 1.9 300 1.2

Note: DMF = decayed, missing or filled ppm = parts per millionS (a) On the chart below plot a graph of DMF against ppm of fluoride concentration. [2]

(b) Does your graph support or contradict the suggestion that fluoride ions in drinking water help to prevent tooth decay? ......................................................................................................................................................................... [1]

(Continued...)

0 0.5 1.0 1.5 2.0 2.5 3.0

400

200

600

800

Fluoride concentration/ppm

DM

F te

eth

per 1

00

child

ren

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QUESTIONSHEET 9 CONTINUED It has been found in a much wider study from many more areas in the UK that similar results are obtained. Also, the presence of small amounts of fluoride in the water does not appear to be at all harmful. As a result, it has been suggested that in areas where there is no natural fluoride in the water, drinking water should undergo fluoridation i.e. should have fluoride added. (c) Give a reason why fluoridation might be a good idea in areas with no natural fluoride in the drinking water. ......................................................................................................................................................................... [1] (d) Give one argument which might be used against fluoridation of water supplies. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) Suggest two other ways, other than fluoridation of water, in which people could take small amounts of fluoride ions .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY NON-METALS Medium Demand Questions QUESTIONSHEET 10 The table below gives some information about six different gases.

Formula of molecule Mass of one mole of molecules/g Volume occupied by 1g at rtp/dm3 CH4 16 1.50 NH3 17 1.40 N2 28 0.86 O2 32 0.76

CO2 44 0.54 SO2 64 0.38

rtp = room temperature and pressure relative atomic masses: H=1, C=12, N=14, O=16, F=19, Ar=40 (a) Give the name of the molecules listed in the first column. CH4 = ................................................................................................................................................... [1] NH3 = ................................................................................................................................................... [1] N2 = ................................................................................................................................................... [1] O2 = ................................................................................................................................................... [1] CO2 = ................................................................................................................................................... [1] SO2 = ................................................................................................................................................... [1] (b) On the chart below plot a graph of volume against mass of one mole. [2]

(Continued...)

10 20 30 40 50 60 70

0.5

0.7

0.9

1.1

1.3

1.5

0.3

mass of one mole/g

Vol

ume

at rt

p/dm

3

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GCSE CHEMISTRY NON-METALS

QUESTIONSHEET 10 CONTINUED (c) Use your graph to find the volume at rtp occupied by: (i) 1g of ethene, C2H4 .................................................................................................................................. [1] (ii) 1g of argon .............................................................................................................................................. [1] (d) (i) What is the mass of one mole of molecules of a gas for which 1g at rtp occupies 0.52 dm3? ......................................................................................................................................................................... [1] (ii) If the molecule is made up of nitrogen and oxygen only, what is its formula? Show your working. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (e) Determine the volume at rtp occupied by 1g of hydrogen fluoride, HF. Show your working. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [5]

TOTAL / 19

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GCSE CHEMISTRY NON-METALS Medium Demand Questions QUESTIONSHEET 11 The following table contains some information about Group VII of the Periodic Table.

Element Formula Atomic number Melting point (oC) Colour fluorine F2 9 -223 pale yellow chlorine C12 17 -103 yellow-green bromine Br2 35 -7 red-brown iodine I2 53 114 purple-black

(a)(i) Name the element with the lowest melting point. ......................................................................................................................................................................... [1] (ii) Chlorine is a diatomic gas. Explain the meaning of ‘diatomic’. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iii) Give the electronic structure of chlorine. ......................................................................................................................................................................... [1] (iv) Explain how chloride ions are formed from chlorine atoms. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Astatine, At, is another member of Group VII with an atomic number of 85. (i) Give the formula for astatine. ......................................................................................................................................................................... [1] (ii) Describe the appearance of astatine. ......................................................................................................................................................................... [1] (iii) Give the number of electrons in the outer shell of astatine. ......................................................................................................................................................................... [1] (iv) Astatine is expected to form a compound with hydrogen in a similar way to chlorine and hydrogen. By means of a labelled diagram, show how the atoms are bonded together. Name this type of bonding. Diagram [2] Type of bonding. .................................................................................................................................. [1]

TOTAL / 11

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Medium Demand Questions QUESTIONSHEET 12 The table below shows some properties of elements A, B, C, D and E. (The letters are not chemical symbols.)

Element Melting point (oC)

Boiling point (oC)

Conducts heat Brittle Reaction with water Shiny

A 119 444 no yes insoluble no B -7 59 no no slightly soluble no C 98 883 yes no reacts yes D 1083 2336 yes no insoluble yes E -259 -253 no no slightly soluble no

(a) Give the letter of the element which is a liquid under room conditions. ...................................[1] (b) Give the letters of all the elements that are non-metals giving two reasons for your answer. (i) The elements that are non-metals are ..........................................[3] (ii) Reasons. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) Elements A and E when heated can react together to give a gas. Name the type of bonding you would expect this compound to have. Give a reason for your answer. Type of bonding ......................................................[1] Reason. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Gas E has no colour or smell. It burns in oxygen giving a vapour which condenses on a cold surface

as a colourless neutral liquid. The gas E has a number of important uses including the industrial manufacture of ammonia. Name the gas E.

Gas E is .....................................[1]

TOTAL / 9

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Medium Demand Questions QUESTIONSHEET 13 Diamond and graphite are two allotropes of the element carbon. (a) Explain the meaning of allotropy .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) Draw the structure of both diamond and graphite. (i) Diamond (ii) Graphite.

[4] (c) Use the above structures to explain the following. (i) Diamond is a very hard substance often used to cut and engrave glass. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Graphite conducts electricity and is used as electrodes in industry and as positive terminals in batteries. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY NON-METALS

Medium Demand Questions QUESTIONSHEET 14 The following box contains non-metals and their atomic numbers. hydrogen 1, helium 2, carbon 6, nitrogen 7, oxygen 8, fluorine 9, sulphur 16, chlorine 17, bromine 35. Use only elements from these given non-metals to answer the following questions. Each element may be used once, more than once or not at all. (a) Name one element which is (i) a liquid at room temperature, .....................................[1] (ii) has four electrons in its outer shell, ....................................[1] (iii) has the electronic structure 2, 8, 7 ....................................[1] (iv) forms an ion with the formula X2-. ....................................[1] (b) Nitrogen reacts with hydrogen to give the gas ammonia. Give the formula and the type of bonding in ammonia. Formula. ....................................[1] Type of bonding. ....................................[1] (c) Name the element which readily burns in air with a pale blue flame giving off an unpleasant smelling gas which is one of the main causes of acid rain. The element is ....................................[1] (d) Two elements X and Y form compounds with hydrogen with the formulae H2X and YH4.

Name the elements X and Y. Element X is ....................................[1] Element Y is ....................................[1]

TOTAL / 9

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GCSE CHEMISTRY NON-METALS Medium Demand Questions QUESTIONSHEET 15 (a) Give two physical properties of hydrogen. (i) ............................................................................................................................................................. [1] (ii) . ........................................................................................................................................................... [1] (b) Some pure hydrogen was carefully burnt on a cold surface as shown in the diagram. (i) Name two chemicals that could be used to make hydrogen in the laboratory. ................................................. and .................................................... [2] (ii) Give the precaution that must be taken before hydrogen is ignited. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iii) Name the liquid A. ......................................[1] (iv) Give a simple chemical test and observation to confirm the identity of the liquid. Test. ................................................................................................................................................................. [1] Observation. ......................................................................................................................................................... ......................................................................................................................................................................... [1] (c) One of the first uses of hydrogen was in airships since it is the lightest of all gases. Unfortunately it reacts violently with the oxygen in the air which has led to a number of disasters. Name the safer gas which is used in present day airships. ......................................................................................................................................................................... [1]

TOTAL / 9

drops of liquid A

cold surface Pure dry hydrogen

hydrogen burning

glass tube

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GCSE CHEMISTRY NON-METALS

Medium Demand Questions QUESTIONSHEET 16 The table below contains some information about four different substances A, B, C and D. (The letters are not chemical symbols.) Study the table carefully and answer the given questions.

Substance Boiling point (oC) Conducts electricity when solid

Conducts electricity when melted

A above 500 yes yes B below 500 no no C above 500 no no D above 500 no yes

(a) State which substance is most likely to be:- (i) diamond, ...............................[1] (ii) iodine, ...............................[1] (iii) copper . ...............................[1] (b) The four substances are diamond, copper, iodine and sodium chloride. Which of these substances best fits the following descriptions? (i) Atoms bonded by sharing electrons to form small molecules. ......................................................................................................................................................................... [1] (ii) Atoms bonded by sharing electrons to form giant covalent structures. ......................................................................................................................................................................... [1] (iii) Atoms bonded by electron transfer to form giant ionic structures. ......................................................................................................................................................................... [1] (c) During the electrolysis of molten sodium chloride the chloride ion, Cl-, is attracted towards the positive electrode and releases chlorine gas, Cl2. (i) Explain the meaning of the term electrolysis. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) Complete the equation that takes place at the positive electrode. __ Cl- → C12 ________ [2]

TOTAL / 9

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GCSE CHEMISTRY NON-METALS Low Demand Questions QUESTIONSHEET 17 The following table gives some information about gases which are found in the air.

Gas Boiling point/oC Soluble in water? nitrogen -196 no oxygen -183 slightly argon -186 no

carbon dioxide -40 (sublimes) fairly neon -246 no

helium -269 no krypton -153 no xenon -108 no

(a) As well as the above, which other gas is normally found in the air? ......................................................................................................................................................................... [1] (b) Which of the above gases becomes liquid at the lowest temperature? ......................................................................................................................................................................... [1] (c) Carbon dioxide sublimes at –40oC. What would you observe if carbon dioxide gas was cooled to this temperature? ......................................................................................................................................................................... [1] (d) If a mixture of liquid nitrogen and liquid oxygen was allowed to warm up, which one would boil first? ......................................................................................................................................................................... [1] (e) What is the name of the process which allows nitrogen and oxygen to be separated from liquid air by warming? ......................................................................................................................................................................... [1] (f) State the approximate percentages by volume of nitrogen and oxygen in the air. [2] Nitrogen ................................% Oxygen .................................% (g) The percentages of nitrogen and oxygen in the air which has been boiled out of water are different to those given in part (f). Why is this? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(Continued...)

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QUESTIONSHEET 17 CONTINUED (h) Nitrogen and oxygen are both obtained by allowing liquid air to warm up. Why is oxygen more expensive than nitrogen? ......................................................................................................................................................................... [1] (i) Green plants need carbon dioxide for photosynthesis. How can some green plants continue to live under water? ......................................................................................................................................................................... [1]

TOTAL / 11

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GCSE CHEMISTRY NON-METALS

Low Demand Questions QUESTIONSHEET 18 The flow chart shows some of the reactions and changes involved in carbon compounds. (a) Name the chemical substances labelled A and B . A is ............................................... [1] B is ............................................... [1] (b) Name the different processes C, D and E. C is ............................................... [1] D is ............................................... [1] E is ............................................... [1] (c) How can carbon dioxide be converted into carbon monoxide? ......................................................................................................................................................................... [2] (d) Give one important use of carbon dioxide. ......................................................................................................................................................................... [1] (e) Carbon is often used as a reducing agent. When a mixture of carbon and copper oxide are heated the

copper oxide is reduced to copper. Complete and balance the equation for the reaction. C + ..... CuO → ... Cu + .......... [2] (f) Carbon and silicon both belong to Group 4 of the Periodic Table of elements. They form oxides with similar formulae CO2 and SiO2. In terms of structures explain why carbon dioxide is a gas at room conditions but silicon dioxide has a very high melting point. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 12

carbon dioxide

CO2

plants

calcium carbonate

solid A

carbon monoxide

CO

solution B goes milky/

cloudy

D

E

C

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GCSE CHEMISTRY NON-METALS

Low Demand Questions QUESTIONSHEET 19 Use The Periodic Table to answer this question. (a) Give the symbol for the element (i) oxygen ......................................................................................................................................................................... [1] (ii) potassium .............................................................................................................................................................................. (b) Give the name of the element with the symbol [1] (i) C .............................................................................................................................................................................. (ii) Na .............................................................................................................................................................................. (c) Complete the following table. [3]

Substance Chemical formula Elements present zinc oxide ZnO zinc and oxygen

iron sulphide FeS sodium hydroxide NaOH

KC1 potassium and chlorine (d) The chemical formula for carbon monoxide is CO. (i) How many different elements are represented in carbon monoxide? ......................................................................................................................................................................... [1] (ii) Give the total number of atoms the formula CO represents. ......................................................................................................................................................................... [1] (e) The chemical formula for sulphuric acid is H2SO4. (i) How many different elements are present in sulphuric acid? ......................................................................................................................................................................... [1] (ii) Give the total number of atoms present in H2SO4. ......................................................................................................................................................................... [1]

TOTAL / 9

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Low Demand Questions QUESTIONSHEET 20 The table below gives some information about halogens.

Element Atomic symbol Atomic number Melting point/oC Boiling point/oC Fluorine F 9 -220 -188 Chlorine C1 17 -101 -35 Bromine Br 35 -7 +58 Iodine I 53 +114 +183

Astatine At 85 (a) As the atomic number increases what happens to the (i) melting point? ......................................................................................................................................................................... [1] (ii) boiling point? ......................................................................................................................................................................... [1] (b) Are these elements solids, liquids or gases at room temperature (20oC)? (i) fluorine is a ............................................................................................................................................. [1] (ii) chlorine is a ............................................................................................................................................ [1] (iii) bromine is a ............................................................................................................................................ [1] (iv) iodine is a ................................................................................................................................................ [1] (c) In which physical state do you think astatine exists at room temperature? ......................................................................................................................................................................... [1] The behaviour of the halogens with water may be summarised as follows: fluorine violent reaction chlorine dissolves fairly readily bromine dissolves slightly iodine almost insoluble (d) What is likely to be the behaviour of astatine with water? ......................................................................................................................................................................... [1] (e) List the five elements in order of reactivity, placing the most reactive first. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 10

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GCSE CHEMISTRY PRODUCTS FROM OIL

High Demand Questions QUESTIONSHEET 1 (a) Crude oil is the raw material of the petrochemical industry. Describe how crude oil was formed. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

(b) The first stage in the processing of crude oil is fractional distillation. The process is illustrated in the diagram below.

(Continued...)

Bottled gas and chemicals Petroleum gases, b.p. –160-40oC

Diesel oil, b.p. 220-250oC

Fuel oil 350oC

Bitumen

Lubricating oil, b.p. 250-350oC

Kerosene (paraffin), b.p. 150-240oC

Naphtha, b.p. 75-150oC

Gasoline, b.p. 40-75oC

Chemicals

Petrol

Jet fuel

Diesel fuel

Lubricants and chemicals

Fuel for ships

Roads and roofing felt

Vapour of crude oil

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GCSE CHEMISTRY PRODUCTS FROM OIL QUESTIONSHEET 1 CONTINUED (i) Explain how fractional distillation can be used to separate crude oil. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) From which fraction is petrol obtained? ......................................................................................................................................................................... [1]

(iii) Which fraction provides the chemical feedstock for the petrochemical industry? ......................................................................................................................................................................... [1]

(c) All of the chemicals in crude oil are hydrocarbons. What are hydrocarbons? ......................................................................................................................................................................... [2] TOTAL / 10

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GCSE CHEMISTRY PRODUCTS FROM OIL

High Demand Questions QUESTIONSHEET 2 Crude oil is a mixture of many different hydrocarbons. The process by which it can be separated can be demonstrated in the laboratory using the apparatus shown below.

(a) (i) What is the name for this process of separation? ......................................................................................................................................................................... [1]

(ii) What is the purpose of the mineral wool? ......................................................................................................................................................................... [1]

(b) In a typical experiment, four different fractions can be collected. The properties of these fractions are summarised below.

fraction b.p. range (oC) viscosity colour how it burns

A up to 80 very low colourless easily clean flame

B 80 to 160 low pale yellow quite easily smoky flame

C 160 to 250 high yellow difficult to light very smoky flame

D 250 to 320

Complete the table. [3]

(c) Suggest, with reasons, which fraction would be used to provide:

(i) fuel for a motor car engine. Fraction ................................................................................................................................................ [1] Reason.................................................................................................................................................. [2]

(ii) a lubricating oil. Fraction ................................................................................................................................................. [1] Reason................................................................................................................................................... [1]

TOTAL / 10

delivery tube

cold water

thermometer

crude oil soaked into

mineral wool

clamp

heat

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GCSE CHEMISTRY PRODUCTS FROM OIL High Demand Questions QUESTIONSHEET 3 Many of the hydrocarbons obtained from crude oil belong to the alkane homologous series. (a) What is a hydrocarbon? ......................................................................................................................................................................... [2] (b) State two general characteristics of any homologous series. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) The first and fourth members of the alkane series are methane, CH4, and butane, C4H10. What is the formula of hexane, the sixth member of the series? ......................................................................................................................................................................... [1] (d) The atoms of the hydrocarbon, C4H10, can be arranged in two different ways. (i) Draw the structural formulae for the two arrangements of this hydrocarbon. [2] (ii) Which of the two structural formulae you have drawn will have the higher boiling point? ......................................................................................................................................................................... [1] (iii) Explain your answer to part (ii). .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 10

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GCSE CHEMISTRY PRODUCTS FROM OIL

High Demand Questions QUESTIONSHEET 4 Crude oil is a mixture of many compounds. In order to convert it into useful products it must pass through a number of processes. (a) One of the products of the first processing stage is naphtha. What is the name of the process by which naphtha is produced? ......................................................................................................................................................................... [1] (b) Naphtha is then subjected to another process that can produce ethene as one of the products. What name is given to this process? ......................................................................................................................................................................... [1] (c) Ethene can be used for a number of other processes, one of which makes poly(ethene). What is the name of this process? ......................................................................................................................................................................... [1] (d) Complete the following structural equation for the formation of poly(ethene). [2] (e) Describe two environmental problems which are associated with the disposal of waste plastics. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

H H

C

H H

Cn

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GCSE CHEMISTRY PRODUCTS FROM OIL High Demand Questions QUESTIONSHEET 5 This question is about the alkene, ethene, C2H4, which is an unsaturated hydrocarbon. (a) What is meant by ‘unsaturated’? ......................................................................................................................................................................... [1] (b) What is the general formula of alkenes? ......................................................................................................................................................................... [1] (c) Ethanol can be produced from ethene by direct hydration. C2H4 + H2O C2H5OH Under what conditions is this reaction carried out? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Draw the structural formula of ethanol [1] (e) Ethane is a saturated hydrocarbon. Describe a simple test that would enable you to distinguish between ethene and ethane. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (f) Chlorethene (vinyl chloride) can be made from ethene. Chloroethene can be used to produce poly(chloroethene) or PVC. Draw a section of a PVC molecule containing four carbon atoms. [2]

TOTAL / 9

Cl H

C

H H

C

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GCSE CHEMISTRY PRODUCTS FROM OIL

High Demand Questions QUESTIONSHEET 6 Cracking is an important process in the petrochemical industry. (a) (i) What are the conditions for carrying out cracking? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Cracking can be demonstrated in the laboratory.

Draw a labelled diagram of an apparatus that would enable you to crack a sample of liquid paraffin and to collect the gaseous product.

[4] (iii) Give one piece of evidence that the product contains smaller molecules than the starting material. ......................................................................................................................................................................... [1] (b) The starting material is said to contain only saturated hydrocarbons, whereas the product will contain unsaturated ones. What is the difference between a saturated and an unsaturated hydrocarbon? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY PRODUCTS FROM OIL High Demand Questions QUESTIONSHEET 7 Ethane is an alkane hydrocarbon. (a) (i) Draw the structural formula of ethane. [1] (ii) Ethane is said to be saturated. What does this term mean? ......................................................................................................................................................................... [1] (iii) Why is it not possible to make polymers from ethane? ......................................................................................................................................................................... [1] (b) Poly(butene) can be made from butene. (i) Draw one possible structure of butene. [1] (ii) Draw a section of a poly(butene) having eight carbon atoms. [1] (c) poly(butene) is a thermosoftening plastic. Other plastics may be described as thermosetting. (i) Suggest one use for a thermosetting plastic. ......................................................................................................................................................................... [1] (ii) Describe how a sample of a plastic could be tested to find out whether it is thermosetting or

thermosoftening. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY PRODUCTS FROM OIL

High Demand Questions QUESTIONSHEET 8 The diagram below shows some of the reactions of ethene, C2H4. (a) Give the names of each of the lettered substances. (i) liquid A ..............................................................................................................................................................................

(ii) gas B .............................................................................................................................................................................. (iii) catalyst C .............................................................................................................................................................................. (iv) catalyst D .............................................................................................................................................................................. (v) solid E .............................................................................................................................................................................. (vi) liquid F ......................................................................................................................................................................... [6] (b) Write a chemical equation for the reaction between ethene and steam to form liquid F. ......................................................................................................................................................................... [2] (c) Ethene can be converted into ethane by reaction with gas B in the presence of catalyst C. State one commercial application of this type of reaction. ......................................................................................................................................................................... [1]

TOTAL / 9

Liquid A ethane, C2H6

gas B, catalyst C

ethene, C2H4

solid E liquid F

steam, catalyst D

bromine

high pressure, heat, initiator

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GCSE CHEMISTRY PRODUCTS FROM OIL Medium Demand Questions QUESTIONSHEET 9 The following table gives some data about the first ten members of the alkane homologous series.

name formula boiling point (oC) methane CH4 -161 ethane C2H6 -88 propane C3H8 -42 butane C4H10 0 (i) C5H12 36 hexane C6H14 69 heptane C7H16 octane (ii) 126 nonane C9H20 151 decane C10H22 174

(a) (i) Give the name of the alkane (i), C5H12. ......................................................................................................................................................................... [1] (ii) Give the formula of the alkane (ii), octane. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY PRODUCTS FROM OIL

QUESTIONSHEET 9 CONTINUED (b) (i) Plot a graph of boiling point (vertical axis) against number of carbon atoms (horizontal axis) [4]

(Continued...)

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GCSE CHEMISTRY PRODUCTS FROM OIL QUESTIONSHEET 9 CONTINUED (ii) Use the graph to estimate the boiling point of heptane. ......................................................................................................................................................................... [1] (c) There are three hydrocarbons with the molecular formula, C5H12. (i) Draw the structural formulae of all three hydrocarbons.

