Question 1

Consider the species N2-, N2, and N2+. Which of these species will be paramagnetic

Accepted Answer

A)   N2 and N2-
B)   N2+ and N2
C)   N2+ and N2-
D)   only N2-
E)   none are paramagneticF) C) and E)
G) A) and C)

Question 2

According to Molecular Orbital Theory, two separate 1s orbitals interact to form what molecular orbital(s)

Accepted Answer

A)   ( σ\sigmaσ )  only
B)   ( σ\sigmaσ )  and  σ\sigmaσ *
C)   ( π\piπ )  only
D)   ( π\piπ )  and  π\piπ *
E)   ( σ\sigmaσ )  and  π\piπF) C) and D)
G) A) and B)

Question 3

Shown here is the correct Lewis structure for PF5. According to VSEPR theory how many electrons are bonded to the P atom 5. According to VSEPR theory how many electrons are bonded to the P atom   A)  Four B)  Eight C)  Ten D)  Twelve E)  None of the above" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Four
B)   Eight
C)   Ten
D)   Twelve
E)   None of the aboveF) B) and C)
G) A) and E)

Question 4

Which one of the following molecules has a non-zero dipole moment

Accepted Answer

A)   BeCl2
B)   Br2
C)   BF3
D)   IBr
E)   CO2F) A) and C)
G) A) and B)

Question 5

A sp2 hybridized terminal oxygen atom (bonded to one other atom only)  with 2 lone pairs of electrons has what type of bonding

Accepted Answer

A)   1  π\piπ  and 1  σ\sigmaσ   bonds
B)   2  π\piπ  and 1  σ\sigmaσ  bonds
C)   1  π\piπ  and 2  σ\sigmaσ  bonds
D)   0  π\piπ  and 2  σ\sigmaσ  bonds
E)   0  π\piπ  and 3  σ\sigmaσ  bonds F) All of the above
G) B) and E)

Question 6

Indicate the type of hybrid orbitals used by the central atom in CCl4.

Accepted Answer

A)   sp
B)   sp2
C)   sp3
D)   sp3d
E)   sp3d2F) A) and D)
G) B) and C)

Question 7

The geometrical structure of PF5 and IF5 are both square pyramidal.

Accepted Answer

A) True 
 B)False

Question 8

Two py orbitals from two different atoms can interact to form a pi bonding molecular orbital.

Accepted Answer

A) True 
 B)False

Question 9

The bond angles in CO32- are expected to be

Accepted Answer

A)   a little less than 109.5 ∘\circ∘ .
B)   109.5 ∘\circ∘ .
C)   a little less than 120 ∘\circ∘ .
D)   120 ∘\circ∘ .
E)   a little more than 120 ∘\circ∘ . F) A) and D)
G) B) and E)

Question 10

The geometry of the ClF3 molecule is best described as:

Accepted Answer

A)   distorted tetrahedron
B)   trigonal planar
C)   tetrahedral
D)   T-shaped
E)   trigonal pyramidalF) A) and C)
G) B) and C)

Question 11

Which of the following correctly lists species in order of increasing bond order

Accepted Answer

A)   C2 2 2 2
B)   Be2 2 2 2
C)   N2 2 2 2
D)   N2 2 2 2
E)   Be2 2 2 2F) B) and E)
G) B) and D)

Question 12

There are no $\pi$-bonds in C2H6.

Accepted Answer

A) True 
 B)False

Question 13

There are two $\pi$-bonds in C2H4.

Accepted Answer

A) True 
 B)False

Question 14

There is one $\pi$-bond in N2H2.

Accepted Answer

A) True 
 B)False

Question 15

Give the number of lone pairs around the central atom and the geometry of the ion NO2-.

Accepted Answer

A)   0 lone pairs, linear
B)   1 lone pair, bent
C)   2 lone pair, bent
D)   3 lone pairs, bent
E)   3 lone pairs, linearF) All of the above
G) A) and B)

Question 16

The number of pi bonds in the molecule below is

Accepted Answer

A)   2
B)   4
C)   6
D)   10
E)   15F) A) and E)
G) B) and E)

Question 17

Valence Bond Theory alone can be used to determine that O2 is paramagnetic.

