alleryBond order in molecular orbital theory is defined as:
A(Bonding e⁻ − Antibonding e⁻) / 2
B(Bonding e⁻ + Antibonding e⁻) / 2
CNumber of bonding electrons alone
D(Antibonding e⁻ − Bonding e⁻) / 2
Answer & Solution
Correct answer: A. (Bonding e⁻ − Antibonding e⁻) / 2
1. Bond order = (N_b − N_a) / 2.
2. Higher bond order → shorter, stronger bond.
3. Examples: H₂ has BO 1 (2 σ_b bonding); He₂ has BO 0 (no net bonding) — that's why He₂ doesn't exist.
_Source: syllabus Chem Ch 4 §4.7 Molecular Orbital Theory_
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