Chapter 7.8, Problem 7.8.2SR

Interpretation Introduction

Interpretation:

The atoms that need hybrid orbitals to describe in ${\text{BCl}}_{\text{3}}$ molecule should be determined.

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 unhybridized 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.