WELCOME TO AP CHEMISTRY!!!
School Year 2011-2012
Hi! My name is Ms. Scheffel. I will be your AP Chemistry teacher next school year. As the school year
is coming to an end, I wanted to get out some information about class for next school year. I am
excited to meet all of you and begin another fun year of AP Chemistry. Over the summer I have an
assignment that I would like you to complete. It is a twofold assignment, see below.
I will be at school over the summer if you want to come in and work with me on the assignment. I
also suggest meeting with others that have signed up for the class so you can work on the assignment
together. There will be a quiz the first day of class so please make sure you see me or use your study
guide to get your questions answered.
AP CHEMISTRY SUMMER ASSIGNMENT
Please Note: This assignment is a requirement, and is NOT for extra credit!
1. Purchase
a. Study Guide: AP Achiever, Chemistry, McGraw Hill, ISBN 978-0-07-892839
(There may be a new version coming out this summer. Best place to purchase this study
guide is online or from one of my previous students. If you are unable to purchase the
study guide please let me know. I have some copies for students to borrow.)
b. Buy color highlighters and sticky notes to mark up your study guide.
2. Read and study Chapter 1-3 in study guide. Highlight and uses sticky notes for the material
that applies to you.
a. Bring your highlighted study book and notes. Points will be assigned to you and then the
book will be returned to you for your further enjoyment.
3. Go to school website and printout the summer assignment. (Or you can email me and I will
send it to you.)
a. Make flashcards
b. Complete naming and writing formulas, and simple stoich problems.
Please feel free to stop in and see me before the end of the school year with any questions that you
may have or email me this summer if you would like to meet for some additional help.
Thank you!
[email protected]
Once you have opened and printed out the summer homework…
Please email me. I would like to start an email list for all those who are
registered for AP Chemistry.
[email protected]
Welcome to AP Chemistry! Most of you already have a background in chemistry from your
Chemistry or Honors chemistry class, but AP Chemistry is very different. Rather than memorizing
how to do particular types of problems, you must really understand the chemistry and be able to
apply it to all sorts of different situations.
It is not all about memorization; however, having these items memorized is essential for success in
learning the concepts covered in the course. Make flashcards, have your friends and family quiz you,
take the lists with you on vacation, or do whatever it takes to get this information firmly planted in
your head. Do not wait until the night before school begins.
NO LATE ASSIGNMENTS WILL BE ACCEPTED!!!
AP CHEMISTRY FIRST WEEK QUIZ
The first week quiz will cover six areas of memorization:
1. Polyatomic Ions (including name, symbol and charge)
2. Variable Valences for Transition Metals
3. Rules for Naming Acids
4. Rules for Naming Ionic Compounds
5. The Solubility Rules
6. Determining Oxidation Numbers
Rules for Determining Oxidation Number
Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion that
indicates the general distribution of electrons among the bonded atoms.
1. The oxidation number of any uncombined element is 0.
2. The oxidation number of a monatomic ion equal the charge on the ion.
3. The more electronegative element in a binary compound is assigned the number equal to the
charge it would have if it were an ion.
4. The oxidation number of fluorine in a compound is always –1
5. Oxygen has an oxidation number of –2 unless it is combined with F, when it is +2, or it is in a
peroxide, when it is –1.
6. The oxidation state of hydrogen in most of its compounds is+1 unless it combined with a metal, in
which case it is –1.
7. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number of +1,
+2, and +3, respectively
8. The sum of the oxidation numbers of all atoms in a neutral compound is 0.
9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion.
Solubility Rules
NaClNOSO
1. All compounds containing alkali metal cations and the ammonium ion are soluble.
2. All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.
3. All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+.
4. All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
5. All hydroxides are insoluble except compounds of the alkali metals, Ca2+, Sr2+, and Ba2+.
6. All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble except those that also
contain alkali metals or NH4+.
