Compared to the bond in the N_2 molecule, is the bond in the N_2^+ ion stronger or weaker?

• A. N_2^+ does not have a bond.
• B. The bond in N_2^+ is weaker than in N_2.
• C. The bond strength is the same in both N_2^+ and N_2.
• D. The bond in N_2^+ is stronger than in N_2.

Answer: (B)

Verified step by step guidance

1. Recall that the bond strength in diatomic molecules like N_2 depends on the bond order, which is related to the number of bonding and antibonding electrons in molecular orbitals.
2. Write the electron configuration for the neutral N_2 molecule using molecular orbital theory. N_2 has 14 electrons filling bonding and antibonding orbitals.
3. Calculate the bond order for N_2 using the formula: \(\text{Bond order} = \frac{(\text{number of bonding electrons}) - (\text{number of antibonding electrons})}{2}\).
4. For the N_2^+ ion, remove one electron from the highest occupied molecular orbital of N_2, then recalculate the bond order using the same formula.
5. Compare the bond orders of N_2 and N_2^+. A higher bond order corresponds to a stronger bond, so determine whether the bond in N_2^+ is stronger or weaker based on this comparison.