Correct Answer - Option 3 : Greater than the number of antibonding electrons
Concept:
Bond factor (BF) is defined as:
BF= \(\frac{1}{2}\) ( Bonding electrons in the molecule – antibonding electrons in the molecule)
Observations:
When the bond factor is “zero”, the molecule is highly unstable. Hence the bond factor must be greater than zero.
Based on this, if the bond factor is assumed as 1, i.e.
1 = \(\frac{1}{2}\) ( Bonding electrons in the molecule – anti-bonding electrons in the molecule)
2 = Bonding electrons in the molecule – antibonding electrons in the molecule
Bonding electrons in the molecule = 2 + antinbonding electrons in the molecule