Chemistry a molecular approach canadian 1st edition tro test bank

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory Multiple Choice Questions 1) Give the approximate bond angle for a molecule with a trigonal planar shape.

A) 109.5° B) 180° C) 120° D) 105° E) 90° Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

2) Give the approximate bond angle for a molecule with a tetrahedral shape.

A) 109.5° B) 180° C) 120° D) 105° E) 90° Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

3) Give the approximate bond angle for a molecule with a linear shape.

A) 109.5° B) 180° C) 120° D) 105° E) 90° Answer: B Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

4) 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 Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

Copyright © 2014 Pearson Canada Inc.

10-1

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 5) Give the approximate bond angle between the axial position and the equatorial position for a molecule with a trigonal bipyramidal geometry.

A) 109.5° B) 180° C) 120° D) 105° E) 90° Answer: E Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

6) Give the approximate bond angle between two equatorial positions for a molecule with a trigonal bipyramidal geometry.

A) 109.5° B) 180° C) 120° D) 105° E) 90° Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.2

7) Determine the electron geometry (eg) and molecular geometry (mg) of BCl3.

A) eg = trigonal planar, mg = trigonal planar B) eg = tetrahedral, mg = trigonal planar C) eg = tetrahedral, mg = trigonal pyramidal D) eg = trigonal planar, mg = bent E) eg = trigonal bipyramidal, mg = trigonal bipyramidal Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

8) 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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

9) Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.

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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

Copyright © 2014 Pearson Canada Inc.

10-2

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 10) 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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

11) 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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

12) 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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

13) Determine the electron geometry (eg) and molecular geometry (mg) of NCl3.

A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = trigonal planar C) eg = trigonal planar, mg = bent D) eg = linear, mg = linear E) eg = tetrahedral, mg = trigonal pyramidal Answer: E Diff: 2

Type: MC

Var: 1

Page Ref: 10.2

14) Give the approximate bond angle for a molecule with trigonal planar electron geometry and bent molecular geometry.

A) <90° B) 90° C) <120° D) <109.5° E) 120° Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

Copyright © 2014 Pearson Canada Inc.

10-3

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 15) Give the approximate bond angle for a molecule with tetrahedral electron geometry and trigonal pyramidal molecular geometry.

A) 180° B) <180° C) <109.5° D) 109.5° E) <120° Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

16) Give the approximate bond angle for a molecule with tetrahedral electron geometry and bent molecular geometry.

A) 180° B) <180° C) <109.5° D) 109.5° E) <120° Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

17) Give the approximate bond angle for a molecule with trigonal bipyramidal electron geometry and seesaw molecular geometry.

A) <120° (equatorial), 90° (axial) B) 120° (equatorial), <90° (axial) C) <90° (equatorial), <90° (axial) D) 120° (equatorial), 90° (axial) E) <120° (equatorial), <90° (axial) Answer: E Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

18) Give the approximate bond angle for a molecule with T-shape molecular geometry.

A) <90° B) 90° C) >90° D) <120° E) 120° Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

19) Give the approximate bond angle for a molecule with trigonal bipyramidal electron geometry and linear molecular geometry.

A) 180° B) <180° C) >180° D) <109.5° E) <120° Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

20) Give the approximate bond angle for a molecule with octahedral electron geometry and square Copyright © 2014 Pearson Canada Inc.

10-4

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory pyramidal molecular geometry.

A) 90° B) 180° C) >120° D) <90° E) >90° Answer: D Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

21) Give the approximate bond angle for a molecule with octahedral electron geometry and square planar molecular geometry.

A) 90° B) 180° C) >120° D) <90° E) <120° Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.3

22) Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.

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 = seesaw E) eg = tetrahedral, mg = trigonal pyramidal Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

23) Determine the electron geometry for the molecule PF3.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

24) Determine the molecular geometry for the molecule PF3.

A) Trigonal pyramidal B) Trigonal planar C) Tetrahedral D) T-shaped E) Bent Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-5

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 25) Determine the electron geometry for the molecule SBr2.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

26) Determine the molecular geometry for the molecule SBr2.

A) Trigonal pyramidal B) Trigonal planar C) Tetrahedral D) T-shaped E) Bent Answer: E Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

27) Determine the electron geometry for the molecule CS2.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

28) Determine the molecular geometry for the molecule CS2.

