Name ____________________
2015 AP Chemistry Summer Assignment
This AP Chemistry packet covers chapters one through three of the Zumdahl Chemistry,
8th edition textbook. You have covered this material in your first year chemistry courses, so we
will wait until classes begin in the fall to distribute textbooks. This summer you will need to:
 Complete this packet and bring it with you the first day of class. There will be limited
instruction time reviewing this material. A test over this material may be scheduled as early
as the end of the first week of school.
 You must clearly show your work if your wish to receive full credit. Some answers are
furnished at the end of this packet to assist you. Final answers must include correct units.
 Additional material may be posted at http://www1.ccs.k12.in.us/chs/science .
 Online resources include:
o http://apchemistrynmsi.wikispaces.com/AP+Chemistry+Class+Lecture+Notes+AND
+instructional+videos
o http://www.khanacademy.org/#Chemistry
o http://www.chemmybear.com/stdycrds.html
 Please contact us if you have questions: vkundrat@ccs.k12.in.us or eshafer@ccs.k12.in.us
Assignment:
I.
Ions: Test your knowledge of ions by filling in the “Ion Formulas” pages of this packet
with no additional resources. Check and correct your work, noting the ones you need to
relearn. When finished, you can check the answers on the CHS website listed above.
II.
Formula Writing: Fill in the missing names or formulas for the compounds listed on the
“Formula Writing” page of this packet.
III.
Problems: Write the solutions to the attached problems on additional sheets of paper.
Number each problem clearly and circle your final answer. Show all of your work and
write thorough explanations.
I) Ions
Write the correct formulas with correct charges for the following ions using no additional
resources. When you are done, check and correct your work using an ion sheet or by
checking the answers on the CHS website listed above.
Name
Formula
Name
acetate
lead (II)
aluminum
lead (IV)
ammonium
lithium
arsenide
magnesium
barium
manganese (II)
beryllium
manganese (III)
bromate
mercury(I)
bromide
mercury(II)
bromite
nickel (II)
calcium
nickel (III)
carbonate
nitrate
1 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
Formula
Name
Formula
Name
cesium
nitride
chlorate
nitrite
chloride
oxide
chlorite
oxalate
chromate
potassium
chromium (II)
perbromate
chromium(III)
perchlorate
cobalt (II)
periodate
cobalt (III)
permanganate
copper(I)
peroxide
copper(II)
phosphate
cyanide
phosphide
dichromate
phosphite
dihydrogen phosphate
rubidium
fluoride
selenide
gallium
silicate
hydride
silver
hydrogen
sodium
*hydrogen carbonate
sulfate
*hydrogen phosphate
sulfide
*hydrogen sulfate
sulfite
*hydrogen sulfite
strontium
hydronium
tartrate
hydroxide
thiocyanate
hypobromite
thiosulfate
hypochlorite
tin (II)
hypoiodite
tin (IV)
iodide
zinc
Formula
iodate
iron (II)
* “Bi” may be substituted for “hydrogen”
in the ion names marked with *.
iron (III)
2 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
II) Formula Writing
Fill in the missing names or formulas for the following substances:
Name
Formula
Formula
barium sulfate
CuSO4
ammonium chloride
PCl3
chlorine monoxide
Li3N
silicon tetrachloride
BaSO3
magnesium fluoride
N2F4
sodium oxide
KClO4
sodium peroxide
NaH
copper (I) iodide
(NH4)2Cr2O7
zinc sulfide
HNO2
potassium carbonate
Sr3P2
hydrobromic acid
Mg(OH)2
perchloric acid
Al2S3
lead (II) acetate
AgBr
sodium permanganate
P4O10
lithium oxalate
HC2H3O2
potassium cyanide
CaI2
iron (III) hydroxide
MnO2
silicon dioxide
Li2O
nitrogen trifluoride
FeI3
chromium (III) oxide
Cu3PO4
calcium chlorate
PCl3
sodium thiocyanate
NaCN
cobalt (III) nitrate
Cs3N
nitrous acid
Zn(NO3)2
ammonium phosphate
N2O
potassium chromate
PCl3
3 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
Name
III) Problems: Chemical Foundations
1. a) There are 365 days per year, 24 hours per day, 12 months per year, and 60 minutes per
hour. Use these data to determine how many minutes are in a month.
b) Now use the following data to calculate the number of minutes in a month: 24 hours per day,
60 minutes per hour, 7 days per week, and 4 weeks per month.
c) Why are these answers different? Which (if any) is more correct? Why?
