Covalent Bonding Concepts Assessment

Refer to the graph.

Which position which represents the most stable bond length?

• A

• B

• C

• Bonds are stable at any point on this graph.

Which choice explains the flow of energy when bonded atoms separate from each other?

• Energy is released.

• Energy is absorbed.

• No energy change occurs.

• One atom released energy while the other atom absorbs energy.

Refer to the graph.

How is bond energy related to bond length?

• As the bond length between atoms decreases, bond energy increases and then decreases

• As the bond length between atoms decreases, bond energy decreases and then increases.

• As the bond length between atoms decreases, bond energy remains the same.

Identify the following bonding interactions as ionic or covalent.

Groups:

(a) Ionically Bonded

,

(b) Covalently Bonded

• Li - N

• Se - F

• Cu - Cl

• N - O

• C - H

Which of the following covalent interactions has the greatest bond dissociation energy?

• C-O

• C=O

• C-N

• C=N

Which of the following covalent interactions results in the longest bond?

• C-C

• C-O

• C-N

• C-H

Which of the following bonds is most polar?

• H-F

• H-C

• H-O

• H-N

Why are polar bonds stronger than nonpolar bonds?

• The atomic radii of the two bonding atoms are similar.

• The atomic radii of the two bonding atoms are different.

• The electronegativity difference between the two bonding atoms is smaller.

• The electronegativity difference between the two bonding atoms is larger.

What is the relationship between bond length and bond energy.?

• Direct relationship - the shorter the bond the lower the bond energy.

• Inverse relationship - the longer the bond the lower the bond energy.

• Exponential relationship - if the bond length increases by 1 nm, the bond energy increases by a factor of 10

• Bond length is not related to bond energy.

Which of the following best describes bond order?

• As bond order increase, fewer electrons are shared and bond length decreases

• As bond order increases, fewer electrons are shared and bond length increases

• As bond order increases, more electrons are shared and bond length increases

• As bond order increases, more electrons are shared and bond length decreases