A) Trigonal planar B) Bent C) Linear D) T-shaped E) Square planar Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

29) Determine the electron geometry for the molecule PCl5.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: D Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-6

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 30) Determine the molecular geometry for the molecule PCl5.

A) Linear B) Seesaw C) Square pyramidal D) Trigonal bipyramidal E) Square planar Answer: D Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

31) Determine the electron geometry for the molecule BrF3.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: D Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

32) Determine the molecular geometry for the molecule BrF3.

A) Square pyramidal B) Seesaw C) T-shaped D) Square planar E) Trigonal planar Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

33) Determine the electron geometry for the molecule XeF4.

A) Linear B) Trigonal planar C) Tetrahedral D) Trigonal bipyramidal E) Octahedral Answer: E Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

34) Determine the molecular geometry for the molecule XeF4.

A) Square planar B) Tetrahedral C) T-shaped D) Square pyramidal E) Trigonal planar Answer: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-7

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 35) Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻.

A) eg = tetrahedral, mg = bent B) eg = tetrahedral, mg = trigonal pyramidal C) eg = trigonal bipyramidal, mg = linear D) eg = trigonal bipyramidal, mg = trigonal planar E) eg = octahedral, mg = linear Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

36) 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 Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

37) Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

38) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom CH3OCH3.

A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

39) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined atom CH3OCH3.

A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-8

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 40) Consider the molecule below. Determine the molecular geometry at each of the two labelled 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 = seesaw Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

41) Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms.

A) 1 = trigonal planar, 2 = tetrahedral, 3 = trigonal pyramidal B) 1 = tetrahedral, 2 = tetrahedral, 3 = tetrahedral C) 1 = trigonal planar, 2 = tetrahedral, 3 = tetrahedral D) 1 = tetrahedral, 2 = tetrahedral, 3 = trigonal planar E) 1 = trigonal planar, 2 = trigonal pyramidal, 3 = trigonal pyramidal Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

42) Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule.

SeO2

SeCl6

SeF2

A) SeCl6 < SeF2 < SeO2 B) SeF2 < SeO2 < SeCl6 C) SeF2 < SeCl6 < SeO2 D) SeO2 < SeF2 < SeCl6 E) SeCl6 < SeO2 < SeF2 Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-9

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 43) 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 Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

44) 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.

N2O

NCl3

NO2⁻

A) NCl3 > NO2⁻ > N2O B) NO2⁻ > N2O > NCl3 C) N2O > NO2⁻ > NCl3 D) NCl3 > N2O > NO2⁻ E) N2O > NCl3 > NO2⁻ Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

45) 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.

CS2

CF4

SCl2

A) CS2 > SCl2 > CF4 B) SCl2 > CF4 > CS2 C) CF4 > SCl2 > CS2 D) CS2 > CF4 > SCl2 E) CF4 > CS2 > SCl2 Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

10-10

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 46) Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule.

HCN

H2O

H3O⁺

A) H3O+ < HCN < H2O B) H3O⁺ < H2O < HCN C) HCN < H3O⁺ < H2O D) H2O < HCN < H3O⁺ E) H2O < H3O⁺ < HCN Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.4

47) A pilot checks for water in the gas before flying a small airplane. How does she do it?

A) She drains a little bit of gas from the bottom and looks for two layers.

B) She smells it.

C) She shakes the wings.

D) She pipets the liquid from the top of the tank and looks for two layers.

E) She checks the gas gauge.

Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.5

48) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3.

A) eg = tetrahedral, mg = trigonal pyramidal, polar B) eg = tetrahedral, mg = tetrahedral, nonpolar C) eg = trigonal planar, mg = trigonal planar, nonpolar D) eg = trigonal bipyramidal, mg = trigonal planar, polar E) eg = trigonal pyramidal, mg = bent, nonpolar Answer: C Diff: 2

Type: MC

Var: 1

Page Ref: 10.5

49) How many of the following molecules are polar?

BrCl3

CS2

SiF4

SO3

Var: 1

Page Ref: 10.5

A) 1 B) 2 C) 3 D) 4 E) 0 Answer: A Diff: 3

Type: MC

Copyright © 2014 Pearson Canada Inc.

10-11

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 50) How many of the following molecules are polar?

