AP Chemistry
Summer Assignment
 Read the letter on the next page
 Email me tonight at christy.rich@acboe.net. Enter your
name and AP Chemistry in the subject line.
 Complete this packet and email me the answers no later than
7/27/15. Answers that cannot be emailed will be due the first
day of class.
 Email me or call me with questions. My number is 334-2022739.
Welcome to AP Chemistry!
I am happy that after taking one year of Chemistry, you have decided that it is a subject that you
would like to learn more about. This class will be challenging, but the biggest factor determining your
success will be the amount of effort you put into the class. If you do the homework assignments and
study, you can definitely be successful in this class and ultimately on the AP exam.
We have a lot of material to cover, so we will start off by making sure that we have all the basics
down. Over the summer, you are responsible for completing the review questions in this review
packet. All questions that can have the answers emailed are due no later than midnight on
7/27/15. The other questions will be due the first day of class. Please bring a copy of the
completed packet with work shown with you on the first day of school. This will be your first
grade! You will have a test on this material at the end of the first week. The material in this
packet should be mostly review from your first year of Chemistry. You will find that much of the AP
Chemistry curriculum consists of the same topics that you covered last year, but more in depth.
If you get stuck on a problem or a certain type of problem, try moving to the next part. These
problems cover a variety of topics, so you might be able to do the next part and then go back to the
previous ones later. There are also many helpful websites where you can find all kinds of chemistry
information and even help you might need. Working together in groups to tackle the more difficult
questions is also a viable option. In addition, please feel free to email me or call me at any point
during the summer if you have questions or concerns. Please remember getting help from resources
is acceptable and encouraged as long as you learn as you go. Simply copying someone else’s work
teaches you nothing and leaves you further behind than where you started.
I am really looking forward to this class, and I hope that you are also. Good luck and have fun with
that stoichiometry!
See you in August!!!
Mrs. Rich
P.S. If this seems like too much work for the summer, please drop this course. Advanced Placement
Chemistry is a college level course. You will need to be dedicated and work hard if you are to be
successful.
P.S.S. A copy of this Summer Packet is located on my school website.
Common Anions and Cations- (Memorize names, formulas, and charges!)
+1
Hydrogen
Lithium
Sodium
Potassium
ETC….
+2
Beryllium
Magnesium
Calcium
Strontium
ETC……
+3
Aluminum
Gallium
+4
Carbon
Silicon
-4
Carbide
Siliconide
-3
Nitride
Phosphide
-2
Oxide
Sulfide
Selenide
-1
Fluoride
Chloride
Bromide
Iodide
Hydride
Polyatomic Ions- (Memorize names, formulas, and charges!)
Name
ammonium
Hydronium
acetate
tartrate
citrate
perbromate
bromate
bromite
hypobromite
perchlorate
chlorate
chlorite
hypochlorite
periodate
iodate
iodite
hypoiodite
cyanide
cyanate
thiocyanate
hydrogen phosphate
dihydrogen phosphate (biphosphate)
hydrogen carbonate (bicarbonate)
hydrogen sulfide (bisulfide)
hydrogen sulfate (bisulfate)
hydrogen sulfite (bisulfite)
Symbol
NH4
H3O
C2H3O2 or (CH3COO)
C4H4O6
C6H5O7
BrO4
BrO3
BrO2
BrO
ClO4
ClO3
ClO2
ClO
IO4
IO3
IO2
IO
CN
CNO
SCN
HPO4
H2PO4
HCO3
HS
HSO4
HSO3
Charge
+1
+1
-1
-2
-3
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-2
-1
-1
-1
-1
-1
Name
hydroxide
azide
nitrate
nitrite
permanganate
carbonate
chromate (yellow)
dichromate (orange)
peroxide
oxalate
selenate
silicate
sulfate
sulfite
thiosulfate
persulfate
phosphate
phosphite
pyrophosphate
borate
tetraborate
arsenate
arsenite
ferricyanide
hexafluorosilicate
amide
Symbol
OH
N3
NO3
NO2
MnO4
CO3
CrO4
Cr2O7
O2
C2O4
SeO4
SiO3
SO4
SO3
S2O3
S2O8
PO4
PO3
P2O7
BO3
B 4O 7
AsO4
AsO3
Fe(CN)6
SiF6
NH2
Charge
-1
-1
-1
-1
-1
-2
-2
-2
-2
-2
-2
-2
-2
-2
-2
-2
-3
-3
-4
-3
-2
-3
-3
-3
-2
-1
Variable Valences for Metals- (Memorize names, formulas, and charges!))
