Question 1

In order to produce sp3 hybrid orbitals, ________ s atomic orbital(s)and ________ p atomic orbital(s)must be mixed.

Accepted Answer

A) one, two 
B) one, three 
C) one, one 
D) two, two 
E) two, three 
A) one, two 
B) one, three 
C) one, one 
D) two, two 
E) two, three

Question 2

When three atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed?

Accepted Answer

A) six 
B) four 
C) five 
D) three 
E) one 
A) six 
B) four 
C) five 
D) three 
E) one

Question 3

The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals.

Accepted Answer

A) sp 
B) sp2 
C) sp3 
D) sp3d 
E) sp3d2 
A) sp 
B) sp2 
C) sp3 
D) sp3d 
E) sp3d2

Question 4

A typical double bond ________.

Accepted Answer

A) is stronger and shorter than a single bond 
B) consists of one σ bond and one π bond 
C) imparts rigidity to a molecule 
D) consists of two shared electron pairs 
E) All of the above answers are correct. 
A) is stronger and shorter than a single bond 
B) consists of one σ bond and one π bond 
C) imparts rigidity to a molecule 
D) consists of two shared electron pairs 
E) All of the above answers are correct.

Question 5

The molecular geometry of the CS2 molecule is ________.

Accepted Answer

A) linear 
B) bent 
C) tetrahedral 
D) trigonal planar 
E) T-shaped 
A) linear 
B) bent 
C) tetrahedral 
D) trigonal planar 
E) T-shaped

Question 6

The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________.

Accepted Answer

A) 90° 
B) 109.5° 
C) 120° 
D) 180° 
E) 60° 
A) 90° 
B) 109.5° 
C) 120° 
D) 180° 
E) 60°

Question 7

Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because ________.

Accepted Answer

A) the bond order in F2 can be shown to be equal to 1. 
B) there are more electrons in the bonding orbitals than in the antibonding orbitals. 
C) all electrons in the MO electron configuration of F2 are paired. 
D) the energy of the π2pMOs is higher than that of the σ2p MO 
E) the F-F bond enthalpy is very low 
A) the bond order in F2 can be shown to be equal to 1. 
B) there are more electrons in the bonding orbitals than in the antibonding orbitals. 
C) all electrons in the MO electron configuration of F2 are paired. 
D) the energy of the π2pMOs is higher than that of the σ2p MO 
E) the F-F bond enthalpy is very low

Question 8

The electron domain and molecular geometry of SO3 are ________.

Accepted Answer

A) trigonal bipyramidal, trigonal planar 
B) trigonal planar, bent 
C) trigonal bipyramidal, T-shaped 
D) trigonal planar, trigonal planar 
E) octahedral, seesaw 
A) trigonal bipyramidal, trigonal planar 
B) trigonal planar, bent 
C) trigonal bipyramidal, T-shaped 
D) trigonal planar, trigonal planar 
E) octahedral, seesaw

Question 9

For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?

Accepted Answer

A) 1 
B) 2 
C) 1 or 2 
D) 3 
E) 1 or 3 
A) 1 
B) 2 
C) 1 or 2 
D) 3 
E) 1 or 3

Question 10

The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s)and ________ bonded electron pair(s)in its valence shell.

Accepted Answer

A) 1, 4 
B) 2, 4 
C) 4, 0 
D) 4, 1 
E) 4, 2 
A) 1, 4 
B) 2, 4 
C) 4, 0 
D) 4, 1 
E) 4, 2

Question 11

The electron-domain geometry of the AsF5 molecule is trigonal bipyramidal. The hybrid orbitals used by the As atom for bonding are ________ orbitals.

Accepted Answer

A) sp2d2 
B) sp3 
C) sp3d2 
D) sp3d 
E) sp2 
A) sp2d2 
B) sp3 
C) sp3d2 
D) sp3d 
E) sp2

Question 12

The combination of two atomic orbitals results in the formation of ________ molecular orbitals.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 0 
A) 1 
B) 2 
C) 3 
D) 4 
E) 0

Question 13

In comparing the same two atoms bonded together, the ________ the bond order, the ________ the bond length, and the ________ the bond energy.

Accepted Answer

A) greater, shorter, greater 
B) greater, greater, greater 
C) greater, longer, greater 
D) smaller, longer, smaller 
E) smaller, greater, greater 
A) greater, shorter, greater 
B) greater, greater, greater 
C) greater, longer, greater 
D) smaller, longer, smaller 
E) smaller, greater, greater

Question 14

The hybridizations of bromine in BrF5 and of arsenic in AsF5 are ________ and ________, respectively.

