Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
CPiepora@saugus.k12.ma.us
Advanced Placement Chemistry
Summer Assignment 2015
Name:
Date:
Period:
Score:
Welcome to your second year of Chemistry! I am excited to work and learn with each of you during the
2015-2016 academic year. As student and instructor, we are part of a team with one primary goal: to
prepare you for your AP Chemistry exam to be given in May of 2016. 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.
An excellent book that I recommend is: REA’s “AP Chemistry: All
Access” & “AP Chemistry: Crash Course.” It will make your
studies a lot easier and is a great summary of all the important
topics we will be covering. It includes online tests with automatic
scoring and timing, e-flashcards, quizzes and more. There are
several of these books that were left for you to use from previous
years students: First come first served.
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 which
need to be completed. Your summer assignment is due the first day of school and no exceptions will be
tolerated for any reason. 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 you will be tested on Chapters 1-3 of your text,
as well as the lists and types of problems included with your summer assignment.
You will be tested on the new 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 Honors Chemistry notes, AP
Chemistry text, fellow AP Students or the internet. If you don’t think you are working harder in AP
Chemistry than any class you have ever taken; you are probably not working hard enough. If all this
sounds like too much work, you need to rethink your commitment to AP Chemistry.
Solubility Rules: the new solubility rules are easy and a snap to remember.
The revised solubility rules for the new AP Chemistry exam make this topic much easier than in previous years.
All you need to know is that all sodium, potassium, ammonium, and nitrate salts are soluble in water.
Polyatomic Ions: You have to remember these ions and their charges too, so you can name and write the
appropriate chemical formulas. Get an early start!!!
Date Due: First Day of School
CHE255 | Summer Assignment
Page 1 of 8
Instructor: Mr. C. F. Piepora, M.S.E.S., M. Ed.
Polyatomic Ions
Name
ammonium
Symbol
acetate
C2H3O2-
bromate
BrO3-
perchlorate
ClO4-
chlorate
ClO3-
chlorite
ClO2-
hypochlorite
ClO-
dihydrogen phosphate
H2PO4-
hydrogen carbonate
(bicarbonate)
hydrogen sulfate
(bisulfate)
hydrogen sulfite
(bisulfite)
hydroxide
HCO3-
iodate
IO3-
nitrate
NO3-
nitrite
NO2-
permanganate
MnO4-
cyanide
CN-
thiocyanate
SCN-
carbonate
CO32-
chromate
CrO42-
dichromate
Cr2O72-
oxalate
C2O42-
selenate
SeO42-
silicate
SiO32-
sulfate
SO42-
sulfite
SO32-
peroxide
O22-
phosphate
PO43-
phosphite
PO33-
Date Due: First Day of School
CPiepora@saugus.k12.ma.us
NH4+
HSO4HSO3OH-
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 metals with hydroxide (OH-) groups.
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. electrolysis of aluminum oxide
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 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