Chapter 10, Problem 10.28QP

(a)

Interpretation Introduction

Interpretation:

• The concept of hybridization of atomic orbitals has to be discussed.
• It is impossible for an isolated atom to exist in the hybridized state. This statement has to be reasoned out.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the different atomic orbitals which results in the formation of a new set of hybrid orbitals that have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

(b)

Interpretation Introduction

Interpretation: The difference between a hybrid orbital and a pure atomic orbital has to be discussed.

Whether two $\text{2p}$ orbitals of an atom hybridize to give two hybridized orbitals or not has to be discussed.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the different atomic orbitals which results in the formation of a new set of hybrid orbitals that have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$