Question

According to Molecular orbital theory, which of the following is correct with respect to bond order?

• A. Bond order of $\text{N}_2^+$ and $\text{O}_2^+$ is less than $\text{O}_2$
• B. Bond order of $\text{N}_2^+$ and $\text{O}_2^+$ is more than $\text{N}_2$
• C. Bond order of $\text{N}_2^+$ is less than $\text{N}_2$ while that of $\text{O}_2^+$ is more than $\text{O}_2$
• D. Bond order of $\text{N}_2^+$ is less than $\text{O}_2$ while that of $\text{O}_2^+$ is more than $\text{O}_2$

Hint:

Remember this straightforward shortcut for diatomic MO configurations:
• Removing an electron from Nitrogen targets a bonding orbital, lowering its bond order from $3$ down to $2.5$.
• Removing an electron from Oxygen targets an antibonding orbital, raising its bond order from $2$ up to $2.5$!

Answer 1

The Correct Option is C