Question

The sum of bond order values of \( C_2 \) and \( O_2^{2-} \) is \( x \), which is equal to the sum of bond order values of \( a, b, \) and \( c \). What are \( a, b, \) and \( c \)?

• A. \( O_2, O_2^+, O_2 \)
• B. \( B_2, N_2, F_2 \)
• C. \( He_2^+, F_2, N_2 \)
• D. \( O_2^{2-}, N_2, Be_2 \)

Hint:

For molecular orbital-based bond orders, sum the bonding and antibonding electrons carefully.

Answer 1

The Correct Option is B

Step 1: Bond Order Calculation Bond order is determined using the formula: \[ \text{Bond Order} = \frac{\text{Number of bonding electrons} - \text{Number of antibonding electrons}}{2} \] Using Molecular Orbital Theory, the bond orders are: \[ \text{Bond Order of } C_2 = 2 \] \[ \text{Bond Order of } O_2^{2-} = 2 \] Summing: \[ x = 2 + 2 = 4 \] Step 2: Finding \( a, b, c \) Looking at the bond orders: \[ \text{Bond Order of } B_2 = 1 \] \[ \text{Bond Order of } N_2 = 3 \] \[ \text{Bond Order of } F_2 = 0 \] Summing: \[ 1 + 3 + 0 = 4 \] Conclusion Thus, the correct answer is: \[ B_2, N_2, F_2 \]