Future AP Chemistry Students—
I want to be the first to welcome you to AP Chemistry as you finish up your last couple of days of
school. I know all of you have worked hard all (or most) of the year to get where you are right now and
probably the last thing that you want to think about is next year, however I want to at least be able to
provide you with some material that will assist in getting us prepared for the beginning of next year.
Even if this is your alternate class, I want to ensure you have the material needed if this ends up being
your class. If it doesn’t, don’t worry about the work and please return the materials during the first
week of school.
Behind this letter you will find your summer work. It is a review over material that you either
covered in my class. Use the textbook provided or your notes from this year to answer the questions. It
should all be there. This will help us prepare for the first exam, which will cover the first three chapters.
Please do not go home today and do the packet. Take some time off!!! You deserve it. Plus, it is a
review to get many of the ideas we learned this year back in your head before the start of school. That
won’t happen if you do it during the next few weeks of summer vacation. It is due the 1st day of school.
No exceptions, no excuses. Your ability to complete the summer assignment is an indicator of how well
you will do in this course. I also expect you to come back knowing the polyatomic ions that we covered
in Pre-AP Chemistry. I attached the list in case you need it to study. We will spend two weeks covering
this material and then we will test on test.
If after looking over this packet and attempting some of the problems you feel that AP
Chemistry my not be for you that is OK. Please let myself or one of your counselors know this ASAP.
Being able to transfer you to a different course becomes exponentially difficult once the beginning of
the year rolls around. Enjoy your summer vacation and if you have any questions, don’t hesitate to
contact me by email.
Sincerely,
Mr. Chuning (Mr. C)
Contact Information—
Email: austin_chuning@isdschools.org
AP Chemistry – Summer Review Assignment
No, you don’t have to spend all summer studying chemistry. However, if you will spend a bit of time
from time to time this summer reviewing the concepts and skills contained in this guide, you will be able
to spend more time learning new material next year and your life (in chem) will be much easier. Plan on
taking a test over this material during the first week of class; if there are concepts that we did not
completely cover in class it is your responsibility to do research on YOUR OWN in order figure out how
to come to an answer. Do not give up because you think you can’t. Find a solution! I know you can!
I. Significant Figures and Basic Chemical Math
1. A piece of poster board measures 1.827 m long and 0.762 m wide. Find its area. Give the
answer with the correct number of significant figures and proper units.
2. For a laboratory experiment, a teacher wants to divide all of a 453.6 g sample of sulfur equally
among the 21 members of her class. How many grams of sulfur should each student receive?
3. Perform the indicated operations and give answers with the proper number of significant figures:
a. 48.2 m + 3.82 m + 48.4394 m
b. 148 g + 2.39 g + 0.0124 g
c. 451 g – 15.46 g – 20.3 g
d. 5.436 L + 5.3 L – 6.24 L – 0.177 L
e. (51.5 m + 2.67 m) X (33.42 m -0.124 m)
f. (125.1 g – 1.22 g) / (52.5 mL + 0.63 mL)
47.5 kg -1.44 kg
g.
h.
10.5 m X 0.35 m X 0.175m
0.307 g - 14.2 mg - 3.52 mg
(1.22 cm - 0.28 mm) X 0.752 cm X 0.51 cm
4. Convert the following:
a. 50 km to m
b. 47.9 ML to L
c. 578 ms to s
d. 1.55 X 102 kg to milligrams
e. 87.4 cm2 to mm2
f. 0.0962 km/min to m/s
5. Density
a. The mass of 325 mL of liquid methanol is found to be 257 g. What is its density?
b. A block of lead is 1.20 cm X 2.41 cm X 1.80 cm and has a mass of 59.01 g. What is the
density of lead?
c. What is the mass, in grams, of 30 mL of syrup that has a density of 1.32 g/mL?
d. a square of aluminum foil (d= 2.70 g/cm3) is 5.10 cm on a side and has a mass of 1.762 g.
Calculate the thickness of the foil, in millimeters.
II. Atomic Structure
1. Complete the table:
Symbol
Atomic Number
Atomic Mass
# protons
# neutrons
# electrons
12
6
C
48
64
197

79
Na1
23
30
66

28
16
2. What are isotopes?
3. What are ions? How are they formed?
18
18
III. Nomenclature and Formulas
1. Ionic Compounds – formed from metal cations and nonmetal anions.
a. Generally named as “metal name + nonmetal name → change ending to “ide”
Example: CaCl2 = calcium chloride
b. While charges are easy to obtain from the Periodic Table for main group elements (groups
1,2,3,4,5,6,7) remember that transition metals may have variable charge and the charge must be
specified in the name. The charge can be determined from the number/charge of the anions
attached.
