Question 1

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CO2H.

Accepted Answer

A)  mg = tetrahedral 
B)  mg = trigonal pyramidal 
C)  mg = trigonal planar 
D)  mg = trigonal bipyramidal 
E)  mg = bent 
A)  mg = tetrahedral 
B)  mg = trigonal pyramidal 
C)  mg = trigonal planar 
D)  mg = trigonal bipyramidal 
E)  mg = bent

Question 2

Match the following.
-sp3d2

Accepted Answer

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

Question 3

Determine the electron geometry (eg) and molecular geometry (mg) of ClF3.

Accepted Answer

A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, mg = trigonal planar 
C)  eg = trigonal planar, mg = bent 
D)  eg = tetrahedral, mg = trigonal pyramidal 
E)  eg = trigonal bipyramidal, mg = T-shaped 
A)  eg = tetrahedral, mg = tetrahedral 
B)  eg = linear, mg = trigonal planar 
C)  eg = trigonal planar, mg = bent 
D)  eg = tetrahedral, mg = trigonal pyramidal 
E)  eg = trigonal bipyramidal, mg = T-shaped

Question 4

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

Accepted Answer

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

Question 5

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

Accepted Answer

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

Question 6

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

Accepted Answer

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 
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

Question 7

Consider the following compound. How many sigma and pi bonds does it contain? CH3CHCHCO2H

Accepted Answer

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 
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

Question 8

Give the approximate bond angle between the axial position and the equatorial position for a molecule with a trigonal bipyramidal geometry.

Accepted Answer

A)  109.5° 
B)  180° 
C)  120° 
D)  105° 
E)  90° 
A)  109.5° 
B)  180° 
C)  120° 
D)  105° 
E)  90°

Question 9

Determine the electron geometry (eg) and molecular geometry (mg) of PF5.

Accepted Answer

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 
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

Question 10

Give the approximate bond angle in CH4.

Accepted Answer

A)  109.5° 
B)  180° 
C)  120.5° 
D)  104.5° 
E)  90.5° 
A)  109.5° 
B)  180° 
C)  120.5° 
D)  104.5° 
E)  90.5°

Question 11

A molecule or ion with two electrons in a bonding orbital and two electrons in an antibonding orbital would have a bond order of ________.

Accepted Answer

A)  0 
B)  1 
C)  1.5 
D)  0.5 
E)  -1 
A)  0 
B)  1 
C)  1.5 
D)  0.5 
E)  -1

Question 12

Determine the electron geometry for the molecule PF3.

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 13

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

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 14

Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF

Accepted Answer

A)  III > I > II 
B)  II > I > III 
C)  I > III > II 
D)  II > III > I 
E)  I = III > II 
A)  III > I > II 
B)  II > I > III 
C)  I > III > II 
D)  II > III > I 
E)  I = III > II

Question 15

How many of the following molecules contain at least one pi bond? C2H6 Cl2CO C2Cl4 SeS3

Accepted Answer

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

Question 16

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

Accepted Answer

An antibonding orbital is formed when tw

Question 17

Give the electron geometry, molecular geometry, and hybridization for both carbons in CH3COOH.

Accepted Answer

eg = tetrahedral; mg

Question 18

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

Accepted Answer

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

Question 19

Match the following.
-SF4

Accepted Answer

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

Question 20

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

Accepted Answer

A)  1 sigma, 0 pi 
B)  0 sigma, 1 pi 
C)  1 sigma, 1 pi 
D)  1 sigma, 2 pi 
A)  1 sigma, 0 pi 
B)  0 sigma, 1 pi 
C)  1 sigma, 1 pi 
D)  1 sigma, 2 pi

Exam 10: Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CO2H.

Match the following. -sp3d2

Determine the electron geometry (eg) and molecular geometry (mg) of ClF3.

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

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

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

Consider the following compound. How many sigma and pi bonds does it contain? CH3CHCHCO2H

Give the approximate bond angle between the axial position and the equatorial position for a molecule with a trigonal bipyramidal geometry.

Determine the electron geometry (eg) and molecular geometry (mg) of PF5.

Give the approximate bond angle in CH4.

A molecule or ion with two electrons in a bonding orbital and two electrons in an antibonding orbital would have a bond order of ________.

Determine the electron geometry for the molecule PF3.

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

Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF

How many of the following molecules contain at least one pi bond? C2H6 Cl2CO C2Cl4 SeS3

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

Give the electron geometry, molecular geometry, and hybridization for both carbons in CH3COOH.

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

Match the following. -SF4

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

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CO₂H.

Match the following. -sp³^d²

Determine the electron geometry (eg) and molecular geometry (mg) of ClF₃.

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

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

Consider the following compound. How many sigma and pi bonds does it contain? CH₃CHCHCO₂H

Determine the electron geometry (eg) and molecular geometry (mg) of PF₅.

Give the approximate bond angle in CH₄.

Determine the electron geometry for the molecule PF₃.

How many of the following molecules contain at least one pi bond? C₂H₆ Cl₂CO C₂Cl₄ SeS₃

Give the electron geometry, molecular geometry, and hybridization for both carbons in CH₃COOH.

Match the following. -SF₄