XeCl2

COF2

PCl4F

SF6

Var: 1

Page Ref: 10.5

A) 0 B) 3 C) 1 D) 2 E) 4 Answer: B Diff: 3

Type: MC

51) How many of the following molecules are polar?

XeO2

SiCl2Br2

C2Br2

SeCl6

Var: 1

Page Ref: 10.5

A) 1 B) 4 C) 2 D) 3 E) 0 Answer: C Diff: 3

Type: MC

52) How many of the following molecules are polar?

PCl5

COS

XeO3

SeBr2

Var: 1

Page Ref: 10.5

A) 2 B) 0 C) 1 D) 3 E) 4 Answer: D Diff: 3

Type: MC

53) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2.

A) eg = tetrahedral, mg = bent, polar B) eg = trigonal planar, mg = bent, polar C) eg = linear, mg = linear, nonpolar D) eg = tetrahedral, mg = tetrahedral, nonpolar E) eg = trigonal pyramidal, mg = trigonal pyramidal, polar Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

Copyright © 2014 Pearson Canada Inc.

10-12

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 54) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SF6.

A) eg = trigonal bipyramidal, mg = trigonal bipyramidal, nonpolar B) eg = tetrahedral, mg = tetrahedral, polar C) eg = trigonal bipyramidal, mg = seesaw, polar D) eg = octahedral, mg = trigonal bipyramidal, nonpolar E) eg = octahedral, mg = octahedral, nonpolar Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

55) Determine the electron geometry (eg), molecular geometry (mg), and polarity of TeCl6.

A) eg = octahedral, mg = octahedral, nonpolar B) eg = trigonal bipyramidal, mg = trigonal bipyramidal, nonpolar C) eg = octahedral, mg = square planar, polar D) eg = trigonal bipyramidal, mg = seesaw, polar E) eg = tetrahedral, mg = trigonal pyramidal, polar Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

56) 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 Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

57) Determine the electron geometry (eg), molecular geometry (mg), and polarity of HBrO2.

A) eg = trigonal bipyramidal, mg = trigonal planar, nonpolar B) eg = octahedral, mg = square planar, nonpolar C) eg = tetrahedral, mg = bent, polar D) eg = tetrahedral, mg = linear, nonpolar E) eg = linear, mg = linear, polar Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

58) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SF6.

A) eg = trigonal bipyramidal, mg = trigonal bipyramidal, nonpolar B) eg = tetrahedral, mg = tetrahedral, polar C) eg = trigonal bipyramidal, mg = seesaw, polar D) eg = octahedral, mg = trigonal bipyramidal, nonpolar E) eg = octahedral, mg = octahedral, nonpolar Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

Copyright © 2014 Pearson Canada Inc.

10-13

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 59) Choose the compound below that contains at least one polar covalent bond but is nonpolar.

A) HCN B) CF4 C) SeBr4 D) ICl3 E) Both B and C are nonpolar and contain a polar covalent bond.

Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

60) Choose the compound below that contains at least one polar covalent bond but is nonpolar.

A) GeH2Br2 B) SCl2 C) AsCl5 D) CF2Cl2 E) All of the above are nonpolar and contain a polar covalent bond.

Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

61) Place the following in order of increasing dipole moment.

I. BCl3

II. BIF2

III. BClF2

A) I < II = III B) II < III < I C) I < II < III D) II < I < III E) I < III < II Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

62) 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 Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

Copyright © 2014 Pearson Canada Inc.

10-14

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 63) Determine the electron geometry (eg), molecular geometry (mg), and polarity of N2O (N central).

A) eg = linear, mg = linear, nonpolar B) eg = tetrahedral, mg = linear, nonpolar C) eg = tetrahedral, mg = bent, polar D) eg = linear, mg = linear, polar E) eg = trigonal planar, mg = bent, polar Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.5

64) Describe a pi bond.

A) side by side overlap of p orbitals B) end to end overlap of p orbitals C) s orbital overlapping with the end of a p orbital D) overlap of two s orbitals E) p orbital overlapping with a d orbital Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

65) Describe a sigma bond.

A) side by side overlap of p orbitals B) end to end overlap of p orbitals C) side by side overlap of d orbitals D) overlap of two s orbitals E) p orbital overlapping with a d orbital Answer: B Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

66) A molecule containing a central atom with sp hybridization has a ________ electron geometry.

