Chapter 10 Chemical Bonding and Molecular Structure


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Chapter 10 Chemical Bonding and Molecular Structure
Multiple Choice
Section 10.1 1. All of the geometries listed below are examples of the five basic geometries for molecules with
more than 3 atoms except
a. planar triangular b. octahedral c. tetrahedral ! d. trihedral e. trigonal bipyramidal
Section 10.1 2. Three different values can be observed for the bond angles in which of the following basic
molecular structures for simple molecules:
a. linear b. planar triangular c. tetrahedral ! d. trigonal bipyramidal e. octahedral
Section 10.1 3. The basic geometry for molecules in the set below which possesses the smallest bond angles is
a. linear b. planar triangular c. tetrahedral d. trihedral ! e. octahedral
Section 10.1 4. The basic geometry for molecules in the set below which possesses the largest bond angles is
! a. linear b. planar triangular c. tetrahedral d. trihedral e. octahedral
211

Section 10.2 5. The concept that electron pairs located in the valence shell of an atom bonded to other atoms tend to
stay as far apart as possible so as to minimize repulsions between them is incorporated in the a. Pauli principle b. Heisenberg uncertainty principle
! c. valence shell electron pair repulsion theory d. electronegativity and polar bonds theory e. Aufbau principle
Section 10.2 6. Which one of the following arrangements would best accommodate three electron domains in the
valence shell of a covalently bonded atom? ! a. planar triangular b. octahedral c. tetrahedral d. trihedral e. trigonal bipyramidal
Section 10.2 7. Which one of the following arrangements would best accommodate five electron domains in the va-
lence shell of a covalently bonded atom? a. planar triangular b. octahedral c. tetrahedral d. trihedral
! e. trigonal bipyramidal
212

Section 10.2 11. Based on the Lewis structure, the number of electron domains in the valence shell of the boron
atom in the BF3 molecule is
a. 1 b. 2 ! c. 3 d. 4 e. 5
Section 10.2 13. Based on the Lewis structure, the number of nonbonding domains in the CO2 molecule is
a. 1 b. 2 c. 3 ! d. 4 e. 5
Section 10.2 16. Application of the concepts of VSEPR theory leads us to conclude that the shape of the SO3 mole-
cule is
a. trigonal pyramidal b. square planar c. regular tetrahedral ! d. triangular planar e. distorted tetrahedron
Section 10.2 19. Application of the concepts of VSEPR theory leads to the prediction that the shape of the PH3 mole-
cule is
a. bent b. linear c. regular tetrahedral d. triangular planar ! e. trigonal pyramidal
213

Section 10.2 20. The geometry of the CS2 molecule is best described as
a. bent ! b. linear
c. regular tetrahedral d. triangular planar e. trigonal pyramidal
Section 10.2 21. The geometry of the ClF3 molecule is best described as
a. distorted tetrahedral b. regular tetrahedral ! c. T-shaped d. trigonal pyramidal e. triangular planar
Section 10.2 22. Application of the concepts of the VSEPR theory suggests that the geometric arrangement of the
atoms in the carbonate ion, CO32- is
a. octahedral b. square planar c. regular tetrahedral ! d. triangular planar e. trigonal pyramidal
Section 10.2 23. Based on conclusions from application of the VSEPR theory, which one of the following species is
linear?
a. BF3 ! b. HCN
c. H2CO d. H2S e. SO2
214

Section 10.2 28. The bond angle in Cl2O is expected to be approximately
a. 90 degrees ! b. 109.5 degrees
c. 120 degrees d. 145 degrees e. 180 degrees Section 10.2 29. The smallest F—S—F bond angle in SF6 is ! a. 90 degrees b. 109.5 degrees c. 120 degrees d. 145 degrees e. 180 degrees
215

Section 10.3 33. Based on observed periodic trends, arrange the following species, HBr, HCl, HF, HI, in order of
increasing dipole moment. a. HF < HCl < HBr < HI b. HBr < HCl < HF < HI c. HI < HF < HCl < HBr
! d. HI < HBr < HCl < HF e. HCl < HBr < HI < HF
Section 10.3 34. Which of the following molecules CO2, CS2, NO2, COS is/are polar?
a. NO2 only b. CS2, NO2, and COS c. CO2 only ! d. COS and NO2 e. COS only Section 10.3 36. Which one of the molecules below is a polar molecule? a. Br2 b. BF3 c. CO2 d. CS2 ! e. IBr
216

Section 10.5 45. Draw a Lewis structure for the CH4 molecule. What is the hybrid orbital set used by the carbon
atom for bonding? a. sp3d2 b. sp c. sp3d
! d. sp3 e. sp2
Section 10.5 46. Draw a Lewis structure for the NH3 molecule. What is the hybrid orbital set used by the nitrogen
atom for bonding? a. sp3d2 b. sp c. sp3d
! d. sp3 e. sp2
Section 10.5 47. Draw a Lewis structure for the C2H6 molecule. What is the hybrid orbital set used by either of the
carbon atoms for bonding? a. sp3d2 b. sp c. sp3d
! d. sp3 e. sp2
217

Section 10.5 48. Draw a Lewis structure for the C2H4 molecule. What is the hybrid orbital set used by either of the
carbon atoms for bonding?
a. sp3d2 b. sp c. sp3d d. sp3 ! e. sp2
Section 10.6 52. Which one of the following hybrid orbital sets is used by the central atom for σ-bonding in the PCl3
molecule?
a. sp b. sp2 ! c. sp3 d. sp3d e. sp3d2
Section 10.6 53. Which one of the following hybrid orbital sets is used by the central atom for σ-bonding in the PCl4-
ion?
a. sp b. sp2 c. sp3 ! d. sp3d e. sp3d2
Section 10.6 54. Which one of the following hybrid orbital sets is used by the central atom for σ-bonding in the SF6
molecule?
a. sp b. sp2 c. sp3 d. sp3d ! e. sp3d2
218

Section 10.8 93. What is the total number of π-bonds in the benzene molecule?
a. 0 b. 1 c. 2 ! d. 3 e. 4
219

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Chapter 10 Chemical Bonding and Molecular Structure