Chapter 5, Problem 5.12P

Interpretation Introduction

Interpretation:

Reason for the differences in bond lengths of the given $C-C$ single bonds has to be explained.

Concept Introduction:

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.

Bond length is the distance between the nuclei in a bond and it is related to the sum of the covalent radii at the bonded atoms.

${\text{sp}}^{\text{3}}$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.

${\text{sp}}^2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.

$\text{sp }$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.

Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.

Pi (π) bonds are 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.