1. No category

2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
electron geometry (eg) – Mother structure of VSEPR
molecular geometry (mg) – Daughter Structure
Ch9
1) Which of the following represent the Lewis structure for N?
A)
B)
C)
D)
E)
Answer: A
2) Which of the following represent the Lewis structure for Cl?
A)
B)
C)
D)
E)
Answer: B
3) Which of the following represent the Lewis structure for Mg?
A)
B)
C)
D)
E)
Answer: C
4) Which of the following represent the Lewis structure for Br⁻?
A)
B)
C)
D)
E)
Answer: D
5) Which of the following represent the Lewis structure for Ca2⁺? No valence electrons
A)
B)
C)
D)
E)
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
Answer: E
6) Give the complete electronic configuration for Br-.
A) 1s22s22p63s23p64s24p6
B) 1s22s22p63s23p64s24d104p6
C) 1s22s22p63s23p64s23d104p6
D) 1s22s22p63s23p64s23d104p5
E) 1s22s2p63s2p64s23d104p6
Answer: C
7) Give the complete electronic configuration for Ca2+.
A) 1s22s22p63s24p6
B) 1s22s22p63s23p6
C) 1s22s22p63s23p5
D) 1s22s23p64s25p6
E) 1s22s2p63s2p6
Answer: B
8) Give the complete electronic configuration for S2-.
A) 1s22s22p63s24p6
B) 1s22s22p63s23p6
C) 1s22s22p63s23p5
D) 1s22s23p64s25p6
E) 1s22s2p63s2p6
Answer: B
9) Place the following in order of decreasing magnitude of lattice energy.
NaF
RbBr
KCl
A) RbBr > NaF > KCl
B) NaF > KCl > RbBr
C) KCl > NaF > RbBr
D) NaF > RbBr > KCl
E) RbBr > KCl > NaF
Answer: B
10) Place the following in order of increasing magnitude of lattice energy.
CaO
MgO
A) MgO < CaO < SrS
B) SrS < MgO < CaO
C) SrS < CaO < MgO
D) CaO < MgO < SrS
E) CaO < SrS < MgO
Answer: C
SrS
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
11) Identify the shortest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) all of the above bonds are the same length
Answer: C
12) Identify the weakest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) all of the above bonds are the same strength
Answer: A
13) Identify the strongest bond.
A) single covalent bond
B) double covalent bond
C) triple covalent bond
D) all of the above bonds are the same strength
Answer: C
14) Identify the number of bonding pairs and lone pairs of electrons in water.
A) 1 bonding pair and 1 lone pair
B) 1 bonding pair and 2 lone pairs
C) 2 bonding pairs and 2 lone pairs
D) 2 bonding pairs and 1 lone pair
E) 3 bonding pairs and 2 lone pairs
Answer: C
15) Identify the compound with the largest dipole moment in the gas phase.( calculate the electron negativity
difference)
A) Cl2
B) ClF
C) HF
D) LiF
Answer: D
16) Identify the compound with the smallest dipole moment in the gas phase.
A) Cl2
B) ClF
C) HF
D) LiF
Answer: A
2014Spring CHEM101 Ch9-10 Review Worksheet
17) Choose the bond below that is most polar.
A) H-I
B) H-Br
C) H-F
D) H-Cl
E) C-H
Answer: C
18) Choose the bond below that is least polar.
A) P-F
B) C-Br
C) C-F
D) C-I
E) C-Cl
Answer: D
19) Choose the best Lewis structure for BeF2.
A)
B)
C)
D)
E)
Answer: D
20) Choose the best Lewis structure for OCl2.
A)
B)
C)
D)
E)
Answer: E
21) Choose the best Lewis structure for CH2Cl2.
A)
B)
C)
D)
Modified by Dr. Cheng-Yu Lai,
2014Spring CHEM101 Ch9-10 Review Worksheet
E)
Answer: B
22) Choose the best Lewis structure for XeI2.
