Question 1

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

Accepted Answer

A) True 
 B)False

Question 2

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 $\pi$ and 2 $\sigma$ bonds 
B)  2 $\pi$ and 1 $\sigma$  bonds 
C)  2 $\pi$ and 2 $\sigma$  bonds 
D)  0 $\pi$ and 2 $\sigma$  bonds 
E)  0 $\pi$ and 3 $\sigma$  bonds 
A)  1 $\pi$ and 2 $\sigma$ bonds 
B)  2 $\pi$ and 1 $\sigma$  bonds 
C)  2 $\pi$ and 2 $\sigma$  bonds 
D)  0 $\pi$ and 2 $\sigma$  bonds 
E)  0 $\pi$ and 3 $\sigma$  bonds

Question 3

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

Accepted Answer

A)  ($\sigma$) only 
B)  ($\sigma$) and $\sigma$* 
C)  ($\pi$) only 
D)  ($\pi$) and $\pi$* 
E)  ($\sigma$) and $\pi$ 
A)  ($\sigma$) only 
B)  ($\sigma$) and $\sigma$* 
C)  ($\pi$) only 
D)  ($\pi$) and $\pi$* 
E)  ($\sigma$) and $\pi$

Question 4

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

Accepted Answer

A) True 
 B)False

Question 5

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

Accepted Answer

A) True 
 B)False

Question 6

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

Accepted Answer

A) True 
 B)False

Question 7

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

Question 8

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

Accepted Answer

A)  BeCl2 
B)  Br2 
C)  BF3 
D)  IBr 
E)  CO2 
A)  BeCl2 
B)  Br2 
C)  BF3 
D)  IBr 
E)  CO2

Question 9

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 $\pi$ and 1 $\sigma$  bonds 
B)  2 $\pi$ and 1 $\sigma$ bonds 
C)  1 $\pi$ and 2 $\sigma$ bonds 
D)  0 $\pi$ and 2 $\sigma$ bonds 
E)  0 $\pi$ and 3 $\sigma$ bonds 
A)  1 $\pi$ and 1 $\sigma$  bonds 
B)  2 $\pi$ and 1 $\sigma$ bonds 
C)  1 $\pi$ and 2 $\sigma$ bonds 
D)  0 $\pi$ and 2 $\sigma$ bonds 
E)  0 $\pi$ and 3 $\sigma$ bonds

Question 10

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 2 
A)  C2 2 2 2 
B)  Be2 2 2 2 
C)  N2 2 2 2 
D)  N2 2 2 2 
E)  Be2 2 2 2

Question 11

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$\circ$. 
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$\circ$.

Question 12

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

Accepted Answer

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

Question 13

The number of pi bonds in the molecule below is

Accepted Answer

A)  2 
B)  4 
C)  6 
D)  10 
E)  15 
A)  2 
B)  4 
C)  6 
D)  10 
E)  15

Question 14

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

Accepted Answer

A) True 
 B)False

Question 15

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

Accepted Answer

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

Question 16

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, linear 
A)  0 lone pairs, linear 
B)  1 lone pair, bent 
C)  2 lone pair, bent 
D)  3 lone pairs, bent 
E)  3 lone pairs, linear

Question 17

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

Question 18

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

Accepted Answer

A) True 
 B)False

Question 19

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$\circ$. 
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$\circ$.

Question 20

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

Accepted Answer

A)  Four 
B)  Eight 
C)  Ten 
D)  Twelve 
E)  None of the above 
A)  Four 
B)  Eight 
C)  Ten 
D)  Twelve 
E)  None of the above

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

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

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

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

There are two π\piπ -bonds in C2H4.

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

There is one π\piπ -bond in N2H2.

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

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

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

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

The bond angles in SF5+ are expected to be

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

The number of pi bonds in the molecule below is

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

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

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

The geometry of the ClF3 molecule is best described as:

There are no π\piπ -bonds in C2H6.

The bond angles in CO32- are expected to be

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

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

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

There are two $\pi$ -bonds in C₂H₄.

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

There is one $\pi$ -bond in N₂H₂.

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

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

The bond angles in SF₅⁺ are expected to be

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

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

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

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

The geometry of the ClF₃ molecule is best described as:

There are no $\pi$ -bonds in C₂H₆.

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

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