Honors Chemistry
Chemical Compounds
Law of Definite Composition
1.
Complete the following table:
FORMULA MOLAR MASS
Name_______________________________
PERCENT COMPOSITION a) NaHCO
3 b) H
3
PO
4 c) (NH
4
)
3
PO
4 d) Al
2
O
3

FORMULA e) Ba(OH)
2
MOLAR MASS PERCENT COMPOSITION
2 f) Ca(ClO
3
)
2 g) Al
2
(SO
4
)
3 h) (NH
4
)
2
SO
4 i) Na
2
CO
3
∙
H
2
O

Binary Ionic Compounds
2.
Write the chemical name and formula for the ionic compound that results when the indicated metals and nonmetals are bonded together.
Nonmetals
Cl S Se P Br N
3
Na
Ca
Li
Al
Ba
Pb 4+

3.
Determine the molar mass of magnesium iodide.
4.
Determine the percent composition of gallium telluride.
Ionic Compounds
5.
rubidium oxide 14.
antimony(III) hydroxide
6.
potassium permanganate
7.
chromium(II) sulfite
15.
16.
Pb(NO
SnS
2
)
2
8.
zinc carbonate
9.
iron(III) dichromate
17.
Ba
3
P
2
18.
Al(C
2
H
3
O
2
)
3
10.
nickel(II) iodide
11.
cadmium bicarbonate
12.
ammonium oxalate
13.
silver arsenate
19.
20.
21.
22.
NaClO
CuBr
(NH
4
)
2
Pb(ClO
2
2
)
SO
4
3
4

23.
CrN
24.
CoAsO
4
25.
manganese(II) iodide
26.
lithium nitrate
27.
nickel(III) perchlorate
28.
cadmium acetate
29.
iron(II) phosphate
30.
beryllium hydrogen carbonate
31.
zinc selenide
32.
ammonium hypochlorite
33.
scandium chromate
34.
lead(IV) nitride
35.
Ag
3
PO
4
36.
Na
2
Cr
2
O
7
37.
NH
4
C
2
H
3
O
2
38.
Mn(CO
3
)
2
39.
Sr(NO
2
)
2
40.
Ga(MnO
4
)
3
41.
Mg(HCO
3
)
2
42.
CuClO
43.
Ba(OH)
2
44.
Rb
2
C
2
O
4
5

45.
Determine the molar mass of copper(II) bromite.
46.
Determine the percent composition of zinc periodate.
Hydrates
47.
Write the name of the following hydrates a. CuCl
2
∙
2H
2
O ______________________________________ b. MgSO
4
∙
7H
2
O ______________________________________ c. Na
2
SO
4
.
10H
2
O ______________________________________
48.
Write the formula for the following hydrates a. copper(II) sulfate pentahydrate b. calcium chloride dihydrate c. iron(III) nitrate nonahydrate
__________________________
__________________________
__________________________
49.
Determine the molar mass of barium hydroxide octahydrate.
50.
Determine the percent composition of zinc chloride hexahydrate.
6

Molecular Compounds
51.
Cl
2
O 54.
sulfur dioxide
52.
NO
2
55.
phosphorus pentachloride
53.
P
4
O
10
56.
diboron trioxide
57.
Determine the molar mass of arsenic pentabromide.
58.
Determine the percent composition of xenon hexafluoride.
Molecular and Ionic
59.
BrCl
60.
CuCl
61.
FeC
2
O
4
62.
Cr(OH)
3
63.
ClO
64.
AgClO
65.
OF
2
66.
MgF
2
67.
lead(IV) perchlorate
68.
dinitrogen tetroxide
69.
manganese(IV) oxide
70.
dibromine pentoxide
71.
cobalt(III) phosphide
72.
nitrogen trichloride
73.
iron(III) chloride
74.
arsenic pentaiodide
7

75.
Determine the molar mass of nickel(III) dichromate
76.
Determine the percent composition of diphoshphorus pentoxide.
Acids
77.
Write the name of the following acids a. HI
(g)
____________________ HI
(aq) b. H
2
CO
3(l)
____________________ H
2
CO
3(aq) c. H
3
PO
3(s)
____________________ H
3
PO
3(aq) d. H
2
S
(g)
____________________ H
2
S
(aq) e. HF
(g)
____________________ HF
(aq)
78.
Write the formula for the following acids
____________________
____________________
____________________
____________________
____________________ a. nitrous acid b. perchloric acid c. hydrobromic acid d. oxalic acid e. hydrophosphoric acid
________________________________
________________________________
________________________________
________________________________
________________________________
79.
Calculate the molar mass of selenous acid.
80.
Calculate the percent composition of hydrotelluric acid.
8

