AP Chemistry Summer Assignment 2012
Mrs. Higgins
higginsk@fultonschools.org
Welcome to AP Chemistry! You already have a background in chemistry from your general
chemistry class, but AP Chemistry is very different. Rather than memorizing how to do
particular types of problems, you must really understand the chemistry and be able to apply it to
different kinds of problems. AP Chemistry is a difficult course. To succeed you must keep up
with the assignments and be willing to spend time working through the material. The College
Board recommends that students spend one hour outside of class studying and practicing for
every hour in class. I think this is an underestimation of what is necessary to be successful.
Like most AP classes, AP Chem comes with a summer assignment. It is due the third day of
school and will count as your first quiz grade. We will have a test over the summer assignment
on the first Friday of the school year. I check my email frequently, so feel free to contact me if
you are having problems doing the summer assignment.
The summer assignment is a review of your first year chemistry course. It covers chapters 1-4 of
the textbook. You should read the chapters and do the corresponding problems/questions. In
addition to your textbook, there are many good online tutorials and websites that you can use to
help you with the assignment. It is very important that you complete this assignment by
yourself. If you just copy the work of another student, it is doubtful you will understand the
concepts well enough to pass the test! Start early on the summer assignment. It may take
longer to learn/relearn this material than you think!
You must pick up your textbook from Mrs. Price in room 3208 before next Thursday. Don’t lose
it as it will be your book for all of next year – and it is expensive.
I hope you will enjoy your AP Chemistry class. Be ready for an academic challenge. I know
you will learn a lot in AP Chemistry and it will be an excellent way for you to prepare for
college, as it will enhance work-habits, organizational skills and your ability to learn
independently and think creatively.
Have a great summer. See you in August!
Mrs. Higgins
You may write your answers on these pages or use notebook paper.
Chapter One
1. Write the following measurements in scientific notation.
A. 369 g
_______________________
B. 540,000 mL (3 sig figs) _______________________
C. 0.4560 mi
_______________________
D. 0.000000060
_______________________
2. Express the following as whole numbers or decimals.
A. 2.85 x 10-3
______________________
8
B. 1.5 x 10
______________________
C. 4.00 x 10-2
______________________
3. How many significant figures are there in each of the following values?
A. 0.01359456
____________
B. 12.0000
____________
C. 133.45
____________
D. 120.3
____________
E. 2200
____________
F. 0.0040
____________
G. 45.006
____________
4. Perform the indicated calculations on the following measured values. Give the answer with
the correct number of significant figures and units.
A. 16.81 m + 3.226 m = ___________________
B. 326.8 N x 4.4 m2 = ______________________
C. 7.442 s – 7.52 s = ______________________
D. 91 g ÷ 1.86 cm3 = _______________________
5. Using conversion factors, convert 4.1 liters to:
A. kiloliters
____________________
B. milliliters
____________________
C. microliters
____________________
D. cubic centimeters ____________________
6. A velocity is 9.21 x 104 cm per minute. Use unit analysis (dimensional analysis) to calculate
the velocity in meters per second.
7. A team of students determined the density of a sample of wood to be 0.62 grams per
centimeter3. A handbook of tree physiology reported the density to be 0.631 for the same
type of wood. What is the percent error of the student’s value?
8. A leaky faucet drips at a rate of 1 drop/s. If one drop of water is 0.1 mL, how many gallons
of water will be wasted in one day?
9. An aluminum bar is 5.0 cm x 4.0 cm x 10.4 mm and has a mass of 54.000 g. Find the density
of the bar in lb/ft3.
10. What is the diameter, in Angstroms, of an atom of element X, if4.82 x 1025 atoms laid side by
side is 1.8000 inches in length?