Accepted Answer

A) sp3, sp3d 
B) sp3d, sp3d2 
C) sp3d, sp3 
D) sp3d2, sp3d 
E) sp3d2, sp3d2 
A) sp3, sp3d 
B) sp3d, sp3d2 
C) sp3d, sp3 
D) sp3d2, sp3d 
E) sp3d2, sp3d2

Question 15

What is the molecular geometry of a molecule that has three bonding and two non-bonding domains?

Accepted Answer

The answer of What is the molecular geometry of a...

Question 16

The electron-domain geometry and molecular geometry of iodine trichloride are ________ and ________, respectively.

Accepted Answer

A) trigonal bipyramidal, trigonal planar 
B) tetrahedral, trigonal pyramidal 
C) trigonal bipyramidal, T-shaped 
D) octahedral, trigonal planar 
E) T-shaped, trigonal planar 
A) trigonal bipyramidal, trigonal planar 
B) tetrahedral, trigonal pyramidal 
C) trigonal bipyramidal, T-shaped 
D) octahedral, trigonal planar 
E) T-shaped, trigonal planar

Question 17

The molecular geometry of the SF2 molecule is ________.

Accepted Answer

A) linear 
B) bent 
C) trigonal planar 
D) tetrahedral 
E) octahedral 
A) linear 
B) bent 
C) trigonal planar 
D) tetrahedral 
E) octahedral

Question 18

Using the VSEPR model, the electron-domain geometry of the central atom in ClO3- is ________.

Accepted Answer

A) linear 
B) trigonal planar 
C) tetrahedral 
D) trigonal bipyramidal 
E) octahedral 
A) linear 
B) trigonal planar 
C) tetrahedral 
D) trigonal bipyramidal 
E) octahedral

Question 19

Using the VSEPR model, the molecular geometry of the central atom in CH4 is ________.

Accepted Answer

A) linear 
B) trigonal planar 
C) tetrahedral 
D) bent 
E) trigonal pyramidal 
A) linear 
B) trigonal planar 
C) tetrahedral 
D) bent 
E) trigonal pyramidal

Question 20

The angles between sp2 orbitals are ________.

Accepted Answer

A) 45° 
B) 180° 
C) 90° 
D) 109.5° 
E) 120° 
A) 45° 
B) 180° 
C) 90° 
D) 109.5° 
E) 120°

Exam 9: Molecular Geometry and Bonding Theories

In order to produce sp3 hybrid orbitals, ________ s atomic orbital(s)and ________ p atomic orbital(s)must be mixed.

When three atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed?

The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals.

A typical double bond ________.

The molecular geometry of the CS2 molecule is ________.

The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________.

Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because ________.

The electron domain and molecular geometry of SO3 are ________.

For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?

The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s)and ________ bonded electron pair(s)in its valence shell.

The electron-domain geometry of the AsF5 molecule is trigonal bipyramidal. The hybrid orbitals used by the As atom for bonding are ________ orbitals.

The combination of two atomic orbitals results in the formation of ________ molecular orbitals.

In comparing the same two atoms bonded together, the ________ the bond order, the ________ the bond length, and the ________ the bond energy.

The hybridizations of bromine in BrF5 and of arsenic in AsF5 are ________ and ________, respectively.

What is the molecular geometry of a molecule that has three bonding and two non-bonding domains?

The electron-domain geometry and molecular geometry of iodine trichloride are ________ and ________, respectively.

The molecular geometry of the SF2 molecule is ________.

Using the VSEPR model, the electron-domain geometry of the central atom in ClO3- is ________.

Using the VSEPR model, the molecular geometry of the central atom in CH4 is ________.

The angles between sp2 orbitals are ________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

In order to produce sp³hybrid orbitals, s atomic orbital(s)and p atomic orbital(s)must be mixed.

The hybrid orbitals used for bonding by the sulfur atom in the SF₄ molecule are ________ orbitals.

The molecular geometry of the CS₂ molecule is ________.

The Cl-Si-Cl bond angle in the SiCl₂F₂ molecule is approximately ________.

Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F₂. This is because ________.

The electron domain and molecular geometry of SO₃ are ________.

The central Xe atom in the XeF₄ molecule has unbonded electron pair(s)and bonded electron pair(s)in its valence shell.

The electron-domain geometry of the AsF₅ molecule is trigonal bipyramidal. The hybrid orbitals used by the As atom for bonding are ________ orbitals.

In comparing the same two atoms bonded together, the the bond order, the the bond length, and the the bond energy.

The hybridizations of bromine in BrF₅ and of arsenic in AsF₅ are and , respectively.

The electron-domain geometry and molecular geometry of iodine trichloride are and , respectively.

The molecular geometry of the SF₂ molecule is ________.

Using the VSEPR model, the electron-domain geometry of the central atom in ClO₃^- is ________.

Using the VSEPR model, the molecular geometry of the central atom in CH₄ is ________.

The angles between sp² orbitals are ________.