Example: CrCl3 – chromium (III) chloride. (It has to be chromium(III) because there are 3
chlorides in the compound and each chloride is -1
2. Polyatomic Ions – MEMORIZE! (Flash cards may be very helpful)
ammonium
NH4+
carbonate
CO32-
acetate
C2H3O2-
hydrogen carbonate
(aka bicarbonate)
HCO3-
hypochlorite
chlorite
chlorate
perchlorate
ClOClO2ClO3ClO4-
oxalate
C2O42-
sulfite
SO32-
cyonate
thiocyanate
OCNSCN-
sulfate
SO42-
hydrogen sulfite
HSO3-
cyanide
CN-
hydrogen sulfate
HSO4-
hydroxide
OHthiosulfate
S2O32-
phosphate
PO43-
nitrite
nitrate
NO2NO3-
permanganate
MnO4-
hydrogen phosphate
HPO42-
chromate
dichromate
CrO42Cr2O72-
dihydrogen phosphate
H2PO4-
You might want to develop your own mnemonics or strategies for internalizing formulas and charges.
For example, if you know sulfuric acid is H2SO4, and you know that each hydrogen has a +1 charge, then
the sulfate must be -2. Note, also, that all “family members” (for lack of a better term) have the same
charge. If you know nitrate is -1, nitrite will also be -1.
1. Name them:
NaCl
Rb2O
CaS
AlI3
CrO
Cr2O3
Al2O3
NaH
CuBr2
ZnCl2
KClO4
Ca3(PO4)2
Al2(SO4)3
Pb(NO3)2
BaSO3
NaNO2
KMnO4
K2Cr2O7
(NH4)2CO3
LiOH
b. Write them:
cesium bromide
barium sulfate
ammonium chloride
potassium nitrate
sodium hydrogen carbonate
calcium dihydrogen phosphate
beryllium oxide
magnesium fluoride
iron(II) oxide
iron(III) oxide
lithium nitride
ammonium acetate
potassium chlorate
cobalt(III) nitrate
lead(IV) sulfide
magnesium hydroxide
copper(II) phosphate
potassium dichromate
sodium thoisulphate
sodium hydrogen sulfite
3. Binary Molecular Compounds – formed from nonmetals
a. First element is named as usual, second element is then named, changing the end to “ide”
b. Greek prefixes are used to indicate the number of atoms present
Example: N2O5 = dinitrogen pentoxide
c. Name them:
PCl5
PCl3
SF6
SO3
SO2
CO2
NI3
SF2
N2F4
P2S5
N2O
CCl4
H2O
d. Write them:
carbon dioxide
iodine pentachloride
chlorine monoxide
tetraphosphorus decoxide
silicon tetraflouride
disulfur dichloride
oxygen diflouride
carbon tetrabromide
phosphorus trichloride
(Note: your quiz over this material will contain “mixed” problems – ionic and molecular together)
4. Acids and Bases – Flash cards?
Strong Acids
HClO4 – perchloric
HI – hydroiodic
HBr – hydrobromic
HCl – hydrochloric
HNO3 – nitric
H2SO4 - sulfuric
Strong Bases
group I hydroxides
hydroxides from group II: Ca, Sr, Ba
Weak Bases
NH3 – ammonia and its organic derivatives
Other acids (weak)
HF – hydrofluoric
H3PO4 – phosphoric **Note that the “ate” ion becomes the “ic” acid.
HC2H3O2 or CH3CO2H – acetic
H2CO3 – carbonic
HCN – hydrocyanic
H2S – hydrosulfuric
HNO2 – nitrous
H2SO3 – sulfurous
H3PO3 – phosphorous
HClO3 – chloric
HClO2 – chlorous
HClO – hypochlorous
5. Formulas for diatomic elements
“Honkelbrif” – HONClBrIF all exist as diatomics
“Mr. H. BrONClIF
H2, O2, N2, Cl2, Br2, I2, F2
Also mercury (I) cation is a diatomic cation – Hg22+
IV. Basic Stoichiometry and Chemical Calculations
1. Balance:
→
Fe
+
O2
SiCl4
+
H2O
→
PCl3
+
H2O
→
CaO
+
P4O10
C2H6 +
O2
H3PO4 +
Ba(NO3)2
FeCl3
+
SiO2
+
HCl
H3PO3 +
→
HCl
Ca3(PO4)2
→
NaCN
+
Fe2O3
CO2
→
H2O
HCN +
Al2(SO4)3
NaOH
+
→
→
Na3PO4
BaSO4 +
Fe(OH)3
+
Al(NO3)3
NaCl
2. Molar Masses (use 2 decimal places with atomic masses)
N2H4
C5H12
Li2O
Mg(NO3)2
Ca(H2PO4)2
K2SbF5
sodium hydrogen sulfite
ammonium perchlorate
chromium(III) sulfate
3. Mole Conversions (1 mole = 6.02 X 1023 items) particles → moles → mass
What is the mass of 0.250 mole of sodium? How many sodium atoms is this?