2. You go to a convenience store to buy candy and find the owner to be odd. He allows you to buy
pieces in multiples of 4 and to buy 4, you need $0.23. He only allows you to do this by using 3
pennies and 2 dimes. You have a bunch of pennies and dimes, and instead of counting them,
you decide to weigh them. You have 636.3 grams of pennies, and each penny weighs 3.03g.
Each dime weighs 2.29g. Each piece of candy weighs 10.23 g.
a) How many pennies do you have?
b) How many dimes do you need to buy as much candy as possible?
c) How much should all these dimes weigh?
d) How many pieces of candy could you buy?
e) How much would this candy weigh?
f) How many pieces of candy could you buy with twice as many dimes?
3. You have water in each graduated cylinder shown. You then add both
samples to a beaker.
a) How would you write the number describing the total volume?
b) What limits the precision of this number?
4. Why is it incorrect to say that the results of a measurement were accurate
but not precise?
5. Which of the following are exact numbers?
a) There are 12 eggs in a carton of one dozen.
b) One meter equals 1.094 yards
c) The announced attendance at a football game was 52,806.
d) π = 3.1415927.
6. How many significant figures are in each of the following?
a) 100 g.
e) 0.0048 L
2
b) 1.0x10 g.
f) 0.00480 L
3
c) 1.00x10 kg.
g) 4.80x10-3 m
d) 100. kg.
h) 4.800x10-3 m
7. Perform the following and express the results to the correct number of significant figures.
a) 6.022 x 1023 x 1.05 x 102
e) (1.00866 – 1.00728)
-34
9
b) 6.6262 x 10 x 2.998 x 10
6.02205 x 1023
2.54 x 10-9
f) 9.875 x 102 – 9.795 x 102 x 100 (100 is exact)
-2
-3
-1
c) 1.285 x 10 + 1.24 x 10 + 1.879 x 10
3
-2
-3
2
d) 1.285 x 10 - 1.24 x 10
g) 9.42 x 10 + 8.234 x 102 + 1.625 x 103 (3 is exact)
3
4 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
8. Perform the following unit conversions.
a) 8.43 cm to millimeters
b) 2.41 x 102 cm to meters
c) 294.5 mm to centimeters
d) 1.445 x 104 m to kilometers
e) 235.3 m to millimeters
f) 903.3 nm to micrometers
9. A chemist, trying to identify the main component of a compact disc cleaning fluid, determines
that 25.00 cm3 of the substance has a mass of 19.625 g at 20.0°C. Use the information in the
table below to identify the main component of the cleaning fluid. Justify your answer with a
calculation.
Compound
Density at 20°C (g/cm3)
Chloroform
1.492
Diethyl ether
0.714
Ethanol
0.789
Isopropyl alcohol
0.785
Toluene
0.867
10. The density of pure silver is 10.5 g/cm3 at 20°C. If 5.25 g of pure silver pellets is added to a
graduated cylinder containing 11.2 mL of water, to what volume level will the water in the
cylinder rise?
11. In each of the following pairs, which has the greater mass?
a) 1.0 kg of feathers or 1.0 kg of lead
b) 1.0 mL of mercury or 1.0 mL of water
c) 19.3 mL of water or 1.00 mL of gold
d) 75 mL of copper or 1.0 L of benzene
12. The density of osmium is 22.57 g/cm3. If a 1.00-kg rectangular block of osmium has two
dimensions of 4.00 cm x 4.00 cm, what is the third dimension of the block?
13. Match each description below with the following microscopic pictures. More than one picture
may fit each description. A picture may be used more than once or not used at all.
a) a gaseous compound
b) a mixture of two gaseous elements
c) a liquid element
d) a mixture of a gaseous element and a gaseous compound
14. Classify the following as physical or chemical changes.
a) Moth balls gradually vaporize in a closet.
b) Hydrofluoric acid attacks glass, and is used to etch calibration marks on glass laboratory
utensils
c) A French chef making a sauce with brandy is able to burn off the alcohol from the brandy,
leaving just the brandy flavoring.
d) Chemistry majors sometimes get holes in the cotton jeans they wear to lab because of acid
spills.
5 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
Atoms, Molecules, and Ions
15. The formula of water is H2O. Which of the following is indicated by this formula? Explain your
answer.
a) the mass of hydrogen is twice that of oxygen in each molecule.
b) there are two hydrogen atoms and one oxygen atom per water molecule.
c) the mass of oxygen is twice that of hydrogen in each molecule.
d) there are two oxygen atoms and one hydrogen atom per water molecule.
16. Dalton assumed that all atoms of the same element were identical in all their properties.
Explain why this assumption is not valid
17. Why do we call Ba(NO3)2 barium nitrate, but we call Fe(NO3)2 iron(II) nitrate?
18. The common name for NH3 is ammonia. What would be the systematic name for NH3?
19. Explain the law of conservation of mass, the law of definite proportion, and the law of multiple
proportions.
20. The following data were collected for several compounds of nitrogen and oxygen. Show how
these data illustrate the law of multiple proportions.
Compound A
Compound B
Compound C
Mass of Nitrogen that
combines with 1 g of Oxygen
1.7500 g
0.8750 g
0.4375 g
21. With some modifications, Dalton’s atomic theory holds up well regarding how we view
elements, compounds, and chemical reactions today. Answer the following questions
concerning Dalton’s atomic theory and the modifications made today.
a) The atom can be broken down into smaller parts. What are the smaller parts?
b) How are atoms of hydrogen identical to each other, and how can they be different from each
other?
c) How are atoms of hydrogen different from atoms of helium? How can H atoms be similar to
He atoms?
d) How is water different from hydrogen peroxide (H2O2) even though both compounds are
composed of only hydrogen and oxygen?
e) What happens in a chemical reaction, and why is mass conserved in a chemical reaction?
22. Distinguish between the following terms.
a) molecule versus ion
b) covalent bonding versus ionic bonding
c) molecule versus compound
d) anion versus cation
23. A sample of chloroform is found to contain 12.0 g of carbon, 106.4 g of chlorine, and 1.01 g of
hydrogen. If a second sample of chloroform is found to contain 30.0 g of carbon, what is the
total mass of chloroform in the second sample?
24. Label each of the following sets of elements as either noble gases, halogens, alkali metals,
alkaline earth metals, or transition metals.
a) Ti, Fe, Ag
b) Mg, Sr, Ba
c) Li, K, Rb
d) Ne, Kr, Xe
e) F, Br, I
6 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
25. Write the atomic symbol ( 𝐴𝑍X) for each of the isotopes described below.
a) number of protons = 27, number of neutrons = 31
b) the isotope of boron with mass number 10
c) Z = 12, A = 23
d) atomic number 53, number of neutrons = 79
e) Z = 9, number of neutrons = 10
f) number of protons = 29, mass number 65.
26. How many protons, neutrons, and electrons are in each of the following atoms or ions?
59 2+
59 3+
59
2+
a) 24
b) 24
c) 27
Co
d) 27
Co
e) 27
Co
12Mg
12Mg
f)
79
34Se
g)
79 2−
34Se
h)
63
28Ni
i)
59 2+
28Ni
27. Complete the following table:
Symbol
# of Protons
# of Neutrons
# of Electrons
26
33
85
125
86
13
14
10
76
54
Net Charge
53 2+
26Fe
3+
2−
28. For each of the following atomic numbers, use the periodic table to write the formula (including
the charge) for the simple ion that the element is most likely to form in ionic compounds.
a) 13
b) 34 c) 56 d) 7
e) 87 f) 35
29. Name each of the following compounds. Assume the acids are dissolved in water.
a) HC2H3O2
b) NH4NO2
c) Co2S3
d) ICl
e) Pb3(PO4)2 f) KClO3
g) H2SO4
h) Sr3N2
i) Al2(SO3)3 j) SnO2 k) Na2CrO4
l) HClO
Stoichiometry
30. An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with
mass 205.9745 u, 22.10% of an isotope with mass 206.9759 u, and 52.40% of an isotope with
mass 207.9766 u. Calculate the average atomic mass, and identify the element.
31. When a sample of natural copper is vaporized and injected into a mass spectrometer, the
results shown below are obtained. Use these data to calculate the average mass of natural
copper. (The mass values for 63Cu and 65Cu are 62.93 amu and 64.93 amu respectively.)
7 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
32. Dimethylnitrosamine, (CH3)2N2O, is a carcinogenic (cancer-causing) substance that may be
formed in foods, beverages, or gastric juices from the reaction of nitrite ion (used as a food
preservative) with other substances.
a) What is the molar mass of dimethylnitrosamine?
b) How many moles of (CH3)2N2O molecules are present in 250 mg dimethylnitrosamine?
c) What is the mass of 0.050 mole of dimethylnitrosamine?
d) How many atoms of hydrogen are in 1.0 mole of dimethylnitrosamine?
e) What is the mass of 1.0 x 106 molecules of dimethylnitrosamine?
f) What is the mass in grams of one molecule of dimethylnitrosamine?
33. Arrange the following substances in order of increasing mass percent of carbon.
a) caffeine, C8H10N4O2
b) sucrose, C12H22O11
c) ethanol, C2H5OH
34. Give the empirical formula for each of the compounds represented below.
35. The most common form of nylon (nylon-6) is 63.68% carbon, 12.38% nitrogen, 9.80%
hydrogen, and 14.14% oxygen. Calculate the empirical formula for nylon-6.
36. Maleic acid is a compound composed of 41.39% C, 3.47% H, and the rest oxygen. If 0.129
mole of maleic acid has a mass of 15.0 g, what are the empirical and molecular formulas?
37. Many homes in rural America are heated by propane gas, a compound that contains only
carbon and hydrogen. Complete combustion of a sample of propane produced 2.641g of carbon
dioxide and 1.442 g of water as the only products. Find the empirical formula of propane.
38. A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the
compound yields 16.01 mg CO2 and 4.37 mg H2O. The molar mass of the compound is 176.1
g/mol. What are the empirical and molecular formulas of the compound?
39. Examine the particle views and explain the differences between the two situations below with
regard to what is or is not reacting and total yield of ammonia. N2(g) + 3H2(g) → 2NH3(g)
8 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
40. Penicillin, the first of a number of antibiotics, was discovered accidentally by the Scottish
bacteriologist Alexander Fleming in 1928. He was never able to isolate it as a pure compound.
This and similar antibiotics have saved millions of lives that might have been lost to infections.
Penicillin F has the formula C14H20N2SO4. Calculate the mass percent of each element.
41. Give the balanced equation for each of the following chemical reactions:
a) Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon dioxide and water
vapor.
b) Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and
hydrogen sulfide gas.
c) Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid
ammonium thiocyanate (NH4SCN).
42. Balance each of the following chemical equations
a) KO2(s) + H2O(l) → KOH(aq) + O2(g) + H2O2(aq)
b) Fe2O3(s) + HNO3(aq) → Fe(NO3)3(aq) + H2O(l)
c) NH3(g) + O2(g) → NO(g) + H2O(g)
d) PCl5(l) + H2O(l) → H3PO4(aq) + HCl(g)
e) CaO(s) + C(s) → CaC2(s) + CO2(g)
f) MoS2(s) + O2(g) → MoO3(s) + SO2(g)
g) FeCO3(s) + H2CO3(aq) → Fe(HCO3)2(aq)
43. The reaction between potassium chlorate and red phosphorus takes place when you strike a
match on a matchbox. If you were to react 52.9 g of potassium chlorate (KClO3) with excess red
phosphorus, what mass of tetraphosphorus decaoxide (P4O10) could be produced?
KClO3(s) + P4(s) → P4O10(s) + KCl(s) (unbalanced)
44. Elixirs such as Alka-Seltzer use the reaction of sodium bicarbonate with citric acid in aqueous
solution to produce a fizz:
3NaHCO3(aq) + C6H8O7(aq) → 3CO2(g) + 3H2O(l) + Na3C6H5O7(aq)
a) What mass of C6H8O7 should be used for every 1.0 x 102 mg NaHCO3?
b) What mass of CO2(g) could be produced from such a mixture?
45. The space shuttle environmental control system handles excess CO2 (which the astronauts
breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets
to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle,
and each exhales 20. L of air per minute, how long could clean air be generated if there were
25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010
g/mL.
46. Ammonia is produced from the reaction of nitrogen and hydrogen according to the following
balanced equation: N2(g) + 3H2(g) → 2NH3(g)
a) What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10 3 g
N2 and 5.00 x 102 g H2?
b) What mass of which starting material would remain unreacted?
47. Consider the following unbalanced equation:
Ca3(PO4)2(s) + H2SO4(aq) → CaSO4(s) + H3PO4 (aq)
What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0
kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?
9 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.
48. Consider the following unbalanced reaction: P4(s) + F2(g) → PF3(g)
What mass of F2 is needed to produce 120. g of PF3 if the reaction has a 78.1% yield?
49. 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 g of chlorobenzene is reacted with 485 g of chloral.
a) What mass of DDT is formed, assuming 100% yield?
b) Which reactant is limiting? Which is in excess?
c) What mass of the excess reactant is left over?
d) If the actual yield of DDT is 200.0 g, what is the percent yield?
50. An ionic compound MX3 is prepared according to the following unbalanced chemical equation:
M + X2 → MX3
A 0.105-g sample of X2 contains 8.92 x 1020 molecules. The compound MX3 consists of 54.47%
X by mass. a) What are the identities of M and X, and what is the correct name for MX3?
b) Starting with 1.00 g each of M and X2, what mass of MX3 can be prepared?
10 | AP Chemistry Summer Assignment (Ch.1-3), Carmel H.S.