Variable Valences for Transition Metals
Name
Symbol
Chromium
Cr
Manganese
Mn
Iron
Fe
Cobalt
Co
Copper
Cu
Lead
Pb
Mercury
Hg
Tin
Sn
Gold
Au
Silver
Ag
Bismuth
Bi
Antimony
Sb
Cadmium
Zinc
Cd
Zn
Charge
+2
+3
+2
+3
+2
+3
+2
+3
+1
+2
+2
+4
+1
+2
+2
+4
+1
+3
+1
+3
+5
+3
+5
+2
+2
Stock Name
Chromium (II)
Chromium (III)
Manganese (II)
Manganese (III)
Iron (II)
Iron (III)
Cobalt (II)
Cobalt (III)
Copper (I)
Copper (II)
Lead (II)
Lead (IV)
Mercury (I)
Mercury (II)
Tin (II)
Tin (IV)
Gold (I)
Gold (III)
Silver
Bismuth (III)
Bismuth (V)
Antimony (III)
Antimony (V)
Cadmium
Zinc
Rules for Naming an Acid
1. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-, the stem of
the anion has the suffix –ic and it is followed by the word acid.
-ide becomes hydro _____ic Acid
Example: Cl- is the chloride ion so HCl = hydrochloric acid
2. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous,
followed by the word acid.
-ite becomes ______ous Acid
Example: ClO2- is the chlorite ion so HClO2. = chlorous acid.
3. When the anion name ends in –ate, the acid name is the stem of the anion with the suffix –ic,
followed by the word acid.
-ate becomes ______ic Acid
Example: ClO3- is the chlorate ion so HClO3 = chloric acid.
Strong Acids
HCl, HI, HBr, HClO4, HNO3, H2SO4
Polyatomic Ions
Name
ammonium
acetate
perbromate
bromate
bromite
hypobromite
perchlorate
chlorate
chlorite
hypochlorite
periodate
iodate
iodite
hypoiodite
cyanide
dihydrogen phosphate
hydrogen carbonate
hydrogen sulfate
hydrogen sulfite
hydrogen sulfide
hydroxide
nitrate
nitrite
permanganate
thiocyanate
carbonate
chromate
dichromate
peroxide
oxalate
selenite
thiosulfate
sulfate
sulfite
phosphate
phosphite
borate
Symbol/Charge
NH4+1
C2H3O2-1
BrO4-1
BrO3-1
BrO2-1
BrO-1
ClO4-1
ClO3-1
ClO2-1
ClO-1
IO4-1
IO3-1
IO2-1
IO-1
CN-1
H2PO4-1
HCO3-1
HSO4-1
HSO3-1
HS-1
OH-1
NO3-1
NO2-1
MnO4-1
SCN-1
CO3-2
CrO4-2
Cr2O7-2
O2-2
C2O4-2
SeO4-2
S2O3-2
SO4-2
SO3-2
PO4-3
PO3-3
BO3-3
Rules for Naming Ionic Compounds
1. Balance Charges (charges should equal zero)
2. Cation is always written first (for name and formula)
3. Change the ending of the anion to –ide
START of AP Chemistry Summer Homework
Part I: Chemical Formulas
1. Write the formulas for the following:
2. Name each of the following:
a. barium sulfate__________________________
a. CuSO4__________________________________
b. ammonium chloride_____________________
b. PCl3____________________________________
c. chlorine monoxide_______________________
c. Li3N___________________________________
d. silicon tetrachloride______________________
d. BaSO3__________________________________
e. magnesium fluoride______________________
e. N2F4___________________________________
f. sodium oxide____________________________
f. KClO4__________________________________
g. sodium peroxide________________________
g. NaH___________________________________
h. copper (I) oxide_________________________
h. (NH4)2Cr2O7____________________________
i. zinc sulfide_____________________________
i. HNO2__________________________________
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__________________________________
Part II: Stoichiometry
Show all of your work for the following problems.
1. Find the mass % 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 the balanced chemical equation for this reaction.
b. How many grams of calcium oxide will be produced after 12.25 g of calcium carbonate is
completely decomposed?
c. What is the volume of carbon dioxide gas produced when 12.25 g of calcium carbonate is
decomposed at STP?
4. Hydrogen gas and bromine gas react to form hydrogen bromide gas.
a. Write the balanced chemical equation for this reaction.
b. 3.20 g of hydrogen react with 9.50 g of bromine gas. Which is the limiting reactant?
c. How many grams of hydrogen bromide gas can be produced using the amount in (b)?
d. How many grams of excess reactant are left unreacted?
5. When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen
cyanide gas and water.
a. Write the balanced chemical equations for this reaction.
b. Calculate the mass of each product produced when 225.00 g of oxygen gas is reacted with an
excess of the other two reactants.
c. If the actual yield of the experiment in (b) is 105.00 g of HCN, calculate the percent yield.