How many moles of carbon dioxide are in 225g?
How many molecules of water are in 4.68 mole water?
How many sulfate ions are in 86.2 g of aluminum sulfate?
How many molecules are in 37.0 mL of ethanol, C2H5OH, d = 0.789 g/mL?
What is the mass of 1.75 X 1034 aluminum atoms?
4. Percent Composition
a. Calculate the mass percent (percent by mass) of each element in ammonium nitrate, ammonium
sulfate, and urea CO(NH2)2. On a kilogram per kilogram basis, which would be the best choice
for fertilizer?
b. How many grams of nitrogen are present in 46.34 g of ammonium nitrate?
5. Empirical and Molecular Formulas from Percent Composition.
The process:
Assume 100 g sample → percents become grams
Convert to moles
Write a “stupid-looking formula” with moles determined above as subscripts
Get integers for subscripts by dividing all subscripts in your SLF by the smallest subscript
If the subscripts are still non-integers, multiply all of them by the smallest number that will
convert them to integers. This is the Empirical Formula.
If finding the molecular formula, one more piece of data is needed – the molecular weight.
Find the ratio between the molecular mass and the empirical formula mass – the integral
value obtained is the multiplier factor the converts the subscripts of the EF to those of the
MF.
a. Cyclohexanol, used in the manufacture of plastics, has the mass percent composition: 71.95%
carbon, 12.08% hydrogen and 15.97% oxygen. What is its empirical formula?
b. TNT has the mass percent composition: 37.00% C, 2.20% H, 18.50% N, and 42.23% O, by
mass. Find its empirical formula.
c. The empirical formula of paradichlorobenzene, used as a moth repellant, is C3H2Cl. Its
molecular mass is 147 u. What is its molecular formula?
d. Resorcinol, used in the manufacture of resins, drugs and other products is 65.44% C, 5.49% H
with the remainder being oxygen. Its molecular mass is 110 amu. What is its molecular
formula?
6. Non-limiting reactant/non-solution Stoichiometry (consult your text for information on limiting
reactant problems. Also consult youtube.com)
a. The final step in the production of nitric acid involves the reaction of nitrogen dioxide with
water. Another product is nitrogen monoxide. How many grams of nitric acid are produced
for every 100.0 g of nitrogen dioxide that reacts?
b. Upon being strongly heated or subjected to severe mechanical shock, ammonium nitrate
decomposes into nitrogen and oxygen gases and water vapor. If 75.5 grams of ammonium
nitrate decomposes, how many grams of each product is made?
c. How many milliliters of liquid water should be produced by the combustion of 775 mL octane
in abundant oxygen? Assume that the volumes of both liquids are measured at 20˚C, where
the densities are 0.7025 g/mL for octane and 0.9982 g/mL for water.
Skeleton: C8H18 (1) + O2 (g) → CO 2(g) + H2O(l)
d. Lead(II) oxide reacts with ammonia, forming solid lead, nitrogen gas and liquid water.
How many grams of ammonia are consumed in the reaction of 75.0 g lead(II) oxide?
If 56.4 g of lead are produced, how many grams of nitrogen are also formed?
e. Ordinary chalkboard chalk is solid mixture with limestone (calcium carbonate) and gypsum
(calcium sulfate) as its principal ingredients. The limestone dissolves in dilute hydrochloric
acid, producing calcium chloride, carbon dioxide and water. Gypsum does not react with
HC1. If a 5.05 g piece of chalk that is 72.0% calcium carbonate is dissolved in excess HC1,
what mass of carbon dioxide will be produced?
Determine the mass percent of calcium carbonate in a 4.38 g piece of chalk that yields 1.31 g
carbon dioxide when it reacts with excess HC1.
Questions: