Chapter 10, Problem 10.55QP

Interpretation Introduction

Interpretation:

By using molecular orbital theory, the bond order in given species has to be compared.

Concept introduction:

Molecular orbital theory

The atomic orbitals involved in bonding actually combine to form new orbitals that are the “property” of the entire molecule, rather than of the individual atoms forming the bonds.  These new orbitals are called molecular orbitals.

• In molecular orbital theory, electrons shared by atoms in a molecule reside in the molecular orbitals.
• If longer the bond the weaker the bond and this rule will help you while analysing this concept.
• Higher the bond order, the more stable the bond.

Bond order

The number of chemical bonds between a pair of atoms i.e., diatomic molecules is said to be bond order.

$\text{Bond}\text{order = }\frac{\text{number}\text{of}\text{bonding}\text{electrons - number}\text{of}\text{atibondiong}\text{electrons}}{\text{2}}$

• We can justify the order of increasing stability by using bond order and molecular orbital diagram.