AP Chemistry Summer Packet
Welcome to AP Chemistry! I’m so glad that you decided to take this course. This
class will be a great challenge for you, but will do wonders in helping to prepare
you for the rigors of college. AP Chemistry builds upon the concepts that were
covered in first year chemistry, and it is my expectation that you remember a
majority of that content. On day 1 of AP Chem, we will begin learning new
material, and in talking with my AP Chem students from this past school year,
they told me that they wished there had been a summer review so that they were
prepared when they entered class the first day. Thus, I have created this packet.
It is your first assignment for AP Chemistry and it is due at the beginning of the
first day of class. With the exception of polyatomic ions, ALL of it is review from
regular chemistry. I have posted the answer key to all of the worksheets on my
website, http://www.usd305.com/Page/9019 as well as including additional
websites, videos, and resources to help you should you need extra help or review
of the content. I realize that you could easily go online and just copy my answers,
but considering you have decided to take one of the most difficult classes offered
to high school students, I know you are the kind of student who wants to be
prepared for such a challenging course, and you will complete the work and use
the answers on my website to check your understanding.
Feel free to contact me if you have any questions via email
(nikki.chamberlain@usd305.com) and I will help explain problems.
Good luck and I’ll see you in a few months! Enjoy your summer break!
Mrs. Chamberlain
1|Page
Symbols
We will take a symbols quiz on the first day of class. Do you remember these
element symbols? It might be helpful to make flashcards or to try out these
online games.



http://education.jlab.org/elementflashcards/index.html
http://quizhub.com/quiz/f-elements.cfm
http://www.syvum.com/cgi/online/serve.cgi/squizzes/chem/periodic2.tdf
1. H
2. Li
3. Na
4. K
5. Rb
6. Cs
7. Fr
8. Be
9. Mg
10. Ca
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
Sr
Ba
Ra
Sc
Ti
Zr
V
Cr
Mo
W
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
Mn
Fe
Ru
Co
Ni
Pd
Pt
Cu
Zn
Cd
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
Hg
B
Al
Ga
C
Si
Ge
Sn
Pb
N
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
O
S
Se
F
Cl
Br
I
At
He
Ne
Sb
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
Ar
Kr
Xe
Rn
La
Ac
U
Pu
Ag
Au
P
2|Page
Polyatomic Ions & Acids
You will take a quiz over these polyatomic ions & acids the second day of class. You did not
have to memorize polyatomic ions in first year chemistry (they were on the back of your
Periodic Table), but in AP you will have to know them. Consider making flash cards.
acetate
acetic acid
ammonium
carbonate
carbonic acid
chlorate
chloric acid
chlorite
chromate
cyanide
dichromate
dihydrogen phosphate
hydrobromic acid
hydrogen carbonate (bicarbonate)
hydrogen sulfate (bisulfate)
hydrogen sulfide
hydrogen sulfite (bisulfite)
hydroiodic acid
hydronium
hydroxide
hypochlorite
iodate
nitrate
nitrite
nitric acid
nitrous acid
oxalate
perchlorate
perchloric acid
permaganate
peroxide
phosphate
phosphite
phosphoric acid
silicate
sulfate
sulfite
sulfuric acid
thiocyanate
3|Page
Significant Figures
Review of the rules:
1. All nonzero numbers are significant (123 has 3 sig figs)
2. Zeros between nonzero numbers are significant (102 has 3 sig figs)
3. Zeros in front of nonzero numbers are not significant (0.0000123 has 3 sig figs)
4. Zeros at the end of a number and to the right of a decimal are significant (1.000 has 4 sig
figs, 0.0002300 has 4 sig figs)
5. Zeros at the end of a number are not significant. If there is a decimal at the end, they are
(100 has 1 sig fig, but 100. Has 3)
6. When multiplying and dividing, your answer has as many sig figs as the number in the
problem with the fewest.
1. Indicate how many significant figures (sig figs) are in the following numbers:
a) 4,000,001
b) 4,000,000
c) 4,000,000.
d) 4.23 x 108
_____
_____
_____
_____
e) 0.000052
_____
f) 0.00005200 _____
g) 0 .000052001 _____
h) 1.280 x 10-5 _____
2. Write the following numbers in scientific notation so that they each have 3 significant figures:
a. 300
_______________________
b. 146,000 _______________________
c. 0.00120 _______________________
3. Round the following numbers so that they contain 3 significant figures.
a. 173,792
______________________
b. 0.0025021
______________________
c. 0.0003192
______________________
4. Solve the following. Use the appropriate sig figs in your answers:
a. 0.000030 x 0.00002 x 0.06 = _______________________
b. 0.276 x 13.76 x 0.0100 = ________________________
c. 1,234 x 3 = ________________________
d. 3.8890/7 = _______________________
e. 1,000/3.9876 = _______________________
4|Page
Chemical Nomenclature
Before you can name a compound or write a formula, you have to identify if it is ionic or
covalent. Ionic is made of metals and nonmetal OR cations (+) and anions (-). Covalent
compounds (molecular) are made of nonmetals only.
Review of Rules:
Type of
Rules for Naming
Compound
Ionic
1. Name the metal (cation)
 If it is a multivalent
element, use a roman
numeral to indicate
charge
2. Name the anion
 If the anion is a nonmetal
use an “ide” ending
 If the anion is a
polyatomic ion, just name
it
Covalent/
Molecular
Rules for Writing Formula
1. Write each ion with its charge
2. Add subscripts to balance the
charges (criss-cross the charges)
3. The overall charge on an ionic
compound should be ZERO!
