Name: ________________________
Oregon City High School AP Chemistry Summer Assignment
Welcome to AP chemistry! This homework is meant to be a review of the material covered in Chemistry A and B as well as some
memorization of ions and solubility rules that you will need throughout the year. Having the following skills will be essential to your
success in AP Chemistry and I will expect that you already have a firm grasp on these topics as we start the year. The following
assignment is to be completed over the summer and brought in COMPLETED on the first day of class.
AP Chemistry is a challenging course. While it is not all about memorization, having these items memorized is essential for
success in learning the concepts covered in the course. I have included several resources in this packet.
1.
There is a list of the ions that you must know on the first day. Utilize the suggestions for making the process of
memorization easier. For instance, many of you will remember that most of the monatomic ions have charges that are
directly related to their placement on the periodic table. There are naming patterns that greatly simplify the learning of
the polyatomic ions as well. I have included a sheet of flashcards for the polyatomic ions that you must learn. I strongly
suggest that you cut them out and begin memorizing them immediately. Use the hints on the common ions sheet to help
you reduce the amount of memorizing that you must do.
**There will be a test on the first day of class to assess your knowledge of these polyatomic ions… Please be prepared!!!
2.
Memorize the solubility rules and be able to identify whether a substance will break into ions when dissolved in water.
**There will be a test on the first day of class to assess your knowledge of these solubility rules… Please be prepared!!!
3.
There are a number of questions that are meant to help you review the information that you learned in Chemistry A and B
and will be expected to know as we begin AP chemistry. These questions will be DUE ON THE FIRST DAY OF
CLASS!!!
While you may need to reference materials to help remind you how to do some of these problems (your notes from chemistry A
and B, your AP Chemistry textbook, the internet, etc.) please make sure that your work is YOUR OWN as you will be the one
responsible for understanding this information.
Also included is a copy of the periodic table used in AP Chemistry. Notice that this is not the table used in first year chemistry.
The AP table is the same that the College Board allows you to use on the AP Chemistry test. Notice that it has the symbols of
the elements but not the written names. You need to take that fact into consideration when studying for the afore-mentioned
quiz!
Do not let the fact that there are no flashcards for monatomic ions suggest to you that the monatomic ions are not
important. They are every bit as important as the polyatomic ions. If you have trouble identifying the charge of monatomic ions
(or the naming system) then I suggest that you make yourself some flashcards for those as well.
Doubtless, there will be some students who will procrastinate and try to do all of this studying just before the start of
school. Those students may even cram well enough to do well on the initial quiz. However, they will quickly forget the ions,
and struggle every time that these formulas are used in lecture, homework, quizzes, tests and labs. All research on human
memory shows us that frequent, short periods of study, spread over long periods of time will produce much greater retention
than long periods of study of a short period of time.
I could wait and throw these at you on the first day of school, but I don’t think that would be fair to you. Use every
modality possible as you try to learn these – speak them, write them, visualize them. Make flashcards, form a study group, have
your friends and family quiz you, take the lists with you on vacation, or do whatever it takes to get this information imbedded in
your head.
I look forward to seeing you all at the beginning of the next school year. If you need to contact me during the summer, you can
call or email me and I will get back to you quickly.
Jenaya Hoffman
OCHS Chemistry Teacher
[email protected]
503-704-9909
1. Nomenclature
Rules for Naming Ionic Compounds (metal +nonmetal)
