AP Chemistry Pre-Course Packet
AP Chemistry, Fall 2015
Roswell High School
Get excited (and ready) for AP Chemistry!
Name:
Included in this packet is information about the exam and information you should KNOW
(memorize or be able to derive from the wonderful periodic table) or know how to CALCULATE.
FYI—the PT on the AP exam has NO NAMES given, only symbols. If you need help SEE me. We
will start class in August with the expectation that you are competent with ALL of this material.
There will be several assessments that cover this material in the first two weeks of school.
Don’t freak out about this packet. You probably know more than you think. The answer key will
be available in my classroom for you to check your work as you go. If you need more practice in
a certain area, let me know. The first two pages are informational and the rest are things you
should already know how to do! This will be due on Friday, August 14th.
Drop by room F123 or email me: chiltonc@fultonschools.org
The 2016 AP Chemistry Exam will be Monday, May 2nd! Registration information for the exam
will be given to you as soon as it is available. FYI: The AP Chemistry exam is the FIRST exam
given, and it is given at the same time as AP Environmental Science. Yes, you can take both
classes & both exams. You will just have to take an alternate exam (different that the one given
on May 2) on a different date as decided by the College Board.
Stuff to KNOW
1. SI base units and prefixes
2. Rules for significant figures
3. Element Names & Symbols (Element symbols 1 to 38 and Ag, Cd, I, Xe, Cs, Ba, W, Hg, Pb, Sn, Rn, Fr, U,
Th, Pu, and Am written correctly—careful with capital letters—Co, not CO!
4. Monatomic Ions
a. Ions with (usually) one oxidation state:
+
+
+
2+
2+
2+
2+
+
2+
2+
Li , Na , K , Mg , Ca , Sr , Ba , Ag , Zn , Cd , Al
32- 2- - N , O , S , F , Cl , Br , I
3+
b. Ions with more than one oxidation state:
+
Cu
2+
Cu
2+
Hg2
2+
Hg
2+
Fe
3+
Fe
2+
Cr
3+
Cr
Copper (I) ion
Copper (II) ion
Mercury (I) ion
Mercury (II) ion
Iron (II) ion
Iron (III) ion
Chromium (II) ion
Chromium (III) ion
2+
Mn
3+
Mn
2+
Co
3+
Co
2+
Sn
4+
Sn
2+
Pb
4+
Pb
Manganese (II) ion
Manganese (III) ion
Cobalt (II) ion
Cobalt (III) ion
Tin (II) ion
Tin (IV) ion
Lead (II) ion
Lead (IV) ion
5. Strong Acids (for all practical purposes, all others are weak acids): HCl, HBr, HI, H2SO4, HNO3, HClO4
6. Strong Bases (for all practical purposes all others are weak):
Group I hydroxides and Group II hydroxides (except Be(OH)2 and Mg(OH)2)
AP Chemistry, Fall 2015
Roswell High School
7. Polyatomic Ions (most you learned in Honors Chemistry)
-1
-2
2C2H3O2 acetate
SO4 sulfate
2NO3 nitrate
SO3 sulfite
2NO2 nitrite
CO3 carbonate
2CN cyanide
C2O4 oxalate
2OCN cyanate
CrO4 chromate
2SCN thiocyanate
Cr2O7 dichromate
2MnO4 permanganate
S2O3 thiosulfate
2OH hydroxide
O2 peroxide
2HSO4 bisulfate
SeO4 selenate
2HCO3 bicarbonate
HPO4 hydrogen phosphate
O2 superoxide
H2PO4 dihydrogen
phosphate
ClO4 perchlorate *
ClO3 chlorate *
ClO2 chlorite *
ClO hypochlorite *
* Br, I and F may be substituted
-3
3PO4 phosphate
3AsO4 arsenate
3AsO3 arsenite
+1
+
NH4 ammonium
8. Colors of common ions in aqueous solution – most common ions are colorless in solution, however,
some have distinctive colors. These colors have appeared on past AP Chemistry exams:
Fe2+ and Fe3+ - various colors
Ni2+ - green
Cu2+ - blue to green
Co2+ - pink
Cr2+ - blue
MnO4- - dark purple
3+
Cr - green or violet
CrO42- - yellow
Mn2+ - faint pink
Cr2O72- - orange
9. Solubility Rules
Soluble Ionic Compounds
+
Group IA and ammonium (NH 4 ) salts
-
-
nitrates (NO3 ) and acetates (C2H3O2 )
Exceptions
none
none
10. Patterns of Reactions
a. Metallic carbonates when heated decompose into metallic oxides and CO2 (g)
Ex: CaCO3(s) → CaO(s) + CO2(g)
b. Most metallic hydroxides, when heated, decompose into metallic oxides and water.
