1
1.
Triple bonds in molecules
a) occur in polyatomic ions.
b) involve sharing three electrons.
c) occur only in atoms having three valence electrons
d) involve sharing six electrons.
e) must be coordinate covalent.
2.
If the electronegativity difference between elements A and X is 0.2, the bond in AX will
most likely be
a) ionic
3.
b) polar covalent
d) pure covalent
Which of the following is an acceptable Lewis structure for NH2NH2?
.
.
a) H - N - N - H
|
H
|
H
.. ..
d) H - N - N - H
| |
H H
4.
c) nonpolar covalent
.
b) H - N = N - H
=N-H
| |
H H
.
c) H - N
|
H
|
H
.. ..
e) H - N = N - H
|
|
H H
Which of the following is the correct Lewis structure for IO3- ?
a) :O = I = O:
..
| ..
:O:
..
b) :O - I = O:
.. | ..
:O:
..
.. .. ..
d) :O - I - O:
.. | ..
:O:
.. ..
e) :O - I - O:
.. | ..
:O:
c) :O - I - O:
.. | ..
:O:
..
2
..
5.
..
The shape of IO3- is
and the bond angles are
. (See question 4.)
a) trigonal planar, exactly 120
b) tetrahedral, exactly 109.5
c) tetrahedral, approximately 109.5
d) trigonal pyramidal, exactly 109.5
e) trigonal pyramidal, approximately 109.5
6.
7.
Which of the following is the correct Lewis structure, conforming to the Lewis octet rule, for
SO3?
..
a) :O = S = O:
..
..
|
:O:
..
..
b) :O - S = O:
.. |
..
:O:
..
.. .. ..
d) :O - S - O:
.. | ..
:O:
..
.. ..
e) :O - S = O:
.. |
..
:O:
..
You just determined the Lewis structure for sulfur trioxid, SO3. How many resonance
forms, conforming to the Lewis octet rule, are there for this molecule?
a) one
8.
..
..
c) :O - S - O:
.. | ..
:O:
..
b) two
c) three
d) four
Which of the following does NOT conform to the Lewis "octet" rule?
1) NO2
2) BeCl2
3) HCN
4) BCl3
5) CO2
3
a) 3
b) 1
c) 4, 5
d) 2, 3, 4
e) 2, 4
4
9.
10.
Which of the following species is trigonal planar?
1) PO33
2) NF3
3) SeO3
4) SO42
5) NO2
a) 3 only
b) 4 only
c) 2 and 3
d) 3 and 5
e) 1 and 3
3) AlCl3
4) BeCl2
5) CHCl3
c) 3, 4
d) 1, 2
e) 1, 2, 5
Which of the following molecules is (are) polar?
1) PCl3
a) 5
11.
2) OF2
b) 2
How many sp hybridized carbon atoms are contained in the following compound?
H - C  C - CH2 - C  C - CH2 - C  C - CH = CH - CH3
a) 6
12.
b) 7
c) 8
d) 9
Which hybrid orbitals give bond angles of 109.5o?
a) sp
b) sp2
c) sp3
d) sp4
e) 10
5
13.
Balance the following equation. What is the sum of the coefficients of the reactants AND
products in the balanced equation? (If present, don't forget the coefficients of 1.)
Al
a) 13
14.
KBrO4
b) 15

c) 18
Al2O3
+
d) 21
KBr
e) 23
Balance the following equation and choose the quantity which is the sum of the coefficients
of reactants AND products. (If present, don't forget the coefficients of 1.)
CS2 +
a) 18
15.
+
NaOH

b) 15
Na2CS3 +
c) 13
Na2CO3 +
d) 11
H2O
e) 9
Balance the following equation and choose the quantity which is the sum of the coefficients
of reactants AND products. (If present, don't forget the coefficients of 1.)
NH3
a) 12
b) 15
+
O2
c) 19

