Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
AP Chemistry | Summer Assignment
Welcome to your second year of Chemistry! I am excited to work and learn with each of you during the
academic year. As student and instructor, we are part of a team with one primary goal: to prepare you for the
AP Chemistry Exam which is given at the beginning of May. To get us started toward this goal, I am assigning
some problems to be worked over the summer to keep your first year of chemistry “fresh” and to reinforce key
topics.
Two excellent books that I recommend highly are: REA’s “AP
Chemistry: All Access” and REA’s “AP Chemistry: Crash Course”.
These will make your studies a lot easier and are a great summary of
all the important topics we will be covering. Included are online tests
with automatic scoring and timing, e-flashcards, quizzes and more.
Your summer assignment will be a combination of lists to be memorized and problems
dealing with first three chapters in your AP Chemistry textbook dealing with naming compounds and
stoichiometry. Your summer assignment is due on the first day of school. All links have been checked
and are working perfectly.
Chapter 1: Introduction - Matter & Measurement
Chapter 2: Atoms, Molecules & Ions
Chapter 3: Stoichiometry
During the first week of school after a review of the material, you will be tested on Chapters 1-3
Along with the lists and problems included with your summer assignment.
You will be tested on solubility rules, polyatomic ions and charges, ionic & covalent nomenclature and
identifying, balancing and writing chemical reactions from the chemical names of the reactants, and
hydrocarbon functional groups. If you need help turn to your Chemistry notes, AP Chemistry text, fellow
AP Students or the internet.
Date Due: First Day of School
CHE255 | Summer Assignment
Page 1 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
Solubility Rules & Polyatomic Ions:
Polyatomic Ions
Name
Symbol
Name
Symbol
ammonium
NH4+
permanganate
MnO4-
acetate
C2H3O2-
cyanide
CN-
bromate
BrO3-
thiocyanate
SCN-
perchlorate
ClO4-
carbonate
CO32-
chlorate
ClO3-
chromate
CrO42-
chlorite
ClO2-
dichromate
Cr2O72-
hypochlorite
ClO-
oxalate
C2O42-
dihydrogen phosphate
hydrogen carbonate
(bicarbonate)
hydrogen sulfate
(bisulfate)
hydrogen sulfite
(bisulfite)
hydroxide
H2PO4-
selenate
SeO42-
HCO3-
silicate
SiO32-
HSO4-
sulfate
SO42-
HSO3-
sulfite
SO32-
OH-
peroxide
O22-
iodate
IO3-
phosphate
PO43-
nitrate
NO3-
phosphite
PO33-
nitrite
NO2-
hydride
H-
Date Due: First Day of School
CHE255 | Summer Assignment
Page 2 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
I. Chemical Formulas: A helpful website: http://www.kentchemistry.com/links/naming/formulawriting.htm
1. Write formulas for the following:
2. Name each of the following:
a. barium sulfate
_________________________
a. NH4Cl
_________________________
b. copper(I) sulfate
_________________________
b. PCl3
_________________________
c. chlorine monoxide
_________________________
c. Li3N
_________________________
d. silicon tetrachloride _________________________
d. BaSO3
_________________________
e. magnesium fluoride
_________________________
e. N2F4
_________________________
f. sodium oxide
_________________________
f. KClO3
_________________________
g. sodium peroxide
_________________________
g. NaH
_________________________
h. copper(I) oxide
_________________________
h. (NH4)2Cr2O7 _________________________
i. zinc sulfide
_________________________
i. HNO3
_________________________
j. potassium carbonate _________________________
j. Sr3P2
_________________________
k. hydrobromic acid
_________________________
k. Mg(OH)2
_________________________
l. perchloric acid
_________________________
l. Al2S3
_________________________
m. lead(II) acetate
_________________________
m. AgBr
_________________________
n. sodium permanganate_________________________
n. P4O10
_________________________
o. lithium oxalate
_________________________
o. HC2H3O2
_________________________
p. potassium cyanide
_________________________
p. CaI2
_________________________
q. iron (III) hydroxide
_________________________
q. MnO2
_________________________
r. silicon dioxide
_________________________
r. Li2O
_________________________
s. nitrogen trifluoride
_________________________
s. FeI3
_________________________
t. chromium(III) oxide
_________________________
t. Cu3PO4
_________________________
u. calcium chlorate
_________________________
u. PCl5
_________________________
v. sodium thiocyanate
_________________________
v. NaCN
_________________________
w. nitrous acid
_________________________
w. HF
_________________________
Date Due: First Day of School
CHE255 | Summer Assignment
Page 3 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
II. Stoichiometry: Show all of your work for the following problems:
You may find the following websites helpful:
http://www.chemtutor.com/mols.htm
http://www.chem.tamu.edu/class/majors/tutorialnotefiles/limiting.htm
http://www.ausetute.com.au/idealgas.html
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 % hydrogen by mass. Find the empirical and molecular formulas of benzene.
3. Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide.
a. Write a balanced chemical equation for this reaction.
b. How many grams of calcium oxide will be produced after 12.25 grams of calcium carbonate are
completely decomposed?
c. What is the volume of carbon dioxide gas produced from 12.25 grams of calcium carbonate at
STP?
d. What is the volume of carbon dioxide in L if the pressure is 785mm Hg and the temperature is
30°C? (R =62.4 mmHg•L/mol•K)
Date Due: First Day of School
CHE255 | Summer Assignment
Page 4 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
4. Molecular hydrogen gas and molecular 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 reagent?
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)?
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 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.
Date Due: First Day of School
CHE255 | Summer Assignment
Page 5 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
III. Chemical Reactions
In AP Chemistry, most of the reaction we write are called “net ionic.” But before we can do that, you need
to review and memorize some basic reaction types. For some basic review, go to the following website:
http://misterguch.brinkster.net/6typesofchemicalrxn.html
Now try naming the type of chemical reaction of these sample problems from the website:
1) NaOH + KNO3 → NaNO3 + KOH
_____________________________________________
2) CH4 + 2 O2 → CO2 + 2 H2O
_____________________________________________
3) 2 Fe + 6 NaBr → 2 FeBr3 + 6 Na
_____________________________________________
4) CaSO4 + Mg(OH)2 → Ca(OH)2 + MgSO4
_____________________________________________
5) NH4OH + HBr → H2O + NH4Br
_____________________________________________
6) Pb + O2 → PbO2
_____________________________________________
7) Na2CO3 → Na2O + CO2
_____________________________________________
You will also need to learn which acids and bases are strong and which are weak.
Strong acids are: HCl, HBr, HI, HNO3, HClO4 and H2SO4. All other acids are considered weak.
Strong bases are group 1A or 2A metal with hydroxide (OH-) groups.
See this document online: http://spiepho.sbc.edu/worksheets/Gen_Chem_2/Chp15,Acids_and_Bases.doc
Learn these types of decomposition reactions:
1. Metallic carbonates, when heated, form metallic oxides and CO2(g).
eg. CaCO3(s) → CaO(s) + CO2(g)
2. Most metallic hydroxides, when heated, decompose into metallic oxides and water.
eg. Ca(OH)2(s) → CaO(s) + H2O(g)
3. Metallic chlorates, when heated, decompose into metallic chlorides and oxygen.
eg. 2KClO3(s) → 2KCl(s) + 3O2(g)
4. Some acids, when heated, decompose into nonmetallic oxides and water.
eg. H2SO4 → H2O(l) + SO3(g)
5. Some oxides, when heated, decompose.
eg. 2HgO(s) → 2Hg(l) + O2(g)
6. Some decomposition reactions are produced by electricity.
eg. 2H2O(l) → 2H2(g) + O2(g)
eg. 2NaCl(l) → 2Na(s) + Cl2(g)
Date Due: First Day of School
CHE255 | Summer Assignment
Page 6 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
Now try these: (Rewrite as a balanced chemical equation and predict the products formed):
1. barium hydroxide (heated)
___________________________________________________________________________________________________________
2. sodium carbonate (heated)
___________________________________________________________________________________________________________
3. lithium chlorate (heated)
___________________________________________________________________________________________________________
4. an electric current is passed through water (electrolyis)
___________________________________________________________________________________________________________
5. sulfuric acid heated gently
___________________________________________________________________________________________________________
Learn these types of synthesis reactions:
1. Metal + oxygen → metal oxide
eg. 2Mg(s) + O2(g) → 2MgO(s)
2. Nonmetal + oxygen → nonmetallic oxide
eg. C(s) + O2(g) → CO2(g)
3. Metal oxide + water → metallic hydroxide
eg. MgO(s) + H2O(l) → Mg(OH)2(s)
4. Nonmetallic oxide + water → acid
eg. CO2(g) + H2O(l) → H2CO3(aq)
5. Metal + nonmetal → salt
eg. 2 Na(s) + Cl2(g) → 2NaCl(s)
6. A few nonmetals combine with each other
eg. 2P(s) + 3Cl2(g) → 2PCl3(g)
Now try these: (Rewrite as a balanced chemical equation and predict the products formed):
1. magnesium burned in oxygen
_______________________________________________________________________________________________________________________
2. hydrogen gas + nitrogen gas
________________________________________________________________________________________________________________________
3. sulfur burned (complete combustion)
________________________________________________________________________________________________________________________
4. calcium oxide added to water
________________________________________________________________________________________________________________________
Date Due: First Day of School
CHE255 | Summer Assignment
Page 7 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
Organic Chemistry - Just the basics: http://www.visionlearning.com/library/module_viewer.php?mid=60
Hydrocarbon
prefix
# of
Carbon
Atoms
Meth
Eth
Prop
But
Pent
Hex
Hept
Oct
Non
Dec
1
2
3
4
5
6
7
8
9
10
Date Due: First Day of School
CHE255 | Summer Assignment
Page 8 of 8