Name
Chromium
Symbol
Cr
Manganese
Mn
Iron
Fe
Cobalt
Co
Copper
Cu
Lead
Pb
Antimony
Sb
Nickel
Ni
Charge
+2
+3
+2
+3
+2
+3
+2
+3
+1
+2
+1
+2
+4
+3
+5
+2
+3
+4
Stock Name
Chromium (II)
Chromium (III)
Manganese (II)
Manganese (III)
Iron (II) (green)
Iron (III) (yellow)
Cobalt (II)
Cobalt (III)
Copper (I) (blue)
Copper (II) (green)
Lead (I)
Lead (II)
Lead (IV)
Antimony (III)
Antimony (V)
Nickel (II) (green)
Nickel (III)
Nickel (IV)
Name
Mercury
Tin
Symbol
Hg2
Hg
Sn
Charge
+2
+2
+2
+4
+1
+3
+1
Stock Name
Mercury (I)
Mercury (II)
Tin (II)
Tin (IV)
Gold (I)
Gold (III)
Silver
Gold
Au
Silver
Ag
Bismuth
Bi
Zinc
Zn
+3
+5
+2
Bismuth (III)
Bismuth (V)
Zinc
Cadmium
Cd
+2
Cadmium
General Solubility Rules- (Memorize these!)
Rules for Assigning Oxidation
Numbers
1. All neutral pure elements have an oxidation of
0
2. All ions have an oxidation equal to their ionic
charge.
3. Hydrogen always has an oxidation number of
-1 unless it is paired with and another element
with a larger electronegativity. Then, it is +1.
4. Fluorine always has on oxidation number of -1.
5. Oxygen usually has an oxidation number of -2.
with Fluorine, it is +2
if in a peroxide, it is -1
6. Group A elements usually have an oxidation
equal to their normal ion charge.
7. The oxidation numbers of all atoms in
polyatomic Ion add up to be equal to the
charge of the polyatomic ion.
8. The oxidation numbers
of all atoms in a neutral
compound/ molecule
add up to be 0.
AP Chemistry Summer Review Worksheet
1. Identify the following changes as physical or chemical.
a. baking soda reacts with vinegar to produce carbon dioxide
b. the copper sheath on the Statue of Liberty turns green
c. Addition of salt melts the ice on the highway
d. Steam condenses on the windowpane
e. Epoxy resin cures and hardens
f. Sugar dissolves in a cup of coffee
g. Natural gas burns in a furnance
2. Identify each of the following as being most like an observation, a law, or a theory.
a. All coastal areas experience two high tides and two low tides each day.
b. The tides in Earth’s oceans are caused mainly by the gravitational attraction of the moon.
c. Yesterday, high tide in San Francisco Bay occurred at 2.43 a.m. and 3.07 p.m.
d. Tides are higher at the full moon and ne moon than at other times of the month.
3. Define the terms: exothermic and endothermic and give an example of each type of reaction.
4. How much heat is required to raise the temperature of 100 grams of water from 250C to 820C?
Density and Significant Figures
5. Round the following numbers to three significant figures.
a. 4325
b. 6.873 x 103
c. 0.17354
d. 4.9034
6. How many significant figures does each of the following numbers contain?
a. 0.0278 m
b. 1020 L
c. 1.300 cm
d. 0.00394 mol
7. The following length measurements were taken by students using several different measuring devices. Find
the average of the measurements. (Make sure your answer has the correct number of significant figures.) The
known length of the wire is 10.4768 cm. Are the measurements accurate? Why? Are the measurements
precise? Why?
