Chapter.14 Acids and Bases Test Bank Answers 2nd Edition - MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen by Julia Burdge, Michelle Driessen. DOCX document preview.
Student name:__________
MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
1) How many lone pairs of electrons need to be added to complete this Lewis structure?
A) 5
B) 8
C) 6
D) 1
E) 16
2) How many lone pairs of electrons need to be added to complete this Lewis structure?
A) 5
B) 10
C) 0
D) 1
E) 6
3) The total number of bonding electrons in a molecule of formaldehyde (H 2CO) is
A) 3.
B) 4.
C) 6.
D) 8.
E) 18.
4) The total number of lone pairs in NCl 3 is
A) 6.
B) 8.
C) 9.
D) 10.
E) 13.
5) The Lewis structure for CS 2 is
A)
.
B)
.
C)
.
D)
.
6) The Lewis structure for a chlorate ion, ClO3–, should show ____ single bond(s), ____ double bond(s), and ____ lone pair(s).
A) 2, 1, 10
B) 3, 0, 9
C) 2, 1, 8
D) 3, 0, 10
E) 2, 1, 9
7) Which of these Lewis structures is incorrect?
A)
B)
C)
D)
E)
8) Which of these choices is the best Lewis structure for ozone, O 3?
A)
B)
C)
D)
E)
9) Which one of the following Lewis structures is definitely incorrect?
A)
B)
C)
D)
E)
10) Hydrazine, N2H4, is a good reducing agent that has been used as a component in rocket fuels. Select its Lewis structure.
A)
B)
C)
D)
E)
F) None of the answers is correct.
11) Select the correct Lewis structure for nitrogen trifluoride, NF 3.
A)
B)
C)
D)
E)
12) Select the correct Lewis structure for NOCl, a reactive material used as an ionizing solvent.
A)
B)
C)
D)
E) None of the answers is correct.
13) The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is
A) 1.
B) 2.
C) 3.
D) 4.
E) None of the answers is correct.
14) The number of resonance structures for the nitrate ion that satisfy the octet rule is
A) 1.
B) 2.
C) 3.
D) 4.
E) None of the answers is correct.
15) In which one of the following is the best Lewis structure a resonance structure?
A) SO 3
B) BF 3
C) I3−
D) SCO (C = central atom)
E) SO32−
16) Which pair of Lewis structures is not a pair of resonance structures?
A)
B)
C)
D) All of these pairs are resonance structures of the same species.
E) None of these pairs is resonance structures of the same species.
17) What is wrong with this Lewis structure?
A) There are too many electrons.
B) There are too few electrons.
C) The O atom does not have an octet.
D) The C atom does not have an octet.
E) There is nothing wrong with this Lewis structure.
18) In which one of the following species is the central atom (the first atom in the formula) likely to violate the octet rule?
A) BF4−
B) XeO 3
C) SiCl 4
D) NH 3
E) CH 2Cl 2
19) How many total resonance structures can be drawn for the sulfate ion, SO42−?
A) 2
B) 3
C) 4
D) 5
E) 6
20) What does the abbreviation VSEPR stand for?
A) Very Specific Electron and Proton Repair
B) Variable Selective of Electron and Protons
C) Valence Shell for Every Proton
D) Very Selective Electron Pair theory
E) Valence-Shell Electron-Pair Repulsion
21) Which of the following is required for the determination of the VSEPR model and the molecular shape?
A) atomic mass
B) number of protons
C) oxidation number
D) lewis structure
E) None of the answers is correct.
22) According to the VSEPR model, the predicted molecular geometry of the SO3 molecule is
A) pyramidal.
B) tetrahedral.
C) trigonal planar.
D) seesaw.
E) square planar.
23) What is the predicted molecular geometry of the CH4 molecule according to the VSEPR model?
A) tetrahedral
B) trigonal pyramidal
C) trigonal planar
D) square planar
E) seesaw
24) Using the VSEPR model, what is the predicted molecular geometry of the PCl3 molecule?
A) linear
B) bent
C) trigonal planar
D) trigonal pyramidal
E) tetrahedral
25) What is the predicted molecular geometry of the H2O molecule according to the VSEPR model?
A) tetrahedral
B) trigonal pyramidal
C) bent
D) square planar
E) seesaw
26) According to the VSEPR model, the molecular geometry of the carbonate ion, CO32−, is
A) square planar.
B) tetrahedral.
