Chemistry II
Summer Homework Assignment
Name: _______________________________________________
1. Metric Conversions.
Remember 1 cm3 = 1 mL
GIVEN METRIC
UNIT
8.43 cm
1 L = 1 dm3
DESIRED METRIC UNIT
mm
2.41 x 102 cm
m
294.5 nm
cm
1.445 x 104 m
km
708 mL
L
9.005 x 10-7 L
nL
456000 cm3
L
3.45 x 10-10 L
cm3
7.60 x 1011 µg
g
0.00593 kg
mg
2. Would you expect the following atoms to gain or lose electrons when
forming ions? What ion (symbol and charge) is most likely in each case?
ELEMENT
K
Ba
P
O
Br
Rb
GAIN OR LOSE
ION FORMED
3. Chemical Nomenclature: You should be able to complete this using a periodic table
and MINIMAL help from other sources.
ITEM
A
B
C
D
E
F
G
H
I
J
K
L
M
N
O
P
Q
R
S
T
U
V
W
X
Y
Z
AA
BB
CC
DD
EE
FF
GG
HH
II
JJ
CHEMICAL FORMULA
NaBr
CaS
AlI3
CHEMICAL NAME
Strontium fluoride
Potassium nitride
Magnesium phosphide
Hg2O
FeBr3
CoS
TiCl4
Tin (II) nitride
Cobalt (III) iodide
Mercury (II) oxide
Chromium (VI) sulfide
BaSO3
NaNO2
KMnO4
K2Cr2O7
Chromium (III) hydroxide
Magnesium cyanide
Lead (IV) carbonate
Ammonium acetate
N2O4
ICl3
SO2
P2S5
Diboron trioxide
Arsenic pentafluoride
Dinitrogen monoxide
Sulfur hexachloride
HC2H3O2
H3PO3
HCl
Hydrofluoric acid
Sulfurous acid
Phosphoric acid
4. Chemical Reactions – Write and balance the following reactions.
a. Glucose (C6H12O6) reacts with oxygen gas to produce gaseous carbon
dioxide and water vapor.
b. Solid iron (III) sulfide reacts with gaseous hydrogen chloride to form solid
iron (III) chloride and hydrogen sulfide gas.
c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide
gas and solid ammonium thiocyanate (NH4SCN).
d. Aqueous solutions of lead (II) nitrate and sodium phosphate are mixed
resulting in the precipitate formation of lead (II) phosphate and aqueous
sodium nitrate as the other product.
e. Solid zinc reacts with aqueous hydrochloric acid to form aqueous zinc
chloride and hydrogen gas.
f. Aqueous calcium hydroxide is neutralized by aqueous phosphoric acid to
produce solid calcium phosphate and water.
5. Chemical Calculations – You must show the work (on a separate sheet of paper)
that leads to your answer to receive credit. Write your answers in the blanks to the
left of the question.
Remember that:1 mole element = 6.022 x 1023 atoms
1 mole compound = 6.022 x 1023 molecules or formula units
❖ molecules refer to covalent compounds while formula
units refer to ionic compounds (mathematically they
mean the same thing)
A. Bauxite, the principle ore used in the production of aluminum, has the
molecular formula of Al2O3·2H2O (aluminum oxide dihydrate).
____________ (i) What is the molar mass of bauxite?
____________ (ii) What is the mass of aluminum in 0.580 mol bauxite?
____________ (iii) How many atoms of aluminum are in 0.580 mol bauxite?
___________ (iv) What is the mass of 2.10 x 1024 formula units of bauxite?
B. Chloral hydrate (C2H3Cl3O2) is a drug formerly used as a sedative and
hypnotic.
____________ (i) Calculate the molar mass of chloral hydrate.
___________ (ii) How many moles of chloral hydrate molecules are in 500.0
g of chloral hydrate?
___________ (iii) What is the mass in grams of 2.00 x 10-2 mol chloral
hydrate?
___________ (iv) What number of chlorine atoms are in 5.00 g chloral
hydrate?
___________ (v) What mass of chloral hydrate would contain 1.00 g Cl?
___________ (vi) What is the mass of exactly 500 molecules of chloral
hydrate?
6. Stoichiometry –Show your work on a separate sheet of paper but write the
answer in the blank to the left of the question. Remember the equation must be
balanced.
A. The reaction between potassium chlorate and red phosphorus (P4) takes
place when you strike a match on a matchbox. The products are
tetraphosphorus decaoxide and potassium chloride. Answer the following
questions using this reaction.
(i) Write the balanced chemical equation for this reaction.
_________(ii) What mass of tetraphosphorus decaoxide is formed when
52.9 g of potassium chlorate reacts with an excess of red phosphorus?
________ (iii) If the reaction produces 32.5 grams of tetraphosphorus
decaoxide, what is the percent yield?
B. Phosphorus (P4) can be prepared from calcium phosphate by the following
reaction:
Ca3(PO4)2 + SiO2 + C
CaSiO3 + P4 + CO
(i) Balance the equation. [Hint: start with phosphorus]
_________ (ii) How many grams of carbon is need to react with 73.5 mg of
silicon dioxide?
