Chapter 3, Problem 3.35P

Interpretation Introduction

Interpretation:

A single bond connecting an $\text{sp}$-hybridized carbon atom to an ${\text{sp}}^{\text{2}}$-hybridized carbon atom from the listed molecules is to be identified.

Concept introduction:

According to the Valence bond (VB) theory, the hybridization of atomic orbitals is used to account for electron and molecular geometry around the central atom. A hybrid orbital is a combination of one or more atomic orbitals from the valence shell of an atom.

The number of hybrid orbitals required is the same as the number of electron groups. If the number of electron groups is two, two-hybrid orbitals are needed. These are formed by a combination of s and one p orbital, giving $\text{sp}$ hybridization. For three electron groups, three hybrid orbitals are required, s and two of the p orbitals giving ${\text{sp}}^2$ hybridization. Four groups require four orbitals giving ${\text{sp}}^{\text{3}}$ hybridization.