[3] TOTAL / 10

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GCSE CHEMISTRY PRODUCTS FROM OIL

Medium Demand Questions QUESTIONSHEET 10 (a) Ethene can be made into poly(ethene). Draw a section of a poly(ethene) molecule containing at least six carbon atoms. [2] (b) Poly(ethene) is a thermsoftening plastic. Draw the structure of a thermosoftening plastic. [2] (c) Explain why poly(ethene) is a good material for use in carrier bags. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) About thirty years ago, most carrier bags were made from paper, whereas most today are made from poly(ethene). Explain why this change has taken place. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY PRODUCTS FROM OIL Medium Demand Questions QUESTIONSHEET 11 The table below gives some information about monomers and the polymers that are made from them. (a) Complete the table. [2] (b) What structural feature do these monomers have which enables them to be polymerised? ......................................................................................................................................................................... [1] (c) Poly(chloroethene) is used to make coverings for electrical cables. It has replaced the use of rubber. (i) State two properties of poly(chloroethene) that are common to plastics in general, and make it suitable

for this use. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) State two ways in which poly(chloroethene) is better than rubber for this use. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Describe two environmental problems that are associated with the disposal of plastics. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 9

name and structure of monomer name and structure of polymer

ethene poly(ethene)

chloroethene poly(chloroethene)

phenylethene

H Cl

C C

H H

H H

C C

H H

H H

C C

H H

H Cl

C C

H H

H C6H5

C C

H H

(ii) (i)

n

n

n

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GCSE CHEMISTRY PRODUCTS FROM OIL

Medium Demand Questions QUESTIONSHEET 12 The table below gives some information about monomers and the polymers that can be made from them. (a) Complete the table. [4] (b) What is meant by the term ‘monomer’? ......................................................................................................................................................................... [1] (c) What is meant by the term ‘polymer’? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Write down the molecular formula of tetrafluoroethene. ......................................................................................................................................................................... [1] (e) Poly(ethene) can sometimes be used in place of steel. Give one advantage of using poly(ethene) in this way. ......................................................................................................................................................................... [1]

TOTAL / 9

monomer structure structure polymer

propene

poly(tetrafluoroethene)

A B

C D

H H

C C

H H

H CH3

C C

H H

H H

C C

H H

F F

C C

F F

ethene poly(ethene)

n

n

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GCSE CHEMISTRY PRODUCTS FROM OIL Medium Demand Questions QUESTIONSHEET 13 (a) To which homologous series does decane belong? ......................................................................................................................................................................... [1] (b) Cracking decane can produce the following products: ethene C2H4 pentane C5H12 propene C3H6 Which of these are unsaturated? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Cracking decane can sometimes produce just two types of molecule. If one of these products is ethene, give the formula and name of the other one. (i) formula ......................................................................................................................................................................... [1] (ii) name ......................................................................................................................................................................... [1] (d) What are the economic advantages of cracking? .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) Name two chemicals that can be made from ethene. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 9

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GCSE CHEMISTRY PRODUCTS FROM OIL

Medium Demand Questions QUESTIONSHEET 14 Some of the products of the distillation of crude oil are used as fuels. To find out the products formed when hydrocarbons burn, the apparatus below is used. (a) Name the product collected in tube A. ......................................................................................................................................................................... [1] (b) What will happen to the limewater? ......................................................................................................................................................................... [1] (c) Some fuels leave a black deposit on the inside of the thistle funnel. (i) What is this deposit? ......................................................................................................................................................................... [1] (ii) Why does it form? ......................................................................................................................................................................... [1] (iii) What other product could be formed under these circumstances? ......................................................................................................................................................................... [1]

TOTAL / 5

A colourless liquid condenses here

Thistle funnel

TUBE A

Limewater

To vacuum pump (this draws the

gaseous combustion products through the

apparatus)

Kerosene (paraffin) in spirit burner

Ice

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GCSE CHEMISTRY PRODUCTS FROM OIL Medium Demand Questions QUESTIONSHEET 15 Ethene can be used to make ethanol, C2H5OH. (a) Write an equation for this reaction. ......................................................................................................................................................................... [2] (b) Ethanol can be used to make substances known as esters. Esters are often used as flavourings. The table shows some esters. (i) Which element is present in esters, which is not present in hydrocarbons? ......................................................................................................................................................................... [1] (ii) An ester found in apple flavouring contains five carbon atoms, ten hydrogen atoms and two oxygen

atoms. Complete the formula of the apple flavouring given below. [1] (iii) Many of the esters are used as flavourings in food additives. Give two arguments for and two against the use of food additives. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [4]

(Continued...)

C3H7 C O

O

C3H7 C O

O

C5H11

C3H7 C O

O

C2H5

CH3 C O

O

C5H11

FLAVOURING

BANANA

APRICOT

PINEAPPLE

FORMULA OF ESTER

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GCSE CHEMISTRY PRODUCTS FROM OIL

QUESTIONSHEET 15 CONTINUED (c) Ethanol can be made from the fermentation of sugars. In Brazil, ethanol produced in this way is added to petrol. The mixture is known as Gasohol. (i) Suggest why this is an economic process in Brazil, but would not be possible in Britain. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Great care is taken in selling Gasohol. What is the danger of making it too freely available? ......................................................................................................................................................................... [1] (d) State another major use of ethanol. ......................................................................................................................................................................... [1]

TOTAL / 12

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GCSE CHEMISTRY PRODUCTS FROM OIL

Medium Demand Questions QUESTIONSHEET 16 (a) Complete the table showing the names, molecular formulae and structural formulae of three compounds

obtained from crude oil.

name molecular formula structural formula

butane C4H10

pentane

hexane

[4] (b) Butane is highly flammable. Suggest two precautions which must be taken when storing it. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Ethane boils at –88oC and ethene at –104oC. Why are they difficult to separate? ......................................................................................................................................................................... [1]

TOTAL / 7

H H H H

C C C C C

H H H H

H

H

H

H

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GCSE CHEMISTRY PRODUCTS FROM OIL

Low Demand Questions QUESTIONSHEET 17 The graph shows the percentage of North Sea crude oil which distils off during fractional distillation at different temperatures. (a) From the graph estimate the percentage which distils:

(i) below 20oC. ......................................................................................................................................................................... [1] (ii) between 40oC and 75oC (petrol fraction).

......................................................................................................................................................................... [1] (iii) between 75oC and 150oC (naphtha fraction).

......................................................................................................................................................................... [1] (b) In what physical state would you expect the fraction below 20oC to be in?

......................................................................................................................................................................... [1]

(c) The table below gives the uses of the products from crude oil.

use % of oil used

heating 44 road transport 37 generating electricity 8 making chemicals

Calculate the percentage of crude oil used for making chemicals. ......................................................................................................................................................................... [1]

TOTAL / 5

100

80

60

40

20

0 100 200 300 400

Distillation temperature (oC)

Percentage of crude oil

distilled

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GCSE CHEMISTRY PRODUCTS FROM OIL Low Demand Questions QUESTIONSHEET 18 Detergents, paints and inks are all made from the components of crude oil. (a)(i) What is a detergent? ......................................................................................................................................................................... [1] (ii) Explain why it is important that detergents are biodegradable. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) (i) Inks are often mixtures of different coloured dyes. What technique could you use to prove this? ......................................................................................................................................................................... [1] Ben and Jessica used this technique to compare the inks from different pens. Their results are shown below. (ii) Why did they draw the starting line in pencil? ......................................................................................................................................................................... [1] (iii) Which dye did the two inks both contain? ......................................................................................................................................................................... [1] (iv) Which colour was only found in ink B? ......................................................................................................................................................................... [1]

TOTAL / 7

A B

BLUE

YELLOW

RED

ORANGE

BLUE

YELLOW

STARTING LINE (DRAWN IN PENCIL)

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GCSE CHEMISTRY PRODUCTS FROM OIL

Low Demand Questions QUESTIONSHEET 19 (a) The table shows some of the uses of plastics.

Complete the table by filling in the best reason for each use from the list below. The first one has been done for you.

REASONS - lightweight, does not conduct electricity, non-toxic, easily moulded, can be coloured, flexible.

use best reason coating for wires does not conduct electricity guttering carrier bags combs sandwich bags

[4] (b) Crude oil, from which plastics are made, is first separated into fractions. Information about some of the fractions is given in the table.

fraction boiling range (oC) number of carbon atoms petroleum gas -160 to 40 1 to 4

petrol 40 to 80 5 to 10 naphtha 80 to 150 8 to 12 kerosene 150 to 240 10 to 16

(i) State a use for kerosene. ......................................................................................................................................................................... [1] (ii) In which fraction would this molecule be found? ......................................................................................................................................................................... [1] (iii) Propene has a boiling point of –47oC. In which fraction would propene be found? ......................................................................................................................................................................... [1]

TOTAL / 7

H C C C C C C

H H H H H H

H H H H H H

H

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GCSE CHEMISTRY PRODUCTS FROM OIL Low Demand Questions QUESTIONSHEET 20 Some fizzy drinks bottles are made from plastics. There are a number of ways of disposing of waste plastic bottles. Some are shown in the table below.

option method A burn them with other household rubbish B fill in quarries with household waste C re-use the bottles D make them into pellets of pure plastic

(a) Which two of the options help to conserve oil reserves? ......................................................................................................................................................................... [1] (b) Describe environmental problems which could be caused by options A or B. (i) Option A .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Option B .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) In option C, the bottles would need to be sterilised before being re-used. Glass bottles are sterilised using superheated steam. Why might this be unsuitable for plastic bottles? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) What could be done with heat produced in option A? ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY RATES OF REACTION

High Demand Questions QUESTIONSHEET 1 Calcium carbonate reacts with dilute hydrochloric acid to produce the gas carbon dioxide. The table below gives the results from a reaction when 40 cm3 dilute hydrochloric acid was added to one marble chip (calcium carbonate) at room temperature of 20oC. The calcium carbonate was in excess. One of the results in the table is unreliable.

Mass of flask and contents (g) 71.00 70.74 70.54 70.40 70.30 70.24 70.26 70.20 70.20 70.20

time (min) 0 1 2 3 4 5 6 7 8 9

(i) On the grid below plot a graph of the results shown in the table above. Draw a smooth curve through the reliable points and label it A. [3]

(Continued...)

Time (min)

Mass of flask and contents

(g)

0 70.00

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GCSE CHEMISTRY RATES OF REACTIONS QUESTIONSHEET 1 CONTINUED (ii) Sketch carefully on the grid the graph that would be obtained if: I. the same reaction was carried out at a temperature of 50oC. Label this graph B. [2] II. when an identical piece of calcium carbonate was reacted with only 20 cm3 of the dilute acid. Label this graph C. [2] (iii) Explain your answer to part (ii) I, in terms of particle collision. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 10

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GCSE CHEMISTRY RATES OF REACTION

High Demand Questions QUESTIONSHEET 2

Some chemical reactions may take place twice as quickly if their temperature is raised by 10oC. (a) If a particular reaction takes 32 minutes at 20oC, how long will it take if the temperature is raised to 50oC? .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Plot a graph of temperature against time taken to complete the reaction. [3]

(c) Explain why the line on your graph does not meet either axis. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

Tem

pera

ture

/ o C

Time / min

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GCSE CHEMISTRY RATES OF REACTIONS High Demand Questions QUESTIONSHEET 3 Carbonates react with acids to produce a salt, carbon dioxide and water. (a) The equation describes the reaction between calcium carbonate and hydrochloric acid. CaCO3 + 2HCl CaCl2 + CO2 + H2O (i) Add state symbols to complete the equation. [1] (ii) Name the salt produced in this reaction. ......................................................................................................................................................................... [1]

(iii) Use the relative atomic masses C =12, Ca = 40 and O=16 to calculate the relative formula mass of calcium carbonate. Show your working.

.............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iv) How much carbon dioxide can be produced from: A 100 g calcium carbonate? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] B 1 g calcium carbonate? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(b) A student wished to measure the production of carbon dioxide in the above reaction. She considered the two methods outlined in the diagram.

(Continued...)

Method A Method B

1 g calcium

carbonate

add 25 cm3

hydrochloric acid

boiling tube with 25 cm3

hydrochloric acid

weigh immediately

leave for 2 minutes

reweigh

weigh

pour acid into beaker, replace boiling tube

in beaker

leave for 2 minutes

reweigh

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GCSE CHEMISTRY RATES OF REACTION

QUESTIONSHEET 3 CONTINUED

(i) Before carrying out the experiment, she performed the calculation in part (a) (iv) B of this question.

Suggest how this information could be of use to her. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Explain why, of the two methods shown, method B would provide a more reliable estimate of the

amount of carbon dioxide produced during the reaction. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY RATES OF REACTIONS High Demand Questions QUESTIONSHEET 4 Raj’s chemistry teacher puts a beaker of sodium thiosulphate on the windowsill. Raj can clearly see a tree on the school field through the beaker. The teacher adds hydrochloric acid to the beaker. After 120 seconds Raj cannot see the tree although he is looking carefully. (a) Explain why. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] The teacher repeats the experiment with three other classes. The tree disappears from view at different times.

Class Time for tree to disappear in seconds

9X 120 9Y 200 9Z 150

The three experiments were identical except for the day on which they were done. (b) Which class did the experiment: - (i) on a warm spring day? ......................................................................................................................................................................... [1] (ii) during a summer heat wave? ......................................................................................................................................................................... [1] (iii) on a January day when the school heating was not working well? ......................................................................................................................................................................... [1]

The following year the local group of schools agree to do the same experiment on the same day under exactly the same conditions using the same chemicals. They look at objects that are the same distance away.

The results are: -

School Time for tree to disappear in seconds

St Peter’s 110 St Paul’s 100 St Mary’s 150

The teachers tested the chemicals used. They found that the sodium thiosulphate was of different concentration in each school.

(c)(i) Which school had the strongest solution? ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY RATES OF REACTION

QUESTIONSHEET 4 CONTINUED

(ii) Give reasons for your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] Hanif decides to use an ultraviolet lamp and an electric motor powered by a photoelectric cell. (d) How could he use this equipment to measure the cloudiness of the liquid in a more objective way? Draw a diagram of how the equipment might be set up. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ..............................................................................................................................................................................

[4]

TOTAL / 12

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GCSE CHEMISTRY RATES OF REACTIONS High Demand Questions QUESTIONSHEET 5 Cotton is starched to make it easier to weave into denim cloth. Before the cloth is made up into clothing the starch is removed so that it can be more easily sewn. Denim from a newly woven roll is tested to find out the best conditions for the removal of starch using the biological catalyst amylase. A solution of amylase is made up and five equal pieces are cut from the roll of denim. Equal quantities of amylase are added to four of the five pieces in separate beakers. The beakers are kept at temperatures of 20oC, 40oC, 60oC and 80oC respectively for 15 minutes. Afterwards all five pieces are tested for starch. (a) (i) What is a catalyst? ......................................................................................................................................................................... [2] (ii) What is the name given to biological catalysts? ......................................................................................................................................................................... [1] (b) (i) Which of the cotton samples would you expect to contain the most starch? ......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (iii) Which sample would you expect to contain the least starch? ......................................................................................................................................................................... [1] (iv) Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (v) What chemical is most often used to detect starch? ......................................................................................................................................................................... [1]

TOTAL / 11

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GCSE CHEMISTRY RATES OF REACTION

High Demand Questions QUESTIONSHEET 6

The following equation shows what happens when magnesium ribbon reacts with hydrochloric acid. Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) (a) What would you see happening to the magnesium ? ......................................................................................................................................................................... [1] (b) 40 cm3 of gas is collected in 10 seconds. What is the rate of reaction? ......................................................................................................................................................................... [1] (c) How would the rate compare if you used very dilute hydrochloric acid? Explain why. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) State two ways in which the reaction could be speeded up besides changing the concentration of hydrochloric acid. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) Calculate how many moles of hydrogen gas are collected. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

[24 dm3 is the volume of 1 mole of gas at room temperature]

TOTAL / 8

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GCSE CHEMISTRY RATES OF REACTIONS High Demand Questions QUESTIONSHEET 7 When 0.15 M sodium thiosulphate solution (Na2S2O3(aq)) is added to hydrochloric acid, sulphur is formed.

(a) What would you observe during the reaction? ......................................................................................................................................................................... [1]

(b) What other products are formed? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(c) Apart from heating it, how else could you speed up the reaction? How would this work?

.............................................................................................................................................................................. ......................................................................................................................................................................... [2]

The following results table was obtained by mixing various amounts of sodium thiosulphate solution, water and 1 M hydrochloric acid.

Na2S2O3(aq) 50 40 30 20 10 H2O(l) 0 10 20 30 40

Volume (cm3) HCl(aq) 5 5 5 5 5

Reaction Time (s) 5 13 27 56 3 min

(d) (i) Plot a graph of the results [3]

(Continued...)

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GCSE CHEMISTRY RATES OF REACTION

QUESTIONSHEET 7 CONTINUED

(ii) Which variable are you testing? ......................................................................................................................................................................... [1] (iii) Why is the volume of acid kept the same? ......................................................................................................................................................................... [1] (iv) What would you observe during the reaction? ......................................................................................................................................................................... [1]

TOTAL / 11

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GCSE CHEMISTRY RATES OF REACTIONS High Demand Questions QUESTIONSHEET 8 Yoghurt is made from milk. Yoghurt contains lactic acid formed from lactose, the sugar present in milk. Recently a new type of yoghurt has appeared in the shops in which bacteria from Russian cosmonauts has been used in the process. (a) Describe a test to show that an acid is formed when milk is turned into yoghurt. State the result of the test. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) For all practical purposes, a solution of lactose does not change into lactic acid. Adding bacteria increases the rate of reaction. What is meant by the phrase ‘rate of reaction’? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Why does the addition of bacteria have this effect? ......................................................................................................................................................................... [1] (d) Describe or draw diagrams to show what is happening to individual molecules of lactose in the reaction to form lactic acid molecules in yoghurt. .............................................................................................................................................................................. ..............................................................................................................................................................................

[3]

(e) After a while the rate of formation of lactic acid decreases. Why is this? ......................................................................................................................................................................... [1] (f) The yoghurt – milk mixture is heated to about 70oC.What effect does this have on the rate of the

production of lactic acid? Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11

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GCSE CHEMISTRY RATES OF REACTION

Medium Demand Questions QUESTIONSHEET 9 The apparatus shown can be used to collect gas formed by reacting magnesium and sulphuric acid. The following table of data was collected. Time (s) 0 2 4 6 8 10 Volume (cm3) 0 10 16 20 - 22

(a) Plot a graph of the results. [3]

(Continued...)

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GCSE CHEMISTRY RATES OF REACTIONS QUESTIONSHEET 9 CONTINUED (b) One experimental result was missed. (i) What value could it have? ......................................................................................................................................................................... [1] (ii) Why is it easy to miss results like this during experiments? ......................................................................................................................................................................... [1] (c) (i) Which gas is formed in the reaction ? ......................................................................................................................................................................... [1] (ii) How could you test for this gas? ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY RATES OF REACTION

Medium Demand Questions QUESTIONSHEET 10 Some cars are fitted with catalytic converters to remove harmful substances from exhaust gases. The platinum catalyst is coated onto a honeycombed ceramic support. It works best when the engine has warmed up. (a)(i) Explain why a honeycombed support is better than a solid one. ......................................................................................................................................................................... [1] (ii) Explain why the catalyst works better when the engine is warm. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Heavy metals may stick to the catalyst and prevent it from working. The catalyst is said to be poisoned. (i) Explain how catalysts work and how poisoning with heavy metals prevents this. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) Why should the owners of cars with catalytic converters always use unleaded petrol? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY RATES OF REACTIONS Medium Demand Questions QUESTIONSHEET 11 Hydrogen peroxide (H2O2) breaks down slowly to form water and oxygen. (a) Write a balanced symbol equation for the reaction. ......................................................................................................................................................................... [2] (b) The reaction can be greatly speeded up by a catalyst. (i) Name a possible catalyst. ......................................................................................................................................................................... [1] (ii) How does the catalyst work? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) How could you show that the catalyst was unchanged at the end of the reaction? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY RATES OF REACTION

Medium Demand Questions QUESTIONSHEET 12 The diagram shows a flask of zinc metal reacting with hydrochloric acid on a chemical balance.

(a) How could this apparatus be used to measure the speed of the reaction? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) (i) What is the gas being produced? ......................................................................................................................................................................... [1] (ii) How would you test the gas to identify it? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Write an equation for the reaction which is taking place. ......................................................................................................................................................................... [2] (c) How would you expect the results to change if: (i) the temperature was increased? ......................................................................................................................................................................... [1] (ii) the zinc was ground into a fine powder? ......................................................................................................................................................................... [1] (iii) the concentration of the hydrochloric acid was increased? ......................................................................................................................................................................... [1]

TOTAL / 10

150 g

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GCSE CHEMISTRY RATES OF REACTIONS

Medium Demand Questions QUESTIONSHEET 13 Chemical reactions are caused when molecules of different chemicals collide. (a) Describe the effect of increasing the pressure of two gases on the rate of reaction using this collision theory. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) Cornflour is used on the production line in some sweet factories. It is carried in the air. Special precautions have to be taken to remove the cornflour from the air as a fire hazard. Why is this fine powder a fire hazard? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) 10 g of magnesium ribbon burns up in 1 minute. How fast would you expect 10 g of magnesium powder to burn? ......................................................................................................................................................................... [1] (d) Why is heat often provided as a means of speeding up chemical reactions? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) Why does food not keep for ever in a freezer? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY RATES OF REACTION

Medium Demand Questions QUESTIONSHEET 14 A research laboratory is investigating the effectiveness of various catalysts for the reduction of pollution in petrol powered car exhausts. They obtain the following results using their own ‘pollution units’, P. [10 P = 10 pollution units.]

Catalyst Petrol P

Carbon monoxide P

Oxides of nitrogen P

None 100 700 500 A 30 150 150 B 50 250 300 C 10 75 90

In his lab notebook the scientist uses the abbreviations ‘CO’, ‘NOx’ and ‘CH’. (a) What do these abbreviations stand for? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) (i) Which catalyst is most effective at reducing total pollution? ......................................................................................................................................................................... [1] (ii) Which is the largest pollutant in the exhaust before a catalyst is used? ......................................................................................................................................................................... [1] (iii) Which is the largest pollutant in the exhaust from the most effective catalyst? ......................................................................................................................................................................... [1]

TOTAL / 6

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GCSE CHEMISTRY RATES OF REACTIONS

Medium Demand Questions QUESTIONSHEET 15 Hydrogen peroxide and a catalyst are mixed in the apparatus below. The hydrogen peroxide decomposes into water and oxygen. The results obtained are represented on the graph below (a) (i) On the same axes, draw a line to represent the volume of oxygen produced when the reaction is repeated with 5 g of a granulated catalyst in the flask. Label this (i). [1] (ii) On the same axes, draw a line to represent the volume of oxygen produced when the reaction is repeated with 5 g of a powdered catalyst in the flask. Label this (ii). [1] (b) John measures the volume of gas produced when 5 g of two chemicals X and Y are added to hydrogen peroxide under identical conditions. His results for this experiment look like this. He claims that they show that Y is a better catalyst than X. John’s partner Steven does not agree.