9
Graham’s Law of Effusion
81.
Rank these gases in order of highest effusion rate to lowest: NO
2
, SO
2
, CO
2
, and O
2
.
82.
Determine the relative rate of effusion between propane (C
3
H
8
) and octane (C
8
H
18
). Write a brief statement interpreting your answer.
83.
A gas is found to effuse 1.35 times faster than sulfur dioxide. Determine the molar mass of the gas.
84.
Determine the relative effusion rate of carbon dioxide and carbon monoxide. Interpret your answer.
85.
It requires 36.0 seconds for 10.0 mL of oxygen to effuse through a certain capillary tube. Under the same conditions of temperature and pressure it requires 50.0 seconds for 10.0 mL of disilane to effuse through the same capillary tube. Calculate the molar mass of disilane.
Review
86.
Calculate the molar mass of beryllium arsenite.
87.
What is the percent composition of manganese(IV) phosphite?

calcium selenide carbon disulfide cobalt(II) nitride copper(I) bromide copper(II) chloride dihydrate dichromic acid disulfur dichloride hydrobromic acid hydrosulfuric acid magnesium chloride nickel(III) oxalate phosphoric acid potassium bicarbonate rubidium sulfide sodium carbonate monohydrate sulfurous acid tin(IV) dichromate
88.
Identify the type of compound (I = ionic, M = molecular, A = acid, H = hydrate) and write the formula or name.
Type Name Formula Type Formula Name cadmium phosphate SnO
10
HClO
P
Ni
2
(aq)
2
O
5
(SO
3
NaI
)
3
Mn
3
N
2
HClO
3(aq)
Li
3
AsO
4
Mg
3
As
2
SbP
Fe(NO
3
)
3
∙
9H
2
O
H
3
P
(g)
H
2
C
2
O
4(aq)
Ga(NO
3
)
3
HCl
(aq)
Co(OH)
2
Cl
2
O
7
BaCl
2
∙ 2H
2
O

89.
Complete the following chart
Name Formula rubidium perchlorate bromine monochloride strontium arsenide cesium arsenate carbonic acid hydroarsenic acid iron(III) sulfite magnesium sulfate heptahydrate perchloric acid hydroiodic acid aluminum nitrate phosphorus pentachloride copper(II) hydroxide chlorous acid iron(III) chloride hexahydrate chromium(III) phosphide lead(II) oxide lithium iodide
Formula
NaHCO
3
CO
AgBr
LiClO
4
H
3
PO
3 (aq)
HF
(g)
Sb
2
(C
2
O
4
)
3
CuSO
4
∙ 5H
2
O
H
2
CrO
4(aq)
H
2
Se
(aq)
ScPO
4
N
2
O
4
Pb(Cr
2
O
7
)
2
H
2
SO
4(aq)
CaCl
2
∙ 2H
2
O
BaCl
2
MgSe
Fr
2
S
Name
11

12
90.
If a gas with a molar mass of 79.5 g/mol can effuse at a rate of 35.0 mL/sec, at what rate will a gas of molar mass 32.6 g/mol effuse?
91.
Determine the relative rate of effusion of 2-butene (C
4
H
8
) and 2,3-dimethylpentane (C
7
H
16
).
Interpret your answer.
92.
Determine the molar mass of an unknown gas that effuses 1.35 times faster than sulfur trioxide.
Cumulative Review Questions
93.
The density of lithium metal is 0.534 g/cm
3
. Using scientific notation, determine the mass, in
pounds, of 1.726 cubic yards of lithium.
94.
A cup of gold colored metal beads was measured to have a mass of 0.951 lb. By water displacement, the volume of the beads was calculated to be 4.80 x 10
−14
km
3
. Given the following densities, identify the metal. Calculate percent error. a.
Gold: 19.3 g/mL b.
Copper: 8.86 g/mL c.
Bronze: 9.87 g/mL

13
95.
How many electrons are in 2.65 g of potassium atoms?
96.
How many protons are in 2.694 moles of seaborgium?
97.
A little aluminum boat (mass of 14.50 g) has a volume of 450.00 cm
3
. The boat is placed in a small pool of water and carefully filled with pennies. If each penny has a mass of 2.50 g, how many pennies can be added to the boat before it sinks?
98.
Determine whether the following are chemical or physical changes. d.
Molding clay _______ e.
Sublimation _______ f.
Cutting a piece of cheese _______ a.
Frying an egg _______ b.
Dissolving sugar in tea _______ c.
Growing a plant _______
99.
Complete the table below:
What is the atomic number?
What is the mass number
How many protons?
How many electrons?
How many neutrons?
What is the charge?
Write the isotopic symbol.
What kind of ion?
Change in electrons?
Ion A
32
17 gain 3
Ion B
30
64
lose 2

14
100.
Write nuclear equations for the following: a.
Electron capture of phosphorus-32. b.
c.
Alpha decay of iridium-195
Formation of nickel-59 from a beta decay.
101.
A 1.05 gram sample of phosphorus-32 (t
1/2
= 14.26 days) remains after 85.56 days of decay.
What was the original sample mass?
102.
How many kilojoules of thermal energy are required to increase the temperature of 25.0 grams of K
2
CO
3
from 22.19°C to 23.85°C?
103.
A gas at a temperature of 33°C and a pressure of 753 mm Hg is in a rigid container with a volume of 1.65 L. As the temperature of the gas is increased to 88°C, what is the new pressure of the gas, in kPa?