Question 1

Possible shapes of AB3 molecules are linear, trigonal planar, and T-shaped.

Accepted Answer

A) True 
 B)False

Question 2

The central iodine atom in IF5 has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell.

Accepted Answer

A) 1, 5 
B) 0, 5 
C) 5, 1 
D) 4, 1 
E) 1, 4 
A) 1, 5 
B) 0, 5 
C) 5, 1 
D) 4, 1 
E) 1, 4

Question 3

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 4

__________ hybrid orbitals are used for bonding by Xe in the XeF4 molecule.

Accepted Answer

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

Question 5

The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________.

Accepted Answer

A) linear, nonpolar 
B) linear, polar 
C) bent, nonpolar 
D) bent, polar 
E) trigonal planar, polar 
A) linear, nonpolar 
B) linear, polar 
C) bent, nonpolar 
D) bent, polar 
E) trigonal planar, polar

Question 6

A typical triple bond __________.

Accepted Answer

A) consists of one σ bond and two π bonds 
B) consists of three shared electrons 
C) consists of two σ bonds and one π bond 
D) consists of six shared electron pairs 
E) is longer than a single bond 
A) consists of one σ bond and two π bonds 
B) consists of three shared electrons 
C) consists of two σ bonds and one π bond 
D) consists of six shared electron pairs 
E) is longer than a single bond

Question 7

The molecular geometry of the SiH2Cl2 molecule is __________.

Accepted Answer

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

Question 8

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

Accepted Answer

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

Question 9

There are __________ unhybridized p atomic orbitals in an sp-hybridized carbon atom.

Accepted Answer

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

Question 10

The hybrid orbital set used by the central atom in NO3- is __________.

Accepted Answer

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

Question 11

Structural changes around a double bond in the __________ portion of the rhodopsin molecule trigger the chemical reactions that result in vision.

Accepted Answer

A) protein 
B) opsin 
C) retinal 
D) cones 
E) rods 
A) protein 
B) opsin 
C) retinal 
D) cones 
E) rods

Question 12

Of the following species, __________ will have bond angles of 120°.

Accepted Answer

A) PH3 
B) ClF3 
C) NCl3 
D) BCl3 
E) All of these will have bond angles of 120°. 
A) PH3 
B) ClF3 
C) NCl3 
D) BCl3 
E) All of these will have bond angles of 120°.

Question 13

The hybridization of the oxygen atom labeled x in the structure below is __________.

Accepted Answer

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

Question 14

The hybrid orbitals used for bonding by Xe in the unstable XeF2 molecule are __________ orbitals.

Accepted Answer

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

Question 15

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 16

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 π2p MOs 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 π2p MOs is higher than that of the σ2p MO 
E) the F-F bond enthalpy is very low

Question 17

There is/are __________ π bond(s)in the molecule below.

Accepted Answer

A) 0 
B) 1 
C) 2 
D) 4 
E) 16 
A) 0 
B) 1 
C) 2 
D) 4 
E) 16

Question 18

Three molecules have similar electron domains, but different molecular shapes. Why?

Accepted Answer

different

Question 19

Of the following molecules, only __________ is polar.

Accepted Answer

A) CCl4 
B) BCl3 
C) NCl3 
D) BeCl2 
E) Cl2 
A) CCl4 
B) BCl3 
C) NCl3 
D) BeCl2 
E) Cl2

Question 20

The molecular geometry of the PF4+ ion is __________.

Accepted Answer

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

Exam 9: Molecular Geometry and Bonding Theories

Possible shapes of AB3 molecules are linear, trigonal planar, and T-shaped.

The central iodine atom in IF5 has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell.

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

__________ hybrid orbitals are used for bonding by Xe in the XeF4 molecule.

The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________.

A typical triple bond __________.

The molecular geometry of the SiH2Cl2 molecule is __________.

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

There are __________ unhybridized p atomic orbitals in an sp-hybridized carbon atom.

The hybrid orbital set used by the central atom in NO3- is __________.

Structural changes around a double bond in the __________ portion of the rhodopsin molecule trigger the chemical reactions that result in vision.

Of the following species, __________ will have bond angles of 120°.

The hybridization of the oxygen atom labeled x in the structure below is __________.

The hybrid orbitals used for bonding by Xe in the unstable XeF2 molecule are __________ orbitals.

The molecular geometry of the CS2 molecule is __________.

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

There is/are __________ π bond(s)in the molecule below.

Three molecules have similar electron domains, but different molecular shapes. Why?

Of the following molecules, only __________ is polar.

The molecular geometry of the PF4+ ion is __________.

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

Possible shapes of AB₃ molecules are linear, trigonal planar, and T-shaped.

The central iodine atom in IF₅ has unbonded electron pairs and bonded electron pairs in its valence shell.

__________ hybrid orbitals are used for bonding by Xe in the XeF₄ molecule.

The molecular geometry of the BeCl₂ molecule is , and this molecule is .

The molecular geometry of the SiH₂Cl₂ molecule is __________.

The hybrid orbital set used by the central atom in NO₃^- is __________.

The hybrid orbitals used for bonding by Xe in the unstable XeF₂ molecule are __________ orbitals.

The molecular geometry of the CS₂ molecule is __________.

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

The molecular geometry of the PF₄⁺ ion is __________.