For the diatomic molecule N2, which has a total of 14 valence electrons, what is its bond order?

• A. 0
• B. 2
• C. 3
• D. 1

Answer: (C)

Verified step by step guidance

1. Identify the total number of valence electrons for the N\textsubscript{2} molecule. Since each nitrogen atom has 7 valence electrons, the total is 14 electrons.
2. Write the molecular orbital (MO) electron configuration for N\textsubscript{2}. Fill the molecular orbitals in order of increasing energy, considering the correct order for diatomic molecules with atomic number 7 (nitrogen).
3. Count the number of electrons in bonding molecular orbitals (such as \$\sigma_{2s}\$, \$\sigma^*_{2s}\$, \$\pi_{2p}\$, and \$\sigma_{2p}\$) and antibonding molecular orbitals (such as \$\sigma^*_{2s}\$, \$\pi^*_{2p}\$, and \$\sigma^*_{2p}\$).
4. Use the bond order formula: \$\text{Bond order} = \frac{(\text{number of bonding electrons}) - (\text{number of antibonding electrons})}{2}\$
5. Substitute the counted bonding and antibonding electrons into the formula to calculate the bond order, which indicates the strength and stability of the bond in N\textsubscript{2}.