Welcome to AP Chemistry!
I hope you are ready for a fun, yet challenging year. You already have a solid
background in basic chemistry from your first year Chem class, and this is critical to
success in AP Chem. As the year progresses and you develop your skills for making
connections and problem solving as we delve into great depth of the study of matter
and the changes it undergoes, you will really begin to understand why chemistry is
called the central science, and you will be able to apply your learning to all sorts of
different situations. Students who finish AP Chemistry come out with a much better
understanding of the world around them. They also come out with a sense of great
accomplishment. AP Chemistry is a difficult class, but with determination and
perseverance, you will surely succeed!
1. Purchase your own copy of 5 Steps to a 5 on the AP: Chemistry, John T
Moore, McGraw Hill. (You can purchase them at Amazon.com Online, probably
the more recent the publication the most current information however any
version will work.)
2. Buy a few color highlighters.
3. Read and study thru the chapter titled ‘How to Approach Each Question Type’.
Highlight material that applies to you. These sections give advice on what to
expect and how to study.
4. Take the Diagnostic test. (Go ahead and write in the book, I will
make an additional copy of this test for you to take before the AP Exam.)
5. Take a look at the AP and other websites given in this summer packet. List the
three most useful in the front cover of your book.
6. Read and study (highlight, take notes in the margin, etc) and do all the review
questions at the end of the chapter for these two sections (Chapters vary
based on publication year of your 5 Steps to a 5).
 Basics
 Stoichiometry
AP Chemistry is a difficult course. It is not all about memorization; however,
having these items memorized is essential for success in learning the concepts
covered in the course. Make flashcards, have your friends and family quiz you,
take the lists with you on vacation, or do whatever it takes to get this
information firmly planted in your head. Do not wait until the night before
school begins.
To give yourself a jump start in the course I recommend seven areas of
memorization before the first day of class:
1. Diatomic molecules (7)
2. Polyatomic Ions (including name, symbol and charge)
3. Variable Valences for Transition Metals
4. Rules for Naming Acids
5. Rules for Naming Ionic Compounds
6. The Solubility Rules
7. Determining Oxidation Numbers
Rules for Determining Oxidation Number
Helpful tutorial: http://www.chemguide.co.uk/inorganic/redox/oxidnstates.html
Oxidation Number: A number assigned to an atom in a molecular compound or
molecular ion that indicates the general distribution of electrons among the
bonded atoms.
1. The oxidation number of any uncombined element is O.
2. The oxidation number of a monatomic ion equal the charge on the ion.
3. The more electronegative element in a binary compound is assigned the
number equal to the charge it would have if it were an ion.
4. The oxidation number of fluorine in a compound is always –1
5. Oxygen has an oxidation number of –2 unless it is combined with F, when it is
+2, or it is in a peroxide, when it is –1.
6. The oxidation state of hydrogen in most of its compounds is+1 unless it
combined with a metal, in which case it is –1.
7. In compounds, the elements of groups 1 and 2 as well as aluminum have
oxidation number of +1, +2, and +3, respectively
8. The sum of the oxidation numbers of all atoms in a neutral compound is O.
9. The sum of the oxidation number of all atoms in a polyatomic ion equals the
charge of the ion.
Solubility Rules
1. All compounds containing 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 Hg2+.
4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
5. All hydroxides are insoluble except compounds of the alkali metals, Ca 2+, Sr2+,
and Ba2+.
6. All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble
except those that also contain alkali metals or NH4+.
Variable Valences for Transition Metals
Name
Symbol
Charge
Stock Name
-ous/-ic
Chromium
Cr
+2
+3
Chromium
(II)
Chromous
Chromic
Chromium
(III)
Manganese
Mn
+2
+3
Manganese
(II)
Manganous
Manganic
Manganese
(III)
Iron
Cobalt
Copper
Lead
Mercury
Tin
Gold
Silver
Bismuth
Fe
Co
Cu
Pb
Hg
Sn
Au
Ag
Bi
+2
Iron (II)
Ferrous
+3
Iron (III)
Ferric
+2
Cobalt (II)
Cobaltous
+3
Cobalt (III)
Cobaltic
+1
Copper (I)
Cuprous
+2
Copper (II)
Cupric
+2
Lead (II)
Plumbous
+4
Lead (IV)
Plumbic
+1
Mercury (I)
Mercurous
+2
Mercury (II)
Mercuric
+2
Tin (II)
Satonnous
+4
Tin (IV)
Stannic
+1
Gold (I)
Aurous
+3
Gold (III)
Auric
+1
Silver
Argentous
+2(rarely)
Silver (II)
Argentic
+3
Bismuth
Bismuthous
(III)
+5
Bismuthic
Bismuth (V)
Antimony
Sb
+3
Antimony
(III)
+5
Stibnous
Stibnic
Antimony
(V)
Cadmium
Cd
+2
Cadmium
Zinc
Zn
+2
Zinc
Polyatomic Ions
Name
Symbol
Charge
ammonium
NH4
+1
acetate
C2H3O2
-1
bromate
BrO3
-1
chlorate
ClO3
-1
chlorite
ClO2
-1
cyanide
CN
-1
dihydrogen phosphate
H2PO4
-1
hypochlorite
ClO
-1
hydrogencarbonate(bicarbonate)
HCO3
-1
hydrogen sulfate (bisulfate)
HSO4
-1
hydrogen sulfite (bisulfite)
HSO3
-1
hydroxide
OH
-1
iodate
IO3
-1
nitrate
NO3
-1
nitrite
NO2
-1
perchlorate
ClO4
-1
permanganate
MnO4
-1
thiocyanate
SCN
-1
carbonate
CO3
-2
chromate
CrO4
-2
dichromate
Cr2O7
-2
oxalate
C2O4
-2
selenate
SeO4
-2
silicate
SiO3
-2
sulfate
SO4
-2
sulfite
SO3
-2
phosphate
PO4
-3
phosphite
PO3
-3
Rules for Naming Ionic Compounds
1. Balance Charges (charges should equal zero)
2. Cation is always written first (in name and in formula)
3. Change the ending of the anion to –ide
Rules for Naming an Acid
1. When the name of the anion ends in –ide, the acid name begins with the
prefix hydro-, the stem of the anion has the suffix –ic and it is followed by the
word acid. -ide becomes hydro _____ic Acid
Cl- is the Chloride ion so HCl = hydrochloric acid
2. When the anion name ends in –ite, the acid name is the stem of the anion
with the suffix –ous, followed by the word acid. -ite becomes ______ous Acid
ClO2- is the Chlorite ion so HClO2. = Chlorous acid.