Accepted Answer

A) True 
 B)False

Question 18

The bond angles in SF5+ are expected to be

Accepted Answer

A)   90 ∘\circ∘ .
B)   120 ∘\circ∘ .
C)   90 ∘\circ∘  and 120 ∘\circ∘ .
D)   90 ∘\circ∘  and 180 ∘\circ∘ .
E)   90 ∘\circ∘ , 120 ∘\circ∘ , and 180 ∘\circ∘ . F) A) and D)
G) C) and D)

Question 19

A sp hybridized terminal nitrogen atom (bonded to one other atom only)  with 1 lone pair of electrons has what type of bonding

Accepted Answer

A)   1  π\piπ  and 2  σ\sigmaσ  bonds
B)   2  π\piπ  and 1  σ\sigmaσ   bonds
C)   2  π\piπ  and 2  σ\sigmaσ   bonds
D)   0  π\piπ  and 2  σ\sigmaσ   bonds
E)   0  π\piπ  and 3  σ\sigmaσ   bonds F) A) and B)
G) D) and E)

Question 20

Indicate the type of hybrid orbitals used by the central atom in TeF4.

Accepted Answer

A)   sp
B)   sp2
C)   sp3
D)   sp3d
E)   sp3d2F) C) and E)
G) A) and B)

Exam 10: Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Which of the following correctly lists species in order of increasing bond order

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There are no π\piπ -bonds in C2H6.

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Two py orbitals from two different atoms can interact to form a pi bonding molecular orbital.

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Which one of the following molecules has a non-zero dipole moment

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Indicate the type of hybrid orbitals used by the central atom in CCl4.

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Consider the species N2-, N2, and N2+. Which of these species will be paramagnetic

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A sp hybridized terminal nitrogen atom (bonded to one other atom only) with 1 lone pair of electrons has what type of bonding

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Give the number of lone pairs around the central atom and the geometry of the ion NO2-.

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The bond angles in SF5+ are expected to be

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The geometrical structure of PF5 and IF5 are both square pyramidal.

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Shown here is the correct Lewis structure for PF5. According to VSEPR theory how many electrons are bonded to the P atom

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There is one π\piπ -bond in N2H2.

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The number of pi bonds in the molecule below is

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The bond angles in CO32- are expected to be

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Valence Bond Theory alone can be used to determine that O2 is paramagnetic.

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A sp2 hybridized terminal oxygen atom (bonded to one other atom only) with 2 lone pairs of electrons has what type of bonding

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According to Molecular Orbital Theory, two separate 1s orbitals interact to form what molecular orbital(s)

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The geometry of the ClF3 molecule is best described as:

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Indicate the type of hybrid orbitals used by the central atom in TeF4.

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There are two π\piπ -bonds in C2H4.

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There are no $\pi$ -bonds in C₂H₆.

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Two p_y orbitals from two different atoms can interact to form a pi bonding molecular orbital.

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Indicate the type of hybrid orbitals used by the central atom in CCl₄.

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Consider the species N₂^-, N₂, and N₂⁺. Which of these species will be paramagnetic

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Give the number of lone pairs around the central atom and the geometry of the ion NO₂^-.

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The bond angles in SF₅⁺ are expected to be

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The geometrical structure of PF₅ and IF₅ are both square pyramidal.

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Shown here is the correct Lewis structure for PF₅. According to VSEPR theory how many electrons are bonded to the P atom

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There is one $\pi$ -bond in N₂H₂.

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The bond angles in CO₃^2- are expected to be

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Valence Bond Theory alone can be used to determine that O₂ is paramagnetic.

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A sp² hybridized terminal oxygen atom (bonded to one other atom only) with 2 lone pairs of electrons has what type of bonding

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The geometry of the ClF₃ molecule is best described as:

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Indicate the type of hybrid orbitals used by the central atom in TeF₄.

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There are two $\pi$ -bonds in C₂H₄.

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