(Continued...)

chemicals A or B added here

heat energy

30 60 90

volume of gas

time in seconds

no catalyst

30 60 90

volume of gas

time in seconds

Y

X

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GCSE CHEMISTRY RATES OF REACTION

QUESTIONSHEET 15 CONTINUED What does Steven find wrong with the results? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) After the experiment Steven recovers 5 g of X and 1 g of Y from the two experiments. He claims that

this shows that John is wrong. Why might he think this? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 8

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GCSE CHEMISTRY RATES OF REACTIONS Medium Demand Questions QUESTIONSHEET 16 200 cm3 of hydrogen peroxide solution are warmed in a flask. The volume of gas produced is measured using a syringe. After 30 seconds 5 g of a chemical A is added to the hydrogen peroxide and the volume of gas continues to be measured. The experiment is then repeated but this time another chemical, B, replaces A. A third experiment has chemical B replaced by chemical C. The graph below shows the volume of gas produced over time when the chemicals A, B and C are added. (a) What is the formula of hydrogen peroxide? ......................................................................................................................................................................... [1] (b) What is the gas produced? ......................................................................................................................................................................... [1] (c) (i) What is a catalyst? ......................................................................................................................................................................... [2] (ii) Which of the three chemicals A, B and C is not a catalyst? (Give a reason for your choice) .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Which of the three chemicals is the best catalyst? (Give a reason for your answer) .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) How much of the compounds B and C should be recovered from the flasks after the experiment? ......................................................................................................................................................................... [1]

TOTAL / 9

chemicals A, B or C added here

heat energy

volume of gas

30 60 time in seconds

A B

C

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GCSE CHEMISTRY RATES OF REACTION

Low Demand Questions QUESTIONSHEET 17 (a) List three ways of increasing the rate of a chemical reaction. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) Explain why it is not possible to light a dead tree with a match. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Why is it difficult to light coal, but coal dust in mines can cause explosions? .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY RATES OF REACTIONS Low Demand Questions QUESTIONSHEET 18 The graph below shows the volume of gas produced in an experiment over a period of time.

(a) Write down the letter which represents: (i) the point at which the reaction has first stopped. ......................................................................................................................................................................... [1] (ii) the point at which the reaction is going at its fastest. ......................................................................................................................................................................... [1] (b) Use the graph to estimate: (i) the volume of gas produced after 60 seconds. ......................................................................................................................................................................... [1] (ii) the time taken for 30 cm3 of gas to be collected. ......................................................................................................................................................................... [1] (c) If the experiment was repeated with a catalyst present, how much gas would you expect to collect in total? ......................................................................................................................................................................... [1] (d) (i) If the experiment in (c) was repeated with twice as much catalyst, how much gas would you expect to collect in total? ......................................................................................................................................................................... [1] (ii) Would the speed of collection of the gas be faster, slower or the same as in experiment (c)? ......................................................................................................................................................................... [1]

TOTAL / 7

A

B

C

D E

0 10 20 30 40 50 60 70 80 90 100 110 120

10

30

40

50

60

70

0

20

Time/s

Vol

ume

of g

as/ c

m3

20

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GCSE CHEMISTRY RATES OF REACTION

Low Demand Questions QUESTIONSHEET 19 Rates of reactions can be measured in a number of ways. (a) Name two pieces of apparatus which could be used to measure volumes of gases. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b)(i) If you were timing how long magnesium took to dissolve in different concentrations of acid, what controls would you use to make sure the experiment was fair? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) Which of the following would be best for timing the reactions? (Underline the correct answer) Stop clock kitchen clock alarm clock egg timer [1] (c) Which of the following pieces of apparatus would be most suitable for weighing a marble chip?

(Underline the correct answer) spring balance balance reading to 4 decimal places balance reading to 2 decimal places balance reading in whole grams [1]

TOTAL / 7

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GCSE CHEMISTRY RATES OF REACTIONS Low Demand Questions QUESTIONSHEET 20 Complete the following sentences. (i) Heat energy is measured in _______. (ii) One thousand of these is called a _______. (iii) A reaction which gives out heat is described as _______. (iv) A reaction which takes in heat is described as _______. (v) A _________ will speed up a chemical reaction without being permanently used up. (vi) Reactions involving gases can be speeded up using _________ pressure. (vii) Powders have a greater ______ _______ than lumps of a solid. (viii) Curtains fading and _______ are examples of reactions which (ix) are triggered by _______.

TOTAL / 9

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GCSE CHEMISTRY REACTIONS & FORMULAE

High Demand Questions QUESTIONSHEET 1 Look at the following section of the periodic table. Use only the elements shown to answer the following questions. (a) When metals react with non-metals they form ionic compounds. (i) How do metal atoms form ions? ......................................................................................................................................................................... [1] (ii) Write the symbol of a metal that forms +1 ions. ......................................................................................................................................................................... [1] (b) Write down the formulae of: (i) an aluminium ion. ......................................................................................................................................................................... [1] (ii) a chloride ion. ......................................................................................................................................................................... [1] (iii) aluminium chloride. ......................................................................................................................................................................... [1] (c) When non-metals react with non-metals they form molecules. (i) What type of bonding is found in molecules? ......................................................................................................................................................................... [1] (ii) Tetrachlormethane is a compound of carbon and chlorine. Write down the formula of tetrachloromethane. ......................................................................................................................................................................... [1] (iii) Ammonia exists as molecules. Draw a dot and cross diagram to show the bonding in ammonia.

[2] TOTAL / 9

6

Ca Sc Ti V Mn Cr Fe Co Ni Cu Zn Ga Ge As Se Br Kr K

Mg Na

Be Li

Al Si P S Cl Ar

B C N O F Ne

He H

1 2 3 4 5

7 0 6

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GCSE CHEMISTRY REACTIONS & FORMULAE High Demand Questions QUESTIONSHEET 2 When calcium carbonate (limestone) is heated it produces calcium oxide and carbon dioxide. (i) Complete the following equation CaCO3 → CaO + ________ [1] (ii) What name is given to this type of reaction? ......................................................................................................................................................................... [1] (b)(i) Calculate the relative molecular mass of calcium carbonate. (relative atomic masses: C=12, O=16, Ca=40) ......................................................................................................................................................................... [1] (ii) How many tonnes of calcium carbonate are needed to produce 280 tonnes of calcium oxide? .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 6

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GCSE CHEMISTRY REACTIONS & FORMULAE

High Demand Questions QUESTIONSHEET 3 (a) When magnesium burns in oxygen it produces magnesium oxide. Balance the following symbol equation. __Mg(s) + O2(g) → __MgO(s) [1] (b) Alison carefully reacted some magnesium with oxygen using the equipment below. She made sure that all the magnesium had reacted. Here are the results of Alison’s experiment. mass of crucible + lid = 40.1 g mass of crucible + lid + magnesium = 44.9 g mass of crucible + lid + magnesium oxide = 48.1 g Use Alison’s results to calculate the empirical formula of magnesium oxide. (relative atomic masses: O = 16, Mg = 24) .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [6]

TOTAL / 7

tongs

lid

heat

crucible coil of magnesium ribbon pipeclay triangle

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GCSE CHEMISTRY REACTIONS & FORMULAE High Demand Questions QUESTIONSHEET 4 The diagram shows an experiment to investigate the effect of heat on copper(II) sulphate crystals. (a)(i) Why is cold water used in the beaker? ......................................................................................................................................................................... [1] (ii) How could you identify the colourless liquid in tube B as water? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) When 2.5 g of blue copper(II) sulphate crystals were heated, 1.6 g of white solid were left in tube A. (i) Calculate the mass of water driven off in the experiment. ......................................................................................................................................................................... [1] (ii) Calculate the percentage of water driven off. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) The equation represents the change taking place on heating blue copper(II) sulphate crystals. CuSO4.5H2O ∏ CuSO4 + 5H2O (i) What type of change is taking place? ......................................................................................................................................................................... [1] (ii) Write an equation to represent what happens when water is added to white copper(II) sulphate. ......................................................................................................................................................................... [1] (ii) What symbol should be used instead of the arrow in the first equation? ......................................................................................................................................................................... [1]

TOTAL / 8

heat tube A

blue copper(ll) sulphate crystals tube B

colourless liquid

cold water

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GCSE CHEMISTRY REACTIONS & FORMULAE

High Demand Questions QUESTIONSHEET 5 Nitrogen is an important element to help plants to grow. Artificial fertilisers contain compounds of nitrogen. Two such compounds are sodium nitrate (NaNO3), ammonium nitrate (NH4NO3). (a) Calculate the relative molecular masses of each of these compounds. (Relative atomic masses: H = 1, C = 12, N = 14, O = 16, Na = 23) (i) sodium nitrate. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) ammonium nitrate. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (b) Calculate the percentage of nitrogen in: (i) sodium nitrate. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) ammonium nitrate. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Which of them would be best for a farmer to use? ......................................................................................................................................................................... [1] (d) Ammonia, NH3 has 82.4% of nitrogen in it. Give two reasons why it would be unsuitable for use as a fertiliser. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 9

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GCSE CHEMISTRY REACTIONS & FORMULAE High Demand Questions QUESTIONSHEET 6 (a) Calculate the empirical formulae of the following compounds. (Relative atomic masses: H=1, C=12, N=14, O=16, S=32, K=39, Fe=56) (i) a compound of 3.5 g nitrogen and 4 g oxygen. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) a compound of 50% oxygen and 50% sulphur. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) a compound of 39% potassium, 1% hydrogen, 12% carbon and 48% oxygen. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) 16.0 g of an oxide of iron formed from 11.2 g iron. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (b) Find (i) the empirical formula and (ii) the molecular formula of a compound containing 4.04% hydrogen, 24.24% carbon and 71.72% chlorine, given the following information: relative atomic masses: H=1, C=12, Cl=35.5 relative molecular mass of the compound = 99 (i) .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (ii) .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 14

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GCSE CHEMISTRY REACTIONS & FORMULAE

High Demand Questions QUESTIONSHEET 7 A chemist finds a compound in an unlabelled bottle. He carries out a number of experiments on it. Here are his results. colour black heat no change add dilute hydrochloric acid solution of green salt heat and pass hydrogen over it brown solid, gas which condenses to colourless liquid (a) Identify the black solid. ......................................................................................................................................................................... [1] (b)(i) Identify the green salt. ......................................................................................................................................................................... [1] (ii) What products would be formed when a solution of the green salt is electrolysed? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) How can the gas produced during electrolysis be identified by a chemical test? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c)(i) Name the brown solid produced in the fourth test. ......................................................................................................................................................................... [1] (ii) Name the liquid which condenses in the fourth test. ......................................................................................................................................................................... [1] (iii) Write an equation for the reaction. ......................................................................................................................................................................... [1] (iv) What is the role of hydrogen in this reaction? ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY REACTIONS & FORMULAE High Demand Questions QUESTIONSHEET 8 Barium chloride contains water of crystallisation (BaCl2.xH2O). Some barium chloride was heated in a basin. The results are shown below. mass of empty basin = 117.8 g mass of basin plus BaCl2.xH2O = 125.9 g mass of basin plus BaCl2 after heating = 124.7 g (a)(i) Why was the empty basin weighed? ......................................................................................................................................................................... [1] (ii) Calculate the mass of BaCl2.xH2O. ......................................................................................................................................................................... [1] (iii) Calculate the mass of BaCl2 after heating. ......................................................................................................................................................................... [1] (iv) Calculate the mass of water lost. ......................................................................................................................................................................... [1] (v) Calculate the percentage of water in the BaCl2.xH2O. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) What could be done to ensure that all the water had been lost? .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) Calculate the relative molecular masses of: (i) BaCl2 .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (ii) H2O .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (Relative atomic masses: H = 1, O = 16, Cl = 35.5, Ba = 137) (d) Use your previous answers to determine the value of x in BaCl2.xH2O. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 14

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 9 The following words describe ten different types of chemical reaction. decomposition precipitation combustion oxidation reduction reversible neutralisation exothermic endothermic displacement Write the correct word after each of the following descriptions of chemical reactions. (a) two solutions are mixed together and form an insoluble product ......................................................................................................................................................................... [1] (b) a reaction in which oxygen is removed from one of the reactants ......................................................................................................................................................................... [1] (c) a reaction which takes in heat from the surroundings ......................................................................................................................................................................... [1] (d) a reaction where products can form the original reactants ......................................................................................................................................................................... [1] (e) a single substance breaks down into two or more simpler ones ......................................................................................................................................................................... [1] (f) a substance loses electrons ......................................................................................................................................................................... [1] (g) one element takes the place of another in a compound ......................................................................................................................................................................... [1] (h) a substance burns in oxygen ......................................................................................................................................................................... [1]

TOTAL / 8

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GCSE CHEMISTRY REACTIONS & FORMULAE Medium Demand Questions QUESTIONSHEET 10 When calcium oxide reacts with water it forms calcium hydroxide (slaked lime). The reaction is exothermic. (a) Explain what is meant by an ‘exothermic reaction’. ......................................................................................................................................................................... [1] (b) The formula for a calcium ion is Ca2+ and that of a hydroxide ion is OH-. Write down the formula for calcium hydroxide. ......................................................................................................................................................................... [1] (c) Write down one use of slaked lime. ......................................................................................................................................................................... [1] (d) When slaked lime is dissolved in water, it produces a solution known as limewater. It is possible to make a small amount of calcium carbonate from limewater. Explain how this can be done. ......................................................................................................................................................................... [1] (e) How can calcium carbonate be converted into quicklime? ......................................................................................................................................................................... [1] (f) The reactions described above are often put together in a diagram called the calcium cycle. Explain the word “cycle” in this context. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 7

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 11 Solutions of different halogens were mixed with solutions of halide salts. The mixtures were shaken with some organic solvent. Halogens dissolve better in the solvent than in water and give distinctive colours. (chlorine - green, bromine - orange, iodine - violet) Here are the results of some experiments.

experiment halogen added halide salt colour after shaking

A chlorine potassium bromide orange B chlorine potassium iodide violet C bromine potassium chloride orange D bromine potassium iodide violet E iodine potassium chloride violet F iodine potassium bromide violet

(a) What type of reaction is taking place? ......................................................................................................................................................................... [1] (b) In which experiments are no reactions taking place? ......................................................................................................................................................................... [3] (c) Write a word equation for experiment A. ......................................................................................................................................................................... [1] (d) Write a symbol equation for experiment A. [2] (e) What do the experiments tell you about the relative reactivities of chlorine, bromine and iodide? .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (f) How would you expect fluorine to react with potassium chloride? ......................................................................................................................................................................... [1] (g) How would you expect chlorine to react with potassium fluoride? ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY REACTIONS & FORMULAE Medium Demand Questions QUESTIONSHEET 12 The table below gives information about the solubilities of a number of salts.

sodium potassium lead barium calcium chloride soluble soluble insoluble soluble soluble sulphate soluble soluble insoluble insoluble slightly

soluble nitrate soluble soluble soluble soluble soluble carbonate soluble soluble insoluble insoluble insoluble

(a) What can you say about the solubility of sodium and potassium salts? ......................................................................................................................................................................... [1] (b) What can you say about the solubility of nitrates? ......................................................................................................................................................................... [1] (c) What can you say about the solubility of lead salts? ......................................................................................................................................................................... [2] (d) Predict the products of the following reactions, underlining any precipitates. (i) sodium carbonate solution with lead nitrate solution .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) calcium chloride solution with potassium nitrate solution .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iii) barium chloride solution with sodium sulphate solution .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (e) Barium salts are poisonous, yet some X-ray patients have to drink barium sulphate. Explain why they can do this without harming themselves. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 13 Five students wanted to find out what would happen when a certain compound was heated. They found that a gas was given off, so they measured the mass of the gas lost. Their results are shown below.

student 1 2 3 4 5 loss in mass (g) 0.032 0.06 0.083 0.09 0.107 volume of gas (cm3) 24 45 62 75 80

(a) Plot the results on the graph. [4]

(Continued...)

loss

in m

ass (

g)

volume of gas (cm3)

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GCSE CHEMISTRY REACTIONS & FORMULAE QUESTIONSHEET 13 CONTINUED (b) Which student’s result is incorrect? ......................................................................................................................................................................... [1] (c) Use your graph to estimate: (i) the volume of 0.05 g of the gas. ......................................................................................................................................................................... [1] (ii) the mass of 15 cm3 of the gas. [1] (d) The gas given off is oxygen. (i) How can the results of the experiment be used to confirm this? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Describe a chemical test that can confirm the identity of the gas. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 11

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 14 Study the diagram below. (a) (i) In which two tubes will the steel go rusty? ......................................................................................................................................................................... [1] (ii) Why does the steel not rust in the other two tubes? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) In which tube will the rusting occur fastest? Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Explain how ships and piers are prevented from rusting. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (d) State how each of the following is prevented from rusting. (i) cutlery ......................................................................................................................................................................... [1] (ii) car bodies ......................................................................................................................................................................... [1]

TOTAL / 10

tube A

tube B

tube C

tube D

distilled water

boiled and cooled water

cotton wool

salt solution

oil

calcium chloride

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 15 Zinc metal can be extracted from the mineral zinc blende (zinc sulphide) Stage 1 - zinc blende heated in air to produce zinc oxide. Stage 2 - zinc oxide reacted with sulphuric acid to make a solution containing zinc ions. Stage 3 - zinc metal is obtained by electrolysis of the solution. The zinc extracted is used to coat other metals and in alloys. (a) Suggest two advantages of alloys over pure metals. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) (i) Name the metal that zinc is often used to protect. ......................................................................................................................................................................... [1] (ii) What is the process of covering a metal with zinc called? ......................................................................................................................................................................... [1] (c) (i) Apart from zinc oxide, what other product is formed when zinc blende is heated in air? ......................................................................................................................................................................... [1] (ii) The formula of zinc oxide is ZnO. The formula of an oxide ion is O2 -. What is the formula of a zinc ion? ......................................................................................................................................................................... [1] (d) What type of reaction occurs when zinc oxide reacts with sulphuric acid? ......................................................................................................................................................................... [1] (e) Zinc can also be extracted from zinc oxide by heating it with coke. (i) What is the main element in coke? ......................................................................................................................................................................... [1] (ii) Write an equation for the reaction between zinc oxide and coke. ......................................................................................................................................................................... [1] (iii) What type of reaction involves the removal of oxygen? ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY REACTIONS & FORMULAE

Medium Demand Questions QUESTIONSHEET 16 The key below is used to identify five carbonates and a hydrogencarbonate. (a) (i) Which soluble compound gives off carbon dioxide, but gives no smell? ......................................................................................................................................................................... [1] (ii) What type of substance will react with any carbonate or hydrogencarbonate to produce carbon dioxide? ......................................................................................................................................................................... [1] (iii) Only one carbonate in the key produces no carbon dioxide when heated. Which one? ......................................................................................................................................................................... [1] (b) Tablets for upset stomachs often contain citric acid and magnesium carbonate. Describe and explain what happens when these tablets are added to water. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) A teaspoon of sodium hydrogencarbonate is added when making gingerbread. (i) What is the purpose of the sodium hydrogencarbonate? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Why would sodium carbonate be unsuitable for this purpose? ......................................................................................................................................................................... [1]

TOTAL / 8

Does it give off carbon dioxide when heated?

Does it dissolve in water?

Is it green?

copper carbonate

ammonium carbonate

Does it smell of ammonia when

heated?

Does it give a red flame test?

sodium hydrogen- carbonate

magnesium carbonate

calcium carbonate

sodium carbonate

No

No

Yes No

No

Yes

Yes

Yes No

Yes

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GCSE CHEMISTRY REACTIONS & FORMULAE

Low Demand Questions QUESTIONSHEET 17 Quicklime, CaO, is made by heating limestone, CaCO3, in a rotating kiln. Limestone is added at the top of the kiln. Turning the kiln lets the limestone move slowly to the bottom as it is heated. Quicklime is formed and is taken from the bottom. (a) Give the chemical name for: (i) quicklime ......................................................................................................................................................................... [1] (ii) limestone ......................................................................................................................................................................... [1] (b) Heat is required for the reaction to take place. What name is given to reactions which take in heat? ......................................................................................................................................................................... [1] (c) James investigated this reaction. He heated a piece of limestone on the edge of a gauze. Describe what he saw. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) Before the rotating kiln was invented, each batch of limestone had to be heated separately. Suggest one advantage that the rotating kiln has over the older method. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (e) There are proposals to extend a limestone quarry. (i) Give two arguments that the quarry owners could use in favour of the proposed extension. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Give two arguments that those against the extension could use. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY REACTIONS & FORMULAE

Low Demand Questions QUESTIONSHEET 18 (a) Some students decided to investigate the chemistry of seashells. They started by adding hydrochloric acid to some pieces of seashell. The mixture fizzed. They decided to find out if the gas was carbon dioxide. (i) Complete the diagram below to show how they could do this. [3] (ii) What result would they see if the gas was carbon dioxide? ......................................................................................................................................................................... [2] (b) They then heated a small piece of shell in a flame. Different substances give different colours when put in a flame.

substance colour of flame sodium chloride yellow potassium chloride pink calcium chloride red copper chloride green

(i) Why is copper wire not used for the test? ......................................................................................................................................................................... [1] (ii) How is the test wire cleaned between each test? ......................................................................................................................................................................... [1] The shells turned the flame a red colour. (iii) Which metal is in the seashells? ......................................................................................................................................................................... [1] (c) Use the results of the two tests to select the chemical name of the substance from which seashells are

made from the list below. sodium chloride sodium carbonate calcium carbonate calcium chloride ......................................................................................................................................................................... [1]

TOTAL / 9

sea shells

hydrochloric acid

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GCSE CHEMISTRY REACTIONS & FORMULAE Low Demand Questions QUESTIONSHEET 19 Some bottles of chemicals were imported from Germany. Their labels are in German. (a) Which bottle contains a potassium compound? ......................................................................................................................................................................... [1] (b) (i) Which bottle contains an element? ......................................................................................................................................................................... [1] (ii) What gas is formed when this element is added to dilute sulphuric acid? ......................................................................................................................................................................... [1] (c) Which bottle contains a flammable substance? ......................................................................................................................................................................... [1] (d)(i) Which bottle contains a compound of four elements? ......................................................................................................................................................................... [1] (ii) What does the hazard label on this bottle mean? ......................................................................................................................................................................... [1] (e) The gas, hydrogen, is known in German as “Wasserstoff”. Wasser means water. Suggest an explanation for the name. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 8

Phosphorsaure H3PO4

Zinc Zn

Ethanol C2H5OH

Kalium hydrogen sulfat

KHSO4

A B

C D

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GCSE CHEMISTRY REACTIONS & FORMULAE

Low Demand Questions QUESTIONSHEET 20 (a) The diagram shows a cross section through a type of blast furnace, which was used in the Iron Age. (i) The charcoal is the fuel for the furnace. Charcoal is mainly carbon. Write an equation for the burning of charcoal in a plentiful supply of air. ......................................................................................................................................................................... [1] (ii) Some carbon monoxide may also be formed. Why is this undesirable? ......................................................................................................................................................................... [1] (b) The iron ore is reduced to iron when the furnace gets hot enough. (i) What is meant by ‘reduced’ in this reaction? ......................................................................................................................................................................... [1] (ii) Name a substance that is oxidised in the process. ......................................................................................................................................................................... [1] (c) When the furnace was opened, the clay had changed. List three of the changes to the clay. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 7

AIR BLASTED HERE

CLAY

IRON FORMED

HERE

CHARCOAL

IRON +CHARCOAL

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GCSE CHEMISTRY THE PERIODIC TABLE

High Demand Questions QUESTIONSHEET 1

The boxes represent particles of different gases. One box shows the particles of elements in group 0 (group 8).