NO
d) 20
+
H2O
e) 22
6
16.
Which of the following is an example of a single-replacement reaction (assume all reactions
occur to give products)?
1) KI (aq) + Cl2 (g) 
2) Pb(NO3)2 (aq) + Na2SO4 (aq) 
3) Mg (s) + O2 (g) 
4) Al (s) + FeCl2 (aq) 
5) CaCl2 (aq) + (NH4)2S (aq) 
a) 1 only
17.
c) 4 only
d) 2 and 5
e) 1 and 4
Which of the reactions in question 16 is (are) an example(s) of a double-replacement
reaction (assume all reactions occur to give products)?
a) 1 only
18.
b) 3 only
b) 3 only
c) 4 only
d) 2 and 5
What are the expected products of the following reaction?
CaCO3 (s) + H2SO4 (aq)
a) Ca(OH)2 + SO3 + CO2
b) CaSO4 + H2 + CO3
c) 4 CaO + 4 CO2 + H2S
d) CaCO3H2SO4
e) CaSO4 + H2O + CO2

e) 1 and 3
7
19.
Arrange the following chlorine containing species in order of increasing oxidation number
of the chlorine atom. What compound occupies the intermediate (middle) position?
a) HClO3
b) Cl2
c) Cl2O7
d) CaCl2
e) ClO2
8
20.
Examine the reaction below and the statements concerning the reaction. Select an answer
which includes ALL of the CORRECT statements given below.
Te
1)
2)
3)
4)
5)
+
4 HNO3
2 H2O
+
4 NO2
b) 1
c) 2, 3, 4
d) 2, 4
e) 1, 5
b) 340.4
c) 345.6
d) 361.2
e) 322.0
Smelling salts contain (NH4)2CO3. To three significant figures what is the weight percent
of nitrogen in the compound?
(Atomic weights: C = 12.01, O = 16.00, H = 1.008, N = 14.01)
a) 33.2
23.
+
Cocaine, an addictive drug, has the molecular formula C17H21NO4. What is the molecular
weight (in amu) of cocaine? (Atomic weights: C = 12.01, H = 1.008, N = 14.01, O = 16.00)
a) 303.3
22.
TeO2
N has been oxidized.
The reducing agent is Te.
The oxidation number of N changed from +5 to +4.
Te has been oxidized.
The reducing agent is HNO3.
a) 1, 2, 5
21.

b) 29.2
c) 17.9
d) 14.6
e) 12.3
For reasons of taste, the maximum chloride ion, Cl-, content of drinking water is set at 0.25 g
per liter. How many chloride ions is this per liter?
(Atomic weight: Cl = 35.45)
a) 4.2 x 1022
b) 4.2 x 1021
d) 8.5 x 1025
e) 1.6 x 1022
c) 1.6 x 1023
9
24.
25.
26.
The lowest limit of MgSO4 that can be detected by taste in drinking water is 0.400 g per
liter. How many moles of MgSO4 is this per liter?
(Atomic weights: Mg = 24.30, O = 16.00, S = 32.06; Mol. Wts.: MgSO4 = 120.36)
a) 3.32 x 10-3
b) 3.32 x 10-4
d) 3.01 x 10-4
e) 3.01 x 10-6
c) 3.32 x 10-2
How many moles of carbon atoms are in 0.0195 g of the amino acid glycine
(NH2CH2CO2H)?
(At. wts.: C = 12.01, O = 16.00, H = 1.008, N = 14.01; Mol. Wt: NH2CH2CO2H = 75.07)
a) 2.60 x 10-4
b) 5.20 x 10-4
d) 1.04 x 10-3
e) 2.60 x 10-3
c) 1.04 x 10-4
Sodium carbonate has the formula, Na2CO3. How many sodium ions are present in 0.10 g
of Na2CO3? (At. Wts.: C = 12.01, O = 16.00, Na = 22.99; Form. Wt.: Na2CO3 = 105.99)
a) 5.7 x 1020
b) 1.1 x 1021
d) 5.7 x 1021
e) 6.4 x 1024
c) 3.2 x 1024
10
27.
A dry cleaning fluid is composed of 14.5% C and 85.5% Cl. What is the empirical formula
of the compound? (Atomic weights: C = 12.01, Cl = 35.45)
a) CCl
28.
c) CCl3
d) C2Cl
e) C3Cl
If the molecular weight of the compound in question 27 is 248.73 amu, what is the
molecular formula of the compound?
a) CCl2
29.
b) CCl2
b) C2Cl2
c) C2Cl4
d) C3Cl6
e) C4Cl8
Calculate the number of moles of NO produced from 0.25 moles of O2 by the following
reaction. (Atomic Weights: N = 14.00, O = 16.00; Mol. Wts.: NO = 30.00, O2 = 32.00)
a) 0.20
4 NH3 + 5 O2