8. The helium gas stored inside a large weather balloon weighs 13.558 grams. What is the volume of the balloon
if the density of helium is 0.1786 g/L?
9. 28.5 grams of iron shot is added to a graduated cylinder containing 45.5 mL of water. The water level rises to
the 49.1 mL mark. From this information, calculate the density of iron.
10. A cube of gold-colored metal with a volume of 59 cm3 and a mass of 980 g. The density of pure gold is 19.3
g/cm3. Is the metal pure gold? Show calculations to justify your answer.
11. Distinguish between potential energy and kinetic energy and give an example of each.
12. Rewrite the following numbers in proper scientific notation.
a. 0.000007345
b. 4,304,000,0.00230
Atomic Theory
13. What is the charge and location of the following subatomic particles?
a. Proton
b. Neutron c. Electron
14. What were the main points of Dalton’s Atomic Theory? Which of these points are still accepted today? Which
ones do we no longer accept? Why?
15. Who discovered protons? Neutrons? Electrons?
16. Summarize the evidence used by J.J. Thomson to argue that cathode rays consist of negatively charged
particles.
17. Define isotope.
18. The atomic number is always equal to the number of _______________ in an atom.
19. Let’s pretend you are holding two atoms of carbon that are isotopes. Describe what the two atoms have in
common and what they have different.
20. List the number of protons, neutrons, and electrons in carbon-13.
21. Determine the number of protons, neutrons, and electrons in each of the following.
a. 39K
b. 23Na+
c. 208Pb
d. 33P322. What is the frequency of ultraviolet light with a wavelength of 2.94 x 10-8 m?
23. What is the wavelength of a gamma ray electromagnetic radiation with a frequency of 2.73 x 1020 Hz?
24. What is the energy of a microwave photon that has a frequency of 1.12 x 1012 Hz?
25. What is the approximate energy of a photon having a frequency of 4.0 x 107 parsecs?
26. What is the frequency of light with a wavelength of 1.0 x 10-6 cm?
The Periodic Table
27. Strontium consists of four isotopes. Listed are its isotopes with masses and the percent abundance of each:
83.9134 amu ( 0.5%), 85.9094 amu (9.9%) , 86.9089 amu (7.0 %) , and 87.9056 amu (82.6 %). Calculate the
atomic mass of Sr ?
28. Nitrogen has two isotopes, N-14 and N-15, with atomic masses of 14.00031 amu and 15.001 amu,
respectively. What is the percent abundance of N-15?
29. Write the electron configuration of the following neutral elements.
a. Mg
b. Al
c. Ar
d. F
30. Make sure you know the names of the first 40 elements just by looking at their symbol. (This one cannot be
emailed.)
31. Rows are called? Columns are called?
32. Write the orbital notations for the following elements. (This one cannot be emailed.)
a. P
b. C
c. Na
d. Ne
33. Identify each of the following as nonmetals, metalloids, or metals.
a. Mg
b. O
c. Ca d. N
e. S
f. Cr
g. B
h. Au
i. Ga
34. Which groups on the periodic table are part of the main group elements?
35. Which of the elements are diatomic in nature?
36. Give the electron configuration for a neutral atom of beryllium.
37. Who is credited with creating the modern periodic table?
38. Identify the number of valence electrons each of the following contain.
a. Halogens
b. the Oxygen family
c. Alkali Metals
d. the Boron family
e. the inert gasses f. Alkaline Earth Metals
g. the Carbon family h. the nitrogen family
39. Define the following: Aufbau Principle, electron configuration, Pauli Exclusion Principle, Hund’s Rule, and
Heisenberg Uncertainty Principle
40. How many orbitals do each of the following contain?
a. s
b. p
c. d
d. f
41. Write the noble gas electron configurations for each of the following elements.
a. F
b. S
c. K
d. Br
42. Write the electron configurations for the following elements and their ions.
a. K and K+
b. P and P- c. O and O2d. Ca and Ca2+
43. Write the electron configurations for Cr and Cu. Explain why they are so different.
44. Write the dot notation that describes the following elements.
a. K+
b. Sr
c. N
d. Br
e. O245. Draw the Lewis structure according to VSEPR and name the following compounds. (This one cannot be
emailed.)
a. Cl4
b. C2Cl2
c. CH4 d. C2Cl4
e. NCl3
f. PBr3
g. ClF
h.