4. Simplify the formula if possible
Examples:
NaCl = sodium chloride
NaNO3 = sodium nitrate
Fe2(CO3)3 = Iron (III) carbonate
1. Name each element and use the
appropriate prefix to tell how
many
 Omit mono on the
first element
2. Put an “ide” ending on the last
element
Examples:
Calcium chloride = Ca+2Cl-1 = CaCl2
Sodium sulfate = Na+1SO4-2 = Na2SO4
Copper (II) oxide = Cu+2O-2 = CuO
1. Use the prefixes to determine the
subscripts in the formula
2. Do NOT simplify molecular
formulas
Examples:
P4O10 = tetraphosphorus
decabromide
CO = carbon monoxide
Examples:
Dinitrogen pentachloride = N2Cl5
Trihydrogen hexabromine octaoxide
= H3Br6O8
Use the rules to write formulas and name the compounds on page 6.
5|Page
Write names:
1. CO2
2. Co(CN)3
3. OF2
4. Zn(OH)2
5. NiCO3
6. CuSO4
7. KMnO4
8. (NH4)3PO4
9. C7F9
10.Mg(C2H3O2)2
Write formulas:
11. Copper (II) sulfate
12.Tricarbon nonachloride
13. Ammonium oxalate
14. Iron (II) oxide
15. Silver sulfate
16. Lead (IV) chromate
17.Calcium carbonate
18. Carbon monoxide
19. Cesium phosphide
20. Sodium hydroxide
6|Page
Molar Conversions
#grams
1 mole
Mass in
Molar
Mass
Grams
PT
1 mole
6.022 X 1023 molecules
Moles 6.022 X 1023
Molecules
Or
Atoms
1. Convert to moles:
a. 32.9 g neon
1.63 moles
b. 6.4 x 10-4 kg aluminum phosphate
5.3 x 10-3
moles
c. 7.12 x 1023 molecules silicon tetrafluoride
1.18 moles
2. Convert to grams:
a. 3.46 moles lithium carbonate
255 g
3. Convert to molecules:
a. 6.72 moles sodium chloride
4.04 x 1024
molecules
7|Page
b. 16.2 kg diphosphorus pentoxide
6.87 x 1025
molecules
4. Convert to grams:
a. 1.06 x 1027 atoms copper
1.12 x 105 g
b. 7.39 x 1023 molecules tin (II) chromate
288 g
5. The density of liquid water is 0.997 g/mL at 25 degrees Celsius.
a. How many moles of water are in 250.0 mL of water?
b. Calculate the volume that would be occupied by 2.00 moles of liquid water at 25
degrees Celsius?
a. 13.85 mol
H2O
b. 36.1 mL
H2O
8|Page
Writing & Balancing Equations
Review of Reaction Types:
Type of Reaction
Relationship
Analogy
Synthesis
Dating
Decomposition
Break Up
Single
Cheating
Replacement
Double
Swapping
Replacement
Combustion
O2 Cute
General Equation
Example
A + X  AX
AX  A + X
AX + B  BX + A
AX + Y  AY + X
AX + BY  AY + BX
N2 + 3H2 2NH3
CaCO3  CaO + CO2
Mg + 2HCl  MgCl2 + H2
NaOH + AgCl  NaCl + AgOH
CxHy + O2  CO2 + H2O
CH4 +2 O2  CO2 + 2H2O
 Remember that decomposition reactions are difficult to predict. For a review of them, visit this
website http://quizlet.com/6084569/types-of-decomposition-reactions-flash-cards/ or access the
link on my website.
 Remember to write water, in a reaction, as H+1OH-1
1. sodium iodide + chlorine 
2. silver nitrate + potassium iodide 
3. rubidium + bromine 
4. sodium + water 
5. magnesium chlorate 
9|Page
6. silver nitrate + calcium 
7. carbon tetrahydride + oxygen 
8. bromine + calcium iodide 
9. nitric acid + zinc 
10. sulfuric acid + sodium chloride 
11. silver carbonate 
12. aluminum + sulfuric acid 
10 | P a g e
Stoichiometry
1. Sodium reacts with water to produce sodium hydroxide and hydrogen gas.
a. How many moles of sodium will react if 4 moles of hydrogen are produced? 8 moles Na
2. In a very violent reaction called a thermite reaction, aluminum metal reacts with iron (III) oxide to
form iron metal and aluminum oxide according to the following equation:
Fe2O3 + 2Al  2Fe + Al2O3
a. If 0.905 mole Al2O3 is produced in the reaction, what mass of Fe is produced? 101 g Fe
b. How many moles of Fe2O3 will react with 99.0 g of Al? 1.83 mole Fe2O3
11 | P a g e
3. Iron (III) chloride, FeCl3, can be made by the reaction of iron and chlorine gas. How much iron, in
grams, will be needed to completely react with 58.0 g of Cl2? 30.4 g Fe
4. Calculate the mass of silver bromide produced from 22.5 g of silver nitrate in the following reaction:
2AgNO3 + MgBr2  2AgBr + Mg(NO3)2
24.9 g AgBr
5. Iron (III) hydroxide decomposes to produce iron (III) oxide and water vapor. If 0.75 L of water vapor
is produced at STP, how many grams of iron (III) hydroxide were produced? 2.4 g Fe(OH)3
6. How many molecules of oxygen are produced by the decomposition of 6.54 g of potassium
chlorate? 4.82 x 1022 molecules O2
12 | P a g e