C) pyramidal.
D) trigonal planar.
E) octahedral.
27) According to the VSEPR model, the predicted molecular geometry of SiCl4 is
A) linear.
B) trigonal planar.
C) bent.
D) tetrahedral.
E) trigonal pyramidal.
28) According to the VSEPR model, the predicted molecular geometry of ammonia, NH3, is
A) linear.
B) trigonal planar.
C) bent.
D) tetrahedral.
E) trigonal pyramidal.
29) According to the VSEPR model, which molecule is predicted to be linear?
A) H2S
B) HCN
C) BF 3
D) H2CO
E) SO 3
30) Using the VSEPR model, predict the molecular geometry around the central atom in PO43−.
A) trigonal planar
B) trigonal pyramidal
C) tetrahedral
D) trigonal bipyramidal
E) octahedral
31) Using the VSEPR model, predict the molecular geometry around the central atom in SO32−.
A) trigonal planar
B) trigonal pyramidal
C) tetrahedral
D) trigonal bipyramidal
E) octahedral
32) What is the number of lone electron pairs on the central atom of a molecule having a trigonal pyramidal molecular geometry, such as NH3?
A) 1
B) 2
C) 3
D) 0
E) 4
33) What is the number of lone electron pairs on the central atom of a molecule having a linear molecular geometry, such as CO2?
A) 1
B) 2
C) 3
D) 0
E) 4
34) What is the number of lone electron pairs on the central atom of a molecule having a linear molecular geometry, such as ClF2−?
A) 1
B) 2
C) 3
D) 0
E) 4
35) According to the VSEPR model, a molecule with the general formula AB3 with no lone pairs on the central atom will have a ______ molecular shape.
A) linear
B) bent
C) trigonal planar
D) tetrahedral
E) trigonal pyramidal
36) According to the VSEPR model, a molecule with the general formula AB2 with two lone pairs on the central atom will have a _____ molecular geometry.
A) linear
B) bent
C) trigonal planar
D) tetrahedral
E) seesaw
37) What is the molecular geometry of N2O as predicted by the VSEPR model?
A) trigonal pyramidal
B) trigonal planar
C) tetrahedral
D) bent
E) linear
38) What is the molecular geometry of the thiocyanate anion, SCN−, as predicted by the VSEPR model? (Carbon is the central atom.)
A) linear
B) bent
C) tetrahedral
D) trigonal planar
E) trigonal pyramidal
39) What is the molecular geometry of BeH2 as predicted by the VSEPR model?
A) tetrahedral
B) bent
C) trigonal planar
D) linear
E) trigonal pyramidal
40) What is the molecular geometry of NOCl as predicted by the VSEPR model?
A) linear
B) trigonal planar
C) bent
D) tetrahedral
E) trigonal pyramidal
41) What is the molecular geometry of NO2− as predicted by the VSEPR model?
A) linear
B) trigonal planar
C) bent
D) tetrahedral
E) trigonal pyramidal
42) What is the molecular geometry of HOF as predicted by the VSEPR model?
A) trigonal pyramidal
B) bent
C) tetrahedral
D) linear
E) trigonal planar
43) What is the molecular geometry of ClF2− as predicted by the VSEPR model?
A) linear
B) bent
C) seesaw
D) T-shaped
E) trigonal bipyramidal
44) According to the VSEPR model, what is the predicted Cl–C–Cl bond angle in CCl4?
A) 90°
B) 109.5°
C) 120°
D) 145°
E) 180°
45) Which is the most reasonable prediction for the H–N–H bond angle in NH3?
A) 90°
B) 109.5°
C) 120°
D) 107°
E) 105°
46) What is the predicted O–C–O bond angle in CO2?
A) 60°
B) 90°
C) 109.5°
D) 120°
E) 180°
47) Which is the most reasonable prediction for the H–O–H bond angle in H2O?
A) 90°
B) 109.5°
C) 120°
D) 107°
E) 105°
48) Which is the most reasonable prediction for the Cl–N–Cl bond angle in NCl3?
A) 120°
B) 111°
C) 109.5°
D) 107°
E) 90°
49) Which is the most reasonable prediction for the H–C–H bond angle in CH4?