A) linear B) trigonal bipyramidal C) trigonal planar D) tetrahedral E) bent Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

67) Identify the number of electron groups around a molecule with sp hybridization.

A) 1 B) 2 C) 3 D) 4 E) 5 Answer: B Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

Copyright © 2014 Pearson Canada Inc.

10-15

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 68) A molecule containing a central atom with sp2 hybridization has a ________ electron geometry.

A) linear B) trigonal bipyramidal C) trigonal planar D) tetrahedral E) bent Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

69) Identify the number of electron groups around a molecule with sp2 hybridization.

A) 1 B) 2 C) 3 D) 4 E) 5 Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

70) A molecule containing a central atom with sp3 hybridization has a(n) ________ electron geometry.

A) linear B) trigonal bipyramidal C) octahedral D) tetrahedral E) bent Answer: D Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

71) Identify the number of electron groups around a molecule with a tetrahedral shape.

A) 1 B) 2 C) 3 D) 4 E) 5 Answer: D Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

72) A molecule containing a central atom with sp3d hybridization has a(n) ________ electron geometry.

A) tetrahedral B) linear C) octahedral D) trigonal planar E) trigonal bipyramidal Answer: E Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

Copyright © 2014 Pearson Canada Inc.

10-16

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 73) Identify the number of electron groups around a molecule with a trigonal bipyramidal shape.

A) 1 B) 2 C) 3 D) 4 E) 5 Answer: E Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

74) A molecule containing a central atom with eight electron groups has a(n) ________ electron geometry.

A) octahedral B) trigonal bipyramidal C) tetrahedral D) trigonal planar E) trigonal pyramidal Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.7

75) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN. 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 Diff: 2

Type: MC

Var: 1

Page Ref: 10.7

76) Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN. 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: A Diff: 2

Type: MC

Var: 1

Page Ref: 10.7

77) Determine the electron geometry (eg) and molecular geometry (mg) of H2CO. 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: E Diff: 2

Type: MC

Var: 1

Page Ref: 10.7

Copyright © 2014 Pearson Canada Inc.

10-17

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 78) Draw the Lewis structure for OF2. What is the hybridization on the O atom?

A) sp B) sp3 C) sp2 D) sp3d E) sp3d2 Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

79) Draw the Lewis structure for H3O+. What is the hybridization on the O atom?

A) sp B) sp3 C) sp2 D) sp3d E) sp3d2 Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

80) Draw the Lewis structure for SO3. What is the hybridization on the S atom?

A) sp B) sp3 C) sp2 D) sp3d E) sp3d2 Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

81) Draw the Lewis structure for BrO4⁻. What is the hybridization on the Br atom?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

82) Draw the Lewis structure for CCl4. What is the hybridization on the C atom?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

83) Draw the Lewis structure for CO2. What is the hybridization on the C atom?

Copyright © 2014 Pearson Canada Inc.

10-18

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

84) Draw the Lewis structure for BF3. What is the hybridization on the B atom?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

85) Draw the Lewis structure for COCl2. What is the hybridization on the C atom?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

86) Draw the Lewis structure for SO2-3. What is the hybridization on the S atom?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

87) Draw the Lewis structure for N2H2. What is the hybridization on the N atoms?

A) sp B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

88) Draw the Lewis structure for C2H2. What is the hybridization on the C atoms?

A) sp Copyright © 2014 Pearson Canada Inc.

10-19

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory B) sp3d2 C) sp3d D) sp3 E) sp2 Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

89) Consider the molecule below. Determine the hybridization at each of the two labelled carbons.

A) C1 = sp3, C2 = sp3d B) C1 = sp, C2 = sp2 C) C1 = sp2, C2 = sp3d D) C1 = sp3d, C2 = sp3d2 E) C1 = sp2, C2 = sp3 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

90) Consider the molecule below. Determine the hybridization at each of the three labelled atoms.

A) 1 = sp2, 2 = sp3, 3 = sp2 B) 1 = sp2, 2 = sp3, 3 = sp3 C) 1 = sp3, 2 = sp3, 3 = sp3 D) 1 = sp3, 2 = sp3, 3 = sp2 E) 1 = sp, 2 = sp2, 3 = sp2 Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

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10-20

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 91) How many of the following molecules have sp hybridization on the central atom?