Ex: Ca(OH)2(s) → CaO(s) + H2O(g)
c. Metallic chlorates, when heated, decompose into metallic chlorides and oxygen.
Ex: 2KClO3(s) → 2KCl(s) + 3O2(g)
d. Some acids, when heated, decompose into nonmetallic oxides and water.
Ex: H2SO4 → H2O(l) + SO3(g)
AP Chemistry, Fall 2015
Roswell High School
e. Some oxides, when heated, decompose.
Ex: 2HgO(s) → 2Hg(l) + O2(g)
f. Some decomposition reactions are produced by electricity.
Ex: 2H2O(l) → 2H2(g) + O2(g)
g. Metal + oxygen → metal oxide
Ex: 2Mg(s) + O2(g) → 2MgO(s)
h. Nonmetal + oxygen → nonmetallic oxide
Ex: C(s) + O2(g) → CO2(g)
i. Metal oxide + water → metallic hydroxide
Ex: MgO(s) + H2O(l) → Mg(OH)2(s)
j. Nonmetallic oxide + water → acid
Ex: CO2(g) + H2O(l) → ; H2CO3(aq)
k. Metal + nonmetal → salt
Ex: 2 Na(s) + Cl2(g) → 2NaCl(s)
l. A few nonmetals combine with each other
Ex: 2P(s) + 3Cl2(g) → 2PCl3(g)
Stuff to know how to CALCULATE (with proper significant figures!!)
1. Use dimensional analysis method to convert the following:
a.
b.
c.
d.
3 meters into centimeters
15,050 milligrams into grams
3,264 milliliters into liters
9,674,444 grams into kilograms
2. Classify each of the following as units of mass, volume, length, density, energy, or
pressure
a.
b.
c.
d.
mg
mL
3
cm
mm
e.
f.
g.
h.
3
kg/m
kJ
atm
cal
3. How many significant figures are in each of the following?
a.
b.
c.
d.
1.92 mm
0.030100 kJ
6.022 x1023 atoms
460.00 L
e.
f.
g.
100
0.001
0.010
c.
d.
0.0000000809 Ǻ
765,400,000,000 atoms
4. Record the following in correct scientific notation:
a.
b.
350,000,000 cal
0.0000721 mol
5. Calculate the following to the correct number of significant figures.
a.
b.
c.
1.27 g / 5.296 cm3
12.235 g / 1.01 L
2.1 x 3.21
d.
e.
200.1 x 120
17.6 + 2.838 + 2.3 + 110.77
6. Calculate the mass of a sample of copper that occupies 4.2x10 3cm3 if the density of
copper is 8.94g/cm3.
AP Chemistry, Fall 2015
Roswell High School
7. Fill in the following table:
Element or ion
Complete Name
# protons
# neutrons
# electrons
Fe-55
+
K
27
25
2-
O
Pb-208
8. Find the average atomic mass of an element if, out of 100 atoms, 5 have a mass of
176amu, 19 have a mass of 177amu, 27 have a mass of 178amu, 14 have a mass of
179amu and 35 have a mass of 180amu.