A) 90°
B) 109.5°
C) 120°
D) 107°
E) 105°
50) Place the following in order of decreasing electronegativity.Mg Cl F
A) Mg > Cl > F
B) F > Cl > Mg
C) Cl > F > Mg
D) Cl > Mg > F
E) F > Mg > Cl
51) Place the following in order of increasing electronegativity.N As K Ca
A) K < Ca < N < As
B) N < As < Ca < K
C) As < Ca < K < N
D) N < K < Ca < As
E) K < Ca < As < N
52) Place the following in order of increasing electronegativity.Se K Cl
A) Cl < Se < K
B) K < Se < Cl
C) K < Cl < Se
D) Se < Cl < K
E) Cl < K < Se
53) Place the following in order of increasing electronegativity.Cs O S
A) O < S < Cs
B) S < O < Cs
C) Cs < S < O
D) Cs < O < S
E) O < Cs < S
54) Which one of the following molecules is nonpolar?
A) NH 3
B) OF 2
C) CH3Cl
D) H2O
E) BeCl 2
55) Predict the molecular geometry and polarity of the SO2 molecule.
A) linear, polar
B) linear, nonpolar
C) bent, polar
D) bent, nonpolar
E) trigonal planar, polar
56) Predict the molecular geometry and polarity of the CS2 molecule.
A) linear, polar
B) linear, nonpolar
C) tetrahedral, nonpolar
D) bent, nonpolar
E) bent, polar
57) Which one of the following molecules is polar?
A) CH 4
B) CHBr 3
C) F 2
D) CBr 4
E) CO 2
58) Which of the following is defined as the attractive forces between polar molecules?
I. dispersion forces |
II. dipole-dipole interactions |
III. ion-dipole interactions |
A) I and III
B) II only
C) III only
D) I, II, and III
E) I only
F) I and II
59) Which substance should exhibit hydrogen bonding in the liquid phase?
A) PH 3
B) He
C) H2S
D) CH 4
E) CH3OH
60) Which substance will exhibit hydrogen bonding between molecules?
A) (CH3)3N
B) CH 3–O–CH 3
C) CH3CH2–OH
D) CH3CH2–F
E) HI
61) Which one of the following pure substances will exhibit hydrogen bonding?
A) CH 4
B) H2C=CH2
C) H2O
D) CHCl 3
E) CHF 3
62) Which of the following atoms does not participate in hydrogen bonding?
A) S
B) O
C) F
D) N
E) H
63) The strongest intermolecular interactions between ethyl alcohol (CH3CH2OH) molecules arise from
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) ion-dipole interactions.
E) carbon-oxygen bonds.
64) The strongest intermolecular interactions between hydrogen fluoride (HF) molecules arise from
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) ion-dipole interactions.
E) ionic bonds.
65) Ammonia's unusually high melting point is the result of
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) covalent bonding.
E) ionic bonding.
66) In which of the following compounds will the molecules not form hydrogen bonds with each other?
A)
B)
C)
D)
E)
67) The strongest intermolecular interactions between pentane (C5H12) molecules arise from
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) ion-dipole interactions.
E) carbon-carbon bonds.
68) Which kinds of intermolecular forces exist between propane molecules?
I. dispersion forces |
II. dipole-dipole interactions |
III. ion-dipole interactions |
A) I only
B) II only
C) III only
D) I, II, and III
E) I and III
69) Helium atoms do not combine to form He2 molecules, yet He atoms do attract one another weakly through
A) dipole-dipole forces.
B) ion-dipole forces.
C) dispersion forces.
D) dipole-induced dipole forces.
E) hydrogen bonding.
70) Which one of the following pure substance has both dispersion forces and dipole-dipole forces?
A) HCl
B) BCl 3
C) Br 2
D) H 2
E) CO 2
71) For which of the following pure substances are the intermolecular interactions entirely due to dispersion forces?
A) C2H6
B) CH3OCH3
C) NO 2
D) H2S
E) Ca(NO3)2
72) Which of the following pure substances has the strongest dispersion forces?
A) C4H10
B) C5H12
C) C6H14
D) C7H16
E) C8H18
73) At a temperature of 27 K, neon condenses due to
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) covalent bonding.
E) intramolecular forces.
74) Octane is a component of fuel used in internal combustion engines. The dominant intermolecular forces in octane are
A) dipole-dipole forces.
B) London dispersion forces.
C) hydrogen bonding.
D) covalent bonds.
E) carbon-hydrogen bonds.
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MCQ Test Bank | Introductory Chemistry - 2nd Edition by Burdge and Driessen
By Julia Burdge, Michelle Driessen