_________ (iii) Phosphorite is a mineral that contains Ca3(PO4)2 plus other
non-phosphorus containing compounds. What is the maximum amount of P4
that can be produced from 1.00 kg of phosphorite if the phosphorite sample
is 75% calcium phosphate by mass? Assume an excess of the other reactants.
C. 500 g sulfuric acid reacts with 400 g barium hydroxide producing a barium
sulfate solid precipitate and water.
(i)Write and balance the equation for this reaction.
_________(ii) Determine the limiting reactant.
_________(iii) Calculate the mass of water produced.
_________(iv) Calculate the mass of the excess reactant remaining after
the reaction goes to completion.
Solubility Rules
1. All compounds containing alkali metal cations and the ammonium ion are
soluble.
2. All compounds containing nitrate, perchlorate, chlorate, and acetate ions
are soluble.
3. All chlorides, bromides, and iodides are soluble except those containing
1+
Ag , Pb2+, or Hg22+.
4. All sulfates are soluble except those containing Hg22+, Pb2+, Sr2+, Ca2+,
or Ba2+.
5. All hydroxides are insoluble except compounds of the alkali metals,
2+
Ca , Sr2+, and Ba2+.
6. All compounds containing PO43-, S2-, CO32-, and SO32- ions are insoluble
except those that also contain alkali metals or NH41+.
SOLUBLE
INSOLUBLE
Alkali metal cations (these are group I
metal ions)
Hydroxides (except: alkali metals,
ammonium, Ca+2, Sr+2, Ba+2)
Ammonium ion
Phosphates, Sulfides, Carbonates, Sulfites,
Chromates (except: alkali metals and
ammonium)
Nitrates, Perchlorates, Chlorates,
Acetates
Chlorides, Bromides, Iodides
(except: Ag+1, Pb+2, Hg22+)
Sulfates (except: Pb+2, Hg22+, Sr+2,
Ca+2, Ba+2)
Both of these have the same information just arranged in a different way. You need to
begin learning these rules. We will begin using these the first week of school and quizzes
related to this information will begin by the second week of school.
You should also know ALL of the polyatomic ions on the next page. Pay attention to those
ions ending in –ite versus – ate. You learned these in Chem I with me.
(CLO)-1
HYPOCHLORITE
(BRO)-1
HYPOBROMITE
(IO)-1
HYPOIODITE
(ClO2)-1
chlorite
(BrO2)-1
bromite
(IO2)-1
iodite
(ClO3)-1
chlorate
(BrO3)-1
bromate
(IO3)-1
iodate
(ClO4)-1
perchlorate
(BrO4)-1
POLYATOMIC ION NAME
Ammonium
Acetate
Cyanide
Hydrogen carbonate
Hydrogen sulfate
Hydroxide
Nitrate
Nitrite
Hypochlorite
Chlorite
Chlorate
Perchlorate
Permanganate
Iodate
Thiocyanate
Oxalate
Carbonate
Chromate
Dichromate
Sulfate
Sulfite
Thiosulfate
Arsenate
Phosphate
Phosphite
perbromate (IO4)-1
periodate
SYMBOL and OXIDATION NO.
( NH4 ) + 1
(CH3COO) –1 or ( C2H3O2) –1
( CN ) - 1
( HCO3 ) -1
( HSO4 ) - 1
( OH ) -1
( NO3 ) -1
( NO2 ) -1
( ClO ) -1
( ClO2 ) -1
( ClO3 ) -1
( ClO4 ) -1
( MnO4 ) -1
( IO3 ) -1
( SCN ) - 1
( C2O4 ) - 2
( CO3 ) -2
( CrO4 ) -2
( Cr2O7 ) -2
( SO4 ) -2
( SO3 ) -2
( S2O3 ) -2
( AsO4 ) -3
( PO4 ) -3
( PO3 ) –3
These problems are all based upon concepts and skills that you learned (or
should have) in Chem I. We will only spend the first 2 weeks reviewing this
material.
If you couldn’t finish this assignment with a periodic table and a calculator
(with 1 or 2 googles allowed-I realize it’s summer), you will find Chem 2 an
uphill climb. I will not be starting from scratch and reteaching you Chem I as
if you’d never seen it before. We will review and refresh your memory. In
addition, the problems we work involving these Chem I topics are written on a
much higher level than these (which are similar to the ones you worked in my
Chem I class).
By the third or fourth week of school, we will move into new topics which will
build upon these concepts and skills as well as add new ones. The course
moves at a college-level pace and you will be expected to keep up with
homework, write lab reports and perform calculations independently, seek
help (I will not chase you). I am happy to see you during my planning period,
during lunch, or before school if you have questions.
GOOD NEWS: No lengthy projects or research papers, just practice
problems and be sure you know what you are doing! If you pay good attention
in class, DON’T MISS CLASS, and keep well-organized notes, your homework
should not take that long.
If I recommended that you take this course, it is because I believe you are
capable of being successful in it. As a college-bound student, you should
appreciate the challenge offered in Chem 2. We will work hard, but we will
also have fun. Plus, there is the added ego boost of knowing you took one of
the hardest classes in high school, ACED IT and got Purdue credits, too!
See you in August!!
Oxygen and Potassium went on a date… It went OK. :D