C2Cl2

CO2

O3

H2O

Var: 1

Page Ref: 10.7

A) 0 B) 1 C) 2 D) 3 E) 4 Answer: C Diff: 3

Type: MC

92) How many of the following molecules have sp3 hybridization on the central atom?

XeCl4

CH4

SF4

C2H2

A) 0 B) 4 C) 3 D) 2 E) 1 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

93) How many of the following molecules have sp3d hybridization on the central atom?

SiCl4

BrF5

AsF5

BrF3

Var: 1

Page Ref: 10.7

A) 2 B) 0 C) 4 D) 1 E) 3 Answer: A Diff: 3

Type: MC

94) How many of the following molecules have sp3d2 hybridization on the central atom?

SeCl6

XeF4

IF5

AsCl5

Var: 1

Page Ref: 10.7

A) 1 B) 3 C) 0 D) 2 E) 4 Answer: B Diff: 3

Type: MC

95) How many of the following molecules have sp2 hybridization on the central atom?

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

HCN

SO2

OCl2

XeCl2

Var: 1

Page Ref: 10.7

A) 4 B) 3 C) 2 D) 1 E) 0 Answer: D Diff: 3

Type: MC

96) Give the electron geometry (eg), molecular geometry (mg), and hybridization for CH3-.

A) eg = tetrahedral; mg = trigonal pyramidal; sp3 B) eg = tetrahedral; mg = tetrahedral; sp3 C) eg = trigonal pyramidal; mg = trigonal pyramidal; sp3 D) eg = trigonal planar; mg = trigonal planar; sp2 Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

97) List the number of sigma bonds and pi bonds in a single bond.

A) 1 sigma, 0 pi B) 0 sigma, 1 pi C) 1 sigma, 1 pi D) 1 sigma, 2 pi Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

98) List the number of sigma bonds and pi bonds in a double bond.

A) 1 sigma, 1 pi B) 2 sigma, 1 pi C) 2 sigma, 2 pi D) 1 sigma, 2 pi Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

99) List the number of sigma bonds and pi bonds in a triple bond.

A) 1 sigma, 1 pi B) 2 sigma, 1 pi C) 2 sigma, 2 pi D) 1 sigma, 2 pi Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 100) Draw the Lewis structure for the molecule CH2CHCH3. How many sigma and pi bonds does it contain?

A) 8 sigma, 1 pi B) 9 sigma, 0 pi C) 9 sigma, 1 pi D) 7 sigma, 2 pi E) 8 sigma, 2 pi Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

101) Draw the Lewis structure for the molecule CH3CH2CCH. How many sigma and pi bonds does it contain?

A) 11 sigma, 0 pi B) 9 sigma, 1 pi C) 8 sigma, 3 pi D) 9 sigma, 2 pi E) 8 sigma, 2 pi Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

102) Consider the following compound. How many sigma and pi bonds does it contain?

CH3CHCHCO2H A) 9 sigma, 4 pi B) 11 sigma, 2 pi C) 9 sigma, 2 pi D) 13 sigma, 0 pi E) 6 sigma, 2 pi Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

103) Draw the Lewis structure for the molecule C3H4. How many sigma and pi bonds does it contain?

A) 7 sigma, 1 pi B) 8 sigma, 0 pi C) 6 sigma, 2 pi D) 10 sigma, 0 pi E) 8 sigma, 2 pi Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.7

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 104) How many of the following molecules contain at least one pi bond?

C2H6

Cl2CO

C2Cl4

SeS3

Var: 1

Page Ref: 10.7

A) 0 B) 1 C) 3 D) 4 E) 2 Answer: C Diff: 3

Type: MC

105) Which of the following statements is TRUE? A) The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the set.

B) A bond order of 0 represents a stable chemical bond.

C) When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals.

D) Electrons placed in antibonding orbitals stabilize the ion/molecule.

E) All of the above are true.

Answer: C Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 106) 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 Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 107) Use the molecular orbital diagram shown to determine which of the following is least stable.

A) F2

B) F22⁺ C) Ne22⁺ D) O22⁺ E) F21⁻ Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

10-26

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 108) Use the molecular orbital diagram shown to determine which of the following is paramagnetic.

A) O22⁻ B) Ne22⁺ C) O22⁺

D) F22⁺

E) None of the above is paramagnetic.

Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

10-27

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 109) Use the molecular orbital diagram shown to determine which of the following is most stable.

A) C22⁺ B) N22⁺ C) B2

D) C22⁻ E) B22⁺ Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

10-28

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 110) Use the molecular orbital diagram shown to determine which of the following is least stable.

A) C22⁺ B) N22⁺ C) B2

D) C22⁻ E) B21⁺ Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

10-29

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 111) Use the molecular orbital diagram shown to determine which of the following is paramagnetic.

A) B22⁺ B) B22⁻

C) N22⁺ D) C22⁻ E) B2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

112) Draw a molecular orbital diagram and use it to determine which of the following is most stable.

A) F2 B) F22⁺

C) Ne22⁺ D) O22⁺ E) F22⁻ Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

10-30

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 113) Draw a molecular orbital diagram and use it to determine which of the following is most stable.

A) C22⁺ B) N22⁺ C) B2

D) C22⁻ E) B22⁺ Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

114) A molecule or ion with four electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of: A) 1 B) 1.5 C) 2 D) 2.5 E) 3 Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

115) A molecule or ion with five electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of: A) 0.5 B) 1 C) 1.5 D) 2 E) 3 Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

116) A molecule or ion with seven electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of: A) 0.5 B) 1 C) 1.5 D) 2 E) 2.5 Answer: E Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

117) A molecule or ion with eight electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of: A) 1 B) 1.5 C) 2 D) 2.5 E) 3 Answer: E Diff: 1

Type: MC

Var: 1

Page Ref: 10.8 Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 118) A molecule or ion with three electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of: A) 0.5 B) 1 C) 1.5 D) 2 E) 3 Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

119) A molecule or ion with two electrons in a bonding orbital and two electrons in an antibonding orbital would have a bond order of: A) 0 B) 1 C) 1.5 D) 0.5 E) -1 Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

120) Draw a molecular orbital diagram and use it to determine which of the following is paramagnetic.

A) O22⁻ B) Ne22⁺ C) O22⁺

D) F22⁺

E) None of the above is paramagnetic.

Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

121) Draw a molecular orbital diagram and use it to determine which of the following is most stable.

A) C22⁺

B) N22⁺ C) B2

D) C22⁻ E) B22⁺ Answer: D Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 122) Draw a molecular orbital diagram and use it to determine which of the following is paramagnetic.

A) B22⁺ B) B22⁻ C) N22⁺ D) C22⁻ E) B2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: 10.8

123) In molecular orbital theory the acronym HOMO stands for A) homogenous orbital-molecular orientation.

B) highly ordered molecular orbital.

C) highest occupied molecular orbital.

D) highest orbital-molecular orientation.

E) It has no meaning.

Answer: C Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

124) In molecular orbital theory the acronym LUMO stands for A) lowest unhybridized molecular orientation.

B) lowest unoccupied molecular orbital.

C) lowest unhybridized molecular orbital.

D) linear-uninteresting molecular orientation.

E) It has no meaning.

Answer: B Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

125) In molecular orbital theory the acronym LCAO stands for A) linear combination of atomic orbitals.

B) lowest combined atomic orbitals.

C) least consumed advanced orientation.

D) linearly created available orbital.

E) It has no meaning.

Answer: A Diff: 1

Type: MC

Var: 1

Page Ref: 10.8

126) Draw the Lewis structure for SF6. What is the hybridization on the S atom?

A) sp B) sp2 C) sp3 D) sp3d E) sp3d2 Answer: E Diff: 3

Type: MC

Var: 1

Page Ref: Content removed

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 127) Draw the Lewis structure for BrF5. What is the hybridization on the Br atom?

A) sp3d2 B) sp3d C) sp3 D) sp2 E) sp Answer: A Diff: 3

Type: MC

Var: 1

Page Ref: Content removed

128) Draw the Lewis structure for BrCl3. What is the hybridization on the Br atom?

A) sp3d2 B) sp3d C) sp3 D) sp2 E) sp Answer: B Diff: 3

Type: MC

Var: 1

Page Ref: Content removed

Algorithmic Questions 1) What geometric arrangement of charge clouds is expected for an atom that has four charge clouds?