9. Strontium consists of four isotopes with masses and percent abundances as follows:
83.9134amu (0.5%), 85.9094amu (9.9%), 86.9089amu (7.0%), and 87.9056amu (82.6%).
Calculate the atomic mass of strontium.
10. Write the complete & Noble gas (abbreviated) ground state electron configurations:
a.
b.
c.
d.
Strontium
Iron
Sulfur
neodymium
11. Write formulas for the following substances:
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
Barium sulfate
Ammonium chloride
Chlorine monoxide
Silicone tetrachloride
Magnesium fluoride
Sodium oxide
Sodium peroxide
Copper (I) iodide
Zinc sulfide
Hydrobromic acid
k.
l.
m.
n.
o.
p.
q.
r.
s.
t.
Lead (II) acetate
Sodium permanganate
Lithium oxalate
Potassium cyanide
Iron (III) hydroxide
Silicone dioxide
Nitrogen trifluoride
Chromium (III) oxide
Cobalt (III) nitrate
Nitrous acid
12. Name each of the following compounds (Give acid names where appropriate)
a.
CuSO4
i.
Al2S3
b.
PCl3
c.
N2F4
j.
k.
AgBr
P4O10
d.
KClO4
l.
HC2H3O2
e.
(NH4)2Cr2O7
f.
HNO2
g.
Sr3P2
h.
Mg(OH)2
m. FeI3
n.
Cu3PO4
o.
Cs3N
p.
HF
13. Find the mass percent (percent composition) of nitrogen in each of the following
compounds:
a.
b.
c.
NO
NO2
N2O4
AP Chemistry, Fall 2015
Roswell High School
14. Complete the Following Table:
Name of Acid
Formula of Acid
Name of Anion
hydrochloric
HCl
chloride
sulfuric acid
H2SO4
sulfate
HC2H3O2 or CH3COOH
15. Predict the products of the following reactions, write balanced chemical equations, include states
of matters and identify the reaction type.
a.
sodium carbonate (heated)
b.
electrolysis of aluminum oxide
c.
magnesium burned in oxygen
d.
Ammonium sulfate reacts with barium nitrate.
e.
Zinc metal is added to a solution of copper (II) chloride.
f.
Propane gas (C3H8) is burned in excess oxygen.
g.
Solid calcium chlorate is heated strongly.
h.
Solutions of lead (II) nitrate and calcium iodide are combined.
i.
Sulfuric acid is combined with sodium hydroxide.
j.
Iron metal shavings are added to hydrochloric acid.
k.
Sodium metal is added to distilled water.
16. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows
the compound to be 7.74 % hydrogen by mass. Find the empirical and molecular formulas of
benzene.
17. Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write a balanced equation for this reaction.
b. 3.2 grams of hydrogen react with 9.5 grams of bromine. Which is the limiting reactant?
c. How many grams of hydrogen bromide gas can be produced using the amounts in (b)?
d. How many grams of excess reactant are left unreacted?
e. What volume of HBr, measured at STP is produced in (b)?
AP Chemistry, Fall 2015
Roswell High School
18. 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 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.
19. When solutions of potassium iodide and lead (II) nitrate are combined, the products are
potassium nitrate and lead (II) iodide.
d. Write a balanced equation for this reaction, including (aq) and (s).
e. 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.
f. Calculate the volume of 0.50M potassium iodide required to react completely with
50.0mL of 0.50M lead (II) nitrate
20. A solution of 2.5 M H2SO4 is reacted with 75.0 mL of 6.2 M NaOH
g. Write a balanced equation.
h. Calculate the volume of H2SO4 required in milliliters.
i.
Calculate the mass of the salt produced.
Recommended AP Chemistry Review books:
5 Steps to a 5, AP Chemistry, 2015 edition, by John Moore and Richard Langley, McGraw-Hill
AP Chemistry Crash Course, 2nd Edition, by Adrian Dingle, Research & Education Association
Cracking the AP Chemistry Exam, 2015 edition, by Paul Foglino, The Princeton Review