Chapter 7.8, Problem 7.8.3SR

Interpretation Introduction

Interpretation:

It should be checked that can hybrid orbital be used to explain how a central atom can form more bonds than the number of unpaired electrons in its ground state configuration.

Concept introduction:

According to valence bond theory,

• The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.
• The each overlapping atomic orbital must be contained with a single unpaired.
• Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

  Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

  Pi (π) bonds: the bonds in which shared un-hybridized orbital’s (p, d, etc.) electron density are concentrated in above and below of the plane of the molecule.

  Double bonds: One sigma bond and one pi bond are together known as a double bond.