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Chem 1100 Pre-Test Fall 2016
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1.
What is the coefficient for HBr when the following equation is balanced with the smallest whole
number coefficients?
Br2 + H2O  HBr + HBrO3
a.
b.
c.
d.
e.
____
2.
Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be
formed from the decomposition of 13.2 moles of ammonium nitrate?
2NH4NO3  2N2 + O2 + 4H2
a.
b.
c.
d.
e.
____
____
6.60
14.0
26.4
13.2
18.0
3.
The thermite reaction is performed using 8.6 g Fe2O3 and 1.8 g powdered Al metal. Which reactant is
in excess and by how much?
Fe2O3 + 2 Al  Al2O3 + 2Fe
a.
b.
c.
d.
e.
____
5
7
8
3
6
Al; 0.3 g
Fe2O3; 2.0 g
Al; 2.1 g
Al; 1.1 g
Fe2O3; 3.3 g
4.
What is the percent yield of elemental sulfur if 7.54 grams of sulfur are obtained from the reaction of
6.16 grams of SO2 with an excess of H2S?
2H2S + SO2  2H2O + 3S
a.
b.
c.
d.
e.
72.6%
40.8%
81.5%
88.4%
91.4%
5.
a.
b.
c.
d.
What is the molarity of 850. mL of a solution containing 46.2 grams of NaBr?
0.495 M
0.506 M
0.516 M
0.528 M
e. 0.545 M
____
6.
Concentrated hydrochloric acid is about 12.1 M. What volume of concentrated HCl is required to
produce 5500 mL of 0.250 M?
a. 980 mL
b. 0.114 L
c. 98 mL
d. 0.211 L
e. 1114 mL
____
7.
a.
b.
c.
d.
e.
____
8.
a.
b.
c.
d.
e.
____
9.
I.
II.
III.
IV.
What volume of 0.130 M HCl solution will just react with 0.424 gram of Ba(OH)2?
2HCl + Ba(OH)2  BaCl2 + 2H2O
38.1 mL
32.6 mL
24.1 mL
18.6 mL
96.7 mL
Which response contains all the molecules below that violate the octet rule, and no others?
SF4, SiCl4, H2Te, AsF5, BeI2
SF4, AsF5, BeI2
BeI2
H2Te, BeI2
SF4, SiCl4
AsF5
Which numbered response lists all the molecules below that exhibit resonance and none that do not?
PF5
HNO3
SO2
H2O
a.
b.
c.
d.
e.
I and II
II and III
III and IV
I and III
II, III, and IV
____
10.
a.
b.
c.
d.
e.
Which one of the following molecules has a central atom that is sp2 hybridized?
BeF2
BCl3
PCl3
H2O
NH3
____
11.
a.
b.
c.
d.
For AsF3, the electronic geometry is ____ and the molecular geometry is ____.
tetrahedral; trigonal planar
trigonal planar; tetrahedral
tetrahedral; tetrahedral
trigonal planar; trigonal planar
e. trigonal planar; linear
____
12.
a.
b.
c.
d.
e.
Which one of the following is a nonpolar molecule with polar bonds?
H2O
NH3
PF5
CHCl3
none of these
____
13.
a.
b.
c.
d.
e.
Which one of the following molecules is octahedral?
BeCl2
SeF6
BF3
PF5
CF4
____
14.
How many sigma ()bonds and how many pi () bonds does the ethene molecule contain?
a.
b.
c.
d.
e.
4 , 2 
5 , 2 
5 , 1 
5 , 0 
8 , 2 
____
15.
a.
b.
c.
d.
e.
Which of the following molecules has an asymetric structure?
XeF4
SF4
SF6
XeF2
BCl3
____
16.
The overlap of the 2p atomic orbitals produces ____ sigma molecular orbitals and ____ pi molecular
orbitals.
a. 2; 3
b. 2; 4
c. 4; 2
d. 1; 2
e. 3; 3
____
17.
a.
b.
c.
d.
What is the best definition of bond order?
A bond resulting from the occupation of a pi molecular orbital.
The amount of energy required to break one mole of bonds.
A bond resulting from the occupation of a sigma molecular orbital.
The number of bonding molecular orbitals minus the number of antibonding molecular
orbitals.
e. Half the number of electrons in bonding molecular orbitals minus half the number of
electrons in antibonding molecular orbitals.
____
18.
a.
b.
c.
d.
e.
According to the Brønsted-Lowry theory, a base is defined as ____.
an electron pair acceptor
a proton acceptor
an electron pair donor
a proton donor
any species that can produce hydroxide ions in aqueous solution
____
19.
a.
b.
c.
d.
e.
Which one of the following is a weak acid?
H2SO4
HClO
HCl
HBr
HI
____
20.
Consider the complete neutralization reactions between the following acid-base pairs in dilute
aqueous solutions. Which one of the reactions produces insoluble salts?
a. CH3COOH + NaOH 
b. HNO3 + Mg(OH)2 
c. H3PO4 + Ca(OH)2 
d. HCl + KOH 
e. H2SO4 + Sr(OH)2 
____
21.