A. Balance Charges (charges should net zero)
B. Cation is always written first (in name and in formula)
C. Change the ending of the anion to –ide (unless polyatomic ion, then named as given).
I. Name these binary compounds of two nonmetals.
IF7__________________________
N2O5____________________________
N2O4________________________
As4O10___________________________
PCl3_________________________
S2Cl2____________________________
XeF2 _____________________________
SF6_______________________________
II. Name these binary compounds with a fixed charge metal.
AlCl3 _______________________
MgO____________________________
KI__________________________
SrBr2 ___________________________
CaF2 ________________________
Al2O3___________________________
BaI2______________________________
Na2S _____________________________
III. Name these binary compounds of cations with variable charge (use roman numerals).
CuCl2 ______________________
Fe2O3____________________________
SnO______________________________
PbCl4_______________________
Cu2S_____________________________ HgS______________________________
AuI3________________________
CoP_____________________________
IV. Name these compounds with polyatomic ions.
Fe(NO3)3_________________________ NaOH__________________________
Ca(ClO3)2________________________ KNO2__________________________
NH4NO2_________________________ Cu2Cr2O7 _______________________
Cu2SO4___________________________
NaHCO3__________________________
Acids-For simplicity, the acids that we will be concerned with naming are really just a special class of ionic compounds where the
cation is always H+. So if the formula has hydrogen written first, then this usually indicates that the hydrogen is an H+ cation
and that the compound is an acid. When dissolved in water, acids produce H+ ions (also called protons, since removing the
single electron from a neutral hydrogen atom leaves behind one proton).
Rules for Naming an Acid
A. 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
HCl ________________________
H2S _______________________
HI _________________________
HF _______________________
B. 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.
C. 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.
**I like to remember this rule as “I ate something and it was icky.”
I.
HNO3, which contains the polyatomic ion nitrate, is called nitric acid.
HNO2, which contains the polyatomic ion nitrite, is called nitrous acid.
Name the following acids using the correct naming rule.
HClO4__________________________
H2SO4__________________________ HC2H3O2_________________________
H3PO4__________________________
HNO2__________________________ H2CrO4__________________________
H2C2O4_________________________
H2CO3__________________________
II. Name these compounds appropriately.
Hint: some of these compounds are covalently bonded (nonmetal + nonmetal) so you will have to use prefixes to indicate
how many of each element is in the compound: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-.
CO____________________________ NH4CN _________________________
HIO3__________________________
NI3____________________________ AlP ____________________________
OF2___________________________
LiMnO4________________________ HClO __________________________
SO2___________________________
CuCr2O7_______________________
K2O____________________________
HF____________________________
FeF3__________________________
KC2H3O2________________________
MnS__________________________
III. Write the chemical formulas.
Tin (IV) phosphide
_____________
copper (II) cyanide
____________
Magnesium hydroxide
_____________
sodium peroxide
____________
Sulfurous acid
_____________
lithium silicate
____________
Potassium nitride
_____________
chromium (III) carbonate ____________
Gallium arsenide
_____________
cobalt (II) chromate
____________
Zinc fluoride
_____________
dichromic acid
____________
2. Composition
Complete the following problems showing all work.
1. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting magnesium oxide weighed 1.560
grams. Determine the percent composition of each element in the compound.
2. Determine the empirical formula given the following data for each compound:
a) Fe = 63.53%, S = 36.47%
b) Fe = 46.55%, S = 53.45%
3. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound.
3. Solubility rules
I. Review solubility rules and identify each of the following compounds as soluble or insoluble in water. You must memorize
the solubility rules given in this packet. You may want to spend time memorizing the solubility rules before you compete
the next two sections, try them without using your solubility chart, and then check them using the chart.
Na2CO3
___________
CoCO3
_____________
Pb(NO3)2
_____________
K 2S
___________
BaSO4
_____________
(NH4)2S
_____________
AgI
___________
Ni(NO3)2
_____________
KI
_____________
FeS
___________
PbCl2
_____________
CuSO4
_____________
Li2O
___________
Mn(C2H3O2)2
_____________
Cr(OH)3_
_____________
AgClO3
___________
Sn(SO3)4
_____________
FeF2
_____________
II. Write out the balanced chemical equation for each of the following double replacement reactions. Predict whether each of
these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the
precipitate.