(a) (i) What name is given to group 0 (8) elements? ......................................................................................................................................................................... [1]

(ii) Name two elements from group 0. ......................................................................................................................................................................... [2]

(b) (i) Which box best represents particles from group 0 elements? ......................................................................................................................................................................... [1]

(ii) Explain the reason for your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(c) A lighted splint is put into a gas jar of helium. What would happen? ......................................................................................................................................................................... [1] (d) Some properties of elements change as you go down their group in the periodic table. For each property listed below, comment on if and how it changes as you go down group 0.

(i) reactivity ......................................................................................................................................................................... [1]

(ii) density ......................................................................................................................................................................... [1]

(iii) metal or non-metal ......................................................................................................................................................................... [1]

(e) Which would be the best method to distinguish between different samples of group 0 gases? Choose from the list below: (i) shake the sample with water and add an indicator, (ii) do a flame test, (iii) put a lighted splint into a sample of each gas, (iv) measure the density of each. ......................................................................................................................................................................... [1]

TOTAL / 10

A B C D

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GCSE CHEMISTRY THE PERIODIC TABLE High Demand Questions QUESTIONSHEET 2 The diagram represents a sodium atom and a sodium ion. (a) (i) Which diagram represents the sodium atom? ......................................................................................................................................................................... [1]

(ii) Give reasons for your choice. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(iii) Sodium is in group 1 of the periodic table. How can you tell this from its electron structure? ......................................................................................................................................................................... [1]

(b) (i) What is an ion? ......................................................................................................................................................................... [1]

(ii) Potassium is also in group 1 of the periodic table. What is the symbol for the potassium ion? Choose from: K K+ K2+ K- K2- ......................................................................................................................................................................... [1]

(c) Group 1 elements are stored in oil. Suggest the reason for this. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

(d) A small piece of potassium is taken out of its bottle and cut. The surface is silver coloured and shiny, but after a few minutes it looked dull and white. A chemical reaction had taken place. (i) With what had the potassium reacted?

......................................................................................................................................................................... [1]

(ii) What is the name of the substance formed on the outside of potassium?

......................................................................................................................................................................... [1]

(iii) Write a word equation for the reaction. ......................................................................................................................................................................... [1]

(iv) Write a balanced symbol equation for this reaction. ......................................................................................................................................................................... [2] TOTAL / 13

x

x x x

x x

x x

x x

x

x x x

x x

x x

x x

x

A B

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GCSE CHEMISTRY THE PERIODIC TABLE

High Demand Questions QUESTIONSHEET 3 Lithium (Li) can be burnt in chlorine (C12) to give lithium chloride. (a) (i) Write a word equation for the reaction. ......................................................................................................................................................................... [1] (ii) Write a balanced symbol equation for the reaction. ......................................................................................................................................................................... [1] (b) (i) Which group in the periodic table does lithium belong to? ......................................................................................................................................................................... [1] (ii) How many electrons are there in its outside shell? ......................................................................................................................................................................... [1] (iii) How many electrons are there in the outside shell of the chlorine? ......................................................................................................................................................................... [1] (c) Use a ‘dot and cross’ diagram to explain how lithium and chlorine react together. Show only the electrons in the outer shell.

[3]

(d) Sodium also reacts with chlorine. (i) Will the reaction be more reactive or less reactive than with lithium? ......................................................................................................................................................................... [1] (ii) What is the common name of the product? ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY THE PERIODIC TABLE High Demand Questions QUESTIONSHEET 4 The diagram below shows the arrangement of particles in a crystal of sodium chloride. (a) (i) Each particle has a charge. What type of particles have a charge? Choose from: atoms, molecules, ions. ......................................................................................................................................................................... [1]

(ii) In sodium chloride what is the name of the particle with the positive charge?

......................................................................................................................................................................... [1]

(iii) What is the name of the particle with the negative charge? ......................................................................................................................................................................... [1]

(iv) What holds the particles together? ......................................................................................................................................................................... [1]

(b) The table below gives some information about sodium and chlorine. Complete the table.

element symbol electron arrangement

number of electrons in outside shell

number of electron shells

periodic table group number

Sodium Na 2.8.1 (i) (iii) (v)

Chlorine C1 2.8.7 (ii) (iv) (vi) [6]

(c) Use the information in the table to explain:

(i) why sodium chloride has positively and negatively charged particles. (Use dot and cross diagrams to help your explanation.) .............................................................................................................................................................................. ......................................................................................................................................................................... [5]

(ii) why the formula for sodium chloride is NaC1. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] TOTAL / 16

Key +

-

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GCSE CHEMISTRY THE PERIODIC TABLE

High Demand Questions QUESTIONSHEET 5 Sarah is diving into a swimming pool. She can smell chlorine. (a) (i) Explain why there is chlorine in the swimming pool. ......................................................................................................................................................................... [1] (ii) Iodine is the same group of the periodic table as chlorine. Give a use of iodine. ......................................................................................................................................................................... [1] (b) (i) Chlorine and iodine are in group 7 of the periodic table. What name is given to group 7 elements? ......................................................................................................................................................................... [1] (ii) Is chlorine a metal or non-metal? ......................................................................................................................................................................... [1] (iii) Is iodine a metal or non-metal? ......................................................................................................................................................................... [1] (c) (i) The atomic number of chlorine is 17. What does this tell you? ......................................................................................................................................................................... [1] (ii) The electron arrangement of chlorine is 2.8.7. How many electron shells does it have? ......................................................................................................................................................................... [1] (iii) Iodine has five electron shells. How many electrons are in the outer shell of iodine? ......................................................................................................................................................................... [1] (iv) The symbol for chlorine is C1, iodine is I and sodium Na. Chlorine combines with sodium to make sodium chloride, NaC1. Iodine also reacts with sodium. What will be the name and formula of the compound formed? ......................................................................................................................................................................... [2]

TOTAL / 10

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GCSE CHEMISTRY THE PERIODIC TABLE High Demand Questions QUESTIONSHEET 6 Emma takes a photograph of a friend. Her friend tells her that the film is coated with silver bromide which is sensitive to light. Silver bromide can be made by reacting silver nitrate with sodium bromide. The chemical reaction can be represented as: Ag+(aq) + Br- (aq) ∧ AgBr(s)

(a) (i) What happens to silver bromide in the light? ......................................................................................................................................................................... [1] (ii) Give another reaction which is affected by light energy. ......................................................................................................................................................................... [1] (b) (i) What type of particle is Br- ? ......................................................................................................................................................................... [1] (ii) Is silver bromide soluble in water? ......................................................................................................................................................................... [1] (c) (i) Suggest what would happen if a sample of silver iodide were left in the light. ......................................................................................................................................................................... [1] (ii) Silver iodide can be made in a similar way to silver bromide. Write an ionic equation to show this reaction. Include the state symbols. ......................................................................................................................................................................... [3]

TOTAL / 8

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GCSE CHEMISTRY THE PERIODIC TABLE

High Demand Questions QUESTIONSHEET 7 The symbols represent two different forms of chlorine atoms. (a) (i) What name is given to atoms of the same element that have different mass numbers? ......................................................................................................................................................................... [1] (ii) Why do the atoms have different mass numbers? ......................................................................................................................................................................... [1] (iii) What two things does the number 17 tell you about the structure of a chlorine atom? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) Calculate the number of neutrons in an atom of chlorine-35. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) A sample of chlorine is found to have a mass of 35.5. Explain why it is not a whole number. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (c) (i) A small amount of sodium was burnt in samples of chlorine-35 and chlorine-37. What difference,

if any, would you expect between the reactions?

......................................................................................................................................................................... [1] (ii) Explain your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Would chlorine-35 and chlorine-37 have the same boiling point? ......................................................................................................................................................................... [1] (iv) Give a reason for your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] TOTAL / 12

C1 35 17 C1 37

17

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GCSE CHEMISTRY THE PERIODIC TABLE High Demand Questions QUESTIONSHEET 8 The table below shows the elements on the third period. Sample of each of the elements were burnt in oxygen and the oxides formed were tested to see whether they were acids or bases.

11 Na

sodium 23

12 Mg

magnesium 24

13 A1

aluminium 27

14 Si

silicon 28

15 P

phosphorus 31

16 S

sulphur 32

17 C1

chlorine 35.5

18 Ar

argon 40

(a) (i) How many electron shells does the third period have? ......................................................................................................................................................................... [1] (ii) The element with atomic number 10 is neon. Explain in terms of electron arrangement why a new period starts after neon. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (b) (i) Which three elements in the third period are metals? ......................................................................................................................................................................... [1] (ii) What trend do you notice about metallic properties as you go across the period? ......................................................................................................................................................................... [1] (c) (i) Oxygen is in group 6. What does this tell you about the number of electrons in the outside shell? ......................................................................................................................................................................... [1] (ii) Write down formulae for the oxides of sodium, magnesium and aluminium. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3]

TOTAL / 9

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GCSE CHEMISTRY THE PERIODIC TABLE

Medium Demand Questions QUESTIONSHEET 9 Farah has balloons filled with three different gases. The symbols for the gases are written on each balloon. She lets go of the balloons. The diagram shows what happens.

(a) To which group of the periodic table do the gases belong? ......................................................................................................................................................................... [1] (b) (i) Predict what would happen to a balloon filled with krypton. ......................................................................................................................................................................... [1] (ii) Explain the reasons for your answer. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) (i) Draw the electron structure of helium.

[1] (ii) Explain how the electron structure is related to the chemical properties of helium. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (d) (i) Helium is often used to fill balloons. Give two reasons why this is a good choice. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Neon, argon and krypton are used to fill light bulbs. Give a reason for this. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] TOTAL / 11

He

Ar

Ne

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GCSE CHEMISTRY THE PERIODIC TABLE Medium Demand Questions QUESTIONSHEET 10 John has three bottles containing salts. One contains sodium chloride, one lithium chloride and one potassium chloride, but the labels have come off. (a) (i) Sodium, potassium and lithium all belong to the same group of the periodic table. What is the group number? ......................................................................................................................................................................... [1] (ii) What is the name of the group? ......................................................................................................................................................................... [1] (iii) What colour are the three salts? ......................................................................................................................................................................... [1] (b) John needs to put the correct labels on the bottles. He does a flame test. Describe exactly how he does the flame test. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [3] (c) John puts his results in a table. Look at the table and fill in the names of the salts.

Bottle Colour of flame Name of salt

A Yellow

B Red

C Lilac

[3]

TOTAL / 9

A

B

C

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GCSE CHEMISTRY THE PERIODIC TABLE

Medium Demand Questions QUESTIONSHEET 11 The table below gives information about some of the elements in group 7.

Element Symbol Atomic No. Melting point (oC)

Boiling point (oC) Appearance

chlorine C1 17 -101 -34 greenish gas

bromine Br 35 -7 58 red liquid

iodine I 53 114 183 black solid (a) (i) Put the three elements in the table in their order of reactivity, with the most reactive first. ......................................................................................................................................................................... [1] (ii) Which property in the table above indicated the order of reactivity for group 7 elements? ......................................................................................................................................................................... [1] (b) (i) How many electrons are in the outside shell of a chlorine atom? ......................................................................................................................................................................... [1] (ii) Does the element chlorine usually exist as free atoms, molecules or ions? ......................................................................................................................................................................... [1] (iii) Explain your answer to (ii). .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (c) Fluorine is also in group 7. Its atomic number is 9. (i) Draw the electron arrangement for fluorine.

[2] (ii) Would you expect fluorine to be a solid, liquid or gas at room temperature? ......................................................................................................................................................................... [1] (iii) Predict what its melting point would be. ......................................................................................................................................................................... [1] (d) A sample of bromine is put in a test tube in a water bath at 60 oC. Suggest what will happen to it. ......................................................................................................................................................................... [1] TOTAL / 11

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GCSE CHEMISTRY THE PERIODIC TABLE Medium Demand Questions QUESTIONSHEET 12

Abdul adds some silver nitrate (AgNO3) solution to a sodium chloride (NaC1) solution. He notices a white precipitate. He leaves the test tube in bright sunlight. The precipitate went dark.

(a) (i) What colour is the sodium chloride solution? ......................................................................................................................................................................... [1] (ii) What is meant by ‘precipitate’? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) What is the name of the precipitate made? ......................................................................................................................................................................... [1] (b) (i) Write a word equation for the reaction. ......................................................................................................................................................................... [1] (ii) What is the state symbol for a solution in water? ......................................................................................................................................................................... [1] (iii) What is the state symbol for a precipitate? ......................................................................................................................................................................... [1] (iv) Write a symbol equation for the reaction, including the state symbols. ......................................................................................................................................................................... [2] (c) Abdul adds some silver nitrate to three more solutions, A, B and C. He puts the results in a table. Put a tick in the column if there was a halide present.

solution observation observation after leaving in sunlight was a halide present?

A no reaction no change B pale yellow precipitate went dark C yellow precipitate went dark

[2]

TOTAL / 11

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GCSE CHEMISTRY THE PERIODIC TABLE

Medium Demand Questions QUESTIONSHEET 13 Below is the first part of the periodic table, giving the elements with their atomic numbers.

0 I

II

H 1

III

IV

V

VI

VII

He 2

Li 3

Be 4

B 5

C 6

N 7

O 8

F 9

Ne 10

Na 11

Mg 12

Al 13

Si 14

P 15

S 16

Cl 17

Ar 18

K 19

Ca 20

Sc 21

Ti22

V 23

Cr 24

Mn25

Fe26

Co27

Ni 28

Cu 29

Zn30

Ga31

Ge32

As33

Se 34

Br 35

Kr36

(a) (i) What is the name given to the group between atomic number 21 and 30? ......................................................................................................................................................................... [1] (ii) Are they metals or non-metals? ......................................................................................................................................................................... [1] (iii) What do the following symbols stand for? ..............................................................................................................................................................................

[3]

(b) Below are some properties of two elements.

element melting point boiling point relative density A 1535 2750 7.87 B 97.5 892 0.97

(i) Which element is from the group between atomic numbers 21 and 30? ......................................................................................................................................................................... [1] (ii) Using the properties in the table, suggest which elements would be most suitable for making a kettle. Give a reason for your answer. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Element number 22 is called titanium. From its position in the periodic table predict three properties you would expect it to have. Put a tick in the box by one property from each pair in the list below. soft hard can be pulled out to make a wire breaks easily when pulled dull surface that cannot be polished shiny surface that can be polished

[3]

TOTAL / 11

Fe: Cu: Zn:

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GCSE CHEMISTRY THE PERIODIC TABLE Medium Demand Questions QUESTIONSHEET 14 Saima heated some copper(II) carbonate (CuCO3) in a test tube. She noticed that the green copper carbonate changed to a black powder. A gas also came off which she passed through a liquid, A. (a) (i) Copper is a transition element. Name another element from this part of the periodic table. ......................................................................................................................................................................... [1] (ii) What is liquid A? ........................................................................................................................................................................ [1] (iii) Describe what Saima saw happening in A. .............................................................................................................................................................................. ......................................................................................................................................................................... [1] (iv) What is the name of the gas? ........................................................................................................................................................................ [1] (b) (i) What is the name of the black powder formed? ......................................................................................................................................................................... [1] (ii) Saima thinks that a chemical reaction has taken place. Give two pieces of evidence to support her idea. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Write a word equation for the reaction. ......................................................................................................................................................................... [1] (iv) Write a balanced symbol equation for the reaction. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY THE PERIODIC TABLE

QUESTIONSHEET 14 CONTINUED (c) Saima heated two more carbonates, zinc carbonate and sodium carbonate. She put her results in the table below.

substance appearance before heating appearance after heating gas given off

A white solid white solid no

B white solid solid yellow when hot, white when cold yes

(i) Which substance was zinc carbonate? ......................................................................................................................................................................... [1] (ii) Explain the reason for your choice. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iii) Explain why no gas was given off with A. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 14

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GCSE CHEMISTRY THE PERIODIC TABLE Medium Demand Questions QUESTIONSHEET 15 Three jars containing metal salts have lost their labels. One contains a salt of copper, one a salt of iron(II) and one a salt of iron(III). They can be distinguished by testing with sodium hydroxide solution. (a) (i) To what part of the periodic table do copper and iron belong? ......................................................................................................................................................................... [1]

(ii) What is the likely colour of the copper salt? ......................................................................................................................................................................... [1] (b) (i) Describe how to carry out the test with sodium hydroxide, and what would you look for. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) The table shows the results of testing the three salts with sodium hydroxide. Complete the table.

salt colour of precipitate metal ion in salt A blue B iron(II) C brown

[2] (c) (i) What is the symbol for the iron(II) ion? ......................................................................................................................................................................... [1] (ii) What is the symbol for the hydroxide ion? ......................................................................................................................................................................... [1] (iii) Write a balanced ionic equation to show the reaction between iron(II) ions and hydroxide ions. ......................................................................................................................................................................... [1]

TOTAL / 9

A B C

? ? ? ?

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GCSE CHEMISTRY THE PERIODIC TABLE

Medium Demand Questions QUESTIONSHEET 16 The table below shows the second and third periods of the periodic table. I II III IV V VI VII 0

3 Li

lithium 7

4 Be

beryllium 9

5 B

boron 11

6 C

carbon 12

7 N

nitrogen 14

8 O

oxygen 16

9 F

fluorine 19

10 Ne

neon 20

11 Na

sodium 23

12 Mg

magnesium 24

13 A1

aluminium 27

14 Si

silicon 28

15 P

phosphorus 31

16 S

sulphur 32

17 C1

chlorine 35.5

18 Ar

argon 40

(a) (i) The first period is not shown. How many elements are in the first period? ......................................................................................................................................................................... [1] (ii) How many elements are in the second period? ......................................................................................................................................................................... [1] (iii) What does the period number tell you about the arrangement of electrons in the atom? ......................................................................................................................................................................... [1] (b) (i) Find carbon in the table. Which period is it in? ......................................................................................................................................................................... [1] (ii) Which group is it in? ......................................................................................................................................................................... [1] (iii) What does the group number tell you about the structure of the carbon atom? ......................................................................................................................................................................... [1] (c) (i) There are two numbers, 6 and 12, in the box with carbon. 6 is the atomic number. What two things does the atomic number 6 tells you about an atom of carbon? .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) What is the number 12 called? ......................................................................................................................................................................... [1] (iii) What does the number 12 tell you about the structure of an atom of carbon? .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

TOTAL / 10

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GCSE CHEMISTRY THE PERIODIC TABLE Low Demand Questions QUESTIONSHEET 17 Below are the first 36 elements in the periodic table with their atomic numbers.

0 I

II

H 1

III

IV

V

VI

VII

He 2

Li 3

Be 4

B 5

C 6

N 7

O 8

F 9

Ne 10

Na 11

Mg 12

Al 13

Si 14

P 15

S 16

Cl 17

Ar 18

K 19

Ca 20

Sc 21

Ti22

V 23

Cr 24

Mn25

Fe26

Co27

Ni 28

Cu 29

Zn30

Ga31

Ge32

As33

Se 34

Br 35

Kr36

(a) Give the symbol for one example of each of the following: (i) a metal ......................................................................................................................................................................... [1] (ii) a gas ......................................................................................................................................................................... [1] (iii) a transition element ......................................................................................................................................................................... [1] (b) Find Cl (chlorine) in the table above. (i) What is the group number? ......................................................................................................................................................................... [1] (ii) Which period is it in? ......................................................................................................................................................................... [1] (iii) How many electron shells does it have? ......................................................................................................................................................................... [1] (iv) How many electrons are there in its outside shell? ......................................................................................................................................................................... [1] (c) Explain what is meant by ‘atomic number’. .............................................................................................................................................................................. ......................................................................................................................................................................... [1]

(Continued...)

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GCSE CHEMISTRY THE PERIODIC TABLE

QUESTIONSHEET 17 CONTINUED (d) (i) What name is given to the elements in group 0? ......................................................................................................................................................................... [1] (ii) What is the main chemical property of group 0 elements? ......................................................................................................................................................................... [1] (iii) How does their electron arrangement explain this chemical property? ......................................................................................................................................................................... [1]

TOTAL / 11

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GCSE CHEMISTRY THE PERIODIC TABLE Low Demand Questions QUESTIONSHEET 18 Group one elements react with water and a gas is given off. Lithium, potassium and rubidium were put in separate troughs of water, A, B and C. The diagrams show the reactions. ‘A’ fizzed gently and a gas was given off. ‘B’ reacted violently, burst into flames and cracked the trough. ‘C’ reacted vigorously and burst into flames. (a) Identify the elements A, B and C by completing the sentences below.