Which of the following reactions is the net ionic equation for the acid-base reaction between H 2CO3
and Sr(OH)2?
a. H2CO3 + Sr2+ + 2OH  SrCO3 + 2H2O
b. H3O+ + OH  2H2O
c. 2H3O+ + Sr2+ + 2OH  Sr2+ + 4H2O
d. H2CO3 + 2OH  2H2O + CO32
e. H2CO3 + Sr(OH)2  2H2O + Sr2+ + CO32
____
22.
a.
b.
c.
d.
e.
How many mL of 0.57 M AgNO3 will completely react with 121 mL of 0.95 M NaI?
AgNO3 + NaI  AgI + NaNO3
72.6 mL
181 mL
202 mL
4.47 mL
0.202 mL
____
23.
If 20 mL of 0.010 M H3PO4 solution is completely neutralized by 60.0 mL of Ca(OH) 2 solution, what
is the molarity of the Ca(OH)2 solution?
a. 0.010 M
b. 0.200 M
c. 0.030 M
d. 0.040 M
e. 0.0050 M
____
24.
What is the oxidation number of arsenic in K3AsO4?
a. +1
b. +2
c. +3
d. +4
e. +5
____
25.
In the following net ionic reaction, ____ is the oxidizing agent and ____ is oxidized.
C + H+ + SO42  CO2 + SO2 (acidic solution)
a.
b.
c.
d.
e.
H+; CO2
C; CO2
SO42; H+
SO42; C
C; SO42
____
26.
a.
b.
c.
d.
e.
Name the molecular compound, HNO3.
ammonia
nitric acid
nitrous acid
nitric oxide
methane
____
27.
a.
b.
c.
d.
e.
Which of the following molecules has the smallest bond angle(s)?
CH4
NH3
H2O
CF4
CO2
____
28.
a.
b.
c.
d.
e.
Which of the following molecules has three lone pairs of electrons on the central atom?
XeF4
SF4
SF6
XeF2
NCl3
Chem 1100 Pre-Test Fall 2016
Answer Section
MULTIPLE CHOICE
1.
ANS:
A
PTS:
1
TOP:
Chemical Equations
2.
ANS:
C
PTS:
1
TOP:
Calculations Based on Chemical Equations
3.
ANS:
E
PTS:
1
TOP:
The Limiting Reactant Concept
4.
ANS:
C
PTS:
1
TOP:
Percent Yields from Chemical Reactions
5.
ANS:
D
PTS:
1
TOP:
Concentrations of Solutions
6.
ANS:
B
PTS:
1
TOP:
Dilution of Solutions
7.
ANS:
A
PTS:
1
TOP:
Using Solutions in Chemical Reactions
8.
ANS:
A
PTS:
1
TOP: Writing Lewis Formulas: Limitations of the Octet Rule for Lewis Formulas
9.
ANS:
B
PTS:
1
TOP:
Resonance
10.
ANS:
B
PTS:
1
TOP:
Trigonal Planar Electronic Geometry
11.
ANS:
A
PTS:
1
TOP:
Tetrahedral Electronic Geometry: AB3U
Species
12.
ANS:
C
PTS:
1
TOP:
Tetrahedral Electronic Geometry: AB3U
Species
13.
ANS:
B
PTS:
1
TOP: Octahedral Electronic Geometry: AB6, AB5U, and AB4U2
14.
ANS:
C
PTS:
1
TOP:
Compounds Containing Double or Triple
Bonds
15.
ANS:
B
PTS:
1
TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3
16.
ANS:
B
PTS:
1
TOP:
Molecular Orbitals
17.
ANS:
E
PTS:
1
TOP:
Bond Order and Bond Stability
18.
ANS:
B
PTS:
1
TOP:
The Brønsted-Lowry Theory
19.
ANS:
B
PTS:
1
TOP:
Strengths of Acids
20.
ANS:
C
PTS:
1
TOP:
Acid-Base Reactions in Aqueous Solutions
21.
ANS:
A
PTS:
1
TOP:
Acid-Base Reactions in Aqueous Solutions
22.
ANS:
C
PTS:
1
TOP:
Calculations Involving Molarity
23.
ANS:
E
PTS:
1
TOP:
Calculations for Acid-Base Titrations
24.
ANS:
E
PTS:
1
TOP:
Balancing Redox Reactions
25.
ANS:
D
PTS:
1
TOP: Adding H+, OH–, or H2O to Balance Oxygen or Hydrogen
26.
ANS:
B
PTS:
1
TOP:
Chemical Formulas
27.
ANS:
C
PTS:
1
TOP:
Tetrahedral Electronic Geometry: AB2U2
Species
28.
ANS:
D
PTS:
1
TOP: Trigonal Bipyramidal Electronic Geometry: AB5, AB4U, AB3U2, and AB2U3