Outline of Review Material
AP Chemistry
Summer 2016
The summer work is mostly review from first year chemistry. We will be testing over this material about two
days into the school year. To help you with this, I have included some review problems. These will be counted
as homework for you and will be due on the first day back from the summer.
Your first task is to join the AP Chem facebook group. No, it’s not an absolute requirement, but it’s just short
of that. Go to my course website - princetonschools.net/dusch, and click on AP Chemistry Facebook Group in
the left-hand navigation. Then ask to join the group. That’ll be the easiest way to get help with these homework
problems. You can also check my site out for help under Chemistry Help. (10 HW pts)
Your second task is to get an AP chemistry review book. You can pick these up for in the range of $10-15 on
Amazon or probably $20 in store at Barnes and Noble or some other book store. The format of and curriculum
for the AP chemistry test changed in 2014, so don’t get anything older than that (ideally, get a 2016 version).
To check, see if the book mentions colligative properties or nuclear chemistry. If it mentions those, it’s old.
Don’t buy it. I particularly recommend AP Chemistry Crash Course, AP Chemistry All Access, or Cracking the
AP Chemistry Exam. There are other good books, but I know these have been updated to the new test format.
(10 HW pts)
Your third task is to visit apstudent.collegeboard.org and visit the AP chemistry course page (under AP
courses). Download the two pdf’s there: Course Overview and Course and Exam Description. Don’t print these
out. One is two pages, but the other is 177 pages long. You will have to show me that you have this
downloaded and available on some device (your phone, a tablet, a laptop if you need to) because we will refer
to the document at weird and spontaneous times next year. (10 HW pts)
Your fourth task is to memorize a few more polyatomic ions. It’s mostly the list from honors but with a few
more included. Check the sheet toward the back of this packet. (no points, but you’ll need them on tests and
quizzes)
Your fifth task is to do the practice problems in the rest of the packet. They’re review from the first year plus
one slightly new application of empirical formulas. (20 HW pts – graded for correctness)
…name compounds - be they ionic, covalent, or acidic – from their formulas or write formulas from their
names…
1. Name the following compounds…
a) HCl
b) H2SO4
c) NaNO3
d) H2S
e) BaBr2
f) Hg2CO3
g) PbCl4
h) CBr4
i) Mn(OH)2
j) KrF4
k) MgO
l) PtSO4
m) Hg2Cl2
n) BaCr2O7
o) XeF6
p) UF6
2. Write formulas for the following compounds…
a) ammonium sulfate
f) sulfurous acid
b) acetic acid
g) manganese (IV) oxide
c) copper (I) bromide
h) disulfur trioxide
d) silicon tetrafluoride
i) lithium cyanide
e) trinitrogen octaoxide
j) chromium (III) phosphate
…write the atomic symbols with charge, atomic number, and atomic mass in the correct places…
3. Write the complete symbols with as much information as possible for these two atoms or ions…
a) p+ = 106 n0 = 157
e- = 106
+
0
b) p = 56
n = 61
e- = 54
(atomic # in bottom left, mass in top left
…write reactions from situations given…
4. Write the reactions for the following situations…include correct subscripts and states of matter along
with any other needed symbols…
a) When sodium metal is placed in water, it makes hydrogen gas and a solution of sodium hydroxide.
b) The combustion of ethyl alcohol, C2H5OH, in oxygen gas is catalyzed by platinum. It results in the
typical combustion products of carbon dioxide water – both in the gaseous states.
c) Solution of barium nitrate and sodium hydroxide produce a precipitate of barium hydroxide while the
sodium nitrate remains in solution.
d) When calcium carbonate is heated strongly, it breaks down into calcium oxide – lime – and carbon
dioxide gas.
e) Copper – as a wire – can replace silver in silver nitrate solution. The solution would then end up
being copper (II) nitrate.
…balance reactions…
5. Balance the reactions from problem #4.
…identify patterns in chemical reactions on the periodic table…
6. Identify the types of reactions present in problems 4. Be warned, however, that a few won’t fit
exactly into the patterns.
…calculate and manipulate molecular weights, atomic weights, formula weight…and identify each as such…
7. Make menus for each of these chemicals.
a) C2H5OH
b) Ba(NO3)2
c) Pt
d) TiO2
e) F2
…calculate the percent by mass of elements in a chemical – and reverse the process by calculating the
empirical and molecular formulas from percents by mass…
8. What is the percent by mass of all the elements in sucrose – C12H22O11?
9. Ethylene glycol – the major component of antifreeze – is made of 38.7% carbon, 9.7% hydrogen,
and 51.6% oxygen. What is the empirical formula of ethylene glycol?
10. If the molar mass of ethylene glycol is 62.1 g/mol, what is the molecular formula?
…calculate the amount of product or reactant made or used up from an amount given…
11. 35.6 grams of heptanol is combusted. How many grams of water should be produced from
complete combustion?
12. How much pure silver can be made from a 1.4 gram wire of copper from the reaction in problem
4e?
…use the concepts of limiting reactants to calculate theoretical yields…
13. 100 grams of each of the reactants in problem 4a are allowed to react fully.
a) Which of the reactants will limit the production?
b) What will be the theoretical yield of calcium metal?
Real AP Questions from past AP tests
I have a little repository of past AP tests. I will – throughout the year – take questions from these and put them
on worksheets and tests for you. This is probably the single most effective thing that I can do to help prepare
you for the AP test. Once you’ve seen the types of questions that they ask, you’ll be more ready to answer
them when they count.
. . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g)
14. When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms,
the coefficient for O2(g) is what?
15. When hafnium metal is heated in an atmosphere of chlorine gas, the product of the reaction is found to
contain 62.2 percent Hf by mass and 37.4 percent Cl by mass. What is the empirical formula for this
compound?