A) trigonal bipyramidal B) octahedral C) tetrahedral D) square planar Answer: C Diff: 1

Type: MC

Var: 5

Page Ref: 10.2

2) What is the molecular geometry of ClF4 -?

A) seesaw B) square planar C) square pyramidal D) tetrahedral Answer: B Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

3) What is the molecular geometry of NCl3?

A) T-shaped B) tetrahedral C) trigonal planar D) trigonal pyramidal Answer: D Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 4) What is the molecular geometry of SF5-?

A) octahedral B) seesaw C) square pyramidal D) trigonal bipyramidal Answer: C Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

5) Which of the following best describes ClF2-? It has a molecular geometry that is A) linear with no lone pairs on the Cl atom.

B) linear with lone pairs on the Cl atom.

C) nonlinear with no lone pairs on the Cl atom.

D) nonlinear with lone pairs on the Cl atom.

Answer: B Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

6) What is the molecular geometry of TeCl4?

A) seesaw B) square planar C) square pyramidal D) tetrahedral Answer: A Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

7) Using the VSEPR model, the electron-domain geometry of the central atom in BrF4- is ________.

A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) octahedral Answer: E Diff: 3

Type: MC

Var: 6

Page Ref: 10.4

8) Using the VSEPR model, the molecular geometry of the central atom in XeF2 is ________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal Answer: A Diff: 3

Type: MC

Var: 9

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 9) Using the VSEPR model, the molecular geometry of the central atom in BF3 is ________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal Answer: B Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

10) Using the VSEPR model, the molecular geometry of the central atom in CF4 is ________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal Answer: C Diff: 3

Type: MC

Var: 6

Page Ref: 10.4

11) Using the VSEPR model, the molecular geometry of the central atom in SO2 is ________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal Answer: D Diff: 3

Type: MC

Var: 7

Page Ref: 10.4

12) Using the VSEPR model, the molecular geometry of the central atom in NCl3 is ________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal Answer: E Diff: 3

Type: MC

Var: 7

Page Ref: 10.4

13) Using the VSEPR model, the molecular geometry of the central atom in XeF4 is ________.

A) tetrahedral B) seesaw C) square planar D) trigonal bipyramidal E) square pyramidal Answer: C Diff: 3

Type: MC

Var: 15

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 14) Using the VSEPR model, the electron-domain geometry of the central atom in BF3 is ________.

A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) octahedral Answer: B Diff: 3

Type: MC

Var: 7

Page Ref: 10.4

15) Using the VSEPR model, the electron-domain geometry of the central atom in SF2 is ________.

A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) octahedral Answer: C Diff: 3

Type: MC

Var: 16

Page Ref: 10.4

16) Using the VSEPR model, the electron-domain geometry of the central atom in SF4 is ________.

A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) octahedral Answer: D Diff: 3

Type: MC

Var: 8

Page Ref: 10.4

17) What is the O-B-O bond angle in BO33-?

A) less than 109.5° B) 109.5° C) 120° D) greater than 120° Answer: C Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

18) What are the F-Po-F bond angles in PoF6?

A) 60° B) 90° C) 109.5° D) 120° Answer: B Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 19) The VSEPR model predicts the H—O—H bond angle in H3O+ to be A) 60°.

B) 90°.

C) less than 109.5° but greater than 90°.

D) 109.5°.

Answer: C Diff: 3

Type: MC

Var: 5

Page Ref: 10.4

20) The orbital hybridization on the carbon atoms in C2H2 is ________.

A) sp B) sp2 C) sp3 D) sp3d2 Answer: A Diff: 2

Type: MC

Var: 5

Page Ref: 10.7

21) The hybrid orbital set used by the central atom in NO3- is ________.

A) sp B) sp2 C) sp3 D) sp3d E) sp3d2 Answer: B Diff: 2

Type: MC

Var: 7

Page Ref: 10.7

22) The hybrid orbital set used by the central atom in NCl3 is ________.

A) sp B) sp2 C) sp3 D) sp3d E) sp3d2 Answer: C Diff: 2

Type: MC

Var: 16

Page Ref: 10.7

23) The hybrid orbital set used by the central atom in KrF2 is ________.

A) sp B) sp2 C) sp3 D) sp3d E) sp3d2 Answer: D Diff: 2

Type: MC

Var: 8

Page Ref: 10.7

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Matching Questions Match the following.