(i) The element in A was: ......................................................................................................................................................................... [1]

(ii) The element in B was: ......................................................................................................................................................................... [1]

(iii) The element in C was: ......................................................................................................................................................................... [1]

(b) The solution left in A was tested with litmus paper. What colour did the litmus paper go? ......................................................................................................................................................................... [1]

(c) The gas coming off in A was collected in a test tube and tested with a lighted splint. What happened? ......................................................................................................................................................................... [1]

(ii) What is the name of the gas? ......................................................................................................................................................................... [1]

(d) Sodium also reacts with water. (i) Will the reaction be more or less vigorous than that with lithium? ......................................................................................................................................................................... [1]

(ii) What are the names of the products of the reaction? ......................................................................................................................................................................... [1]

(e) Group 1 elements are called ‘alkali metals’. Suggest the reason for this. .............................................................................................................................................................................. .............................................................................................................................................................................. ......................................................................................................................................................................... [2]

TOTAL / 10

A B C

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GCSE CHEMISTRY THE PERIODIC TABLE

Low Demand Questions QUESTIONSHEET 19 Iron and copper are both transition elements. They can both be used to make pans. (a) (i) Give two physical properties of most transition elements that make them suitable for pans. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (ii) Why is copper not often used for pans? ......................................................................................................................................................................... [1] (iii) Copper is often used for electric wires. Give two properties of copper that make copper a good choice for this use. .............................................................................................................................................................................. ......................................................................................................................................................................... [2] (iv) Iron is used to make cars but not aeroplanes. Give one property of iron that makes it good to use for cars. ......................................................................................................................................................................... [1] Give one property of iron that makes it unsuitable for planes. ......................................................................................................................................................................... [1] (b) (i) Iron is used as a catalyst in the Haber process to make ammonia. What is the purpose of a catalyst? ......................................................................................................................................................................... [1] (ii) Platinum is used as a catalyst in catalytic converters in cars. Where in the periodic table would you expect to find platinum? ......................................................................................................................................................................... [1] (c) (i) Copper and iron both form ions with non-metals. What type of ions do they form? ......................................................................................................................................................................... [1] (ii) Write the symbols for a copper(II) ion and an iron(III) ion. ......................................................................................................................................................................... [2] TOTAL / 12

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GCSE CHEMISTRY THE PERIODIC TABLE Low Demand Questions QUESTIONSHEET 20 The following diagram shows part of the periodic table in which letters represent some elements. (These are not chemical symbols)

A B C D E

F G

You may use each letter once, more than once or not at all in this question. (i) Give the letter that represents the element that I is an unreactive gas .................................................................................................................... [1] II has one electron in its outside shell ........................................................................................... [1] III is in the same group as F ............................................................................................................ [1] IV is a yellow/green gas .................................................................................................................. [1] V is in the same period as E ........................................................................................................... [1] VI forms several coloured compounds ............................................................................................ [1] VII is used in light bulbs .................................................................................................................. [1]

TOTAL / 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) (i) change pH to 7 1 (ii) burette/measuring cylinder/syringe 1 (b) (i) 1 g 1 (ii) 30/10 1 = 3 g 1 (iii) concentration of sodium hydroxide 1 (c) 6 g in 100g 1 ⇒ no 1 TOTAL 8 QUESTIONSHEET 2 (a) 1. magnesium 2. zinc 3. nickel 4. copper 2 4 correct answers score 2 marks 2 correct answers score 1 mark (b) (i) hydrogen 1 (ii) burning splint/ignite/burn the gas squeaky pop 2 (c) (i) magnesium chloride 1 (ii) ionic 1 (iii) the forces of attraction/bonding between the ions are very strong large amount of energy required to break them 2

TOTAL 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES QUESTIONSHEET 3 (a) (i) sodium + oxygen → sodium oxide 1 (ii) Na2O 1 (iii) solid 1 (iv) purple 1 (b) (i) O2 (g) 2 (ii) accept answer between 4 and 6 1 (iii) any two from corrodes buildings/statues/metalwork kills/damages trees causes lakes to become acidic/kills animal and plant life 2

TOTAL 9

QUESTIONSHEET 4 (a) (i) covalent 1 (ii)

N

H

HH

8 electrons around N scores 1 mark correct bonding pairs scores 1 mark 2 (iii) forces between the molecules/ particles are weak these forces are easily overcome 2 (b) (i) particles move/ have kinetic energy randomly/in all directions or diffusion takes place from high concentration to low concentration 2 (ii) molecules/particles of ammonia are lighter 1 (iii) ammonium chloride 1

TOTAL 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) (i) carbon dioxide 1 limewater turns milky/white/cloudy 1 (ii) calcium sulphate 1 (b) (i) increases 1 (ii) greater surface area 1 particles collide more often 1 (c) (i) hydrogen 1 (ii) burning splint/produces squeaky pop 2 (iii) manufacture of ammonia/manufacture of margarine 1

TOTAL 10 QUESTIONSHEET 6 (a) One mark each for: yellow colourless yellow blue 4 (b) (i) bromophenol blue 1 (ii) bromophenol blue and thymol blue 2

TOTAL 7 QUESTIONSHEET 7 (a) calcium hydroxide 1 (b) 8 5 10 5 125 1 = 10 000 g/10 kg 1 (c) calcium oxide is corrosive/harms skin 1 (d) (i) Ca(OH)2 + 2HNO3 Ca(NO3) 2 + 2H2O 2 (ii) 1 mol Ca(OH)2 neutralises 2 mol HNO3 1 74 g Ca(OH)2 neutralises 126 g HNO3 1 37 g Ca(OH)2 is needed to neutralise 63 g HNO3 1

TOTAL 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES QUESTIONSHEET 8 (a) SO2 + Cl2 + 2H2O H2SO4 + 2HCl 2 (correct formulae 1, balancing 1) (b) 71g Cl2 react with 64 g SO2 1 so 71 mg Cl2 react with 64 mg SO2 1

and 1 mg Cl2 reacts with 7164 = 0.9 mg SO2 1

(c) A 10 / 2 = 5 B 50 / 5 = 10 1 B is greater 1

TOTAL 7

QUESTIONSHEET 9 (a) (i) 12 1 (ii) lemon juice 1 (iii) 7 1 (b) red or orange 1 (c) (i) accept any pH greater than 7 up to 14 1 (ii) neutralisation 1 (iii) water 1

TOTAL 7

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) green 1 (b) (i) neutralisation 1 (ii) reaction is faster/increases rate of the reaction increases surface area/more collisions between particles 2 (c) (i) 2 CO2 2 (ii) turns milky/white/cloudy 1 (iii) 24 + 12 + (16 5 3) 1 = 84 1

TOTAL 9

QUESTIONSHEET 11 (a) (i) burette 1 (ii) neutralisation 1 (iii) 7 1 (b) (i) hydrogen ion/H

+ 1 (ii) hydroxide ion/OH- 1 (iii) H+ + OH- → H2O 1 (c) (i) it is corrosive 1 (ii) any two from safety goggles plastic gloves wear lab coat use a tray to catch spillage 2

TOTAL 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES QUESTIONSHEET 12 (a) (i) red 1 (ii) hydrogen 1 (b) (i) blue/purple 1 (ii) hydroxide ion 1 (c) (i) 7 1 (ii) sodium sulphate 1 (iii) 2NaOH 2H2O 2 (d) a fertiliser 1

TOTAL 9

QUESTIONSHEET 13 (a) remains of dead plants became buried action of heat and pressure in the absence of oxygen over millions of years any three marks 3 (b) (i) gain of oxygen/loss of hydrogen/loss of electrons 1 (ii) sulphur dioxide 1 (c) H2O + SO2 ∏ H2SO3 2 (d) limestone is a carbonate 1 acids react with carbonates 1

TOTAL 9

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 14 (a) A 1 (b) B 1 (c) C 1 (d) F 1 (e) D 1 (f) B 1 (g) A 1

TOTAL 7

QUESTIONSHEET 15 (a) MgCO3 1 calcium carbonate fizzes 2 (b) MgCl2 1 (c) (i) add acid slowly/ from a burette 1 until indicator changes colour 1 (ii) as a control/ for a fair test 1 (d) (i) 0.7 5 16 = 11.2 p 1 1.2 5 11 = 13.2 p 1 0.6 5 7.5 = 4.5 p 1 0.4 5 22 = 8.8 p 1 (ii) magnesium hydroxide 1 cheapest 1 no gas given off 1

TOTAL 14

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES QUESTIONSHEET 16 (a) (i) does not react with acid 1 (ii) substance A 1 very high pH – dangerous 1 (iii) a carbonate 1 (b) (i) seasoning 1 preserving foods 1 (ii) two from: sodium carbonate, chlorine, sodium, sodium hydrogencarbonate 2 (iii ) to melt ice 1

TOTAL 9

QUESTIONSHEET 17 (a) add universal indicator/litmus 1 red ⇒ acid 1 (b) vinegar is acid 1 ammonia is alkaline 1 they neutralise the stings 1 (c) water dilutes acid 1 washing soda neutralises it 1

TOTAL 7

QUESTIONSHEET 18 (a) field C 1 (b) A beans, onion, leek 3 B beans, leek 2 C potato 1 (c) field C 1

TOTAL 8

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GCSE CHEMISTRY ACIDS, BASES & SALTS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 19 (a) MgSO4 1 (b) I magnesium & sulphuric acid 2 II magnesium carbonate & sulphuric acid 2 III magnesium hydroxide & sulphuric acid 2 (c) boil off/evaporate the water 1

TOTAL 8

QUESTIONSHEET 20 (i) seven/7 1 (ii) neutral/ neutralised 1 (iii) hydrogen/ hydrogen ions 1 (iv) carbon dioxide 1 (v) ethanoic acid 1 (vi) lemons/car batteries/nettles etc 1 (vii) sodium hydroxide/potassium hydroxide/ammonia etc 1 (viii) corrosive 1

TOTAL 8

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) oxygen 2 6 (0) 1 sulphur 2 8 6 1 (b) (i) correct nucleus 1 correct electronic arrangement 1 (ii) lose 6 electrons 1 gain 2 electrons 1 (c) (i) chlorine radicals have unpaired electrons 1 are chlorine atoms 1 OR chlorine molecules have no unpaired electrons 1 are pairs of chlorine atoms 1 (ii) CFCs/chlorofluorocarbons 1 (NOT – aerosols, fridges etc as these are not substances) TOTAL 9 QUESTIONSHEET 2 (a) (i) outer shell electron 1 furthest from nucleus 1 (ii) all electrons in same shell 1 (iii) nearest electrons to nucleus 1 (b) 1 three electrons in outside shell 1 after this removing from next shell in 1

TOTAL 7

8P 8N

1 2 3 4 number of electrons

energy

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES QUESTIONSHEET 3 (a) (i) relative atomic mass/mass number = 40 1 atomic number/proton number = 20 1 (ii) protons – 20 1 neutrons – 20 1 electrons – 20 1 (b)

protons neutrons electrons 1 0 0 4 5 2

26 30 23 53 74 54 34 45 36

8 ½ mark each rounded to whole number

TOTAL 13

QUESTIONSHEET 4 (a) correct and same electronic arrangement 1 correct and same protons in each 1 correct neutrons 1 (b) 90/100 × 20 = 18 1 10/100 × 22 = 2.2 1 relative atomic mass = 18 + 2.2 = 20.2 1 (correct answer alone scores 3) Note: that the answer alone scores full marks. Always show working as an incorrect answer with no working will score zero. Correct working will gain some marks. (c) all chemical properties are the same 1 chemical properties depend on number of electrons 1 electrons are the same in both isotopes 1

TOTAL 9

10P 10N

10P 12N

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) (i) 18 1 (ii) argon 1 (b) (i) 20 1 (ii) Calcium ion/Ca2+ 1 (c) (i) 1/ one 1 (ii) 20 1 (d) (i) 7/ seven 1 (ii) 37 1

TOTAL 8 QUESTIONSHEET 6 (a) 13 protons 11 neutrons 1 13 electrons 1 (b) atoms with same number of protons/ atoms of same element 1 with different numbers of neutrons 1 (c) both isotopes have same number of electrons/ arrangement of electrons 1 it is number/arrangement of electrons that determines chemical behaviour 1 (d) 25/100 × 24 = 6 1 75/100 × 28 = 21 1 6 + 21 = 27 1 (correct answer alone scores 3) Note: that the answer alone scores full marks. Always show working as an incorrect answer with no working will score zero. Correct working will gain some marks. (e) aluminium/Al 1 TOTAL 10

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES QUESTIONSHEET 7 (a) B 1 (b) E 1 (c) A 1 (d) F 1 (e) A 1 (f) B & C/C & B 1 (g) D & E/E & D/D & F/F & D 1

TOTAL 7 QUESTIONSHEET 8 (a) (i) 2,8,8,2 1 (ii) 2,8,7 1 (b) (i) atoms become stable by obtaining full outer shells 1 calcium loses 2 electrons 1 chlorine gains one electron 1 electrons transferred from calcium atoms to chlorine atoms 1 (ii) Ca2+, Cl− 2

(iii) CaCl2 1 (c) ionic bonds/forces between ions/particles are very strong 1 they take a lot of energy to break/overcome 1

TOTAL 11 QUESTIONSHEET 9 (a) covalent 1 (b) (i) bonds between atoms are very strong 1 require a lot of energy to break 1 (ii) atoms arranged in layers 1 forces between layers weak/layers slide past each other easily 1 (c) free electrons 1 move along the layers 1

TOTAL 7

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) regular pattern of ions 1 tightly packed 1 free electrons 1 hold structure together 1 (All four marks could be obtained from a clearly labelled diagram) (b) (i) forces holding lattice together are strong 1 ions/atoms in lattice tightly packed 1 (ii) layers of ions/atoms can slide past each other 1 (c) free electrons take in heat 1 passed on as electrons collide 1 (d) alloy 1

TOTAL 10 QUESTIONSHEET 11 (a) (i) 2,8,1 1 (ii) 2,8,7 1 (b) (i) Na+ 1 (ii) Cl− 1 (c) NaCl 1 (d) (i) ions able to move freely 1 (ii) melt it 1 (e) (i) inert/noble gas/ Group 0 1 (ii) has a full outer shell 1

TOTAL 9

+ + +

+

+

+ + +

+ + + +

- - - -

- - - -

-- - -

Electrons

Positively charged metal ions

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES QUESTIONSHEET 12 (a) (i) two sodium with 1+ needed to cancel 2- in sulphate 1 Na2SO4 1 (ii) one potassium with 1+ needed to cancel 1- in nitrate 1 KNO3 1 (iii) one calcium 2+ needed to cancel 1- in two chlorines 1 CaC12 1 (iv) one magnesium 2+ needed for two nitrates 1- 1 Mg(NO3) 2 1 (v) one potassium 1+ needed for one chloride 1- 1 KC1 1 (b) (i) ionic 1 (ii) electrons are transferred from one atom 1 to another 1 (c) (i) I- 1 (ii) Sr2+ 1 (iii) SrI2 1

TOTAL 16

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES

QUESTIONSHEET 13 (a) (i) simple molecular 1 (ii) giant atomic 1 (iii) simple molecular 1 (iv) giant metallic 1 (v) giant ionic 1 (b) both will be low 1 (c) regular arrangement of cobalt ions 1 surrounded by free electrons 1

TOTAL 8 QUESTIONSHEET 14 (a) A & E/E & A 2 (b) B 1 (c) B & D/D & B 2 (d) C 1 (e) F 1 (f) E 1 (g) F 1 Note: that you may use each atom once, more than once or not at all. This is sometimes stated on the question paper. Students often go wrong by thinking that they must use all the alternatives at some point in the answer.

TOTAL 9

Co2+ Co2+Co2+ Co2+

Co2+

Co2+

Co2+Co2+

Co2+Co2+

Co2+

Co2+

Sea of electrons

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES QUESTIONSHEET 15 (a) (i) 4 1 (ii) 4 1 (b) 1 1 (c) (i) 4 1 (ii) 2 1 (d) (i) carbon & silicon/silicon & carbon/C & Si/Si & C 1 (ii) four electrons in outer shell of both 1 means they are both in group 4 1

TOTAL 8 QUESTIONSHEET 16 (a) (i) nucleus 1 (ii) protons 1 neutrons 1 (iii) positive/+/+12 1 (b) (i) 12 1 (ii) 2,8,2 1 (c) (i) two/2/II 1 has two electrons in outer shell 1 (ii) three/3/III 1 outer electrons in third shell/energy level 1

TOTAL 10

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES

QUESTIONSHEET 17 (a) (i) K2O 1 (ii) MgO 1 (iii) Al2O3 1 (b) (i) FeO 1 Fe2O3 1 (ii) iron(II) oxide & iron(III) oxide 1

TOTAL 6 QUESTIONSHEET 18 (a) (i) sodium chloride 1 (ii) sodium sulphate 1 (iii) sodium hydrogencarbonate 1 (b) (i) sodium sulphate/ Na2SO4 1 (ii) 7 1 (c) (i) sodium hydrogencarbonate/ NaHCO3 1 (ii) sodium (no marks as given in question) hydrogen 1 carbon 1 oxygen 1

TOTAL 9

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GCSE CHEMISTRY ATOMIC STRUCTURE & BONDING ANSWERS AND MARK SCHEMES QUESTIONSHEET 19 One mark each for the following in the correct order smallest neutrons positive negative nucleus equal ion atomic number mass number/atomic mass different protons electrons neutrons

TOTAL 13 QUESTIONSHEET 20 one mark each

Name of element neon magnesium sodium nitrogen carbon symbol Ne Mg Na N C

mass number 20 24 23 14 12 atomic number 10 12 11 7 6

number of neutrons 10 12 12 7 6

TOTAL 9

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) butane is easier to light 1 charcoal is less expensive/is easier to store 1 (b) (i) random arrangement of molecules, quite close together 1 able to move freely in body of liquid 1 (ii) widely spaced random arrangement 1 able to move freely in whole container 1 (c) evaporation 1 (d) (i) 2 (ii) separate molecules with low attraction 1 (e) energy needed to start reaction 1 called activation energy 1

TOTAL 12 QUESTIONSHEET 2 (a) (i) to allow gases to pass through 1 (ii) as a conductor 1 (b) produce electricity directly from fuel 1 (c) 2H2 + O2 2H2O 2 (one for formulae, one for balancing) (d) do not run down as quickly 1 produce water for use by astronauts 1 (e) solar cell 1

TOTAL 8

H C C C C

H H H H

H H H H

H

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES QUESTIONSHEET 3 (a) (i) burns quicker/more completely 1 (ii) heat transferred to water more efficiently 1 (b) (i) 6H2O 1 + 6CO2 1 (ii) 31 200 × 100/2 1 = 1 560 000 J or 1560 kJ 1

TOTAL 6 QUESTIONSHEET 4 (a) (i) 1 energy taken in 1 from surroundings 1 (ii) breaking bonds in ammonium nitrate takes in energy 1 making bonds between ions and water molecules gives out energy 1 former exceeds the latter 1 (b) (i) 2Al + Fe2O3 Al2O3 + 2Fe 2 (ii) match supplies activation energy 1 the reaction supplies it after that 1

TOTAL 10 QUESTIONSHEET 5 (a) treacle pudding contains carbohydrate for energy 1 sumo wrestler needs protein for muscle 1 (b) sugar is a simple carbohydrate 1 may cause obesity 1

TOTAL 4

crystals

solution

energy

time

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 6 (a) Bond breaking = 436 + 151 = 587 1 Bond making = 2 × 298 = 596 1 Difference = -9 kJ 1 (b) Exothermic 1 (c)

3

TOTAL 7 QUESTIONSHEET 7 (a) Heat energy = 4.2 × 15 × 20 1 = 1260 J = 1.26 kJ 1

(b) Moles = 1000

10 × 0.1 = 0.001 1

= 1 ×10-3 1 (c) HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) 1 (d) 1000 × (a) 1 = 1260 kJ 1

TOTAL 7 QUESTIONSHEET 8 (a) (i) Br-Br + H-H/193 + 436 1 = 629 1 (ii) 2 × H-Br/2 × 366 1 = 732 1 (iii) overall energy change = energy in – energy out/ 629 – 732 1 = -103 1 (+ 103 scores 1 mark.) (b) exothermic/ energy given out/ energy supplied to surroundings 1 (give follow through mark) (c) b 1

TOTAL 8

H2 +I2

2HI

energy

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES QUESTIONSHEET 9 (a) (i) to find out how much fuel was used 1 (ii) to ensure an even temperature 1 (iii) the temperature of the water 1 (iv) the volume of water 1 distance of burner from beaker 1 (b) (i) 12oC/g 1 (ii) propanol 1 propanol is bigger molecule 1 contains more carbon 1

TOTAL 9 QUESTIONSHEET 10 (a) bubbling/ fizzing/ slight movement of calcium 1 clouding of water 1 (b) (i) energy produced = 4.2 × 5 × 50 1 =1050 J (or 1.050 kJ) 1 (ii) Exothermic 1 (c) Ca(s) + 2H2O(1) ™ Ca(OH)2(aq) + H2(g) 2 Ignore state symbols

TOTAL 7 QUESTIONSHEET 11 (a) (i) open 1 (ii) more oxygen mixes with the methane 1 (b) (i) hydrogen carbon 2 (ii) carbon dioxide water 2 (c) (i) the minimum energy for a reaction to happen 2 (ii) lowers the activation energy 1

TOTAL 9

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 12 (a) (i) exothermic heat is given out/ temperature rises 2 (ii) 17oC 1 (iii) paraffin 1 (iv) to make the test fair/ so the results are comparable 1 (b) oxygen 1 (c) causes global warming/ greenhouse effect polar ice caps melt causing flooding 2 (d) carbon monoxide 1

TOTAL 9 QUESTIONSHEET 13 (a) ethanol 1 smallest temperature rises 1 (b) to make the test fair 1 different amounts of water require different amounts of heat to raise temperature by 1oC 1 (c) 100 × 4.2 × 39 1 = 16380 J for 1.0 g 1 for 2.0 g: 16380 × 2 = 32760 J (=32.76 kJ) 1

TOTAL 7

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES QUESTIONSHEET 14 (a) reactants and products labelled 1 (b) activation energy labelled 1 (c) (i) formula mass of MgO = 24 + 16 = 40 1 40 g MgO produced from 24 g Mg 1 100 g MgO produced from (24 × 100)/ 40 = 60 g Mg 1 (ii) 32 g O2 reacts with 48 g Mg 1 8 g O2 reacts with 12 g Mg 1 8 g O2 occupies 6 dm3 1

