Question 1

Which of the following statements is TRUE?

Accepted Answer

A)   The total number of molecular orbitals formed doesn't always equal the number of atomic orbitals in the set.
B)   A bond order of 0 represents a stable chemical bond.
C)   When two atomic orbitals come together to form two molecular orbitals, one molecular orbital will be lower in energy than the two separate atomic orbitals and one molecular orbital will be higher in energy than the separate atomic orbitals.
D)   Electrons placed in antibonding orbitals stabilize the ion/molecule.

Question 2

Use the molecular orbital diagram shown to determine which of the following is most stable. 22⁺ B)  N22⁺ C)  B2 D)  C22⁻ E)  B22⁺" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   C22⁺
B)   N22⁺
C)   B2
D)   C22⁻
E)   B22⁺

Question 3

How many of the following molecules are polar? 
XeO2 SiCl2Br2 C2Br2 SeCl6

Accepted Answer

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

Question 4

Determine the electron geometry (eg)  and molecular geometry (mg)  of XeF4.

Accepted Answer

A)   eg = tetrahedral, mg = tetrahedral
B)   eg = linear, mg = linear
C)   eg = tetrahedral, mg = bent
D)   eg = trigonal bipyramidal, mg = tetrahedral
E)   eg = octahedral, mg = square planar

Question 5

A molecule or ion with seven electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of ________.

Accepted Answer

A)   0.5
B)   1
C)   1.5
D)   2
E)   2.5

Question 6

Determine the molecular geometry for the molecule PF3.

Accepted Answer

A)   Trigonal pyramidal
B)   Trigonal planar
C)   Tetrahedral
D)   T-shaped
E)   Bent

Question 7

In molecular orbital theory the acronym LCAO stands for ________.

Accepted Answer

A)   linear combination of atomic orbitals
B)   lowest combined atomic orbitals
C)   least consumed advanced orientation
D)   linearly created available orbital
E)   It has no meaning.

Question 8

Use the molecular orbital diagram shown to determine which of the following is least stable. 22⁺ B)  N22⁺ C)  B2 D)  C22⁻ E)  B2⁺" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   C22⁺
B)   N22⁺
C)   B2
D)   C22⁻
E)   B2⁺

Question 9

Draw the Lewis structure for COCl2. What is the hybridization on the C atom?

Accepted Answer

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

Question 10

Draw the Lewis structure for N2H2. What is the hybridization on the N atoms?

Accepted Answer

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

Question 11

What is the molecular geometry of Te Cl4?

Accepted Answer

A)   seesaw
B)   square planar
C)   square pyramidal
D)   tetrahedral

Question 12

Give the approximate bond angle for a molecule with a tetrahedral shape.

Accepted Answer

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

Question 13

Determine the molecular geometry (mg)  of the bolded and underlined atom CH3CH2OH.

Accepted Answer

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

Question 14

Place the following in order of increasing dipole moment. I. BCl3 II. BIF2  III. BClF2

Accepted Answer

A)   I 
B)   II 
C)   I 
D)   II 
E)   I < III < II

Question 15

Give the approximate bond angle for a molecule with trigonal bipyramidal electron geometry and linear molecular geometry.

Accepted Answer

A)   180°
B)   
C)   >180°
D)   
E)   <120°

Question 16

Draw the Lewis structure for S 3d2 C)  sp3d D)  sp3 E)  sp2" class="answers-bank-image d-inline" rel="preload" > . What is the hybridization on the S atom?

Accepted Answer

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

Question 17

Give the approximate bond angle in H2O.

Accepted Answer

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

Question 18

Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Accepted Answer

Yes. The polarity of a molecule depends ...

Question 19

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Accepted Answer

A)   GeH2Br2
B)   SCl2
C)   AsCl5
D)   CF2Cl2

Question 20

Consider the molecule below. Determine the molecular geometry at each of the two labelled carbons.

Accepted Answer

A)   C1 = tetrahedral, C2 = linear
B)   C1 = trigonal planar, C2 = bent
C)   C1 = bent, C2 = trigonal planar
D)   C1 = trigonal planar, C2 = tetrahedral
E)   C1 = trigonal pyramidal, C2 = seesaw

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

Use the molecular orbital diagram shown to determine which of the following is most stable.

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Place the following in order of increasing dipole moment. I. BCl3 II. BIF2 III. BClF2

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Choose the compound below that contains at least one polar covalent bond but is nonpolar.

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Which of the following statements is TRUE?

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Give the approximate bond angle for a molecule with trigonal bipyramidal electron geometry and linear molecular geometry.

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In molecular orbital theory the acronym LCAO stands for ________.

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Draw the Lewis structure for COCl2. What is the hybridization on the C atom?

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Draw the Lewis structure for S . What is the hybridization on the S atom?

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Determine the molecular geometry (mg) of the bolded and underlined atom CH3CH2OH.

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Give the approximate bond angle in H2O.

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A molecule or ion with seven electrons in bonding orbitals and two electrons in an antibonding orbital has a bond order of ________.

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Is it possible for a molecule to be nonpolar even though it contains polar bonds? Explain your answer and give an example.

Correct AnswerverifiedYes. The polarity of a molecule depends ...View AnswerShow Answer

Draw the Lewis structure for N2H2. What is the hybridization on the N atoms?

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What is the molecular geometry of Te Cl4?

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Determine the molecular geometry for the molecule PF3.

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How many of the following molecules are polar? XeO2 SiCl2Br2 C2Br2 SeCl6

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Give the approximate bond angle for a molecule with a tetrahedral shape.

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Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

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Consider the molecule below. Determine the molecular geometry at each of the two labelled carbons.

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Use the molecular orbital diagram shown to determine which of the following is least stable.

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Place the following in order of increasing dipole moment. I. BCl₃ II. BIF₂ III. BClF₂

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Draw the Lewis structure for COCl₂. What is the hybridization on the C atom?

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Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH.

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Give the approximate bond angle in H₂O.

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Yes. The polarity of a molecule depends ...
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Draw the Lewis structure for N₂H₂. What is the hybridization on the N atoms?

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What is the molecular geometry of Te Cl₄?

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Determine the molecular geometry for the molecule PF₃.

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How many of the following molecules are polar? XeO₂ SiCl₂Br₂ C₂Br₂ SeCl₆

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Determine the electron geometry (eg) and molecular geometry (mg) of XeF₄.

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