Which of the following conversion, product bond order increases compared to reactant bond order? 

CONCEPT:

Bond Order

Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2

• The bond order of a molecule is defined as the difference between the number of bonding electrons and antibonding electrons, divided by 2:
• A higher bond order indicates a stronger and shorter bond, while a lower bond order indicates a weaker and longer bond.
• When an electron is removed (oxidation) or added (reduction) to a molecule, the bond order may change depending on whether the electron is removed from or added to a bonding or antibonding molecular orbital.

EXPLANATION:

• For the given options, we will calculate the bond order of the reactant and product:
•  N₂ → N₂⁺
  • N₂ bond order = (14 - 8) / 2 = 3
  • N₂⁺ bond order = (13 - 8) / 2 = 2.5
  • The bond order decreases in this case, so this is incorrect.
•  O₂ → O₂^-
  • O₂ bond order = (10 - 6) / 2 = 2
  • O₂⁺ bond order = (16 - 7) / 2 = 1.5
  • The bond order increases in this case, so this is incorrect.
    
•  NO → NO⁺
  • NO bond order = (10 - 5) / 2 = 2.5
  • NO⁺ bond order = (10 - 4) / 2 = 3
  • The bond order increases in this case, so this is correct.
    
•  NO → NO^-
  • NO bond order = (10 - 5) / 2 = 2.5
  • NO^- bond order = (10 - 6) / 2 = 2
  • The bond order decreases in this case, so this is incorrect.

Correct Answer: Option 3