11. A. Compare and contrast the Kelvin scale and the Celsius scale.
B. Convert 450. Kelvin to Celsius
C. Convert 200. Celsius to Kelvin
D. Convert -230 Celsius to Kelvin
In addition to the above items from Chapter 1, be sure you know



The difference between accuracy and precision
How to determine the uncertainty of a measurement
Metric prefixes (mega, kilo, hector, deka, deci, centi, milli, micro, nano, pico)
Chapter Two
12. How many protons, neutrons and electrons are in each of the following ions?
A. Fe3+ (mass # 56) ____p____n____e
B. Ca2+ (mass # 40) ____p____n____e
C. F- (mass # 19) ____p____n____e
D. P3- (mass# 31) ____p____n____e
E. I- (mass # 127) ____p____n____e
13. Name the family or group of the Periodic Table to which each of the following elements
belong:
A. Ar ________________________
B. Sr _________________________
C. Fe _________________________
D. Cl _________________________
E. Nd ________________________
F. Rb _________________________
14. Name each of the following compounds:
A. PbI2
__________________________________________
B. NH4Cl
__________________________________________
C. Fe2O3
__________________________________________
D. LiH
__________________________________________
E. CsCl
__________________________________________
F. NaH
__________________________________________
G. Cr(OH)3 __________________________________________
H. NaC2H3O2 __________________________________________
I. K2Cr2O7 __________________________________________
J. Na2SO4 ___________________________________________
K. KH2PO4 ___________________________________________
15. Name each of the following compounds:
A. NI3
__________________________________________
B. PCl5
__________________________________________
C. CO
__________________________________________
D. P4O10
__________________________________________
E. N2O4
__________________________________________
F. NH3
__________________________________________
16. Write formulas for each of the following compounds:
A. iron (III) oxide ____________________________________
B. hydrogen iodide ____________________________________
C. tin (II) fluoride) ____________________________________
D. calcium phosphate ___________________________________
E. lead (II) nitrate ____________________________________
F. sodium cyanide ____________________________________
G. sodium hydrogen sulfate ______________________________
H. sodium bromate ____________________________________
17. Write formulas for each of the following compounds:
A. rubidium nitrate ________________________________________
B. sodium iodate ________________________________________
C. dinitrogen tetroxide ______________________________________
D. tin (IV) oxide
________________________________________
E. potassium carbonate ______________________________________
F. iron (III) chloride ________________________________________
G. sulfurous acid ___________________________________________
H. magnesium hydroxide ____________________________________
I. carbon tetrachloride ______________________________________
J. potassium hydrogen phosphate ______________________________
K. potassium permanganate ___________________________________
L. potassium chlorate ________________________________________
M. hypoiodous acid __________________________________________
N. ammonium acetate ________________________________________
O. hydroiodic acid __________________________________________
18. Give the names of the following acids:
A. H2SO3 _____________________________________________
B. HI ________________________________________________
C. HBr _______________________________________________
D. HNO2______________________________________________
E. H3PO4 _____________________________________________
F. HCl _______________________________________________
19. Give formulas for the following acids:
A. hydrocyanic acid ____________________________________
B. hydrofluoric acid ____________________________________
C. acetic acid _________________________________________
D. sulfuric acid ________________________________________
E. nitric acid __________________________________________
F. hydrosulfuric acid ___________________________________
20. Give the names of the seven diatomic elements.
21. Define the word isotope.
22. What does the law of definite composition say?
23. What does the law of multiple proportions say?
In addition to the above items from Chapter 2, be sure you read about and understand
the following:
 Dalton’s Atomic Theory
 Thomson’s cathode ray tube experiment
 Rutherford’s gold foil experiment
 The difference between a molecule and an ion
Chapter Three
24. An element, E, has only two naturally occurring isotopes. E-10 has a mass of 10.01 amu and
a natural abundance of 19.78%. E-11 has a mass of 11.01 amu and a natural abundance of
80.22%. What is the average atomic mass of E?
25. Chlorine has two stable isotopes. The mass of one isotope is 34.97 amu. Its relative
abundance is 75.53%. What is the mass of the other stable isotope?
26. How many atoms are in 2.4 moles of neon gas? How many grams?
27. How many grams of zinc are in 1.16 x 1022 atoms of zinc?
28. How many mg of Br2 are 4.6 x 1020 molecules of bromine?
29. How many grams are there in 0.36 moles of cobalt (III) acetate , Co(C2H3O2)3? How many
grams of cobalt are in the sample? How many atoms of cobalt?