A)
B)
C)
D)
E)
Answer: C
23) Give the number of valence electrons for ICl5.
A) 36
B) 40
C) 42
D) 44
E) 46
Answer: C
24) Choose the best Lewis structure for ICl5.
A)
B)
C)
D)
E)
Modified by Dr. Cheng-Yu Lai,
2014Spring CHEM101 Ch9-10 Review Worksheet
Answer: D
25) Choose the best Lewis structure for SF4.
A)
B)
C)
D)
E)
Answer: E
26) Choose the best Lewis structure for NO3⁻.
A)
B)
C)
D)
E)
Modified by Dr. Cheng-Yu Lai,
2014Spring CHEM101 Ch9-10 Review Worksheet
Answer: A
27) Choose the best Lewis structure for SO42⁻.
A)
B)
C)
D)
E)
Answer: A
28) Choose the best Lewis structure for PO43⁻.
A)
B)
Modified by Dr. Cheng-Yu Lai,
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
C)
D)
E)
Answer: C
29) Draw the Lewis structure for CO32- including any valid resonance structures. Which of the following
statements is TRUE?
A) The CO32- ion contains one C—O single bond and two C=O double bonds.
B) The CO32- ion contains two C—O single bonds and one C=O double bond.
C) The CO32- ion contains three C—O double bonds.
D) The CO32- ion contains two C—O single bonds and one C≡O triple bond.
E) None of the above are true.
Answer: B
30) Using Lewis structures and formal charge, which of the following ions is most stable?
OCN⁻
ONC⁻
NOC⁻
A) OCN⁻
B) ONC⁻
C) NOC⁻
D) None of these ions are stable according to Lewis theory.
E) All of these compounds are equally stable according to Lewis theory.
Answer: A
31) Rank the following molecules in decreasing bond energy.
Cl2
Br2
F2
A) I2 > Br2 > Cl2 > F2
B) Cl2 > Br2 > F2 > I2
C) I2 > Cl2 > Br2 > F2
D) Cl2 > I2 > F2 > Br2
Answer: B
I2
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
32) Use the bond energies provided to estimate ΔH°rxn for the reaction below.
Bond
Cl-Cl
P-Cl
PCl3(g) + Cl2(g) → PCl5(l) ΔH°rxn = ?
Bond Energy (kJ/mol)
243
331
A) -243 kJ
B) -419 kJ
C) -662 kJ
D) -67 kJ
E) -905 kJ
Answer: B
33) Use the bond energies provided to estimate ΔH°rxn for the reaction below.
Bond
C-H
C-O
C=O
O=O
O-H
CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(g)
Bond Energy (kJ/mol)
414
360
799
498
464
ΔH°rxn = ?
A) +473 kJ
B) -91 kJ
C) -486 kJ
D) -392 kJ
E) +206 kJ
Answer: D
34) Use the bond energies provided to estimate ΔH°rxn for the reaction below.
Bond
Xe-F
F-F
XeF2 + 2 F2 → XeF6
Bond Energy (kJ/mol)
147
159
ΔH°rxn = ?
A) -429 kJ
B) +159 kJ
C) -660 kJ
D) +176 kJ
E) -270 kJ
Answer: E
Ch10
35) Give the approximate bond angle for a molecule with an octahedral shape.
A) 109.5°
B) 180°
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
C) 120°
D) 105°
E) 90°
Answer: E
36) How many of the following molecules are polar?
BrCl3
CS2
SiF4
SO3
A) 1
B) 2
C) 3
D) 4
E) 0
Answer: A
37) How many of the following molecules are polar?
PCl5
COS
XeO3
SeBr2
A) 2
B) 0
C) 1
D) 3
E) 4
Answer: D
electron geometry (eg) – VSPER Mother structure geometry
38) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3.
A) eg=tetrahedral, mg=trigonal planar, sp2
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=trigonal pyramidal, mg=tetrahedral, sp3
E) eg=trigonal planar, mg=trigonal planar, sp2
Answer: C
39) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O.