OF2
i. NH3
j. CCl4
k. O2
l. N2
46. Which groups are part of the s- block? p- block? d- block?
47. What orbital is filled when iodine gains an electron to become a negative ion?
48. Define the following and describe their trends.: Atomic radius, ionization energy, electron affinity, ionic
radius, and electronegativity
49. Name the elements that match the following descriptions.
a. Has 5 outer electrons on the third row of the periodic table
b. Has a 4s24p5 electron configuration
c. The noble gas on the fifth row
d. Group 6A element in the fourth period
50. Which group of elements has the highest electronegativity values on the periodic table?
51. Be familiar with nomenclature. It will be the first quiz of the year!!! (This one cannot be emailed.)
52. Write the formula of the following compounds.
a. Calcium sulfate.
b. Ammonium Phosphate
c. Lithium Nitrite
d. potassium perchlorate.
e. Barium Oxide
f. Zinc sulfide.
g. Sodium Perbromate
h. Calcium Iodide
i. Aluminum Carbonate
53. The hormone, thyroxine is secreted by the thyroid gland, and has the formula: C15H17NO4I4. How many
milligrams of Iodine can be extracted from 15.0 Grams of thyroxine?
54. Define Oxidation number.
55. Find the Oxidation number of each of the following.
a. Carbon in CO2.
b. Sulfur in H2SO4.
c. Phosphorus in PO43d. Manganese in MnO42-
Stoichiometry
56. Calculate the percentage by mass of each element in the following substances.
a. A. SO3
b. CH3COOCH3
c. Ammonium Nitrate
57. Calculate the molecular formulas of the following substances given their empirical formulas and molar
masses.
a. C2H5 and 58 g/mol
b. CH and 78 g/mol
c. HgCl and 236.1 g/mol
d. CH2 and 84 g/mol
e. NH2Cl and 51.5 g/mol
58. Determine the number of molecules present in a 4.56 mol sample of methane gas. How many hydrogen atoms
are present in the sample?
59. Determine the formula weight for each of the following.
a. N2O5
b. CuSO4
c. Ca(HCO3)2
d. CaSO4•2H2O
60. Calculate the mass in grams of each of the following.
a. 6.02 x 1023 atoms of Mg
b. 3.01 x 1023 formula units of CaCl2
c. 12.4 x 1015 molecules of CH2O
61. Mercury has an atomic mass of 200.59 amu. Calculate the:
a. Mass of 3.0 x 1010 atoms Hg
b. Number of atoms in exactly one gram of Hg.
62. The molecular formula of morphine, a pain-killing narcotic, is C17H19NO3.
a. What is its molar mass?
b. What fraction of atoms in morphine is accounted for by carbon?
c. Which element contributes the lease to the molar mass?
63. In an experiment, a student gently heated a hydrated copper compound to remove the water of hydration. The
following data was recorded:
a. Mass of crucible, cover, and contents before heating 23.4 g.
b. mass of empty crucible and cover
18.82 g.
c. mass of crucible, cover, and contents after heating to constant mass 20.94 g.
Calculate the experimental percent of water in the compound.