3. When the anion name ends in –ate, the acid name is the stem of the anion
with the suffix –ic, followed by the word acid. -ate becomes ______ic Acid
ClO3- is the Chlorate ion so HClO3 = Chloric acid.
Practice:
1. Write formulas for the following
substances:
a. Barium sulfate __________________
b. Ammonium chloride__________________
c. Chlorine monoxide __________________
d. Silicone tetrachloride_________________
e. Magnesium fluoride _________________
f. Sodium oxide __________________
g. Sodium peroxide__________________
h. Copper (I) iodide __________________
i. Zinc sulfide __________________
j. Potassium carbonate _________________
k. Hydrobromic acid __________________
l. Perchloric acid __________________
m. Lead (II) acetate __________________
n. Sodium permanganate _______________
o. Lithium oxalate __________________
p. Potassium cyanide __________________
q. Iron (III) hydroxide _________________
r. Silicone dioxide __________________
s. Nitrogen trifluoride __________________
t. Chromium (III) oxide ________________
u. Calcium chlorate __________________
v. Sodium thiocyanate _________________
w. Cobalt (III) nitrate __________________
x. Nitrous acid __________________
y. Ammonium phosphate _______________
z. Potassium chromate _________________
2. Name each of the following compounds
(Give acid names where appropriate)
a. CuSO4 ____________________________
b. PCl3 ____________________________
c. Li3N ____________________________
d. BaSO3 ____________________________
e. N2F4 ____________________________
f. KClO4 ____________________________
g. NaH ____________________________
h. (NH4)2Cr2O7 ________________________
i. HNO2 ____________________________
j. Sr3P2 ____________________________
k. Mg(OH)2 __________________________
l. Al2S3 ____________________________
m. AgBr ____________________________
n. P4O10 ____________________________
o. HC2H3O2 __________________________
p. CaI2 ____________________________
q. MnO2 ____________________________
r. Li2O ____________________________
s. FeI3 ____________________________
t. Cu3PO4 ____________________________
u. PCl3 ____________________________
v. NaCN ____________________________
w. Cs3N ____________________________
x. Zn(NO3)2 __________________________
y. N2O ____________________________
1) Find the mass percent of nitrogen in each of the following compounds:
a. NO
b. NO2
c. N2O4
d. N2O
2) Benzene contains only carbon and hydrogen and has a molar mass of 78.1
g/mol. Analysis shows the compound to be 7.74% H by mass. Find the
empirical and molecular formulas of benzene.
3) Calcium carbonate decomposes upon heating, producing calcium oxide and
carbon dioxide gas.
a. Write a balanced chemical equation for this reaction.
b. How many grams of calcium oxide will be produced after 12.25 g of calcium
carbonate is completely decomposed?
c. What volume of carbon dioxide gas is produced from this amount of calcium
carbonate, at STP?
4) Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write a balanced chemical equation for this reaction.
b. 3.2 g of hydrogen gas and 9.5 g of bromine gas react. Which is the limiting
reagent?
c. How many grams of hydrogen bromide gas can be produced using the
amounts in (b)?
d. How many grams of the excess reactant is left unreacted?
e. What volume of HBr, measured at STP, is produced in (b)?
5) When ammonia gas, oxygen gas and methane gas (CH4) are combined, the
products are hydrogen cyanide gas and water.
a. Write a balanced chemical equation for this reaction.
b. Calculate the mass of each product produced when 225 g 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 g of HCN, calculate the
percent yield.
6) When solutions of potassium iodide and lead (II) nitrate are combined, the
products are potassium nitrate and lead (II) iodide.
a. Write a balanced equation for this reaction, including (aq) and (s).
b. Calculate the mass of precipitate produced when 50.0mL of 0.45M
potassium iodide solution and 75mL of 0.55M lead (II) nitrate solution are
mixed.
c. Calculate the volume of 0.50M potassium iodide required to react
completely with 50.0mL of 0.50M lead (II) nitrate.