Question 1

Consider the skeletal structure shown below:
N-C-C-N
Draw the Lewis structure and answer the following:
-How many of the atoms are sp hybridized?

Accepted Answer

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

Question 2

Which of the following substances contains two pi bonds?

Accepted Answer

A) C2H4 
B) C3H8 
C) C2H2 
D) C2H6 
E) CH4 
A) C2H4 
B) C3H8 
C) C2H2 
D) C2H6 
E) CH4

Question 3

The hybridization of I in IF4- is

Accepted Answer

A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3 
A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3

Question 4

Whenever a set of equivalent tetrahedral atomic orbitals is required,an atom will adopt a set of sp3 orbitals.

Accepted Answer

A) True 
 B)False

Question 5

A(n)__________ molecular orbital is lower in energy than the atomic orbital of which it is composed.

Accepted Answer

The answer of A(n)__________ molecular orbital is lower in energy...

Question 6

Which of the following are paramagnetic?
O2 O2- O22- B2 C2 N2 F2 CN- P2

Accepted Answer

Question 7

In the molecule C2H4 the valence orbitals of the carbon atoms are assumed to be

Accepted Answer

A) not hybridized 
B) sp hybridized 
C) sp2 hybridized 
D) sp3 hybridized 
E) dsp hybridized 
A) not hybridized 
B) sp hybridized 
C) sp2 hybridized 
D) sp3 hybridized 
E) dsp hybridized

Question 8

Which of the following statements is incorrect?

Accepted Answer

A) For the molecule NO,the molecular orbital model is preferred over the localized electron model because NO contains an unpaired electron. 
B) Electrons in antibonding orbitals will cause a molecule to be paramagnetic. 
C) According to the molecular orbital model,when bonding occurs between hydrogen and bromine to make HBr,the 1s orbital of the hydrogen atom no longer exists. 
D) Antibonding electrons are higher in energy than the atomic orbitals from which they came. 
E) At least two of the above are incorrect. 
A) For the molecule NO,the molecular orbital model is preferred over the localized electron model because NO contains an unpaired electron. 
B) Electrons in antibonding orbitals will cause a molecule to be paramagnetic. 
C) According to the molecular orbital model,when bonding occurs between hydrogen and bromine to make HBr,the 1s orbital of the hydrogen atom no longer exists. 
D) Antibonding electrons are higher in energy than the atomic orbitals from which they came. 
E) At least two of the above are incorrect.

Question 9

Which of the following species has the largest dissociation energy?

Accepted Answer

A) O2 
B) O2- 
C) O22- 
D) O2+ 
E) O22+ 
A) O2 
B) O2- 
C) O22- 
D) O2+ 
E) O22+

Question 10

Consider the molecule and the following hybridization choices:  
-What is the hybridization of the carbon atom that is double-bonded to oxygen?

Accepted Answer

A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3 
A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3

Question 11

Tetracyanoethylene has the skeleton shown below:   From its Lewis structure determine the following:
-How many nonbonded electron pairs are in the molecule?

Accepted Answer

A) 0 
B) 2 
C) 4 
D) 5 
E) 8 
A) 0 
B) 2 
C) 4 
D) 5 
E) 8

Question 12

The hybridization of Cl in ClF2+ is

Accepted Answer

A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3 
A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3

Question 13

Which of the following species is paramagnetic?

Accepted Answer

A) C2 
B) O2 
C) F2 
D) Li2 
E) none of these 
A) C2 
B) O2 
C) F2 
D) Li2 
E) none of these

Question 14

What is the bond order of Ne2?

Accepted Answer

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

Question 15

A $\pi$ (pi)bond is the result of the

Accepted Answer

A) overlap of two s orbitals 
B) overlap of an s orbital and a p orbital 
C) overlap of two p orbitals along their axes 
D) sidewise overlap of two parallel p orbitals 
E) sidewise overlap of two s orbitals 
A) overlap of two s orbitals 
B) overlap of an s orbital and a p orbital 
C) overlap of two p orbitals along their axes 
D) sidewise overlap of two parallel p orbitals 
E) sidewise overlap of two s orbitals

Question 16

The H2- ion is more stable than H2 since it has an additional electron to produce a net lowering of energy.

Accepted Answer

A) True 
 B)False

Question 17

The concept of __________ is required for certain molecules because the localized electron model assumes electrons are located between a given pair of atoms in a molecule.

Accepted Answer

The answer of The concept of __________ is required for...

Question 18

Larger bond order means greater bond strength.

Accepted Answer

A) True 
 B)False

Question 19

Which of the following has a bond order of 1.5?

Accepted Answer

A) O2+ 
B) N2 
C) O2- 
D) C2 
E) none of these 
A) O2+ 
B) N2 
C) O2- 
D) C2 
E) none of these

Question 20

The hybridization of Se in SeF6 is

Accepted Answer

A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3 
A) sp 
B) sp2 
C) sp3 
D) dsp3 
E) d2sp3

Exam 9: Covalent Bonding: Orbitals

Consider the skeletal structure shown below: N-C-C-N Draw the Lewis structure and answer the following: -How many of the atoms are sp hybridized?

Which of the following substances contains two pi bonds?

The hybridization of I in IF4- is

Whenever a set of equivalent tetrahedral atomic orbitals is required,an atom will adopt a set of sp3 orbitals.

A(n)__________ molecular orbital is lower in energy than the atomic orbital of which it is composed.

Which of the following are paramagnetic? O2 O2- O22- B2 C2 N2 F2 CN- P2

In the molecule C2H4 the valence orbitals of the carbon atoms are assumed to be

Which of the following statements is incorrect?

Which of the following species has the largest dissociation energy?

Consider the molecule and the following hybridization choices: -What is the hybridization of the carbon atom that is double-bonded to oxygen?

Tetracyanoethylene has the skeleton shown below: From its Lewis structure determine the following: -How many nonbonded electron pairs are in the molecule?

The hybridization of Cl in ClF2+ is

Which of the following species is paramagnetic?

What is the bond order of Ne2?

A π\piπ (pi)bond is the result of the

The H2- ion is more stable than H2 since it has an additional electron to produce a net lowering of energy.

The concept of __________ is required for certain molecules because the localized electron model assumes electrons are located between a given pair of atoms in a molecule.

Larger bond order means greater bond strength.

Which of the following has a bond order of 1.5?

The hybridization of Se in SeF6 is

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Filters

The hybridization of I in IF₄^- is

Whenever a set of equivalent tetrahedral atomic orbitals is required,an atom will adopt a set of sp³ orbitals.

Which of the following are paramagnetic? O₂O₂^-O₂²^-B₂C₂N₂F₂CN^-P₂

In the molecule C₂H₄ the valence orbitals of the carbon atoms are assumed to be

The hybridization of Cl in ClF₂⁺ is

What is the bond order of Ne₂?

A $\pi$ (pi)bond is the result of the

The H₂^- ion is more stable than H₂ since it has an additional electron to produce a net lowering of energy.

The hybridization of Se in SeF₆ is