64. Name the7 types of general inorganic reactions with example of each?
65. Write the balanced chemical equations for the reaction of sodium with the following. (Don’t forget state!)
a. Nitrogen
b. Oxygen
c. Sulfur
d. Bromine
66. Write a balanced chemical equation for each of the following. (Don’t forget state!)
a. The reaction of magnesium oxide with iron to form iron (III) oxide and magnesium.
b. The decomposition of dinitrogen oxide gas to its elements.
c. The reaction of solid calcium carbide with water to form calcium hydroxide and acetylene gas, (C2H2).
d. The reaction of solid calcium cyanamide (CaCN2) with water to form calcium carbonate and ammonia
gas.
e. The burning of propane .
f. Nitrogen gas reacts with hydrogen to form ammonia.
g. Sodium reacts with iodine gas to form sodium iodide.
h. Sodium oxide reacts with water to form sodium hydroxide and hydrogen.
i. The synthesis of magnesium nitride from magnesium and nitrogen gas.
j. Concentrated hydrochloric acid reacts with concentrated sodium hydroxide to form sodium chloride
and water.
k. Carbon dioxide combines with water to form carbonic acid.
l. Mg(OH)2 + HNO3 →
67. Define limiting reagent, theoretical yield , and actual yield
68. Calculate the mass of O2 produced if 3.450 g potassium chlorate is completely decomposed by heating in
presence of a catalyst (Manganese Dioxide).
69. Chlorine and Fluorine react to form gaseous chlorine trifluoride. If you start with 1.75 mol of chlorine and
3.68 mol of fluorine. What is the limiting reactant? How much trifluoride is produced?
70. When benzene reacts with bromine, bromobenzene and bromic acid is obtained:
a. What is the theoretical yield of bromobenzene in this reaction when 30.0g of benzene reacts with 65.0
g of bromine?
b. If the actual yield of bromobenzene was 56.7 g what was the percentage yield?
Gas Laws
71. Convert:
a. 25˚C to K
b. 200 K to ˚C
c. 128 K to ˚C
72. A balloon filled with helium has a volume of 30.0 L at a pressure of 100 torr and a temperature of 15.0˚C.
What will the volume of the balloon be if the temperature is increased to 80.0˚C and the pressure remains
constant?
73. A gas has a volume of 590 mL at a temperature of -55.0˚C. What volume will the gas occupy at 30.0˚C?
74. A gas has a pressure of 710 mmHg at 227˚C. What will its pressure be at 27˚C, if the volume does not
change?
75. What is the pressure exerted by 32 g of O2 in a 22.0 L container at 30.0˚C?
76. A mixture of gasses at a total pressure of 95 torr contains N2, CO2, and O2. The partial pressure of CO2 is 24
torr and the partial pressure of N2 is 48 torr. What is the partial pressure of the O2?
77. A nitrogen sample at 30˚C has a volume of 1.75 L. If the pressure and the amount of gas remain unchanged,
determine the volume when the Celsius temperature is doubled.
78. On a warm day, an amusement park balloon is filled with 47.8 g He. The temperature is 33˚C and the pressure
inside the balloon is 2.25 atm. Calculate the volume of the balloon.
79. Convert 6.75 atm to:
a. torr
b. kilopascals
c. mm of Hg
Molarity
80. Calculate the molarity of a solution that contains 0.0345 mol NH4Cl in 400. mL of solution.
81. Calculate the molarity of a solution that contains 20.0 g of sodium hydroxide in 200. mL of solution.
82. How many grams of solute are present in 50.0 ml of 0.360 M sodium chloride?
Acid/ Base
83. Name and write the formulas for 7 strong acids.
84. Name and write the formula for all the strong bases.
85. Use (A) to indicate an acid only, (B) to indicate a base only, and (C) to indicate both.
a. Is a good conductor
b. Has a pH of 3 _____
c. Feels slippery _____
d. Tastes sour _____
e. Tastes bitter _____
f. Produced when sodium reacts with water _____
g. Reacts with zinc to produce hydrogen _____
h. Reacts with carbonates to produce CO2 _____
86. Acids tend to __________________ H+ ions.
87. Bases tend to __________________ H+ ions.
88. Acids tend to have a pH ______________ 7.
89. Bases tend to have a pH ______________ 7.
90. Water generally has a pH of __________.
91. Complete the following chart:
pH
pOH
[H3O+] / [H+] in molarity
6.1 x 10-8 M
2.5 x 10-10 M
1.0
[OH-] in molarity
1.4 x 10-3M
12.3
1.0 M
3.2
1.93 x 10-13 M
7.41
Acid or Base