Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

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

Accepted Answer

A) True 
 B)False

Question 3

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) B) and C)
G) None of the above

Question 4

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) D) and E)
G) A) and D)

Question 5

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

Accepted Answer

A) True 
 B)False

Question 6

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

Accepted Answer

A) True 
 B)False

Question 7

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

Accepted Answer

A) True 
 B)False

Question 8

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 B)
G) B) and E)

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) B) and C)
G) A) and B)

Question 10

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) B) and D)
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) D) and E)
G) A) and D)

Question 12

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

Accepted Answer

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

Question 13

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) None of the above
G) B) and C)

Question 14

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) A) and B)
G) A) and C)

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) A) and C)
G) A) and E)

Question 16

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) None of the above
G) A) and C)

Question 17

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) B) and C)
G) B) and D)

Question 18

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 E)

Question 19

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

Accepted Answer

A) True 
 B)False

Question 20

The number of pi bonds in the molecule below is

Accepted Answer

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

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

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

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There are no π\piπ -bonds in C2H6.

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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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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 number of pi bonds in the molecule below is

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

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The geometry of the ClF3 molecule is best described as:

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

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

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The bond angles in SF5+ are expected to be

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

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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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The bond angles in CO32- are expected to be

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

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

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

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There are two π\piπ -bonds in C2H4.

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There is one π\piπ -bond in N2H2.

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

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There are no $\pi$ -bonds in C₂H₆.

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

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The geometry of the ClF₃ molecule is best described as:

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

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

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The bond angles in SF₅⁺ are expected to be

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

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

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

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There are two $\pi$ -bonds in C₂H₄.

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There is one $\pi$ -bond in N₂H₂.

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