Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
84. A sp hybridized terminal oxygen atom (bonded to one other atom only) with 1 lone pair of
electrons has what type of bonding?
85. A sp2 hybridized terminal oxygen atom (bonded to one other atom only) with 2 lone pairs
of electrons has what type of bonding?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
86. A sp3 hybridized central nitrogen atom with 1 lone pair of electrons has what type of
bonding?
87. Which of the following species have the same geometries?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
88. Which of the following molecules have the same geometries?
89.
The number of pi bonds in the molecule below is
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
90.
The number of pi bonds in the molecule below is
91. The number of pi bonds in the oxalate ion (C2O42–) is
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
92. According to Molecular Orbital Theory, two separate 1s orbitals interact to form what
molecular orbital(s)?
93. According to Molecular Orbital Theory, two separate px orbitals interact about the x-axis
to form what molecular orbitals?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
94. According to Molecular Orbital Theory, two separate px orbitals interact about the y-axis
to form what molecular orbitals?
95. Consider the species Cl2+, Cl2, and Cl2–. Which of these species will be paramagnetic?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
96. Consider the species O2–, O2, and O2+. Which of these species will be paramagnetic?
97. Consider the species N2–, N2, and N2+. Which of these species will be paramagnetic?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
98. In which of the following would the bonding be strengthened with the addition of an
electron to form the negative molecular ion?
99. In which of the following would the bonding be weakened with the subtraction of an
electron to form a positive molecular ion?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
101. What is the bond order of Cl2–?
102. What is the bond order of CO+?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
103. In which of the following would the bonding be weakened with the addition of an
electron to form the negative molecular ion?
104. Which of the following is not true of molecular orbitals?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
105. The electrons in the delocalized molecular orbitals of benzene (C6H6)
106. Which of the following correctly lists species in order of increasing bond length?
107. Which of the following correctly lists species in order of increasing bond length?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
108. Which of the following correctly lists species in order of increasing bond order?
109. Select True or False: In VSEPR theory the molecular geometry of H3O+ (hydronium ion)
Bloom’s Level: 4. Analyze
Difficulty: Medium
Gradable: automatic
Section: 10.01
Subtopic: Valence-Shell Electron-Pair Repulsion Theory (VSEPR) and Molecular Shape
Topic: Molecular Shape
110. Select True or False: In VSEPR theory the molecular geometry of CO32– is distorted
tetrahedron (seesaw).
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
111. Select True or False: In VSEPR theory the molecular geometry of SF4 (sulfur
112. According to VSEPR theory, which of the following triatomic ions should be linear: N3–,
I3–, NO2–, ClO2–, SCN–?
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
113. Using periodic trends, arrange the following molecules in order of increasing dipole
moment: NH3, PH3, AsH3.
Chapter 10 – Chemical Bonding II: Molecular Geometry and Hybridization of Atomic
115. Which of the following molecules has polar bonds but is a nonpolar molecule? PCl5,
PCl3, NCl3, CO2
116. Which of the following molecules has polar bonds but is a nonpolar molecule? BF3,
CCl4, CO, SF4