Chapter 1, Problem 1.51SP

1.

Interpretation Introduction

To determine: The hybridization and approximate bond angles around each of the given atom except hydrogen.

Interpretation: The hybridization and approximate bond angles around each of the given atom except hydrogen are to be shown.

Concept introduction: The hybridization is a theoretical phenomenon which explains the bonding pattern within the molecule. There are various types of hybridization involved in chemical bonding. Generally three main types are as follows,

• $\text{sp}$
• ${\text{sp}}^2$
• ${\text{sp}}^3$

In the first type one “s” and one “p” orbitals are mixed with each other and form two new “$\text{sp}$” hybridized orbitals of new energies.

In the second type one “s” and two “p” orbitals are mixed with each other and form three new “${\text{sp}}^2$” hybridized orbitals of new energies.

In the third type one “s” and three “p” orbitals are mixed with each other and form four new “${\text{sp}}^3$” hybridized orbitals of new energies.

The bond angles in “$\text{sp}$”, “${\text{sp}}^2$” and “${\text{sp}}^3$” hybridization are $180°,120°$ and $109.5°$ respectively.

2.

Interpretation Introduction

To determine: The three-dimensional diagrams of the given compounds with the representation of lone pairs of electron.

Interpretation: The three-dimensional diagrams of the given compounds with the representation of lone pairs of electron are to be shown.

Concept introduction: The three-dimensional representation of the molecule is described by the type of hybridization present in the molecule. On the basis of hybridization the bonding and non-bonding electrons are calculated. The bonding electrons are represented by single, double or triple bonds. The non-bonding electrons are represented by lone pairs of electron.