TOTAL 8

QUESTIONSHEET 15 (a) (i) exothermic 1 (ii) they are being used up faster than they can be replaced so they will eventually run out 2 (iii) wood/ paper/ peat/ biogas/ charcoal any two 2 (b) (i) C-H O=O 2 (ii) C=O H-O 2 (iii) bonds broken =4 C-H + 2 O=O bonds formed = C=O + 4 H-O 1 energy in = (4 × 435) = (2 × 497) energy out = (2 × 803) + (4 × 464) 1 energy change = 2734 – 3462 1 energy change = -728 kJ 1 correct answers score 4 marks

TOTAL 13

energy

products

activation energy reactants

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 16 (a) the reading would increase 1 (b) (i) substance which speeds up/ increases the rate of a chemical reaction is chemically unchanged/ remains the same 2 (ii) reading goes up to the same point as before reading goes up quicker 2

TOTAL 5 QUESTIONSHEET 17 (a) (i) thermometer 1 (ii) 57 – 19 = 38 1 (iii) any temperature at least 5 degrees above 38 1 (b) exothermic 1 (c) (i) any combustion, any displacement etc 1 (ii) can be used to supply energy 1 (iii) can be used to cool injuries etc. 1

TOTAL 7 QUESTIONSHEET 18 (a) Two from state of health, age, type of job 2 (b) 325 + 1430 + 660 + 200 1 = 2615 J 1 (c) (i) man would be fatter 1 farmer more muscular 1 (ii) he does not take in enough energy 1 (iii) eat less 1 take exercise 1

TOTAL 9

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GCSE CHEMISTRY ENERGETICS ANSWERS AND MARK SCHEMES QUESTIONSHEET 19 (a) larger surface area of coal oxygen/air can mix with it more easily 2 (b) less coal for amount of air/oxygen mixes better to burn more easily 2 (c) oxygen needed for combustion air only contains 20% oxygen 2 (d) carbon dioxide carbon monoxide 2

TOTAL 8 QUESTIONSHEET 20 (a) Three from lights easily, easy to store, safe to store, continues to burn, no pollution 3 (b) (i) heat same mass of water with each fuel 1 measure temperature rise 1 weigh burners before and after experiment 1 to calculate amount of fuel used 1 (ii) coal does not light and continue to burn as easily 1 (iii) difficult to measure amount of gas used 1 (c) we don’t know how much fuel was used 1

TOTAL 10

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) proteins /amino acids 1 (b) nitrate will be used up eventually / will run out 1 (c) (i) 23 + 14 + (3 × 16) = 85 1 (ii) 14 / 85 × 100 = 16.5 (16.47) 2 if incorrect, one mark is given for the correct fraction (ii) is marked consequentially on part (i) (d) (i) air 1 (ii) water / natural gas / methane 1 (e) (i) iron acts as a catalyst 1 (ii) this increases surface area 1 and increases the rate of reaction 1 (f) sulphuric acid 1 (g) increase in plant/algal growth 1 plants/algae die and rot 1 the rotting process uses up oxygen in the water 1 lack of oxygen results in death of fish and other wildlife 1

TOTAL 15

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 2 (a) provides raw materials to make useful products 1 provides jobs for people 1 adds valuable income to the local community 1 (b) THREE from : -removes a mineral that cannot be replaced -damages habitats of plants and/or animals -spoilheaps produced that are unsightly -named form of pollution from mining eg.noise/more lorries/dust 3 (c) (i) (s) = solid 1 (g) = gas 1 (ii) CaCO3 : 100 1 CaO : 56 1 CO2 : 44 1 (d) (i) 100 tonnes limestone 56 tonnes calcium oxide 300 tonnes 168 tonnes 3,000 tonnes 1680 tonnes 2 marked consequentially on the masses given in (c) (ii) some limestone remains unreacted/does not get hot enough 1 (e) glass making / cement making / building material / neutralising agent for soils 1

TOTAL 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 3 (a) anode correctly labelled – electrode on left 1 (b) Test – use damp litmus paper 1 Result - turns white / bleached 1 (c) kill bacteria in drinking water or swimming pools / manufacture of PVC or bleach or disinfectants 1 (d) 2Cl - → Cl2 + 2e- 1 (e) hydrogen 1 (f) (i) solution is alkaline 1 (ii) sodium hydroxide 1 (g) FIVE from : - run cell with known concentration of salt solution - measure volume of gas collected after specified time/ time how long to collect a specified volume of gas - repeat experiment with weaker/stronger concentration of salt solution - use same volume of solution - use same electrodes - use same current 5 (h) increase current of cell 1 use different electrodes 1

TOTAL 15

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 4 (a) Al3+ 1 O2- 1 (b) lowers melting point of the aluminium oxide 1 (c) ions need to be free to move towards the electrodes 1 ions are able to move as a liquid / ions unable to move as a solid 1 (d) (i) Al3+ + 3e- Al 1 (ii) oxide ions are attracted to the anode 1 oxide ions lose electrons 1 to form oxygen gas 1 (e) method of extraction from the ores is related to a metal's position in the reactivity series 1 metals at the top of the series need more energy than those lower down 1 (f) (i) United Kingdom 1 (ii) TWO from:

- large amount of electricity not available - money for construction of plant not available - lack of suitable trained workforce 2

TOTAL 14

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) C + O2 CO2 1 (b) sulphur dioxide reacts with oxygen in the air and dissolves in water 1 forming sulphuric acid or 'acid rain' 1 making the soil too acidic and damages the roots of the trees/ rain water is very acidic and attacks or damages leaves 1 (c) (i) neutralisation 1 (ii) CaO : 56 1 SO2 : 64 1 (iii) 32 / 64 × 56 = 28 tonnes 2 if incorrect, 1 mark is given for the fraction mark consequentially on answers to (ii) (iv) TWO from : -do not want sulphur dioxide to escape so best to have excess calcium oxide -would be difficult to ensure thorough mixing of reactants -impurities may be present in calcium oxide / may be impure 2 (d) (i) reaction is reversible/products break up to reform reactants 1 (ii) sulphur trioxide 1 (iii) sulphuric acid 1 TOTAL 14

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 6 (a) + 189 kJ 1 (b) (i) the minimum amount of energy needed to start a reaction 1 (ii) line drawn from the reactants to the top of the curve 1 (iii) speeds up the reaction / makes the reaction go faster 1 (c) (i) 70 % 1 (ii) 70 / 100 × 300 = 210 tonnes 2 if incorrect one mark is awarded for the correct fraction mark consequentially on the answer to (c) (i) (iii) low rate of reaction / slow reaction low temperature makes the catalyst less effective 1 (d) (i) SO3 + H2SO4 H2S2O7 2 one mark for correct reactants, one mark for correct products (ii) the reaction is too violent / too exothermic 1 (e) (i) transition metal / transition element 1 (ii) vanadium catalyst is not used up in the reaction 1 TOTAL 13

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 7 (a) amount or percentage of copper present is very small 1 (b) reacts in air to form sulphuric acid 1 this is the cause of 'acid rain' 1 poisonous / causes pollution scores one mark (c) sulphur dioxide reacted with air or oxygen 1 to form sulphur trioxide 1 sulphur trioxide absorbed into concentrated sulphuric acid 1 (d) (i) copper from the anode/impure electrode forms copper ions or dissolves 1 copper ions turn to copper on cathode/deposited on cathode/pure copper 1 impurities are left behind/fall to the bottom of the cell 1 (ii) 2e- 1 (iii) ‘reduction’ is electron gain 1 copper ions gain two electrons 1 (iv) 'anode slime' contains precious metals/named metals eg. silver, gold 1 (e) high melting points 1 form coloured compounds 1 TOTAL 15 QUESTIONSHEET 8 (a) (i) 1.03% 1 (ii) oxygen 1 (b) (i) fractional distillation 1 (ii) argon 1 (iii) oxygen 1 (c) carbon dioxide & water vapour 2 (d) (i) in electric bulbs, for risky welding jobs, etc. 1 (ii) fast freezing food, for packing food, making ammonia, etc. 1 (e) convert iron to steel (1) by burning impurities (1) 2

TOTAL 11

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 9 (a) air 1 (b) (i) NO 1 (ii) O2 1 (iii) NO2 1 (c) platinum 1 (d) gases are cooled using water 1 (e) reacted with water 1 and oxygen 1 (f) (i) ammonia solution / ammonium hydroxide 1 (ii) neutralisation 1 (iii) nitrogen is converted into plant protein 1 crop yield is therefore increased 1 (iv) 10% nitrogen 1 5% potassium 1 no phosphorus is present 1

TOTAL 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) iron 1 (b) 3H2 1 2NH3 1 (c) a reaction in which the products reform the reactants 1 (d) (i) increases as the pressure increases 1 decreases as the temperature increases 1 (ii) temperature 300oC pressure 225 atmospheres 1 (iii) line drawn between 300oC and 500oC lines and is closer to 300oC line 1 (e) Two from: - more expensive plant or pipelines as they need to be thicker/stronger - greater risk of explosion / greater danger to workforce - higher power costs for compressor 2 (f) lower rate of reaction / reaction takes a long time 1 (g) cool down the mixture of gases 1 ammonia will be the first to turn into a liquid 1 (h) recycled 1 TOTAL 14

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 11 (a) haematite/magnetite 1 (b) (i) carbon reacts with oxygen to form carbon dioxide 1 this reacts with more carbon 1 (ii) oxygen is removed 1 (c) (i) CaCO3 CaO + CO2 2 (ii) limestone removes acid/sandy impurities 1 (d) molten iron 1 slag 1 (e) need for shift work / unsociable hours 1 (f) THREE from : -near to supply of coal/coke or near to coalfield -near to a port for import of ore -good communication links eg. good road or rail links -availability of skilled workforce 3 (g) steel 1 girders for construction / motor car bodies / shipbuilding 1

TOTAL 15

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 12 (a) TWO from : - large amount of impurities present in ore/ only one tonne of metal formed from every 4 tonnes of ore - large amounts of energy required in the extraction process/ uses large amounts of electricity - special equipment required to cope with the high temperatures involved 2 (b) THREE from : - high demand reduces the Earth's resources - more fuel burnt that adds to atmospheric pollution/greenhouse effect/increase in carbon dioxide levels - bauxite ore will run out/is a non-renewable resource - problems involved in more recycling to meet the increased demand - more waste produced from purification of bauxite - more land used to build HEP plants to meet electricity demand 3 (c) (i) anode connected to +; cathode to − 1 electrolyte – the solution 1 aluminium metal – the bottom layer 1 (ii) oxygen formed at the anode 1 reacts with the carbon forming carbon dioxide gas 1 (d) (i) Al3+ + 3e- Al 1 (ii) molar mass of oxygen = 32 g 1 each O2 releases 4 electrons to form 4/3 aluminium 1 4/3 × 27 × 10 = 360 tonnes 1

TOTAL 14

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 13 (i) oxygen 1 (ii) vanadium(V) oxide 1 (iii) water 1 (iv) (s) O2 (g) 2 (v) toxic nature of the gas/forms acid rain 1 (vi) hydrogen, sulphur and oxygen 1 (vii) dangerous reaction/ a sulphuric acid mist is formed 1 (viii) paints/fertilisers/car batteries/detergents/plastics/cleaning metals/ many more 1

TOTAL 9

QUESTIONSHEET 14 (a) (i) N2 (1) 3 2 (l) 2 (ii) iron behaves as a catalyst in speeding up the reaction 1 (iii) heat speeds up the reaction l (b) (i) as the pressure increases % of ammonia also increases 1 as the temperature increases % of ammonia decreases 1 (ii) construction cost or plant too dangerous 1 (c) sulphuric acid 1

TOTAL 8 QUESTIONSHEET 15 (a) (i) (I) coke 1 (II) limestone 1 (ii) slag 1 (b) (i) carbon monoxide 1 (ii) 2×56 + 3 ×16 1 =160 1 (iii) 1 mole of Fe2O3 gives 2 moles of Fe 1

320 tonnes gives 224 tonnes of iron 1

TOTAL 8

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 16 (a) (i) cost of electricity 1 (ii) breaking down a substance by electricity 1 (iii) reduce energy/lower the melting point of the aluminium oxide 1 (iv) ions must be mobile 1 (v) oxide O2 − 1 (b) (i) near power station (1) electrolysis needs electricity (1) OR good transport system (1) import of bauxite/export of aluminium (1) 2 (ii) making our resources last longer/cheaper metals/ lower energy costs 1 (c) (i) conducts heat 1 (ii) conducts electricity 1 (iii) does not corrode 1

TOTAL 11 QUESTIONSHEET 17 (a) (i) One each for: sodium ----- electrolysis zinc ----------reduction with coke copper ------heat sulphide with oxygen 3 (ii) most reactive metals need electrolysis 1 least reactive by heating 1 (iii) carbon 1 (b) (i) displacement/ oxidation – reduction/ reduction 1 (ii) sodium more reactive than titanium 1

TOTAL 8

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GCSE CHEMISTRY INDUSTRIAL PROCESS ANSWERS AND MARK SCHEMES QUESTIONSHEET 18 (a) (i) C 1 (ii) E 1 (iii) D 1 (iv) B 1 (b) (i) heating up incoming air 1 (ii) Two from: nitrogen, carbon dioxide, carbon monoxide 2 (c) carbon 1

TOTAL 8

QUESTIONSHEET 19 (a) nitrogen is very unreactive 1 (b) products turn back into reactants 1 (c) a catalyst/ iron catalyst 1 (d) returned to reaction/recycled/used again 1 (e) strong smell 1 alkaline/ red litmus paper turns blue 1 (f) (i) ammonium nitrate 1 (ii) contain a lot of nitrogen 1 improves crop yield 1

TOTAL 10

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GCSE CHEMISTRY INDUSTRIAL PROCESSES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 20 (a) (i) sodium chloride 1 (ii) Two from: on roads in winter, seasoning, preserving food, glazing earthenware, curing bacon 2 (b) (i) strong alkali 1 (ii) Two from: soap, paper, dyes, rayon 2 (c) (i) gas 1 bleach 1 (ii) Two from: treating water, swimming pools, making plastics, dyes, hydrochloric acid, solvents, refrigerants,bleaches 2

TOTAL 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) voltmeter 1 (b) greater difference between the reactivity of the metals 1 the greater the voltage 1 references between more reactive metal & greater voltage 1 (c) accept any value between 0.6 and 1.6 volts 1 (d) stays at 1.6 volts 1 (e) silver is slightly less reactive than copper 1 (f) liquid will spill out of the container / not portable 1

TOTAL 8 QUESTIONSHEET 2 (a) D A B C (2 for all correct, 1 for one mistake) 2 (b) A = magnesium B = iron C = platinum D = calcium (4 correct – 3 marks, 3 correct – 2 marks 2 correct – 1 mark) 3 (c) (i) 2 HCl 1 (ii) MgCl2 contains Mg2+ 1 formula is MgSO4 1 (iii) magnesium nitrate 1

TOTAL 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 3 (a) (i) reaction 1 zinc sulphate + copper 1 (ii) no reaction 1 (iii) reaction 1 magnesium sulphate + zinc 1 (b) (i) loss of oxygen/gain of hydrogen/gain of electrons 1 (ii) magnesium + copper oxide magnesium oxide + copper 1 (iii) magnesium circled 1 (iv) the minimum energy 1 required for a reaction to happen 1 (c) (i) lead oxide/copper oxide 1 (ii) calcium oxide/potassium oxide 1

TOTAL 12

QUESTIONSHEET 4 (a) lithium barium magnesium aluminium all correct – 2 marks, 2 correct – 1 mark 2 (b)

solution aluminium barium lithium magnesium aluminium nitrate barium nitrate lithium nitrate magnesium nitrate

4 correct - 3 marks 3 correct - 2 marks 2 correct – one mark 3 (c) aluminium reacts with oxygen/air 1 forms layer of aluminium oxide 1 coating prevents aluminium from reacting 1

TOTAL 8

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) (i) bauxite 1 (ii) lowers melting point of aluminium oxide 1 process uses less energy/cheaper 1 (iii) anode 2O2- O2 + 4e- 1 cathode Al3+ + 3e- Al 1 (b) (i) haematite 1 (ii) loss of oxygen/gain of hydrogen/gain of electrons 1 (iii) 3CO + Fe2O3 3CO2 + 2Fe 2 (iv) road building/fertiliser 1 (c) aluminium higher than carbon in series 1 carbon not reactive enough to reduce aluminium oxide 1

TOTAL 12 QUESTIONSHEET 6 (a) TEST - use of a named indicator 1 eg.Universal or pH indicator RESULT - correct colour for the indicator used eg.turns blue/purple 1 (b) M2O 1 (c) GROUP – 1 1 REASON - forms compounds with similar formula to group 1 metals/ (accept named metal)/forms single positive ions 1 NOT - reacts violently with water (this could be a group 2 metal) (d) REACTIVITY SERIES - correct order, placing mancunium at the top 1 REASON - group 1 metals appear at the top of the reactivity series 1 (e) copper + mancunium sulphate 1 (f) (i) mancunium sulphate 1 (ii) 2 MOH + H2SO4 M2SO4 + 2H2O 2 (1 mark for correct formulae for products) (1 mark for balancing)

TOTAL 11

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 7 (a) (i) iron + aluminium oxide 1 (ii) 2 Al and 2 Fe BOTH REQUIRED 1 (b) aluminium is more reactive / higher in reactivity series than iron 1 metals will therefore swap places / displacement occurs 1 (c) gives a larger surface area 1 therefore gives a higher rate of reaction / reacts more quickly 1 (d) (i) copper is less reactive than iron / is lower in the reactivity series 1 therefore no reaction will take place 1 (ii) magnesium / zinc 1

TOTAL 9 QUESTIONSHEET 8 (a) measuring cylinder / burette/ pipette 1 (b) chemical balance / balance NOT weighing machine or scales 1 (c) temperature would rise 1 brown / pink solid formed 1 solution becomes colourless / blue colour of solution fades 1 (d) Cu + ZnSO4 BOTH REQUIRED 1 (e) some zinc will be left over / unreacted at the end of the reaction / more than enough zinc to react with the copper sulphate 1 (f) (i) no reaction would take place 1 (ii) zinc is less reactive than magnesium / magnesium is more reactive than zinc 1 zinc will not be able to displace magnesium 1

TOTAL 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 9 (a) ONE FROM: metal A - reaction with air - colour change metal B - reaction with air - colour change metal B - reaction with water - fizzing/bubbles/effervesces metal D - reaction with air - colour change metal D - reaction with water - fizzing/bubbles/effervesces 1 (b) MOST REACTIVE D B A LEAST REACTIVE C 2 (1 mark for C being placed as least reactive) (c) D 1 REASON - reacts vigorously with water/ most reactive metal 1 (d) C 1 (e) copper + oxygen copper oxide 2 (1 mark for identifying oxygen as a reactant) (1 mark for identifying the oxide as the sole product) (f) metal D is very reactive with water 1 metals react more vigorously with acid than with water 1 (references to 'too dangerous' scores 1 mark)

TOTAL 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) one per connection 3 (b) (i) potassium 1 (ii) magnesium/ iron 1 (c) (i) hydrogen 1 (ii) lighted splint 1 pops/explodes 1

TOTAL 8 QUESTIONSHEET 11 (a) aluminium zinc iron lead (4 correct – 2 marks, 2 correct – 1 mark) 2 (b) (i) MgSO4(aq) + Cu(s) Mg(s) + CuSO4(aq) 2 (ii) Any two from: magnesium dissolves brownish copper metal precipitated blue colour of solution fades 2 (iii) copper – last/bottom 1 magnesium – first/top 1 (c) (i) no reaction 1 (ii) reaction aluminium sulphate + iron 1

TOTAL 10

copper

iron

magnesium

potassium

reacts with steam

vigorous reaction in cold water

no reaction with steam or water

reacts reversibly with steam

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 12 (a) (i) Any two from: sodium melts/becomes molten ball moves across water quickly increased amount of fizzing 2 (ii) 2Na + 2H2O 2NaOH + H2 1 (iii) purple/dark blue 1 pH 12 – 14 1 (b) Any two from: potassium moves across water at increased speed burns with lilac flame sparks/explodes 2 (c) (i) alkali metals 1 (ii) have one electron in outer shell 1 (iii) reactivity increases down group 1 outer electron becomes further from nucleus 1 nucleus has less force of attraction on outer electron/ increased shielding 1 outer electron is lost more easily 1

TOTAL 13

QUESTIONSHEET 13 (a) oxygen and water BOTH REQUIRED 1 (b) zinc corrodes instead of the iron NOT forms a protective barrier 1 (c) zinc is more reactive than iron/ zinc is higher in the reactivity series. 1 (d) sea water is needed to complete the circuit 1 (e) arrow points away form the zinc block 1 (f) PREDICTION : iron would rust faster 1 REASON : iron is more reactive than copper and so will corrode first 1 (g) nails placed in salt water and in deionised water 1 some form of observation or measurement of rusting after a period of time 1 use of 'fair' test or comparison between the two results 1

TOTAL 10

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 14 (a) the less reactive metals were discovered first or earlier 1 (b) (i) TWO FROM : brown solid formed blue solution will fade/become colourless zinc dissolves 2 (ii) copper + zinc sulphate BOTH REQUIRED 1 (c) (i) 13oC 1 (ii) exothermic 1 (iii) TWO FROM: add greater mass of zinc use a more concentrated solution of copper sulphate use a more reactive metal than zinc/accept a named metal 2

TOTAL 8 QUESTIONSHEET 15 (a) brown solid is copper metal 1 magnesium is more reactive than copper 1 (b) no reaction takes place 1 copper is less reactive than zinc 1 (c) THREE FROM : carbon is more reactive than iron carbon will displace iron from its oxide forming iron metal carbon is less reactive than aluminium carbon and aluminium oxide will therefore not react 3 (d) zinc is more reactive than hydrogen 1 zinc will displace hydrogen from an acid to form hydrogen gas 1 copper is less reactive than hydrogen 1 (e) stability of carbonates is linked to the position of metals in the reactivity series 1 carbonates of metals that are lower decompose more easily 1

