AP Chemistry Summer Assignment
Due Date: Thursday, September 1st, 2011
Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number
of significant figures.
Part I: Chemical Formulas
Write the chemical formulas for each of the
following substances.
Write the name of each of the following compounds.
1. Barium sulfate
__________
1. CuSO4
______________________________
2. Ammonium chloride
__________
2. PCl3
______________________________
3. Chlorine monoxide
__________
3. Li3N
______________________________
4. Silicon tetrachloride
__________
4. BaSO3
______________________________
5. Sodium oxide
__________
5. KClO4
______________________________
6. Sodium peroxide
__________
6. NaH
______________________________
7. Copper (I) iodide
__________
7. (NH4)2Cr2O7 ______________________________
8. Zinc sulfide
__________
8. HNO2
______________________________
9. Potassium carbonate
__________
9. Sr3P2
______________________________
10. Hydrobromic acid
__________
10. Mg(OH)2
______________________________
11. Perchloric acid
__________
11. Al2S3
______________________________
12. Lead (II) acetate
__________
12. H2O2
______________________________
13. Sodium permanganate
__________
13. AgBr
______________________________
14. Lithium oxalate
__________
14. P4O10
______________________________
15. Potassium cyanide
__________
15. CH3COOH ______________________________
16. Copper (II) chloride dihydrate
__________
16. CaI2
______________________________
17. Silicon dioxide
__________
17. MnO2
______________________________
18. Pentanitrogen nonafluoride
__________
18. Li2O
______________________________
19. Calcium chlorate
__________
19. FeI3
______________________________
20. Sodium thiocyanate
__________
20. Cu3PO4
______________________________
21. Cobalt (III) nitrate
__________
21. MgSO4
______________________________
22. Nitrous acid
__________
22. NaCN
______________________________
23. Ammonium phosphate
__________
23. Zn(NO3)2
______________________________
24. Hypochloric acid
__________
24. HF
______________________________
25. Potassium chromate
__________
25. HClO2
______________________________
1|P ag e
Part II: Chemical Equations
For each equation below, identify the type of chemical reaction (synthesis, decomposition, single replacement,
double replacement, or combustion), predict the products and write the balanced equation.
1. Ammonium sulfate reacts with barium nitrate.
Reaction Type: _____________________
2. Zinc metal is added to a solution of copper (II) chloride.
Reaction Type: _____________________
3. Propane gas (C3H8) is burned in excess oxygen.
Reaction Type: _____________________
4. Solid calcium chlorate is heated strongly.
Reaction Type: _____________________
5. Magnesium and nitrogen gas are heated together.
Reaction Type: _____________________
6. Chlorine gas is bubbled through a solution of sodium bromide.
Reaction Type: _____________________
7. Solutions of lead nitrate and calcium iodide are combined.
Reaction Type: _____________________
8. Sulfuric acid is combined with sodium hydroxide.
Reaction Type: _____________________
9. Isopropyl alcohol (C3H7OH) is burned in oxygen.
Reaction Type: _____________________
10. Iron metal shavings are added to hydrochloric acid.
Reaction Type: _____________________
11. Solid sodium carbonate is heated in a crucible.
Reaction Type: _____________________
12. Sodium metal is added to distilled water.
Reaction Type: _____________________
2|P ag e
Part III: Stoichiometry
1. Find the mass percent of nitrogen in each of the following compounds.
a. NO
b. NO2
c. N2O4
d. N2O
2. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the
compound to be 7.74% hydrogen by mass. Find the empirical and molecular formulas of benzene.
3. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of calcium oxide will be produced after 12.25 g of calcium carbonate is completely
decomposed?
c. What volume of carbon dioxide gas is produced from this amount of calcium carbonate at STP?
3|P ag e
4. Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write a balanced chemical equation for this reaction.
b. 3.20 g of hydrogen gas and 9.50 g of bromine gas react. Which is the limiting reagent?
c. How many grams of hydrogen bromide gas can be produced using the amounts in (b)?
d. How many grams of the excess reactant is left unreacted?
e. What volume of HBr, measured at STP, is produced in (b)?
5. When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen
cyanide gas and water.
a. Write a balanced chemical equation for this reaction.
b. Calculate the mass of each product produced when 225 g of oxygen gas is reacted with an excess
of the other two reactants.
4|P ag e
c. If the actual yield of the experiment in (b) is 105 g of HCN, calculate the percent yield.
6. When solutions of potassium iodide and lead (II) nitrate are combined, the products are potassium
nitrate and lead (II) iodide.
a. Write a balanced equation for this reaction, including (aq) and (s).
b. Calculate the mass of precipitate produced when 50.0mL of 0.45M potassium iodide solution and
75mL of 0.55M lead (II) nitrate solution are mixed.
c. Calculate the volume of 0.50M potassium iodide required to react completely with 50.0mL of
0.50M lead (II) nitrate.
Part IV: Structure of Matter
Describe how you would separate and recover into four separate containers the following four components of a
mixture: liquid water (H2O (l)) + iron filings (Fe (s)) + sodium chloride dissolved in water (NaCl (aq)) + beach sand
grains (SiO2 (s)).
Part V: E-mail
E-mail me at [email protected] with the e-mail address you prefer me to contact you at throughout the
year. Include the name of the AP Chemistry review book you have purchased to use throughout the year.
5|P ag e