Download Summer Assignment

Summer Assignment
Please Note: This assignment is a requirement, and is NOT for extra credit!
1. Purchase your own copy of 5 Steps to a 5 on the AP: Chemistry, John T Moore,
McGraw Hill, 2008-2009 Edition.
2. Buy a few color highlighters.
3. Read and study Chapter 1 and 2. Highlight material that applies to you.
4. Take the diagnostic test on Page 23. (Go ahead and write in the book, I will make
an additional copy of this test for you to take before the AP Exam.)
5. Take a look at the AP and other websites. List the three most useful in the front
cover of your book
6. Read and study (highlight, take notes in the margin, etc) and do all the review
questions at the end of the chapter for Chapter 3 (Basics) and Chapter 5
(Stoichiometry)
7. Bring your highlighted book, notes and diagnostic test to school the first day of class
in August. Points will be assigned to you and then the book will be returned to you
for your further enjoyment.
NO LATE ASSIGNMENTS WILL BE ACCEPTED!!!
AP CHEMISTRY FIRST DAY TEST
AP Chemistry is a difficult course. 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. The first day test 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. Solubility Rules
6. Determining Oxidation Numbers
If this seems like too much work for the summer, please drop the course. Advanced
Placement Chemistry is a college level course. You will need to be dedicated and work very
hard if you are to be successful.
Rules for Naming an Acid
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
Cl- is the Chloride ion so HCl = hydrochloric acid
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
ClO2- is the Chlorite ion so HClO2 = Chlorous acid.
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
ClO3- is the Chlorate ion so HClO3 = Chloric acid.
Rules for Naming Ionic Compounds
1. Balance Charges (charges should equal zero)
2. Cation is always written first (in name and in formula)
3. Change the ending of the anion to -ide
Solubility Rules
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+.
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 O.
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 O.
9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the
ion.
Examples: (use your periodic table, group #’s are columns)
CO: (Sum will equal 0 since it is a neutral molecule)
O will have a -2 ox. number.
1C+1O=0
(C?) + (-2) = 0
C? = +2
Oxidation number of C in CO is +2
Oxidation number of O in CO is -2 (known)
Check ox. number to see if it falls within range:
+2 is in between the maximum value of C, +4, (Group #) and the minimum value of C, 4, (Group # - 8).
So okay.
Cr2O72-: (Sum of all oxidation numbers will equal -2 since it is an ion.)
2 Cr + 7 O = -2
2(Cr?) + 7(-2) = -2
2(Cr?) + (-14) = -2
2(Cr?) = +12
Cr? = +6
Oxidation number of each Cr in Cr2O72- is +6
Oxidation number of each O in Cr2O72- is -2 (known)
Check ox. number to see if it falls within range:
+6 is the maximum value that Cr can have (Group#). So okay.
CS2: (Sum will equal 0 since it is a neutral molecule)
C will have the positive oxidation number since it is less EN than S
S will have a -2 charge since it is Gr # 6, (6 - 8 = -2)
C+2S=0
(C?) + 2 (-2) = 0
(C?) + (-4) = 0
C? = +4
Oxidation number of C in CS2 is +4
Oxidation number of each S in CS2 is -2 (known)
Check ox. number to see if it falls within range:
+4 is the maximum value that C can have, (Gr#). So okay.
NH4+: (Sum will equal +1 since it is an ion)
H will have a +1 ox. number since it is bonded to N, a nonmetal.
N + 4 H = +1
(N?) + 4(+1) = +1
N? = -3
Oxidation number of N in NH4+ is -3
Oxidation number of each H in NH4+ is +1 (known)
Check ox. number to see if it falls within range:
-3 is the minimum value that N can have, (Group # - 8). So okay.
H5IO6: (Sum will equal 0 since it is neutral species.)
H will have a +1 ox. number since it is combined w/ nonmetals
Iodine will have a + charge since it is less EN than Oxygen
5H+I+6O=0
5(+1) + (I?) + 6(-2) = 0
(+5) + (I?) + (-12) = 0
(I?) + (-7) = 0
I? = +7
Oxidation number of I in H5IO6 is +7
Oxidation number of each H in H5IO6 is +1 (known)
Oxidation number of each O in H5IO6 is -2 (known)
Check ox. number to see if it falls within range:
+7 is the maximum value that I can have, (Gr#). So okay.