TOTAL 12

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 16 (a) bubbles of gas / fizzing / effervescence/ iron dissolves 1 (b) aluminium metal has a layer of oxide present 1 this makes it resistant to attack / is a protective layer /prevents reaction 1 (c) students were investigating the effects of acid rain 1 this contains sulphuric acid / formed from sulphur dioxide 1 (d) (i) lead and copper nitrate (ANY ORDER - 1 mark each) 2 (ii) brown / pink solid or deposit 1 (iii) lead + copper nitrate → copper + lead nitrate 1 (iv) lead has displaced the copper in the compound 1 (accept replaced or changed places with)

TOTAL 10 QUESTIONSHEET 17 (a) silver 1 (b) sodium 1 (c) mercury 1 (d) sodium 1 (e) magnesium 1 (f) iron 1 (g) zinc 1 (h) sodium 1 (i) calcium 1

TOTAL 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 18 (a) iron 1 aluminium oxide 1 (b) energy is given out in the reaction / reaction is exothermic 1 temperature rises above 1500oC to melt the iron 1 (c) increases the surface area 1 reaction rate is increased / reaction happens faster 1 (d) to allow the molten iron to run into the gap between the rails 1 (e) clay is able to withstand the high temperatures reached 1 (f) aluminium is more reactive than iron 1 copper is less reactive than iron 1 displacement only occurs when the metal is more reactive 1

TOTAL 11 QUESTIONSHEET 19 (a) magnesium copper silver 1 (b) (i) gain oxygen/lose hydrogen/lose electrons 1 (ii) magnesium + oxygen magnesium oxide OR copper + oxygen copper oxide 1 (c) (i) copper becomes black/coated in silver 1 (ii) copper more reactive than silver 1 displaced silver from solution 1 (d) (i) no visible reaction 1 (ii) copper is less reactive than magnesium 1 cannot displace magnesium 1

TOTAL 9

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GCSE CHEMISTRY METALS & THE REACTIVITY SERIES ANSWERS AND MARK SCHEMES

QUESTIONSHEET 20 (a) (i) hydrogen 1 (ii) magnesium hydroxide (allow oxide) 1 (b) (i) hydrogen 1 (ii) Two from: calcium, zinc, iron, lead, nickel 2 (iii) copper/silver/gold/platinum 1 (c) gold & silver are unreactive 1 do not tarnish easily/retain shine 1 iron would rust/corrode 1

TOTAL 9

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) (i) increases 1 (ii) decreases 1 (b) 105 kJ per mole 1 (c) while bond length increases 1 bond energy decreases 1 (d) none 1 because astatine is likely to be insoluble 1 (e) C1, Br, I, At 2 or if one out of order 1 (f) no 1 as bond energy decreases 1 expect reactivity to increase 1

TOTAL 12 QUESTIONSHEET 2 (a) sulphur dioxide 1 (b) -10oC 1 (c) the gas has been dried 1 pH paper reacts to aqueous solutions 1 (d) pH falls below 7 / paper becomes yellow/orange/red 1 (e) 2SO2 + O2 � 2SO3 2 (f) catalyst 1 (g) heat given out 1 (h) SO3 + H2O → H2SO4 2 (i) the bulk of the liquid absorbs the heat 1 so no spray is caused 1

TOTAL 13

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES QUESTIONSHEET 3 (a) (i) yellow/green gas 1 (ii) iron(III) chloride 1 (iii) 2Fe(s) + 3Cl2(g) → 2FeCl3(s) 2 (iv) chlorine is poisonous 1 (b) less vigorous 1 (c) (i) 2Na(s) + Br2(l) → 2NaBr(s) 2 (ii) potassium and fluorine 1 potassium is the most reactive metal (1), fluorine the most reactive non-metal (1) 2

TOTAL 11 QUESTIONSHEET 4 (i) glowing splint - relights in oxygen but not in nitrogen 2 (ii) flame - 'pop' noise in hydrogen only or litmus paper goes red and then bleached in chlorine only 2 (iii) lime water goes white/milky in carbon dioxide only 3 (iv) litmus goes blue in ammonia solution only 3 [ The above will perhaps be the most common answers - there are alternative answers!]

TOTAL 10 QUESTIONSHEET 5 (a) (i) S : O mass(g) 3.2 : 3.2 1 moles: 3.2/32=0.1 : 3.2 / 16 = 0.2 1 ratio 1 : 2 So formula is SO2 1 (ii) oxygen 1 (b) (i) a reaction that can go backwards or forwards 1 (ii) SO2

+ 2O2 � 2SO3 2 (c) in oxygen there is less distance between the nucleus and the outer shell/orbit (1), therefore more easy to gain electrons (1) 2

TOTAL 9

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 6 (a) N,P,K are the chemical symbols of nitrogen, phosphorus, potassium 1 fertilisers contain these 1 (b) (i) nitrogen 1 (ii) nitrogen 1 (iii) potassium 1 (c) magnesium 1 (d) Mr for NH4NO3 = 14+4+14+48 = 80 1 80 g NH4NO3 contains 28 g nitrogen 1

N content = 1008028

× = 35% 1

(e) the nitrate also supplies potassium 1

TOTAL 10

QUESTIONSHEET 7 (a) 2, 8, 5 1 (b) H P H

2 Formula PH3 1 (c) (i) gas 1 (ii) covalent bonding 1 weak attraction between molecules 1 (d) fertilisers 1

TOTAL 8

H

xo

xo

x o

x x

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES QUESTIONSHEET 8 (a) appearance: thin/ mobile amber/yellow 1 structure: short chains of sulphur atoms 1 appearance: liquid becomes thicker 1 structure: chains of sulphur atoms tangle 1 (b) allotropes 1 (c) must have cooled slowly 1 trapping crystals under surface 1 (d) (i) needle structure disappears/ become lozenge-shaped 1 (ii) none 1

TOTAL 9 QUESTIONSHEET 9 (a) points plotted correctly 1 best fit curve 1 (b) support 1 (c) appears to help prevent tooth decay 1 (d) involves enforced "mass medication" / too much fluoride is harmful 1 (e) tablet form 1 toothpaste 1

TOTAL 7

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) methane, ammonia, nitrogen, oxygen, carbon dioxide, sulphur dioxide 6 (b) points correctly plotted 1 best fit curve 1 (c) (i) 0.86 dm3 1

(ii) 0.60 dm3 1

(d) (i) 46 g 1 (ii) N = 14, & O = 16, so sum = 30 1 to make 46 one more O is needed 1 so formula = NO2 1 (e) HF = 1 + 19 = 20 1 line drawn on graph from 20 on x axis to curve 1 line drawn on graph from curve to y axis 1 from graph, volume = 1.2 1 dm3 1

TOTAL 19 QUESTIONSHEET 11 (a) (i) fluorine 1 (ii) two atoms per molecule 1 (iii) 2,8,7. 1 (iv) Cl atom gains an electron (1) to become a negative Cl ion/Cl- (1) 2 (b) (i) At2 1 (ii) black solid 1 (iii) seven 1 (iv) H At or H-At 2 Type of bonding – covalent 1

TOTAL 11

x x

x x

x x

x o

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES QUESTIONSHEET 12 (a) B 1 (b) (i) A, B & E 3 (ii) do not conduct heat/not shiny/low boiling point - any two 1 (c) Type of bonding: covalent/electrons shared by the two non-metals 1 Reason: atoms covalently bonded together give molecules 1 forces of attraction between molecules are weak/molecules are easily seperated 1 (d) hydrogen 1 [A = sulphur, B = bromine, C = sodium, D = copper, E = hydrogen]

TOTAL 9

QUESTIONSHEET 13 (a) the existence of an element in two or more forms 1 (b) (i) (ii) (2) (2) 4 (c) (i) carbon atoms are linked by very strong covalent bonds 1 in a three-dimensional/ macromolecular structure 1 (ii) carbon atoms use only three of their outer electrons to form covalent bonds 1 remaining electrons are delocalised/ can move along the layers and therefore conduct electricity 1

TOTAL 9 QUESTIONSHEET 14 (a) (i) bromine 1 (ii) carbon 1 (iii) chlorine 1 (iv) sulphur or oxygen 1 (b) NH3 covalent 2 (d) sulphur 1 (d) X = sulphur or oxygen 1 Y = carbon 1

TOTAL 9

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES

QUESTIONSHEET 15 (a) no smell/tasteless/colourless/almost insoluble in water/lighter than air - any two 2 (b) (i) zinc (1) hydrochloric acid (1) [and many more!] 2 (ii) make sure that there is no air/oxygen left in the apparatus before igniting 1 (iii) water 1 (iv) anhydrous copper sulphate (1) goes from white to blue (1) or anhydrous cobalt chloride (1) goes from blue to purple (1) 2 (c) helium 1

TOTAL 9 QUESTIONSHEET 16 (a) (i) C (ii) B (iii) A 3 (b) (i) iodine (ii) diamond (iii) sodium chloride 3 (c) (i) the breaking down of a substance by electricity 1 (ii) 2 in front of the Cl

-(1), + 2e- (1) 2

TOTAL 9 QUESTIONSHEET 17 (a) water vapour 1 (b) helium 1 (c) becomes solid 1 (d) nitrogen 1 (e) fractional distillation 1 (f) N = 78%, O = 21% 2 (g) some oxygen dissolves in water 1 nitrogen does not 1 (h) less of it in air 1 (i) carbon dioxide is soluble in water 1

TOTAL 11

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GCSE CHEMISTRY NON-METALS ANSWERS AND MARK SCHEMES QUESTIONSHEET 18 (a) A = carbon, B = lime water/calcium hydroxide 2 (b) C = decomposition, D = photosynthesis, E = oxidation/burning 3 (c) heat (1) with carbon (1) 2 (d) fizzy drinks/fire extinguisher/'dry ice' - any one 1 (e) CO2 (1) 2 2 (1) 2 (f) CO2 has a simple molecular structure, SiO2 has a giant molecular structure 2

TOTAL 12

QUESTIONSHEET 19 (a) (i) O, (ii) K 1 (b) (i) carbon (ii) sodium 1 (c) iron and sulphur 1 sodium, oxygen and hydrogen 1 potassium chloride 1 (d) (i) two 1 (ii) two 1 (e) (i) three 1 (ii) seven 1

TOTAL 9 QUESTIONSHEET 20 (a) (i) increase 1 (ii) increase 1 (b) (i) gas 1 (ii) gas 1 (iii) liquid 1 (iv) solid 1 (c) solid 1 (d) insoluble 1 (e) F, C1, Br, I, At 2 1 if 1 out of order

TOTAL 10

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) Any three from: bodies of sea creatures that died millions of years ago decayed anaerobically under high temperature and pressure 3 (b) (i) compounds with different numbers of carbon atoms have different boiling points heating vaporises crude oil different compounds condense at different temperatures 3 (ii) gasoline 1 (iii) naphtha 1 (c) compounds containing only 1 the elements carbon & hydrogen 1 TOTAL 10 QUESTIONSHEET 2 (a) (i) distillation 1 (ii) contains oil/stop oil running about/safety 1 (b) very high 1 dark yellow 1 does not burn 1 (c) (i) A 1 Any two from low b.p./volatile easy to burn clean flame 2 (ii) C 1 high viscosity 1 TOTAL 10

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES QUESTIONSHEET 3 (a) a compound containing carbon & hydrogen 1 only 1 (b) Any two from: compounds have same general formula physical properties show gradation chemical properties are similar 2 (c) C6H14 1 (d) (i) 2 (ii) straight chain version 1 (iii) Any two from: has greatest contact with neighbouring molecules therefore greater intermolecular forces of attraction greater forces mean more energy/heat needed to separate molecules 2

TOTAL 10 QUESTIONSHEET 4 (a) fractional distillation 1 (b) cracking 1 (c) polymerisation 1 (d) single bond 1 indication of long chain 1 (e) non-biodegradable/stays in ground for a long time 1 toxic fumes when burnt 1

TOTAL 7

H C C C C

H H H H

H H H H

H

H

C H H H H

H H C C C

H H H

C C

H H

H H n

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) contains carbon – carbon double bond 1 (b) CnH2n 1 (c) Any two from: 300oC/raised temperature/heat 60 atmospheres/high pressure phosphoric acid/catalyst 2 (d) 1 (e) shake each gas with bromine water 1 bromine loses colour with ethene/not with ethane 1 (f) 2

TOTAL 9

H H

C OH

H

H

H

C

C C C C

H Cl Cl H

H H H H

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES QUESTIONSHEET 6 (a) (i) high temperature 1 named catalyst (aluminium oxide/silicon dioxide/broken pot) 1 (ii) liquid paraffin in mineral wool 1 catalyst 1 heat 1 collection over water 1 (iii) product is gas, starting material is liquid 1 (b) saturated have only carbon-carbon single bonds 1 unsaturated have at least one carbon-carbon double bond 1 TOTAL 9

pieces of broken porcelain

heat mineral wool soaked with

liquid paraffin

water

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 7 (a) (i) 1 (ii) has only carbon-carbon single bonds 1 (iii) needs a double bond to form polymers 1 (b) (i) 1 (ii) 1 (c) (i) cups/electrical fittings/kettles 1 (ii) heat sample of the plastic 1 if it melts it is thermoplastic 1 if it chars it is thermosetting 1

TOTAL 9 QUESTIONSHEET 8 (a) (i) 1,2-dibromoethane 1 (ii) hydrogen 1 (iii) nickel/platinum 1 (iv) phosphoric acid/sulphuric acid 1 (v) poly(ethene) /polythene 1 (vi) ethanol 1 (b) C2H4 + H2O C2H5OH 2 (c) making margarine 1

TOTAL 9

H H

H

H

H

H C C

C

H H

C

CH3

C

H

C

CH3

H

H

H H H H

H H

H C C C C

H H H H

H H

H C C C C H or

H

C

C2H5 H

C

H

C

C2H5

H

C

H

H

or

CH3 CH3

Page 312: GCSE/IGCSE Chemistry Question Bank with Answers

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES QUESTIONSHEET 9 (a) (i) pentane 1 (ii) C8H18 1 (b) (i) sensible scales 1 axes labelled + units 1 points plotted correctly 1 smooth curve drawn through points 1 (ii) 99oC (+/- 1oC) 1 (c) 3 TOTAL 10

1 2 3 4 5 6 7 8 9 10 0

20

40

60

80

100

120

140

160

180

- 20

- 40

- 60

- 100

- 80

- 120

- 140

- 160

- 180

X

X

X

X

X

X

X

X

X

H H H H

C C C C C

H H H H

H

H

H

H

H H

H

H

H C C C

C

H H H H

H

H

C

H

H

C H H

C C C

H H

H H

H H

C

H

H H

H

Page 313: GCSE/IGCSE Chemistry Question Bank with Answers

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) 2 (b) 2 (c) it is light/low density 1 strong 1 (d) poly(ethene) is stronger than paper 1 can be mass produced/ethene is now readily available 1

TOTAL 8 QUESTIONSHEET 11 (a) (i) poly(phenylethene) 1 (ii) 1 (b) double bond 1 (c) (i) flexible 1 electrical insulator 1 (ii) rubber perishes/cracks in time 1 poly(chloroethene) is fire-resistant 1 (d) non-biodegradable 1 toxic fumes when burned 1 TOTAL 9

C C C C C C

H H H H H H

H H H H H H

H C6H5 H

C C

H H

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES QUESTIONSHEET 12 (a) A poly(propene) 1 B 1 C tetrafluoroethene 1 D 1 (b) the simplest compound from which a polymer is made 1 (c) a molecule/compound made by joining thousands of monomers 2 (d) C2F4 1 (e) it does not rust/lighter/lower density 1

TOTAL 9 QUESTIONSHEET 13 (a) alkanes 1 (b) ethene and propene 2 (c) (i) C8H18 1 (ii) octane 1 (d) Two from: makes use of less useful fractions produces more petrol produces alkenes/raw materials for the petrochemical industry 2 (e) Two from: poly(ethene) ethanol bromoethane ethane-1, 2-diol 2

TOTAL 9

H CH3

C

H H

C

n

F F

C C

F F

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 14 (a) water 1 (b) turn cloudy/milky 1 (c) (i) carbon 1 (ii) incomplete combustion 1 (iii) carbon monoxide 1

TOTAL 5 QUESTIONSHEET 15 (a) C2H4 + H2O C2H5OH 2 (b) (i) oxygen 1 (ii) 1 (iii) For Two from: help to preserve food help food processing attractive colours 2 Against Two from: can have side effects lack of consumer choice can lead to bad food being sold 2 (c) (i) sugar cane needs warm climate to grow 1 Brazil’s climate is more suitable that Britain’s 1 (ii) people may drink it 1 (d) solvent 1

TOTAL 12

C3H7 C O

O

CH3

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES QUESTIONSHEET 16 (a) 1 C5H12 1 C6H14 1 1 (b) keep it cool 1 keep away from flames & sparks 1 (c) they would tend to boil off together 1

TOTAL 7 QUESTIONSHEET 17 (a) (i) 13% (± 2%) 1 (ii) 16% (± 3%) 1 (iii) 24% (± 3%) 1 (b) liquid 1 (c) 11% 1

TOTAL 5

H H H H

H C C C C

H H H H

H

H C C C C C C

H H H H H H

H H H H H H

H

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GCSE CHEMISTRY PRODUCTS FROM OIL ANSWERS AND MARK SCHEMES

QUESTIONSHEET 18 (a) (i) a substance which helps in cleaning processes 1 (ii) Two from: if not, will stay in water causing rivers to foam harming aquatic life 2 (b) (i) chromatography 1 (ii) ink would run in solvent 1 (iii) yellow 1 (iv) orange 1

TOTAL 7 QUESTIONSHEET 19 (a) guttering – easily moulded 1 carrier bags – can be coloured or lightweight 1 combs – easily moulded 1 sandwich bags – non-toxic 1 (b) (i) jet aeroplane fuel 1 (ii) petrol 1 (iii) petroleum gas 1

TOTAL 7 QUESTIONSHEET 20 (a) C & D (both) 1 (b) (i) produces carbon dioxide 1 may produce toxic gases 1 (ii) last for a long time/may cause pollution of water supplies 1 eyesore 1 (c) they may melt 1 if they are thermoplastics 1 (d) used to heat homes/factories 1

TOTAL 8

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (i) scales 1 plotting all the points accurately 1 drawing a smooth curve ignoring the 6 min point 1 (ii) I curve drawn to the left of curve A 1 curve to start at 71.00 g and to finish at 70.20 g 1 II curve drawn to the right of curve A 1 curve to start at 71.00 g and to finish at 70.60 g 1 (iii) particles have more energy 1 greater chance of successful collision 1 therefore greater rate of reaction 1

TOTAL 10

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES QUESTIONSHEET 2 (a) halve time three times 1 4 mins 1 (b) sensible scales 1 correct plotting 1 correct line drawn 1 (c) impossible to have reaction in zero time 1 too cold and reaction will stop 1

TOTAL 7

0 10 20 40 50 30 60 70 0

10

20

30

40

50

60

70

Time/min

Tem

pera

ture

/ 0 C

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES

QUESTIONSHEET 3 (a) (i) All state symbols correct: CaCO3(s) + 2HCl(aq) CaCl2(aq) + CO2(g) + H2O(l) 1 (ii) calcium chloride 1 (iii) 40 + 12 +(3 × 16) = 100 1 (iv) A Idea that 1 mole / 1 molecule of CaCO3 produces 1 mole / molecule of CO2 1 mass of 1 mole of CO2 = 44 g 1 B 0.44 g / 1% of candidate’s answer to A 1 (b) (i) would know how much CO2 could be produced 1 if very different result obtained, could indicate error/could be used to monitor reliability of technique 1 (ii) in method A, some CO2 would escape before apparatus was placed on balance/ before initial reading could be taken 1 would lead to underestimate of CO2 produced 1

TOTAL 10

QUESTIONSHEET 4 (a) sulphur is produced 1 clouds up the beaker/ sulphur is insoluble 1 (b) (i) 9Z 1 (ii) 9X 1 (iii) 9Y 1 (c) (i) St Paul’s 1 (ii) concentration affects rate of reaction 1 St Paul’s is fastest 1 (d) shine lamp through beaker 1 set photocell on other side 1 time how long it takes for motor to stop 1

1

TOTAL 12

M

uv lamp photo cell motor

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES QUESTIONSHEET 5 (a) (i) a substance which speeds up a reaction 1 but is not used up/ still present at the end of the reaction 1 (ii) enzymes 1 (b) (i) sample at 80oC 1 (ii) enzyme denatured at 80oC 1 leaving the reaction without a catalyst 1 so very slow 1 (iii) sample at 40oC 1 (iv) reaction is fastest at this temperature/ reaction is slower at lower temperatures 1 most starch digested 1 (v) iodine 1

TOTAL 11 QUESTIONSHEET 6 (a) fizzes / bubbles/ gradually disappears 1

(b) s10

cm40 3

= 4 cm3 s-1 1

(c) much slower 1 fewer particles, so fewer collisions 1 (d) increase temperature / heat it 1 change surface area of magnesium → powder 1

(e) moles of hydrogen =000,24

40 1

= 1.67 × 10-3 1 TOTAL 8

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES

QUESTIONSHEET 7 (a) yellow precipitate/ goes cloudy 1 (b) sodium chloride, water, sulphur dioxide (any 2) 2 (c) increase concentration of either reactant 1 more particles closer together/ more collisions 1 (d) (i) plot of either volume of Na2S2O3 or water v time 1 points plotted 1 smooth curve 1 (ii) concentration 1 (iii) to keep concentration of acid constant 1 (iv) goes cloudy/ solid forms 1

TOTAL 11

QUESTIONSHEET 8 (a) add universal indicator solution/paper/test with pH meter 1 universal indicator turns orange/pink/pH falls 1 (b) the amount/mass of lactic acid 1 produced in 1 second/specified time 1 (c) bacteria produce an enzyme/biological catalyst 1 (d) statements or diagrams showing: lactose molecules colliding with enzyme molecules 1 lactose and enzyme molecules bonded together 1 lactic acid molecules released from enzyme molecules 1 (e) the concentration of lactose decreases/ the lactic acid destroy the enzyme/kills the bacteria 1 (f) the rate of reaction decreases 1 because the high temperature destroys the enzyme/kills the bacteria 1

TOTAL 11

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES QUESTIONSHEET 9 (a) pxes labelled 1 points plotted 1 smooth curve 1 (b) (i) take value from graph (about 21) 1 (ii) reaction is so fast 1 (c) (i) hydrogen 1 (ii) ‘pops’ with lighted splint 2

