WELCOME TO AP CHEMISTRY!Mrs. Tolentino

Summer Assignment 2017

This course is designed to give you the equivalent of a general chemistry course that is typically taken during the first year of college. The text, Chemistry by Zumdahl contains 22 chapters, seven of which were topics already covered in Chemistry R.

Due DateThis assignment is due in full on Wednesday, September 6, 2017.Ten points per day will be deducted for late assignments.

GradingThis assignment will be equivalent to one major test. Woodbridge Board of Education Policy states that marking period grades for Advanced Placement courses are determined using the following formulas:

75% Major AssessmentsTests, Major Laboratory Reports, Summer Assignment

25% Minor AssessmentsQuizzes, Weekly Participation grade/minor labs

AssignmentThe assignment is divided into four parts: I. Writing Names and FormulasMemorize the names, symbols, and charges of the ions by making flashcards (or other memorization learning devices). You should be able to name and write formulas of ionic compounds, covalent compounds and acids.

II. Stoichiometry/Problems and Short Answer QuestionsRead Chapters 1 to 4 of the textbook. These problems were taken from the End-of-Chapter section of the textbook. Check out the answers to the odd-numbered problems at the back. The Solubility Rules (page 144 Zumdahl) and the list of strong acids and bases (page 131 Zumdahl) should be memorized.

III. Chemical Equations and Predicting Products Predict the products and balance the equations. For each type of reaction, use as your guide the examples given.

IV. AP Insight Performance Tasks: Geometry, Nonpolar, Dipole Forces, and IMF's(Get from me the Part IV Hard copy together with your books by June 19. Copyright laws prevent me from posting these online.)

Suggestions: Complete this assignment as soon as possible! Complete Parts 1 and 2 by end of July and submit

scanned answers and solutions/work via email or google classroom. You may email me for any concerns or questions at maria.tolentino@woodbridge.k12.nj.us Join and check google classroom periodically Class Code: g8wnof Looking forward to seeing you in September!

Part I. Writing Names and FormulasWrite the chemical formula for the following:

1. sodium sulfate ____________________

2. manganese dioxide ____________________

3. potassium carbonate ____________________

4. calcium phosphate ____________________

5. ammonium chloride ____________________

6. sodium hydroxide ____________________

7. iron (III) chloride ____________________

8. dinitrogen monoxide ____________________

9. lead (II) sulfide ____________________

10. potassium chlorate ____________________

11. hydrochloric acid ____________________

12. nitric acid ____________________

13. sulfuric acid ____________________

14. perchloric acid ____________________

15. potassium dichromate ____________________

16. potassium permanganate ____________________

17. carbon tetrachloride ____________________

18. acetic acid ____________________

19. zinc nitrate ____________________

20. chromium(II) oxide ____________________

Write the chemical name for the following

1. NaHCO3 ____________________

2. PCl3 ____________________

3. BaSO4 ____________________

4. AgCl ____________________

5. H2S ____________________

6. CuCl ____________________

7. Li3N ____________________

8. Na2SO3 ____________________

9. HF ____________________

10. NaCN ____________________

11. NaH ____________________

12. P4O10 ____________________

13. KOH ____________________

14. NH3 ____________________

15. CaCO3 ____________________

16. SnCl4 ____________________

17. Fe2O3 ____________________

18. H2CO3 ____________________

19. H3PO4 ____________________

20. (NH4)2SO4 ____________________

Part II. Stoichiometry / Conversions / ProblemsSolve the following problems. Encircle your final answer. All solutions should be shown. The AP College Board gives partial points for correct solutions.

Cham R Chapter 3 Measurements and Dimensional Analysis1. Gasoline has a density of 0.73 g/cm3. How many liters of gasoline would be required to increase the mass of an automobile from 1271 kg to 1305 kg?(Note: 1 cm3 = 1 mL )

2. Pure gold can be made into extremely thin sheets called gold leaf. Suppose that 50 kg of gold is made into gold leaf having an area of 3620 m2. The density of gold is 19.3 g/cm3.a) How thick in micrometers is the gold leaf? (106 micrometers = 1 meter)

b) A gold atom has a radius of 1.44 x 10-10 m. How many atoms thick is the gold leaf?