b) 0.25
c) 0.30
4 NO + 6 H2O
d) 0.50
e) 0.15
11
30.
Which of the following setups is correct to calculate the number of grams of KClO3
produced from the reaction of 0.150 moles of Cl2.
(Atomic weights: K = 39.1, Cl = 35.45, O = 16.00)
3 Cl2
+
6 KOH

5 KCl
1 mole KClO3
a) 0.150 moles Cl2 x
KClO3
+
3 H 2O
122.6 g KClO3
x
3 moles Cl2
1 mole KClO3
3 moles Cl2
122.6 g KClO3
b) 0.150 moles Cl2 x
x
1 mole KClO3
1 mole KClO3
1 mole KClO3
c) 0.150 moles Cl2 x
1 mole KClO3
x
3 moles Cl2
122.6 g KClO3
3 moles Cl2
1 mole KClO3
d) 0.150 moles Cl2 x
x
1 moles KClO3
31.
+
122.6 g KClO3
How many grams of HClO3 can be produced from 7.2 grams of ClO2 according to the
following reaction? (Atomic weights: Cl = 35.45, H = 1.008, O = 16.00;
Mol. Wts.: ClO2 = 67.45, H2O = 18.02, HClO3 = 84.46, HCl = 36.46)
6 ClO2 + 3 H2O
a) 6.6
b) 6.9

c) 7.1
5 HClO3 + HCl
d) 7.5
e) 7.9
12
32.
A 357.0 ml sample of O2 is collected at 728 mm Hg. What would be the volume (ml) at
1.00 atm assuming that the temperature remains constant ?
a) 331
33.
c) 350
d) 339
e) 342
At STP, a gas has a volume of 2.25 L. What will be the new pressure (torr) if the
temperature is raised to 50C and the volume is increased to 4.00 L?
a) 410
34.
b) 328
b) 440
c) 485
d) 506
e) 552
Lactic acid is produced in the muscles when insufficient oxygen is available during vigorous
exercise. A 0.33 g sample of lactic acid is vaporized in a sealed 300 mL container at 150C
and the resulting pressure is 326 torr. What is the molecular weight of lactic acid?
a) 73
b) 78
c) 84
d) 89
e) 102
13
35.
A 5.73 L flask at 25C contains 0.0388 moles of N2, 0.147 moles of CO and 0.0803 moles of
H2. What is the partial pressure of the CO in atmospheres?
(atomic weights: N = 14.01, C = 12.01, O = 16.0, H = 1.008)
a) 0.166
36.
b) 0.343
c) 0.628
d) 0.921
e) 1.14
Which one of the following statements is FALSE?
a) The average kinetic energies of molecules of different kinds of ideal gases are the same
at a given temperature.
b) Under ordinary conditions of temperature and pressure, ideal gas molecules are widely
separated.
c) Ideal gases conform to the ideal gas equation, PV=nRT, under all conditions.
d) The volume occupied by an ideal gas molecules themselves under ordinary conditions is
large in comparison to the total volume occupied by the gas.
e) Real gases behave ideally at high temperatures and low pressures.
14
USEFUL INFORMATION
R = 0.0821 L-atm/mol-K
1 amu = 1.66 x 10-24 g
Avogadro's number = 6.02 x 1023 particles/mole
molar volume at STP = 22.41L
1 atm = 760 mm Hg = 760 torr = 14.7 lb/in2