TOTAL 8

QUESTIONSHEET 10 (a) (i) creates larger surface area of catalyst 1 (ii) rate of reaction increases 1 as temperature rises 1 (b) (i) reactants stick to surface of catalyst 1 products separate from catalyst after reaction 1 heavy metals block surface to reactants 1 (ii) lead is a heavy metal 1 would ruin catalyst 1

TOTAL 8 QUESTIONSHEET 11 (a) 2H2O(l) 2H2O(l) + O2(g) formulae correct 1 balancing 1 (b) (i) manganese(IV) oxide / manganese dioxide 1 (ii) lowers activation energy 1 provides surface for reaction 1 (iii) weigh before and after 1 then test its catalysing properties again 1

TOTAL 7

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES

QUESTIONSHEET 12 (a) measure loss of mass as gas lost 1 over a period of time 1 (b) (i) hydrogen 1 (ii) lighted splint 1 produces pop / explosion 1 (iii) Zn + 2HCl ZnCl2 + H2 2 (formulae – 1, balancing – 1) (c) (i) rate increased/faster 1 (ii) rate increased/faster 1 (iii) rate increased/faster 1

TOTAL 10 QUESTIONSHEET 13 (a) pressure forces gases into smaller space 1 molecules more likely to collide 1 (b) large surface area of powder 1 can create explosions when it burns/ causes very rapid combustion 1 (c) in less than one minute/faster than ribbon 1 (d) heat gives molecules more energy 1 collisions more likely to produce reaction 1 (e) cooling slows down reactions 1 but does not stop them 1

TOTAL 9 QUESTIONSHEET 14 (a) CO = carbon monoxide 1 NOx = oxides of nitrogen 1 CH = hydrocarbons 1 (b) (i) C 1 (ii) carbon monoxide 1 (iii) oxides of nitrogen 1

TOTAL 6

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES QUESTIONSHEET 15 (a) (i) steeper line 1 same volume of oxygen 1 (ii) much steeper line 1 same volume of oxygen 1 (b) more gas produced with Y 1 catalyst does not affect outcome of reactions 1 (c) some Y used up 1 catalysts are not used up 1

TOTAL 8

QUESTIONSHEET 16 (a) H2O2 1 (b) oxygen 1 (c) (i) susbtance which speeds up a reaction 1 but does not get permanently used up/ can be recovered unchanged at the end 1 (ii) A 1 does not change speed/rate 1 (iii) C 1 changes speed the most 1 (d) 5 g 1

TOTAL 9

30 60 90

volume of gas

time in seconds

(i) (ii)

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES

QUESTIONSHEET 17 (a) Three from: add catalyst heat/warm reaction use higher concentration of reactants use solid reactants with greater surface area / stir more increase pressure of gaseous reactants 3 (b) not enough activation energy supplied by a match 1 heat from the match is conducted away by the rest of the tree 1 (c) dust has greater surface area 1 burns more easily 1

TOTAL 7 QUESTIONSHEET 18 (a) (i) D 1 (ii) B 1 (b) (i) 60 cm3 1 (ii) 20 s 1 (c) 66 cm3 1 (d) (i) 66 cm3 1 (ii) the same 1

TOTAL 7

QUESTIONSHEET 19 (a) Two from: (gas) syringe, measuring cylinder, burette 2 (b) (i) Three from: use same sized pieces of magnesium/ use same mass of magnesium use same volume of acid keep temperature the same stir the same amount 3 (ii) stop clock 1 (c) balance reading to 2 decimal places 1

TOTAL 7

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GCSE CHEMISTRY RATES OF REACTION ANSWERS AND MARK SCHEMES QUESTIONSHEET 20 One mark for each of the following (in correct order) (i) joules 1 (ii) kilojoule 1 (iii) exothermic 1 (iv) endothermic 1 (v) catalyst 1 (vi) increased 1 (vii) surface area 1 (viii) photography/sunburn 1 (ix) light 1

TOTAL 9

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) (i) lose one or more electrons 1 (ii) Li/Na/K/Cu 1 (b) (i) Al3+ 1 (ii) Cl

- 1 (iii) AlCl3 1 (c) (i) covalent 1 (ii) CCl4 1 (iii) (1 for bond pairs, 1 for lone pair) 2

TOTAL 9 QUESTIONSHEET 2 (a) (i) CO2 1 (ii) thermal decomposition 1 (b) (i) 100 1 (ii) Mr of CaO = 56 1 56 t CaO produced from 100 t calcium carbonate 1 280 t CaO produced from 500 t calcium carbonate 1

TOTAL 6 QUESTIONSHEET 3 (a) 2 and 2 1 (b) mass of magnesium = 44.9 - 40.1 = 4.8 g 1 mass of magnesium oxide = 48.1 - 40.1 = 8.0 g 1 so, mass of oxygen = 8.0 - 4.8 = 3.2 g 1 moles of oxygen = 3.2/16 = 0.2 1 moles of magnesium = 4.8/24 = 0.2 1 ratio Mg:O = 1:1 therefore MgO 1

TOTAL 7

H

H H N x •

x x

x • x •

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES QUESTIONSHEET 4 (a) (i) to condense water 1 (ii) find boiling point/boiling point is 100oC/ find freezing point/freezing point is 0oC/ blue cobalt chloride paper goes pink 1 Note: Cobalt chloride paper test only shows the presence of water, not that the substance is water. It could be dilute acid, salt solution etc. (b) (i) 2.5 - 1.6 = 0.9 g 1 (ii) 0.9 / 2.5 1

= 36% 1 (c) (i) dehydration 1 (ii) CuSO4 + 5H2O ∏ CuSO4.5H2O 1 (iii) � 1

TOTAL 8 QUESTIONSHEET 5 (a) (i) 23 + 14 + (3 × 16) = 85 1 (ii) 14 + (4 × 1) + 14 + (3 × 16) = 80 1 (b) (i) 14/85 × 100 1 = 16.5% 1 (ii) 28/80 × 100 1 = 35% 1 (c) ammonium nitrate 1 (d) Two from: alkaline/gas/poisonous/very soluble/smelly 2

TOTAL 9

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 6 (a) (i) 3.5/14 = 0.25 4/16 = 0.25 1 NO 1 (ii) 50/16 = 3.1 50/32 = 1.5625 1 SO2 1 (iii) 39/39 = 1 1/1 = 1 12/12 = 1 48/16 = 3 1 KHCO3 1 (iv) mass of oxygen = 16.0 − 11.2 = 4.8 1 4.8/16 = 0.3 11.2/56 = 0.2 1 Fe2O3 1 (b) (i) 4.04/1 = 4.04 24.24/12 = 2.02 71.72/35.5 = 2.02 1 ratio of H:C:Cl = 2:1:1 1 CH2Cl 1 (ii) relative mass of CH2Cl = 49.5 1 99/49.5 = 2 therefore C2H4Cl2 1

TOTAL 14 QUESTIONSHEET 7 (a) copper(II) oxide 1 (b) (i) copper(II) chloride 1 (ii) copper and chlorine 2 (iii) bleaches 1 moist indicator paper 1 (c) (i) copper 1 (ii) water 1 (iii) CuO + H2 → Cu + H2O 1 (iv) reducing agent 1

TOTAL 10

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES QUESTIONSHEET 8 (a) (i) to allow you to find mass of substances in it 1 (ii) 125.9 - 117.8 = 8.1 g 1 (iii) 124.7 - 117.8 = 6.9 g 1 (iv) 8.1 - 6.9 = 1.2 g 1 (v) 1.2/8.1 × 100 1 = 14.8% 1 (b) heat the crucible again 1 cool and reweigh 1 repeat until weight is constant 1 (c) (i) 208 1 (ii) 18 1 (d) moles of BaCl2 = 6.9/208 = 0.0332 1 moles of water = 1.2/18 = 0.0667 1 ratio of 1:2 therefore x = 2 1

TOTAL 14 QUESTIONSHEET 9 (a) precipitation 1 (b) reduction 1 (c) endothermic 1 (d) reversible 1 (e) decomposition 1 (f) oxidation 1 (g) displacement 1 (h) combustion 1 Note: In a question of this type it is not necessary to use all the available terms. Sometimes, a term will be required more than once.

TOTAL 8

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 10 (a) energy/ heat transferred to surroundings 1 (b) Ca(OH)2 1 (c) neutralise acidity in lakes/soil/swimming pools 1 (d) bubble carbon dioxide through it 1 (e) heating it strongly 1 (f) compounds can be formed from each other 1 any substances added are given off at a later stage 1

TOTAL 7 QUESTIONSHEET 11 (a) displacement 1 (b) c, e, f 3 (c) chlorine + potassium bromide → bromine + potassium chloride 1 (d) Cl2 + 2KBr ς 2KCl + Br2 2 (e) chlorine most reactive, then bromine, last iodine 1 (f) fluorine displaces chlorine 1 (g) no reaction 1

TOTAL 10

QUESTIONSHEET 12 (a) all are soluble 1 (b) all are soluble 1 (c) all except nitrate 1 are insoluble 1 (d) (i) lead carbonate + sodium nitrate 2 (ii) no precipitate formed/ no reaction 1 (iii) barium sulphate + sodium chloride 2 (e) barium sulphate is very insoluble 1 not absorbed into bloodstream 1

TOTAL 11

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES QUESTIONSHEET 13 (a) labelled axes 1 sensible scales 1 accurate plotting 1 line of best fit 1 (b) student 4 1 (c) (i) 38 cm3 (+/- 1 cm3) 1 (ii) 0.02 g (+/- 0.005 g) 1 (d) (i) find the density of the gas / mass/volume 1 compare to data book 1 (ii) glowing splint 1 relights 1 Note: Always include the result of a chemical test. It is not sufficient to say, for example, “Use the glowing splint test”.

TOTAL 11

x

x

x x

x

0 10 20 30 40 50 60 70 80 90

0.01

0.02

0.03

0.04

0.05

0.06

0.07

0.08

0.09

0.10

0.11

0.12

0.13

0.14

Volume of gas (cm3)

Loss in mass (g)

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 14 (a) (i) A and D 1 (ii) rusting requires water/moisture 1 and oxygen/air 1 (b) tube D 1 salt/ions in salt accelerates rusting 1 (c) zinc/magnesium attached to hull/pier 1 zinc/magnesium more reactive than iron 1 corrodes in preference to iron 1 (d) (i) alloyed with another metal/electroplated 1 (ii) coated in paint/plastic/electroplated 1

TOTAL 10 QUESTIONSHEET 15 (a) Two from: alloys may resist corrosion alloys may look more attractive alloys have lower meting points 2 (b) (i) iron/steel 1 (ii) galvanising 1 (c) (i) sulphur dioxide 1 (ii) Zn2+ 1 (d) neutralisation 1 (e) (i) carbon 1 (ii) ZnO + C → Zn + CO 1 (iii) reduction 1

TOTAL 10

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES QUESTIONSHEET 16 (a) (i) sodium hydrogencarbonate 1 (ii) acid 1 (iii) sodium carbonate 1 (b) the acid and carbonate react together 1 and fizz/produce carbon dioxide 1 (c) (i) raising agent 1 because it decomposes when heated to give carbon dioxide gas 1 (ii) does not produce carbon dioxide when heated 1

TOTAL 8 QUESTIONSHEET 17 (a) (i) calcium oxide 1 (ii) calcium carbonate 1 (b) endothermic 1 (c) limestone glowed brightly 1 crumbled 1 (d) process is continuous/less energy loss/ time-saving 1 (e) (i) Two from: jobs created money brought into area extension better than starting new quarry 2 (ii) Two from: loss of animal habitats eyesore dust noise extra lorries on roads 2

TOTAL 10

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GCSE CHEMISTRY REACTIONS & FORMULAE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 18 (a) (i) delivery tube on end of test tube 1 delivery tube through cork 1 end of delivery tube in limewater 1 (ii) limewater 1 goes cloudy/milky 1 (b) (i) copper produces a green flame 1 (ii) dipped in acid 1 (iii) calcium 1 (c) calcium carbonate 1

TOTAL 9 QUESTIONSHEET 19 (a) D 1 (b) (i) A 1 (ii) hydrogen 1 (c) C 1 (d) (i) D 1 (ii) irritant/harmful 1 (e) hydrogen burns to make water 1 wasserstoff = water maker 1

TOTAL 8 QUESTIONSHEET 20 (a) (i) C + O2 → CO2 1 (ii) poisonous 1 (b) (i) oxygen is removed 1 (ii) carbon 1 (c) harder 1 lighter in colour 1 rougher texture 1

TOTAL 7

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 1 (a) (i) noble/inert/rare gases 1 (ii) two out of helium, neon, argon, krypton, xenon, radon. 2 (b) (i) C 1 (ii) atoms do not combine/monatomic atoms/inert gas so atoms don’t join/ A, B and C show molecules and group 0/8 elements do not form molecules 1 (c) splint goes out/does not burn 1 (d) (i) all unreactive/stays the same 1 (ii) density increases 1 (iii) all non metals/stays the same 1 (e) (iv) measure the density of each 1

TOTAL 10

QUESTIONSHEET 2 (a) (i) A 1 (ii) ‘A’ has 11 electrons and atomic number of sodium is 11 1 ‘A’ has one electron in outside shell but ions have full outer shell 1 (iii) one electron in outside shell 1 (b) (i) charged atom/group of atoms 1 (ii) K+ 1 (c) Any two from: very reactive react with air react with oxygen in the air react with water in the air 2 (d) (i) oxygen (in the air) 1 (ii) potassium oxide 1 (iii) potassium + oxygen → potassium oxide 1 (iv) 4K + O2 → 2K2O 2

TOTAL 13

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 3 (a) (i) lithium + chlorine → lithium chloride 1 (ii) 2Li + Cl2 → 2LiCl 1 (b) (i) group 1 1 (ii) 1 1 (iii) 7 1 (c) diagram to show: chlorine seven electrons 1 lithium one electron being transferred to chlorine 1 lithium ion one positive charge, chloride ion one negative charge 1 (d) (i) more reactive 1 (ii) common/table/cooking salt 1

TOTAL 10

Li x

+ C1 ς Li+

x C1 -

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 4 (a) (i) ions 1 (ii) sodium ion 1 (iii) chloride ion 1 (iv) attraction of opposite charges/ electrostatic attraction 1 (b) (i) 1 (ii) 7 (iii) 3 (iv) 3 (v) 1 (vi) 7 6 (c) (i) sodium needs to lose one electron 1 to empty outside shell/ to give full/complete outer shell/octet/stable electron arrangement 1 sodium transfers electron to chlorine atom 1 which completes its octet 1 1 (ii) one sodium ion electrically balances one chloride ion 1

TOTAL 16

Na x

+ C1 ς Na+

x C1

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 5 (a) (i) to kill bacteria/germs in water 1 (ii) antiseptic/put on cuts to kill bacteria/germs 1 (b) (i) halogens 1 (ii) non-metal 1 (iii) non-metal 1 (c) (i) 17 protons in nucleus/17 electrons in uncombined atom 1 (ii) 3 1 (iii) 7 1 (iv) sodium iodide 1 NaI 1

TOTAL 10

QUESTIONSHEET 6 (a) (i) goes dark 1 (ii) photosynthesis/colour fading 1 (b) (i) ion/anion/negative ion 1 (ii) no 1 (c) (i) go dark 1 (ii) Ag+(aq) + I- (aq) ς AgI(s) 3 (2 marks for correct equation; only 1 if ions not shown. 1 mark for state symbols)

TOTAL 8

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 7 (a) (i) isotopes 1 (ii) different number of neutrons 1 (iii) number of protons 1 number of electrons in uncombined atom 1 (iv) 35 (neutrons + protons) –17 (protons) 1 18 neutrons 1 (b) mixture if different isotopes/chlorine-35 and chlorine-37 1 (c) (i) no difference 1 (ii) Any two from: chemical properties stay the same both elements have 7 electrons/same number of electrons in their outside shell chemical properties depend on number of electrons in outside shell 2 (iii) no 1 (iv) different masses/physical properties depend on the mass 1

TOTAL 12

QUESTIONSHEET 8 (a) (i) 3 1 (ii) second electron shell is full 1 next electron has to go into third shell/one electron in outside shell 1 (b) (i) sodium, magnesium and aluminium/Na, Mg and Al (all three needed for mark) 1 (ii) go from metallic (left hand side) to non-metallic (right hand side) 1 (c) (i) 6 (electrons) 1 (ii) sodium oxide: Na2O magnesium oxide: MgO aluminium oxide: Al2O3 3

TOTAL 9

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 9 (a) group 0/8 / noble gases/inert gases 1 (b) (i) drop/go down/fall 1 (ii) Any two from: lower down in the group group 0/8 elements get denser as the atomic number increases krypton denser/heavier for the same volume than the gases in the other balloons/air 2 (c) (i)

1 (ii) outer shell complete 1 helium does not combine/react with anything 1 (d) (i) very light/less dense than air 1 unreactive/does not react with air/non-flammable 1 (ii) unreactive/inert/full outer electron shells 1 won’t react with hot filament of light bulb 1

TOTAL 11 QUESTIONSHEET 10 (a) (i) group 1 1 (ii) alkali metals 1 (iii) white 1 (b) Any three from: use platinum/nichrome wire clean wire/by dipping in hydrochloric acid and putting into a hot flame dip wire into salt/solution of salt/hydrochloric acid and then salt put into blue flame/hottest part of flame/side of a blue flame look at colour of flame. 3 (c) A = sodium chloride 1 B = lithium chloride 1 C = potassium chloride 1

TOTAL 9

x

x

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 11 (a) (i) chlorine, bromine, iodine 1 (ii) atomic number 1 (b) (i) 7 1 (ii) molecules 1 (iii) Any two from: outer shell incomplete each chlorine atom needs one more electron to complete its octet each atom shares one electron 2 (c) (i) diagram to show: two electron shells 1 two electrons in first shell, seven in outside shell 1 (ii) gas 1 (iii) -220

oC (accept –200

oC to –250

oC) 1

(d) boils/becomes a gas/vapour 1

TOTAL 11

QUESTIONSHEET 12 (a) (i) colourless 1 (ii) Any two from: a solid in a liquid very small particles of solid. 2 (iii) silver chloride 1 (b) (i) silver nitrate + sodium chloride → silver chloride + sodium nitrate 1 (ii) (aq) 1 (iii) (s) 1 (iv) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) 2

(c) B and C 2

TOTAL 11

x x

x x

x

x x x x

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 13 (a) (i) transition elements/ transition metals 1 (ii) metals 1 (iii) Fe = iron, Cu = copper, Zn = zinc 3 (b) (i) A 1 (ii) A 1 high melting point/B would melt when the water boiled 1 (iii) hard 1 can be pulled out to make a wire 1 shiny surface that can be polished 1

TOTAL 11

QUESTIONSHEET 14 (a) (i) one out of scandium, titanium, vanadium, chromium, manganese, iron, cobalt, nickel, zinc, or between atomic numbers 39-48, 57, 72-80 including silver, gold, platinum and mercury 1 (ii) limewater 1 (iii) lime water went cloudy/milky/white precipitate 1 (iv) carbon dioxide 1 (b) (i) copper(II) oxide 1 (ii) gas made 1 copper carbonate changed colour 1 (iii) copper carbonate → copper oxide + carbon dioxide 1 (iv) CuCO3 → CuO + CO2 1 (c) (i) B 1 (ii) Any two from: there was a reaction in B/no reaction in A zinc carbonate/transition metal carbonate breaks down on heating sodium carbonate/group 1 metal carbonates do not break down on heating zinc oxide is yellow when hot and white when cold 2 (iii) Any two from: A was sodium carbonate sodium carbonate does not break down on heating group 1 metal carbonates do not break down on heating 2

TOTAL 14

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 15 (a) (i) transition elements 1 (ii) blue/green 1 (b) (i) add a small amount of sodium hydroxide solution 1 colour of precipitate indicates which metal ion is present 1 (ii) A = copper B = green C = iron(III) (all three for 2 marks one or two for one mark) (c) (i) Fe2+ 1 (ii) OH- 1 (iii) Fe2+ + 2OH- → Fe(OH)2 1

TOTAL 9

QUESTIONSHEET 16 (a) (i) 2 1 (ii) 8 1 (iii) the number of electron shells 1 (b) (i) 2 1 (ii) 4 1 (iii) the number of electrons in the outside shell 1 (c) (i) 6 protons in atom/ in the nucleus 1 6 electrons in uncombined atom 1 (ii) mass number/ relative atomic mass 1 (iii) number of neutrons plus number of protons 1

TOTAL 10

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 17 (a) (i) One out of: Li, Be, Na, Mg, Al, K, Ca, Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, Zn, Ga, Ge. 1 (ii) One out of: H, N, O, F, Cl, He, Ne, Ar, Kr. 1 (iii) One out of: Ti, V, Cr, Mn, Fe, Co, Ni, Cu. (allow Sc and Zn) 1 (b) (i) 7 1 (ii) 3 1 (iii) 3 1 (iv) 7 1 (c) number of protons/number of electrons in neutral (uncombined) atom 1 (d) (i) inert/noble/rare gases 1 (ii) unreactive/do not react 1 (iii) outer electron shell contains 8 electrons/ complete octet 1

TOTAL 11

QUESTIONSHEET 18 (a) (i) lithium 1 (ii) rubidium 1 (iii) potassium 1 (b) blue 1 (c) (i) burnt with a ‘pop’/small explosion 1 (ii) hydrogen 1 (d) (i) more reactive 1 (ii) hydrogen and sodium hydroxide 1 (e) Any two from: react with water to give alkalis all metals hydroxides are alkalis hydroxides all dissolve in water to give alkaline solutions 2

TOTAL 10

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GCSE CHEMISTRY THE PERIODIC TABLE ANSWERS AND MARK SCHEMES

QUESTIONSHEET 19 (a) (i) Any two from: high melting point good conductors of heat strong/high tensile strength 2 (ii) expensive/copper compounds are poisonous 1 (iii) good conductor of electricity 1 ductile/high tensile strength 1 (iv) cars: strong/high tensile strength/(relatively) cheap 1 planes: high density 1 (b) (i) speeds up a reaction 1 (ii) with transition elements 1 (c) (i) positive/cation 1 (ii) Cu2+ Fe3+ 2

TOTAL 12

QUESTIONSHEET 20 (i) I C or E 1 II F or A 1 III A 1 IV D 1 V D 1 VI G 1 VII E 1

TOTAL 7