A) eg=tetrahedral, mg=bent, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=bent, mg=bent, sp2
E) eg=trigonal planar, mg=trigonal planar, sp2
Answer: A
40) Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4.
A) eg=tetrahedral, mg=tetrahedral, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
C) eg=octahedral, mg=square planar, sp3d2
D) eg=octahedral, mg=octahedral, sp3d2
E) eg=trigonal bipyramidal, mg=seesaw, sp3d
Answer: C
41) Give the approximate bond angle for a molecule with an octahedral shape.
A) 109.5°
B) 180°
C) 120°
D) 105°
E) 90°
Answer: E
42) Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.
A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar
Answer: D
43) Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.
A) eg=tetrahedral, mg=trigonal pyramidal
B) eg=octahedral, mg=square planar
C) eg=trigonal bipyramidal, mg=trigonal pyramidal
D) eg=tetrahedral, mg=bent
E) eg=tetrahedral, mg=tetrahedral
Answer: E
44) Determine the electron geometry (eg) and molecular geometry (mg) of PF5.
A) eg=trigonal bipyramidal, mg=trigonal bipyramidal
B) eg=octahedral, mg=octahedral
C) eg=trigonal bipyramidal, mg=tetrahedral
D) eg=tetrahedral, mg=trigonal pyramidal
E) eg=trigonal planar, mg=octahedral
Answer: A
45) Determine the electron geometry (eg) and molecular geometry (mg) of CO2.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, mg=trigonal planar
C) eg=trigonal planar, mg=bent
D) eg=linear, mg=linear
E) eg=trigonal planar, mg=trigonal planar
Answer: D
46) Determine the electron geometry (eg) and molecular geometry (mg) of ICl3.
A) eg=trigonal planar, mg=trigonal planar
B) eg=trigonal bipyramidal, mg= T-shape
C) eg=trigonal planar, mg=bent
D) eg=trigonal bipyramidal, mg=see-saw
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
E) eg=tetrahedral, mg=trigonal pyramidal
Answer: B
47) Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.
A) eg=trigonal bipyramidal, mg=bent
B) eg=linear, mg=linear
C) eg=tetrahedral, mg=linear
D) eg=trigonal bipyramidal, mg=linear
E) eg=tetrahedral, mg=bent
Answer: D
48) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
Answer: E
49) Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.
A) C1 = tetrahedral, C2 = linear
B) C1 = trigonal planar, C2= bent
C) C1 = bent, C2 = trigonal planar
D) C1 = trigonal planar, C2 = tetrahedral
E) C1 = trigonal pyramidal, C2 = see-saw
Answer: D
50) Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each
molecule.
PF3
OF2
PF4⁺
A) PF3 < OF2 < PF4⁺
B) OF2 < PF3 < PF4⁺
C) OF2 < PF4⁺ < PF3
D) PF4⁺ < OF2 < PF3
E) PF4⁺ < PF3 < OF2
Answer: B
51) Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X
represents the outer atoms in each molecule.
2014Spring CHEM101 Ch9-10 Review Worksheet
N2O
NCl3
Modified by Dr. Cheng-Yu Lai,
NO2⁻
A) NCl3 > NO2⁻ > N2O
B) NO2⁻ > N2O > NCl3
C) N2O > NO2⁻ > NCl3
D) NCl3 > N2O > NO2⁻
E) N2O > NCl3 > NO2⁻
Answer: C
52) How many of the following molecules are polar?
BrCl3
CS2
SiF4
SO3
A) 1
B) 2
C) 3
D) 4
E) 0
Answer: A
53) Determine the electron geometry (eg), molecular geometry (mg), and polarity of PCl3.
A) eg=tetrahedral, mg=bent, polar
B) eg=trigonal planar, mg=trigonal planar, nonpolar
C) eg=linear, mg=linear, nonpolar
D) eg=tetrahedral, mg=trigonal pyramidal, polar
E) eg=trigonal pyramidal, mg=trigonal pyramidal, polar
Answer: D
54) Determine the electron geometry, molecular geometry and polarity of SF6.