NaBH4: (Sum will equal 0 since it is neutral species.)
H will have a -1 ox. number since it is combined w/ metals
Na will have a +1 charge (+ Gr# = +1)
Na + B + 4 H = 0
(+1) + (B?) + 4(-1) = 0
(+1) + (B?) + (-4) = 0
(B?) + (-3) = 0
B? = +3
Oxidation number of B in NaBH4 is +3
Oxidation number of each Na in NaBH4 is +1 (known)
Oxidation number of each H in NaBH4 is -1 (known)
Check ox. number to see if it falls within range:
+3 is the maximum value that B can have, (Gr#). So okay.
H2MnO4: (Sum will equal 0 since it is neutral species.)
H is a +1 ox. number since it is combined w/ nonmetals (ignore metal)
Mn will have a + charge since it is less EN than Oxygen
2 H + Mn + 4 O = 0
2(+1) + (Mn?) + 4(-2) = 0
(+2) + (Mn?) + (-8) = 0
(Mn?) + (-6) = 0
Mn? = +6
Oxidation number of Mn in H2MnO4 is +6
Variable Valences For Transition Metals
Name
Chromium
Cr
+2
Stock Name
Chromium (II)
Manganese
Mn
+3
+2
Chromium (III)
Manganese (II)
Iron
Fe
+3
+2
Manganese (III)
Iron (II)
Co
+3
+2
Iron (III)
Cobalt (II)
Copper
Cu
+3
+1
Cobalt (III)
Copper (I)
Lead
Pb
+2
+2
Copper (II)
Lead (II)
Mercury
Hg
+4
+1
Lead (IV)
Mercury (I)
Sn
+2
+2
Mercury (II)
Tin (II)
Gold
Au
+4
+1
Tin (IV)
Gold (I)
Silver
Ag
+3
+1
Gold (III)
Silver
Bismuth
Bi
+3
Bismuth (III)
Antimony
Sb
+5
+3
Bismuth (V)
Antimony (III)
Cadmium
Cd
+5
+2
Antimony (V)
Cadmium
Zinc
Zn
+2
Zinc
Cobalt
Tin
Symbol
Charge
Polyatomic Ions
Name
ammonium
acetate
bromate
chlorate
chlorite
cyanide
dihydrogen phosphate
hypochlorite
hydrogencarbonate(bicarbonate)
hydrogen sulfate (bisulfate)
hydrogen sulfite (bisulfite)
hydroxide
iodate
nitrate
nitrite
perchlorate
permanganate
thiocyanate
carbonate
chromate
dichromate
oxalate
selenate
silicate
sulfate
sulfite
phosphate
phosphite
Symbol
NH4
C2H3O2
BrO3
ClO3
ClO2
CN
H2PO4
ClO
HCO3
HSO4
HSO3
OH
IO3
NO3
NO2
ClO4
MnO4
SCN
CO3
CrO4
Cr2O7
C2O4
SeO4
SiO3
SO4
SO3
PO4
PO3
Charge
+1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-1
-2
-2
-2
-2
-2
-2
-2
-2
-3
-3
1. Write 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. PCl3 _______________________
v. sodium thiocyanate ___________
v. NaCN ______________________
w. nitrous acid _________________
w. HF _______________________
2. Find the mass percent (percent compostion) of nitrogen in each of the following
compounds:
a. NO
b. NO2
c. N2O4
d. N2O
3. Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol.
Analysis shows the compound to be 7.74 % by mass. Find the empirical and molecular
formulas of benzene.
4. 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 12.25 grams of
calcium carbonate at STP?
d. What is the volume of carbon dioxide in (c) if the pressure is pressure is
785mm Hg and the temperature is 30oC? (R =62.4 mm x L/mol x K)
5. Hydrogen gas and 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)?
6. 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.