10 HI + 2 KMnO4 + 3 H2SO4 --> 5 I2 + 2 MnSO4 + K2SO4 + 8 H2O
16. According to the balanced equation above, how many moles of HI would be necessary to produce 2.5 mol
of I2, starting with 4.0 mol of KMnO4 and 3.0 mol of H2SO4?
17. The simplest formula for an oxide of nitrogen that is 36.8 percent nitrogen by weight is what?
18.
__ CH3CH2COOH(l) + __ O2(g) ---> __ CO2(g) + __ H2O(l)
How many moles of O2 are required to oxidize 1 mole of CH3CH2COOH according to the reaction
represented above?
19. In which of the following compounds is the mass ratio of chromium to oxygen closest to 1.62 to 1.00?
(A) CrO3
(B) CrO2
(C) CrO
(D) Cr2O
(E) Cr2O3
20. Elemental analysis of an unknown pure substance indicates that the percent composition by mass is as
follows:
Carbon - 49.02%
Hydrogen - 2.743%
Chlorine - 48.23%
Determine the empirical formula of the unknown substance.
Combustion Analysis (aka The One Sort of New Topic)
In honors chem you found the empirical and molecular formulas. You did this by me telling you how many
grams of, for example, hydrogen and of carbon were in a compound. That rarely happens in the lab. Instead,
the initial compound is burned and the products collected and measured for mass. Chemists then figure out
how many grams of hydrogen and of carbon are in those products. From there, they then find the empirical
formula.
1. Before August 1, post two videos showing how to solve combustion analysis problems to find empirical
formulas. Post them to the AP Facebook group. Make sure one deals with at least H and C. The other can
have H and C, too, but it should also have oxygen in the compound.
2. Share links to two websites that explain how to find the empirical formula by combustion analysis.
Solve these problems…
21. Nicotine is composed of carbon, hydrogen, and nitrogen. A 5.250 mg sample of nicotine was combusted,
producing 14.242 mg of CO2 and 4.083 mg of H2O. What is the empirical formula of nicotine?
22. A carbohydrate is a compound composed solely of carbon, hydrogen and oxygen. When 10.7695 g of an
unknown carbohydrate (MW = 128.2080 g/mol) was subjected to combustion analysis with excess
oxygen, it produced 29.5747 g CO2 and 12.1068 g H2O. What is its molecular formula?
23. A 1.000 g sample of a compound is combusted in excess oxygen and the products are 2.492 g of CO2 and
0.6495 g of H2O.
24. A 1.50 g sample of hydrocarbon undergoes complete combustion to produce 4.40 g of CO2 and 2.70 g of
H2O. What is the empirical formula of this compound?
Polyatomic Ions and Their Charges
*Ammonium
NH4+1
+1 Charge
*Mercury (I)
Hg2+2
* Acetate
? Aluminate
Amide
Azide
Benzoate
* Bicarbonate
Bisulfite
Bromate
? Borohydride
* Chlorate
* Chlorite
? Chromite
Cyanate
* Cyanide
Dihydrogen Phosphate
Dihydrogen Phosphite
Formate
Glutamate
* Hydrogen Carbonate
Hydrogen Sulfate
C2H3O2-1
AlO2-1
NH2-1
N3-1
C6H5COO-1
HCO3-1
HSO3-1
BrO3-1
BH4-1
ClO3-1
ClO2-1
CrO2-1
OCN-1
CN-1
H2PO4-1
H2PO3-1
HCOO-1
C5H8NO4-1
HCO3-1
HSO4-1
-1 Charge
Hydrogen Sulfide
Hydrogen Sulfite
* Hydroxide
Hypobromite
*Hypochlorite
Hypoiodite
Iodate
Iodite
Lactate
* Nitrate
* Nitrite
Perbromate
* Perchlorate
Periodate
* Permanganate
Sorbate
Superoxide
* Thiocyanate
Triiodide
? Vanadate
HS-1
HSO3-1
OH-1
BrO-1
ClO-1
IO-1
IO3-1
IO2-1
C3H5O3-1
NO3-1
NO2-1
BrO4-1
ClO4-1
IO4-1
MnO4-1
C6H7O2-1
O2-1
SCN-1
I3-1
VO3-1
-2 Charge
* Peroxide
? Peroxydisulfate
Phthalate
? Selenate
Silicate
* Sulfate
* Sulfite
Tartrate
? Tellurate
Tetraborate
* Thiosulfate
? Tungstate
? Zincate
O2-2
S2O8-2
C8H4O4-2
SeO4-2
SiO3-2
SO4-2
SO3-2
C4H4O6-2
TeO4-2
B4O7-2
S2O3-2
WO4-2
ZnO2-2
-3 Charge
? Hypophosphite
* Phosphate
Phosphite
PO2-3
PO4-3
PO3-3
-4 Charge
? Pyrophosphate
P2O7-4
* Carbonate
Carbide
* Chromate
* Dichromate
? Disulfate
Hexafluorosilicate
Hydrogen Phosphate
Hydrogen Phosphite
Imide
Manganate
? Metasilicate
? Molybdate
Monohydrogen phosphate
* Oxalate
-2
CO3
C2-2
CrO4-2
Cr2O7-2
S2-2
SiF6-2
HPO4-2
HPO3-2
NH-1
MnO4-2
SiO3-2
MoO4-2
HPO4-2
C2O4-2
-3
Arsenate
? Arsenite
Borate
Citrate
AsO4
AsO3-3
BO3-3
C6H5O7-3
Orthosilicate
SiO4-4
? Tripolyphosphate
P3O10-5
-5 Charge