30. Calculate the mass percent of chlorine in each of the following compounds:
A. ClF
B. CuCl2
31. Chlorophyll a is essential for photosynthesis. It contains 2.72% magnesium by mass. What
is the molar mass of chlorophyll a assuming there is one atom of magnesium in every
molecule of chlorophyll a?
32. Which of the following formulas can be empirical? Circle them.
A. CH4
F. NH4Cl
B. CH2
G. Sb2S3
C. KMnO4
H. N2O
D. N2O5
I. CH2O
E. B2H8
33. A compound is found to contain 49.67 % carbon, 48.92 % chlorine, and 1.39 % hydrogen.
The molar mass of the compound is 289.9 g/mole. Determine the empirical and molecular
formulas of the compound.
34. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide.
A. Write a balanced chemical equation for this reaction.
B. How many grams of calcium oxide will be produced after 12.25 grams of calcium
carbonate are completely decomposed?
C. What is the volume of carbon dioxide gas produced when the 12.25 grams of
calcium carbonate completely decompose at STP?
35. When ammonia gas, oxygen gas and methane (CH4) gas are combined, the products are
hydrogen cyanide gas and water.
A. Write a balanced chemical equation for the reaction.
B. Calculate the mass of each product produced when 225 grams of oxygen gas is
reacted with an excess of the other two reactants.
C. If the actual yield of the experiment in (B) is 105 grams of HCN, calculate the
percent yield.
36. DDT, an insecticide harmful to fish, birds and humans, is produced by the following
reaction:
2C6H5Cl
+
C2HOCl3  C14H9Cl5 + H2O
chlorobenzene
chloral
DDT
In a government lab, 1142 grams of chlorobenzene is reacted with 485 grams of chloral.
A. What mass of DDT is formed?
B. Which reactant is limiting? Which is excess?
C. What mass of the excess reactant is left over?
D. If the actual yield of DDT is 200.0 grams, what is the percent yield?
Chapter Four (Sections 1-3 only)
37. Differentiate between what happens when the following are dissolved in water.
A. Polar solute versus nonpolar solute
B. KF versus C6H12O6
C. RbCl versus AgCl
38. Write a reaction to show how solid calcium chloride breaks apart when dissolved in water.
39. What is molarity?
40. Calculate the molarity of the solution made by dissolving 5.263 grams of NaHCO3 in enough
water to make 250.0 mL of solution.
41. A solution of ethanol (C2H5OH) in water is prepared be dissolving 75.0 mL of ethanol
(density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity
of the solution?
42. Which of the following solutions of strong electrolytes contains the largest number of moles
of chloride ions?
A. 100.0 mL of 0.30 M AlCl3
B. 50.0 mL of 0.60 M MgCl2
C. 200.0 mL of 0.40 M NaCl
43. How would you prepare 2.00 L of 0.250 M NaOH
A. from a 1.00 M stock solution?
B. from solid NaOH?
In addition to the above, know the following:
 the difference between an electrolyte and a nonelectrolyte
 the difference between a strong electrolyte and a weak electrolyte
 three strong acids and three strong bases
 one weak acid and one weak base
Know your solubility rules! They are not easy to memorize, but you have to do it!!!!!! You
can find some helpful hints for memorizing them online. There are also flashcards online
that you might find useful. You do need to know these for the first test. 
Solubility Rules:
1. All compounds containing the alkali metal cations and the ammonium ion are soluble.
2. All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.
3. All chlorides, bromides and iodides are soluble except those containing Ag+, Pb2+ or Hg22+
4. All sulfates are soluble except those containing, Hg22+, Pb2+, Sr22+, Ca2+, or Ba2+.
5. All hydroxides are insoluble except compounds of the alkaline earth metals, Sr22+, Ca2+, and
Ba2+.
6. All compounds containing PO43-, S2-, CO32-, and SO32- are insoluble except those that also
contain alkali metals or NH4+.
You also need to know the following polyatomic ions. You need to know the name, formula
and charge of each. You do need to know these for the first test. 