Molecular Orbital Theory

Let’s break this down step by step to calculate the bond orders and unpaired electrons for the O species and determine why option (1) is the correct answer.
Step 1: Determine the molecular orbital configuration and bond order
O has 12 valence electrons. Using molecular orbital (MO) theory:

• O (12 valence electrons):
  Bonding electrons = 8, antibonding = 4, bond order = , unpaired electrons = 2.
• O (11 valence electrons):
  Bonding electrons = 8, antibonding = 3, bond order = , unpaired electrons = 1.
• O (13 valence electrons):
  Bonding electrons = 8, antibonding = 5, bond order = , unpaired electrons = 1.
• O (14 valence electrons):
  Bonding electrons = 8, antibonding = 6, bond order = , unpaired electrons = 0.

Assuming O is included:

• O (10 valence electrons):
  Bonding electrons = 8, antibonding = 2, bond order = , unpaired electrons = 0.

Step 2: Sum the bond orders and unpaired electrons

• Bond orders:
• Unpaired electrons:

Step 3: Confirm the correct answer
The sum of bond orders is 10, and the sum of unpaired electrons is 4, matching option (1).
Thus, the correct answer is (1) 10, 4.