silver nitrate and potassium chloride
____________
magnesium nitrate and sodium carbonate
____________
strontium bromide and potassium sulfate
____________
cobalt (III) bromide and potassium sulfide
____________
ammonium hydroxide and copper (II) acetate
____________
lithium chlorate and chromium (III) fluoride
____________
4. Balancing Equations
I. Balance the following equations with the lowest whole number coefficients.
____S8
+ ____ O2
 ____ SO3
____C10H16 + ____ Cl2
 ____ C
____Fe
 ____ Fe2O3
+ ____ O2
____C7H6O2 + ____ O2
____KClO3  ____ KCl
 ____CO2
+ ____ HCl
+ ____ H2O
+ ____ O2
____H3AsO4 ____As2O5 + ____ H2O
____V2O5
+ ____ HCl
 ____VOCl3
+ ____ H2O
____Hg(OH)2 + ____ H3PO4  ____ Hg3(PO4)2 + ____ H2O
II. Balance the following equations and indicate the type of reaction taking place:
+ ____ H3PO4

1)
____ NaBr
2)
____ Ca(OH)2 + ____ Al2(SO4)3 
3)
____ Mg
+ ____ Fe2O3
4)
____ C2H4
+ ____ O2
5)
____ PbSO4
____ PbSO3
6)
____NH3
+____I2
____ Na3PO4 + ____ HBr
Type of reaction: ____________________
____ CaSO4 + ____ Al(OH)3
Type of reaction: ____________________

____ Fe
+ ____ MgO
Type of reaction: ____________________

____ CO2
+ ____ H2O
Type of reaction: ____________________
+
____ O2

____N2I6
Type of reaction: ____________________
+ ____H2
Type of reaction: ____________________
5. Stoichiometry and Limiting Factor
1. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide?
Na2O + H2O  2NaOH
2.
2NaClO3  2NaCl + 3O2
What mass of sodium chloride is formed along with 45.0g of oxygen gas?
3. 4NH3 + 5O2  4NO + 6 H2O
What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen?
4.
If the reaction in #3 is done with 25.0g of each reactant, which would be the limiting factor?
5. Na2S + 2AgNO3  Ag2S + 2NaNO3
If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate, which is the limiting factor?
What mass of the excess reactant remains?
What mass of silver sulfide would precipitate?
6. 6NaOH + 2Al  2Na3AlO3 + 3H2
What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of aluminum?
You will need to memorize this first table for the rest of the year… start memorizing over the summer!
SOLUBILITY GUIDELINES
Compounds
Solubility
Exceptions
Salts of alkali metals (group 1A) and
Soluble
Some lithium compounds
ammonium (NH4+)
All nitrate, chlorate and acetate salts
Soluble
Sulfate salts
Soluble
Cation is Pb, Ag, Hg, Ba, Sr, or Ca
Halide (group 7A halogen ions) salts
Soluble
Cation is Ag, Hg or Pb
Acids (H in front)
Soluble
carbonates, phosphates, chromates,
Cation is alkali metal (group 1A) or
Insoluble
sulfides, hydroxides and oxides
ammonium
*salts = ionic compounds
SOLUBILITY CHART
sulfide
sulfate
phosphate
soluble
Perchlorate
I
S
S
S
I
I
I
S
I
S
S
S
I
Oxide
S
S
S
S
S
S
S
S
S
S
I
S
S
S
Nitrate
Hydroxide
S
S
S
S
S
S
S
S
S
S
S
S
S
S
Iodide
Chloride
S
S
S
S
S
S
S
I
S
S
I
S
S
S
S
I
S
S
S
S
sS
S
S
I
S
S
S
sS
I
I
S
S
S
S
S
I
S
S
I
S = Soluble
Key: sS = slightly
I = insoluble
Chlorate
Carbonate
Bromide
Acetate
Al
NH4+
Ba
Ca
Cu2+
Fe2+
Fe3+
Li
Mg
K
Ag
Na
Sr
Zn
S
S
I
S
I
S
d
S
S
S
S
S
S
S
S
sS
S
I
I
d
S
S
sS
S
I
sS
I
S
S
I
S
I
S
I
S
S
I
S
I
S
I
S
S
I
S
I
sS
d
S
S
S
S
sS
S
S
S
S
I
S
I
S
d
S
S
S
S
S
S
S
I
S
I
S
I
sS
I
S
S
S
S
S
S
S
S
S
S
S
I
I
I
S
S
I
S
I
S
I
d = decomposes in water
- = no such compound exists
Common Ions and Their Charges
A mastery of the common ions, their formulas and their charges, is essential to success in AP Chemistry. You
are expected to know all of these ions on the first day of class, when I will give you a quiz on them. You will
always be allowed a periodic table, which makes indentifying the ions on the left “automatic.” For tips on learning
these ions, see the opposite side of this page.