1. AP Chemistry Summer Assignment
2012 – 2013 School Year
Ms. Megonigal J204
megonigale@calvertnet.k12.md.us
Primary Textbook: Chemistry, 6th Edition, Author: S. Zumdahl
Secondary Textbook (to purchase): Cracking the AP Chemistry Exam (The Princeton Review)
Part 1: (20 problems total)
Read Chapter 1 in the textbook and take notes as you read.* Be sure to look at the pictures,
graphs, tables and figures as you read. Complete the following problems at the end of the
chapter: 16, 19, 20, 21, 23, 25, 26, 28, 29, 30, 32, 33, 48, 50, 57, 58, 59, 66, 67 and 70.
You must show all work for math related problems.
Part 2 (22 problems total)
Read Chapter 2 in the textbook and take notes as you read. Be sure to look at the pictures,
graphs, tables and figures as you read. Complete the following problems at the end of the
chapter: 6, 12, 13, 19, 20, 21, 24, 37, 38, 44, 46, 50, 51, 57, 58, 60, 61, 64, 66, 68, 70 and 72.
You must show all work for math related problems.
Part 3
Memorize the following common monatomic ions and polyatomic ions:
Table 2.3 on pg. 62
Table 2.4 on pg. 63
Table 2.5 on pg. 67
This will make the course easier for you as we learn new concepts throughout the year. I
suggest making flashcards as a study aid. You will be tested on these the first week back.
Part 4 (30 problems total)
Read Chapter 3 in the textbook and take notes as you read. Be sure to look at the pictures,
graphs, tables and figures as you read. Complete the following problems at the end of the
chapter: 9, 12, 15, 18, 22, 23, 25, 28, 29 and 30 (10 problems)
In addition, complete the attached multiple choice problems (20 problems).
You must show all work for problems!!
*It is extremely important to read the textbook as opposed to simply skimming it. When
example problems are given, take the time to analyze them; do not just skip over them!
Be prepared to turn in all work (chapter notes and problems) in a spiral notebook on the
first day of school. Make sure your work is neat, legible and clearly labeled in the same order
as listed above.
Be prepared for a test on the material in Chapters 1 – 3 at the end of the first week of school
and several graded assignments the first week as well.
All questions in blue have the answers in the back of the textbook. Do NOT be tempted to
simply copy the answers, as it will do you no good. I specifically chose these questions so you
can check yourself periodically to make sure you are doing the problem/questions correctly.

2. Name_____________________________________________________________________________________
AP Chemistry Summer Assignment 2011 – 2012 School Year
Part 4 Assignment continued
Multiple Choice Questions
You MUST show all work for any problems involving math!
1. Which one of the following elements has been selected as the current atomic weight standard?
a. O
b. C
c. H
d. Na
2. Bromine is composed of two isotopes. One of the isotopes, Br-X, makes up 49.7% of the total
while the other, Br-78.9 makes up 50.3% of the total. Calculate the atomic mass of Br-X
a. 80.0
b. 80.9
c. 89.7
d. 78.9
3. Four beakers containing potassium nitrate dissolved in water are allowed to evaporate to
dryness. Beakers 1 through 4 contain 2.3, 1.91, 5.985, and 0.52 g of dry potassium nitrate.
How many moles of potassium nitrate were recovered after the water evaporated?
a. 0.106 moles
b. 0.212 moles
c. 0.500 moles
d. 2.35 moles
4. How many atoms of uranium (U) are present in 1 nanogram of uranium?
a. 2.5 x 1020
b. 5.0 x 1010
c. 2.5 x 1012
d. 5.0 x 1031
5. Calculate the percent composition of hydrogen in sucrose (C12H22O11).
a. 6%
b. 10%
c. 33%
d. 20%
6. Two of the three forms of vitamin B6 are pyridoxine (C8H11NO2) and pyridoxamine
(C8H12N2O2). Calculate the respective percentage of nitrogen in each compound.
a. 8.8%, 17%
b. 9.3%, 18%
c. 9.2%, 17%
d. 18%, 9.2%
7. Determine the molecular formula of a compound that contains 26.7% P, 12.1% N, 61.2% Cl,
and a molecular weight of 580 g/mol.
a. (PNCl)3
b. (PNCl2)5
c. (P2NCl2)5
d. (PNCl2)

3. 8. Calculate the empirical formula for a compound that contains 32.2% Ca and 67.8% N by mass.
a. Ca(N3)2
b. CaN2
c. CaN
d. CaN4
9. Find the empirical formula of the compound that contains 15.8% Al, 28.1% S and 56.1% O.
a. Al2(SO4)3
b. AlSO2
c. AlSO
d. Al2SO3
10. 505 grams of KOH are required to completely react with 4.50 moles of sulfuric acid. How many
moles of K2SO4 are produced? (make sure to correctly predict products)
11. What are the coefficients necessary to balance the following equations?
b. __C3H8 + ___F2  ___C3F8 + ___HF
12. For every liter of sea water that evaporates, 3.7 g of magnesium hydroxide are produced. How
many liters of sea water must evaporate to produce 5.00 moles of magnesium hydroxide?
13. A solution of copper sulfate is treated with zinc metal. How many grams of copper are
produced if 2.9 g of zinc are consumed?
CuSO4 + Zn  ZnSO4 + Cu
a. 2.9 g
b. 2.8 g
c. 5.7 g
d. 3.7 g
14. How many grams of carbon dioxide are produced from the burning of 1368 g of sucrose
according to the following equation?
C12H22O11 + 12O2  12CO2 + 11H2O
a. 342 g
b. 176 g
c. 1056 g
d. 2112 g
15. How many grams of sulfur dioxide are produced when 90.0 g of thionyl chloride reacts with
excess water according to the following equation?
SOCl2 + H2O  2HCl + SO2
a. 96.8 g
b. 90.0 g
c. 24.2 g
d. 48.4 g

4. 16. Calcium oxide is a basic oxide that is not very soluble in water. Calcium oxide can react with
carbon dioxide to form calcium carbonate (according to the equation below). Calcium
carbonate is an insoluble salt that forms stalactites and stalagmites. How many moles of
carbon dioxide are removed from water if a 400.0 lb stalagmite is formed?
CaO + CO2  CaCO3
a. 1816
b. 908
c. 4000
d. 2258
17. Calculate the number of grams of TiOCl2 required to react with 134 g of carbon.
___TiOCl2 + ___C  ___Ti + ___CO2 + ___CCl4
18. Calculate the number of grams of methane (CH4) required to react with 25.0 g of chlorine
according to the following equation:
___CH4 + ___Cl2  ___CH3Cl + ___CH2Cl2 + ___HCl
19. Identify the limiting reactant and calculate the number of grams left over in excess for the
following equation:
___Cr2O3 + ___CCl4  ___CrCl3 + ___COCl2
The reaction began with 5.00 g of Cr2O3 and 12.0 g of CCl4.
a. Limiting: CCl4, 1.05 g Cr2O3 left over
b. Limiting: Cr2O3, 10.0 g CCl4 left over
c. Limiting: CCl4, 3.70 g Cr2O3 left over
d. Limiting: Cr2O3, 6.75 g CCl4 left over
20. Identify the limiting reactant and the number of grams left over in excess if 1.9 grams of
phosgene and 1.9 grams of sodium hydroxide are combined in the following reaction:
COCl2 + 2NaOH  2NaCl + H2O + CO2
a. Limiting: COCl2, 0.588 g NaOH left over
b. Limiting: COCl2, 0.4 g NaOH left over
c. Limiting: NaOH, 0.520 g COCl2 left over
d. Limiting: NaOH, 0.355 g COCl2 left over