3. Precious metals are commonly measured in troy ounces. A troy ounce is equivalent to 31.1 g. How many moles are in a troy ounce of silver?

Chem R Chapter 12 Stoichiometry / Mole Ratios 4. A combustion reaction involves the reaction of a substance with oxygen gas. The complete combustion of any hydrocarbon (binary compound of carbon and hydrogen) produces carbon dioxide and water as the only products. Octane is a hydrocarbon that is found in gasoline. Complete combustion of octane produces 8 moles of carbon dioxide for every 9 moles of water vapor. What is the molecular formula of octane?

Chem R Chapter 4 Atomic Structure5. The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 amu and 153Eu has a mass of 152.9209 amu. The average atomic mass of europium is 151.96 amu. Calculate the relative abundance of the two europium isotopes.

Chem R Chapter 10 Chemical Quantities6. Ascorbic acid, or vitamin C (C6H8O6), is an essential vitamin. It cannot be stored by the body and must be present in the diet.

a) What is the molar mass of ascorbic acid?

b) Vitamin C tablets are taken as a dietary supplement. If a typical tablet contains 0.500 g (equivalent to 500 milligrams) of vitamin C, how many moles of vitamin C does it contain?

c) how many molecules of vitamin C does it contain?

7.A compound contains only C, H, and N. Combustion of 35.0 mg of the compound produces 33.5 mg CO2 and 41.1 mg H2O. What is the empirical formula of the compound?

8. The compound cisplatin, Pt(NH3)2Cl2, has been studied extensively as an antitumor agent. Calculate the elemental percent composition by mass of cisplatin.

%Pt

%N

%H

%Cl

9. The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. What is the molecular formula of styrene?

How many H atoms are present in a 2.00g sample of styrene?

Chem R Chapter 16 Solutions pages 525-52710. Calculate the molarity of a solution prepared by dissolving a 5.623g sample of NaHCO 3 in enough water to make 250mL.

III. Chemical Equations and Predicting Products Predict the products and balance the equations. ALL reactions will occur. Make sure to write the correct formulas for the reactants and products.

Synthesis/Combination

A metal combines with a nonmetal to form a binary saltExample: A piece of lithium metal is dropped into a container of nitrogen gas.

6Li + N2 → 2Li3N

Metallic oxides and water form bases (metallic hydroxides)Example: Solid sodium oxide is added to water

Na2O + HOH → 2NaOH

Nonmetallic oxides and water form acidsExample: Carbon dioxide is bubbled into water

CO2 + H2O → H2CO3

Metallic oxides and nonmetallic oxides form saltsExample: Solid sodium oxide is added to carbon dioxide

Na2O + CO2 →Na2CO3

1. A strip of aluminum foil is placed in liquid bromine.

2. Magnesium metal is burned in nitrogen gas.

3. Solid magnesium oxide is added to water.

4. Powdered magnesium oxide is added to a container of carbon dioxide gas.

5. Sulfur trioxide gas is added to excess water.

6. Calcium metal heated in nitrogen gas.

7. Excess chlorine gas is passed over hot iron filings.

DecompositionA binary compound may break down to produce two elements usually through the process of electrolysis Example: 2NaCl → 2Na + Cl2

metallic carbonates metallic oxides + carbon dioxideExample: A sample of magnesium carbonate is heated

MgCO3 → MgO + CO2

metallic chlorates metallic chlorides + oxygen gasExample: A sample of magnesium chlorate is heated

Mg(ClO3)2 → MgCl2 + 3O2

hydrates → compound and water

1. A solution of hydrogen peroxide is decomposed catalytically.

Identify the oxidation state of oxygen in hydrogen peroxide.

2. Molten aluminum chloride is electrolyzed

3. Solid mercury(II) oxide decomposes as it is heated in an open test tube in a fume hood.

After the reaction is complete, is the mass of the material in the test tube greater than, less than, or equal to the mass of the original sample? Explain.

