Question

What is incorrect for Bond order?

• A. Represents the number of bonds present between a compound/molecule
• B. Bond order decreases with bond energy
• C. Bond order increases with bond energy
• D. Bond order inversely proportional to bond length

Hint:

Bond order is a key concept in molecular orbital theory. Higher bond order generally indicates a stronger, shorter bond, whereas lower bond order corresponds to weaker, longer bonds.

Answer 1

The Correct Option is B

Bond order refers to the number of bonds between two atoms in a molecule. It can be calculated as: \[ \text{Bond order} = \frac{1}{2} \left( \text{number of electrons in bonding orbitals} - \text{number of electrons in anti-bonding orbitals} \right) \] Now let's analyze the options:
- (A) This is correct. Bond order represents the number of bonds.
- (B) This is incorrect. Bond order increases with bond energy because stronger bonds (higher bond energy) correspond to higher bond orders.
- (C) This is correct. Bond order increases with bond energy.
- (D) This is correct. Bond order is inversely proportional to bond length. The greater the bond order, the shorter the bond length.

Thus, the incorrect statement is \( (B) \), as bond order increases with bond energy.