A) eg=trigonal bipyramidal, mg=trigonal bipyramidal, nonpolar
B) eg=tetrahedral, mg=tetrahedral, polar
C) eg=trigonal bipyramidal, mg=see-saw, polar
D) eg=octahedral, mg=trigonal bipyramidal, nonpolar
E) eg=octahedral, mg=octahedral, nonpolar
Answer: E
55) Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3.
A) eg=trigonal planar, mg=trigonal planar, nonpolar
B) eg=tetrahedral, mg=trigonal pyramidal, polar
C) eg=trigonal planar, mg=trigonal pyramidal, polar
D) eg=trigonal bipyramidal, mg=trigonal planar, nonpolar
E) eg=octahedral, mg=tetrahedral, nonpolar
Answer: B
56) Place the following in order of increasing dipole moment.
I. BCl3
A) I < II = III
II. BIF2
III. BClF2
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
B) II < III < I
C) I < II < III
D) II < I < III
E) I < III < II
Answer: E
57) Place the following in order of decreasing dipole moment.
I. cis-CHCl=CHCl
II. trans-CHCl=CHCI
III. cis-CHF=CHF
A) III > I > II
B) II > I > III
C) I > III > II
D) II > III > I
E) I = III > II
Answer: A
58) Give the electron geometry (eg), molecular geometry (mg), and hybridization for NH3.
A) eg=tetrahedral, mg=trigonal planar, sp2
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=trigonal pyramidal, mg=tetrahedral, sp3
E) eg=trigonal planar, mg=trigonal planar, sp2
Answer: C
59) Give the electron geometry (eg), molecular geometry (mg), and hybridization for H2O.
A) eg=tetrahedral, mg=bent, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=bent, mg=bent, sp2
E) eg=trigonal planar, mg=trigonal planar, sp2
Answer: A
60) Give the electron geometry (eg), molecular geometry (mg), and hybridization for XeF4.
A) eg=tetrahedral, mg=tetrahedral, sp3
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=octahedral, mg=square planar, sp3d2
D) eg=octahedral, mg=octahedral, sp3d2
E) eg=trigonal bipyramidal, mg=seesaw, sp3d
Answer: C
61) Give the hybridization for the O in OF2.
A) sp
B) sp3
C) sp2
D) sp3d
E) sp3d2
Answer: B
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
62) Give the hybridization for the S in SO3.
A) sp
B) sp3
C) sp2
D) sp3d
E) sp3d2
Answer: C
63) Give the hybridization for the Br in BrO4⁻.
A) sp
B) sp3d2
C) sp3d
D) sp3
E) sp2
Answer: D
64) Give the hybridization for the S in SF6.
A) sp
B) sp2
C) sp3
D) sp3d
E) sp3d2
Answer: E
65) Give the hybridization for the Br in BrF5.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
Answer: A
66) Give the hybridization for the Br in BrCl3.
A) sp3d2
B) sp3d
C) sp3
D) sp2
E) sp
Answer: B
66) How many of the following molecules have sp2 hybridization on the central atom?
HCN
A) 4
B) 3
SO2
OCl2
XeCl2
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
C) 2
D) 1
E) 0
Answer: D
67) Use the molecular orbital diagram shown to determine which of the following is most stable.
A) F2
B) F22⁺
C) Ne22⁺
D) O22⁺
E) F22⁻
Answer: D
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
68) Use the molecular orbital diagram shown to determine which of the following are paramagnetic.
A) O22⁻
B) Ne22⁺
C) O22⁺
D) F22⁺
E) None of the above are paramagnetic.
Answer: D
2014Spring CHEM101 Ch9-10 Review Worksheet
Modified by Dr. Cheng-Yu Lai,
69) Use the molecular orbital diagram shown to determine which of the following are paramagnetic.
A) B22⁺
B) B22⁻
C) N22⁺
D) C22⁻
E) B2
Answer: E