Chapter 8, Problem 112A

Interpretation Introduction

(a)

Interpretation:

Molecular shape, bond angle and hybrid orbital of ${\text{SCl}}_{\text{2}}$ needs to be explained.

Concept introduction:

Lewis structure is also called as Lewis dot structure. In this structure, valence electrons are represented by dot symbol around the central atom. This structure shows the bonding between molecule and the lone pairs which may occur in the molecule.

Answer to Problem 112A

Molecular shape of ${\text{SCl}}_{\text{2}}$ is bent, its bond angle is $104.5°$ and hybridization is $s{p}^3$.

Explanation of Solution

Valence electron of Cl is 7 and S is 6. Total number of valence electrons in ${\text{SCl}}_{\text{2}}$ is $6+7\times 2=20$. Total number of bonding pair is $\frac{20\text{electrons}}{2\text{electrons}}=10\text{pairs}$. Hence, 10 electron pairs are available for bonding. Lewis structure of ${\text{SCl}}_{\text{2}}$ as follows:

Central atom contains total 4 pair of electrons, two non bonding pairs and 2 bonding electron pairs. The molecular shape of ${\text{SCl}}_{\text{2}}$ is bent, its bond angle is $104.5°$ and hybridization is $s{p}^3$.

Interpretation Introduction

(b)

Interpretation:

Molecular shape, bond angle and hybrid orbital of ${\text{NH}}_2\text{Cl}$ needs to be explained.

Concept introduction:

Lewis structure is also called as Lewis dot structure. In this structure, valence electrons are represented by dot symbol around the central atom. This structure shows the bonding between molecule and the lone pairs which may occur in the molecule.

Answer to Problem 112A

Molecular shape of ${\text{NH}}_2\text{Cl}$ is trigonal pyramidal, its bond angle is $107.3°$ and hybridization is $s{p}^3$.

Explanation of Solution

Valence electron of both N is 5, Cl is 7 and H is 1. Total number of valance electrons in ${\text{NH}}_2\text{Cl}$ is $5+7+1\times 2=14$. Total number of bonding pair is $\frac{14\text{electrons}}{2\text{electrons}}=7\text{pairs}$. Hence, 7 electron pairs are available for bonding. Lewis structure of ${\text{NH}}_2\text{Cl}$ as follows:

Central atom contains total 4 pair of electrons, one non bonding pair and 3 bonding electron pairs. The molecular shape of ${\text{NH}}_2\text{Cl}$ is trigonal pyramidal, its bond angle is $107.3°$ and hybridization is $s{p}^3$.

Interpretation Introduction

(c)

Interpretation:

Molecular shape, bond angle and hybrid orbital of $\text{HOF}$ needs to be explained.

Concept introduction:

Lewis structure is also called as Lewis dot structure. In this structure, valence electrons are represented by dot symbol around the central atom. This structure shows the bonding between molecule and the lone pairs which may occur in the molecule.

Answer to Problem 112A

Molecular shape of $\text{HOF}$ is bent, its bond angle is $104.5°$ and hybridization is $s{p}^3$.

Explanation of Solution

Valence electron of both O is 6, F is 7 and H is 1. Total number of valence electrons in $\text{HOF}$ is $6+7+1=14$. Total number of bonding pair is $\frac{14\text{electrons}}{2\text{electrons}}=7\text{pairs}$. Hence, 7 electron pairs are available for bonding. Lewis structure of $\text{HOF}$ as follows:

Central atom contains total 4 pair of electrons, two non bonding pair and 2 bonding electron pairs. The molecular shape of $\text{HOF}$ is bent, its bond angle is $104.5°$ and hybridization is $s{p}^3$.

Interpretation Introduction

(d)

Interpretation:

Molecular shape, bond angle and hybrid orbital of ${\text{BF}}_{\text{3}}$ needs to be explained.

Concept introduction:

Lewis structure is also called as Lewis dot structure. In this structure, valence electrons are represented by dot symbol around the central atom. This structure shows the bonding between molecule and the lone pairs which may occur in the molecule.

Answer to Problem 112A

Molecular shape of ${\text{BF}}_{\text{3}}$ is trigonal planar, its bond angle is $120°$ and hybridization is $s{p}^2$.

Explanation of Solution

Valance electron of B is 3 and F is 7. Hence, total number of valance electron is $3+3\times 7=24$. Total number of bonding pair is $\frac{24\text{electrons}}{2\text{electrons}}=12\text{pairs}$. Hence, 12 electron pairs are available for bonding. Lewis structure of ${\text{BF}}_{\text{3}}$ as follows:

Central atom contains total 3 bonding electron pairs. The molecular shape of ${\text{BF}}_{\text{3}}$ is trigonal planar, its bond angle is $120°$ and hybridization is $s{p}^2$.