Welcome to WQE Taster Activities 2020

ChemistrySubject level

A-level

Resource site

www.wqe.ac.uk/tasteractivities

Awarding body

AQA

Assignment details

From GCSE to A-level Chemistry:

Studying Chemistry after GCSEs really develops your practical and mathematical skills. If you enjoy experimenting in a lab, you’ll love it.

At first, the jump from GCSE to A-level may be a little daunting however if you follow the tips and advice in this guide, you will soon adapt.

Where does studying A-level Chemistry take you?

Chemistry students get to investigate a huge range of ideas therefore the career opportunities are endless. Some of the possible career opportunities are highlighted below:

Analytical chemist Chemical engineer Clinical biologist Pharmacologist Doctor Research scientist Toxicologist Patent attorney Science writer Environmental consultant

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Specification at a glance:

The A-level chemistry course is split up into three parts, physical chemistry, inorganic chemistry and organic chemistry. Below is the overview of the specification:

Year 1:

Physical Inorganic OrganicAtomic Structure Periodicity Introduction to organic

chemistryAmount of Substance Group 2 AlkanesBonding Group 7 Haloalkanes Energetics AlkenesKinetics AlcoholsEquilibria Organic AnalysisRedox

Year 2:

Physical Inorganic OrganicThermodynamic Period 3 Optical isomerismRate Equations Transition Metals Aldehydes and

KetonesEquilibrium constants Reactions of ions in

aqueous solutionCarboxylic Acids

Electrode potentials Aromatic ChemistryAcid and Bases AminesEquilibria Polymers

Amino AcidsOrganic synthesisNMRChromatography

Places to go for help throughout your course:

Websites:

Full Specification: https://www.aqa.org.uk/subjects/science/as-and-a-level/chemistry-7404-7405/specification-at-a-glance

https://www.chemguide.co.uk/

https://www.physicsandmathstutor.com/

https://www.youtube.com/channel/UCPtWS4fCi25YHw5SPGdPz0g

https://www.youtube.com/channel/UCps4gUjfZsu6-b-7mwK41lg

http://www.a-levelchemistry.co.uk/

https://chemrevise.org/

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Activity 1: Important vocabulary for practical work

Match the correct word to the definition:

Accurate A statement suggesting what might happen in the future

Data An experiment that gives the same result when a different person carries it out, or a different technique or set of equipment is used

Precise A measurement that is close to the true value

Prediction An experiment that gives the same results when the same experimenter uses the same method and equipment

Range Physical, chemical or biological quantitates or characteristics

Repeatable A variable that is kept constant during an experiment

Reproducible A variable that is measured as the outcome of an experiment

Resolution This is the smallest change in the quantity being measured (input) of a measuring instrument that gives a perceptible change in the reading

Uncertainty The interval within the true value can be expected to lie

Variable The spread of data, showing the maximum and minimum values of the data

Control variable Measurements where repeated measurements show very little spread

Dependant variable Information, in any form that has been collected.

Activity 2: The Periodic Table3

The periodic table of elements is shown on the back page of this booklet. The A-level course will build on what you have learned in GCSEs

1. Draw a line showing the metals and non-metals 2. Colour the transition metals in blue 3. Colour the halogens in yellow4. Colour the alkali metals in red 5. Colour the noble gases in green6. Draw a blue arrow showing the direction of the periods7. Draw a red arrow showing the direction of the groups.

Activity 3: Writing ionic formula

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Below are some common ions and the charges they carry, you need to be able to write correct ionic formulae. Use the table to write the correct formula for the following ionic compounds.

Copper oxide Aluminium oxide Magnesium oxide

Lead nitrate Potassium nitrate Copper carbonate

Sodium hydroxide Lithium iodide Zinc fluoride

Calcium carbonate Barium oxide Barium sulphate

Iron (II) oxide Iron (III) oxide Silver iodide

Activity 4: Bonding

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Write the key concepts regarding the following type of bonding:

Ionic Bonding:

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Covalent Bonding:

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Metallic Bonding:

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_______________________________________________________________________

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Explain the differences in bonding between graphite and diamond?

Explain how and why sodium chloride can conduct electricity?

Describe the properties of aluminium?

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Activity 5: Writing and balancing equations

Throughout your GCSEs you have come across common reactions between acids and metals complete the following chemical reactions by writing balanced symbol equations.

Magnesium + hydrochloric acid

Sodium + sulphuric acid

Hydrochloric acid + sodium hydroxide

Potassium hydroxide + hydrochloric acid

Sodium hydroxide + sulphuric acid

Calcium carbonate + hydrochloric acid

Potassium Carbonate + Hydrochloric Acid

Calcium hydroxide + nitric acid

Nitric acid + calcium

Magnesium carbonate + Hydrochloric Acid

Zinc + sulphuric acid

Calcium + water

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Activity 6: Re-arranging formula

Rearrange this equation so that each of the following is the subject of the equation:

Pv=nRt

A) VB) nC) TD) p

Make the bracketed symbol the subject of the equation:

A) c=fλ (λ)

B) c=nv (v)

C) Q= MCΔT (ΔT)

D) n=V1000

xc (V)

E) n=V1000

xc (c)

F) E=hf (h)

G) ∆G=∆H−T ∆ S (∆ S ¿

Re arrange the following equation so that each of the following is the subject of the equation:

KE=12mv2

a) m b) v

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Activity 7: Calculating the number of moles of a solid

You can find the number of moles of a substance if you are given its mass and you know its molar mass:

number of moles = mass/molar mass

n = m/Mr

Mass MUST be measured in grams!

Molar mass has units of gmol-1

1. Calculate the number of moles present in:

2. Calculate the mass of:

3. Calculate the molar mass of the following substances:

a) 2.3 g of Na a) 0.05 moles of Cl2 a) 0.015 moles, 0.42 g

b) 2.5 g of O2 b) 0.125 moles of KBr b) 0.0125 moles, 0.50 g

c) 240 kg of CO2 c) 0.075 moles of Ca(OH)2

c) 0.55 moles, 88 g

d) 12.5 g of Al(OH)3 d) 250 moles of Fe2O3 d) 2.25 moles, 63 g

e) 5.2 g of PbO2 e) 0.02 moles of Al2(SO4)3

e) 0.00125 moles, 0.312 g

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Activity 8: Equations and Molar Ratios

1. The equation: S + O2 → SO2 tells us that 1 mole of sulphur reacts with 1 mole of oxygen to give 1 mole of Sulphur Dioxide.

How many moles of oxygen would react with a) 2 moles of sulphurb) 10 moles of sulphurc) 0.5 moles of sulphur

How many moles of SO2 would be made by burningd) 2 moles of sulphure) 10 moles of sulphurf) 0.5 moles of sulphur

2. The equation: CH4 + 2O2 → CO2 + 2H2O tells us that 1 mole of methane reacts with 2 moles of oxygen to give 1 mole of carbon dioxide and 2 moles of water

How many moles of oxygen would react with a) 2 moles of methaneb) 10 moles of methanec) 0.5 moles of methane

How many moles of CO2 would be made by reacting d) 2 moles of methanee) 10 moles of methanef) 0.5 moles of methane

How many moles of CH4 would react with

g) 2 moles of O2

h) 4 moles of O2

i) 0.5 moles of O2

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