4. Solid potassium chlorate is heated in the presence of manganese dioxide catalyst

5. A solution of hydrogen peroxide is heated.

6. Solid calcium carbonate is strongly heated.

7. Solid copper(II) sulfate pentahydrate, CuSO4·5H2O is gently heated.

How many grams of water are present in 1.00 mol of copper(II) sulfate pentahydrate?

8. Electrolysis of water

Single DisplacementActive metals replace less reactive metals from their compounds in aqueous solutionExample: Magnesium turnings are added to a solution of iron(III) chloride.

3Mg + 2FeCl3 → 2Fe + 3MgCl2

Active metals replace hydrogen in waterExample: A pea-sized lithium is added to water

2Li + 2HOH → H2 + 2LiOH

Active metals replace hydrogen in acidsExample: Lithium is added to hydrochloric acid

2Li + 2HCl → H2 + 2LiCl

Active nonmetals replace less active nonmetals from their compounds in aqueous solution Example: Chlorine gas is bubbled into a solution of potassium iodide

Cl2 + 2KI → I2 + 2KCl

1. Calcium metal is added to a dilute solution of hydrochloric acid.

2. Liquid bromine is added to a solution of potassium iodide.

3. Pellets of lead are dropped into hot sulfuric acid.

4. Chlorine gas is bubbled into a solution of sodium bromide.

What is the oxidation number of chlorine before the reaction occurs?

What is the oxidation number of chlorine after the reaction occurs?

5. Solid zinc strips are added to a solution of copper sulfate.

6. Lead foil is immersed in silver nitrate solution.

7. Hydrogen gas is passed over hot iron(III) oxide

8. Aluminum metal is added to a solution of copper(II) chloride.

9. Small chunks of solid sodium are added to water.

The reaction is exothermic, and sometimes small flames are observed as the sodium reacts with the water. Identify the product of the reaction that burns to produce the flames.

10. Chlorine gas is bubbled into a solution of potassium iodide.

11. A strip of magnesium is added to a solution of silver nitrate.

12. A piece of cadmium metal is added to a solution of copper(II) chloride.

List two visible changes that would occur in the reaction container as the reaction is proceeding.

13. A copper wire is dipped into a solution of silver(I) nitrate.

Describe what is observed as the reaction proceeds.

14. Sulfuric acid is added to mossy zinc.

The gas generated by this reaction was tested using a glowing splint (a wooden stick with one end that has been ignited ). Describe the result.

Double Displacement

1. Dilute sulfuric acid is added to a solution of barium acetate.

2. Ammonium chloride crystals are added to a solution of sodium hydroxide.

3. Hydrogen sulfide gas is bubbled through a solution of lead(II) nitrate.

4. Solutions of silver nitrate and sodium chromate are mixedIf the contents of the reaction mixture described above are filtered, what substance(s), if any, would remain on the filter paper?

5. A barium nitrate solution and a potassium fluoride solution are combined and a precipitate forms.

If equal number of moles (equimolar) of barium nitrate and potassium fluoride are combined, which reactant, if any, is the limiting reactant? Explain.

6. A solution of ammonium sulfate is added to a saturated solution of barium hydroxide.

7. Excess nitric acid is added to solid calcium carbonate.

Briefly explain why statues made of marble (calcium carbonate) displayed outdoors in urban areas are deteriorating.

8. Solid potassium oxide is added to water.

If a few drops of phenolphthalein indicator are added to the resulting solution, what would be observed? Explain.

9. A piece of solid strontium carbonate is dropped into a solution of hydrochloric acid

Indicate one thing that would be observed as the reaction occurs.

CombustionCompounds containing carbon and hydrogen (and oxygen) burn in oxygen to produce carbon dioxide and water. If sulfur is present, SO2 is formed. 1. Ethanol (CH3CH2OH) is completely burned in the air.

2. Lithium metal is burned in air.

3. The hydrocarbon hexane (C6H14) is burned in excess oxygen.

4. Magnesium metal is strongly heated in oxygen gas.

What is the oxidation number of magnesium before the reaction occurs, and what is the oxidation number of magnesium after the reaction is complete?