A) tetrahedral B) nonpolar, but contains a polar covalent bond C) sp hybridized central atom D) trigonal bipyramidal E) trigonal planar F) polar G) linear H) seesaw molecular geometry I) octahedral J) octahedral electron geometry K) polar, but contains no polar bonds L) sp2 hybridized central atom 1) SF4 Diff: 3

2)XeCl4 Diff: 3

Type: MA

Var: 1

Page Ref: 10.4

Type: MA

Var: 1

Page Ref: 10.4

Type: MA

Var: 1

Page Ref: 10.5

Type: MA

Var: 1

Page Ref: 10.5

Type: MA

Var: 1

Page Ref: 10.7

Type: MA

Var: 1

Page Ref: 10.7

Type: MA

Var: 1

Page Ref: 10.7

Type: MA

Var: 1

Page Ref: 10.7

Type: MA

Var: 1

Page Ref: 10.7

Var: 1

Page Ref: 10.7

3) CH2F2 Diff: 2

4) BCl3 Diff: 2

5) sp Diff: 1

6) sp2 Diff: 1

7) sp3 Diff: 1

8) sp3d Diff: 1

9) sp3d2 Diff: 1

10) BeF2 Diff: 2

Type: MA

Answers: 1) H 2) J 3) F 4) B 5) G 6) E 7) A 8) D 9) I 10) C Copyright © 2014 Pearson Canada Inc.

10-39

Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Short Answer Questions 1) Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Answer: Yes. The polarity of a molecule depends on the molecular geometry and whether or not all of the dipoles (polar bonds) cancel one another. If the molecular geometry causes all of the dipoles to cancel, the molecule will be nonpolar. An example is CF4, where there are four polar bonds but the dipoles sum to 0, making the molecule nonpolar.

Diff: 1

Type: SA

Var: 1

Page Ref: 10.5

2) Explain why oil and water do not mix.

Answer: Water molecules are polar and oil molecules are nonpolar.

Diff: 1

Type: SA

Var: 1

Page Ref: 10.5

3) Determine the molecular geometry about each interior atom in the following structure. Sketch the three-dimensional structure and label the interior atoms with the corresponding molecular geometry.

CH2CHCCCH3 Answer: The sketch should show all of the appropriate multiple bonds, with a double bond between carbons 1 and 2 and a triple bond between carbons 3 and 4. The first two carbons are trigonal planar, the second carbons are linear, and the last carbon is tetrahedral.

Diff: 3

Type: SA

Var: 1

Page Ref: 10.7

4) Give the electron geometry, molecular geometry, and hybridization for both carbons in CH3COOH. Answer: eg = tetrahedral; mg = tetrahedral; sp3 and eg = trigonal planar; mg = trigonal planar; sp2 Diff: 3

Type: SA

Var: 1

Page Ref: 10.7

5) Determine the hybridization about each interior atom in the following structure. Sketch the threedimensional structure and label the interior atoms with their corresponding hybridization.

CH2CHCCCH3 Answer: The sketch should show all of the appropriate multiple bonds, with a double bond between carbons 1 and 2 and a triple bond between carbons 3 and 4. The first two Cs are sp2 hybridized, the next 2 Cs are sp hybridized , and the last C is sp3 hybridized.

Diff: 3

Type: SA

Var: 1

Page Ref: 10.7

6) According to molecular orbital theory, what is an antibonding orbital?

Answer: An antibonding orbital is formed when two orbitals destructively interfere with one another.

An antibonding orbital is usually higher in energy than the two separated atoms and has a node in the internuclear region.

Diff: 2

Type: SA

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

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Chemistry: A Molecular Approach, 1ce Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory 7) Use molecular orbital theory to determine whether He22⁺ or He2⁺ is more stable. Draw the molecular orbital diagram for each and explain your answer.

Answer: The molecular orbital diagram should show He22⁺ with two electrons in the bonding orbital and the molecular orbital diagram of He2⁺ should show two electrons in the bonding molecular orbital

and one electron in the antibonding molecular orbital. The He22⁺ ion is more stable since it has a higher bond order (bond order =1) than He2⁺ (bond order = 1/2).

Diff: 3

Type: SA

Var: 1

Page Ref: 10.8

Copyright © 2014 Pearson Canada Inc.

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