Chapter 10, Problem 10.70QP

(a)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{BeCl}}_{\text{2}}$ is ${180}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{BeCl}}_{\text{2}}$.

Lewis structure of the given molecule is drawn below.

${\text{BeCl}}_{\text{2}}$ is a triatomic molecule . Here the central atom beryllium atom does not have any lone pair of electrons whereas both terminal chlorine atoms have 3 pairs of electron. It is a ${\text{AB}}_{\text{2}}$ type molecule. Since there are only two bonds, there is only one bond angle. Since there is no lone pair on the central atom, to minimize the repulsion, they form a linear geometry. So the bond angle between two atoms is ${180}^0$.

(b)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{BCl}}_3$ is ${120}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{BCl}}_3$.

Lewis structure of the given molecule is drawn below.

${\text{BCl}}_3$ contains four atoms. Here the central atom boron atom does not have any lone pair of electrons whereas the terminal chlorine atoms have 3 pairs of electron. It is a ${\text{AB}}_3$ type molecule. Since there are only three bonds, there are  two bond angle. Since there is no lone pair on the central atom, to minimize the repulsion, they form a trigonal planar geometry. So the bond angle between two atoms is ${120}^0$.

(c)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{CCl}}_4$ is ${109.5}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{CCl}}_4$.

Lewis structure of the given molecule is drawn below.

${\text{CCl}}_4$ contains five atoms. Here the central atom carbon atom does not have any lone pair of electrons whereas the terminal chlorine atoms have 3 pairs of electron. It is a ${\text{AB}}_4$ type molecule. Since there is no lone pair on the central atom, to minimize the repulsion, they form a tetrahedral geometry. So the bond angle between two atoms is ${109.5}^0$.

(d)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{CH}}_3\text{Cl}$ is ${109.5}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{CH}}_3\text{Cl}$.

Lewis structure of the given molecule is drawn below.

${\text{CH}}_3\text{Cl}$ contains five atoms. Here the central atom carbon atom does not have any lone pair of electrons whereas the terminal chlorine atom has 3 pairs of electron. It is a ${\text{AB}}_4$ type molecule. Since there is no lone pair on the central atom, to minimize the repulsion, they form a distorted tetrahedral geometry because of the size difference of terminal chlorine and hydrogen atoms. So the bond angle between two atoms is ${109.5}^0$.

(e)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{Hg}}_{\text{2}}{\text{Cl}}_{\text{2}}$ is ${180}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{Hg}}_{\text{2}}{\text{Cl}}_{\text{2}}$.

Lewis structure of the given molecule is drawn below.

In the case of ${\text{Hg}}_{\text{2}}{\text{Cl}}_{\text{2}}$, both mercury atom does not have any lone pair of electrons whereas the terminal chlorine atoms have 3 pairs of electron. Both the mercury atom is of ${\text{AB}}_2$ type molecule. . Since there is no lone pair on the central atom, to minimize the repulsion, they form a linear geometry. So the bond angle between two atoms is ${180}^0$.

(f)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{SnCl}}_{\text{2}}$ is ${120}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{SnCl}}_{\text{2}}$.

Lewis structure of the given molecule is drawn below.

In the case of ${\text{SnCl}}_{\text{2}}$, the central atom tin atom have a lone pair of electron whereas the terminal chlorine atoms have 3 pairs of electron and is a ${\text{AB}}_2$ with one lone pair of electron type molecule. There are only two bonds so there is only one bond angle. Since there is one lone pair on the central atom, to minimize the repulsion, they form a bent geometry. So the bond angle between two atoms is ${120}^0$.

 (g)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{H}}_{\text{2}}{\text{O}}_{\text{2}}$ is ${109.5}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{H}}_{\text{2}}{\text{O}}_{\text{2}}$.

Lewis structure of the given molecule is drawn below.

In the case of ${\text{H}}_{\text{2}}{\text{O}}_{\text{2}}$, both oxygen atom have any two lone pair of electrons and is a ${\text{AB}}_2$ with two lone pair of electron type molecule.. Since there is two lone pair on each oxygen atom, to minimize the repulsion, they form a tetrahedral geometry. So the bond angle between two atoms is ${109.5}^0$.

(h)

Interpretation Introduction

Interpretation: The bond angle of the given molecule should be found.

Concept Introduction:

• Bond angle measured that made between two nearby bonds. The angles between two adjacent bonds are known as bond angle.
• Using VSEPR theory and Lewis structure, the exact geometry of a molecule can be obtained.
• In VSEPR, the geometry of the molecule is explained based on minimizing electrostatic repulsion between the molecules’ valence electrons around a central atom
• Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Answer to Problem 10.70QP

The bond angle of ${\text{SnH}}_4$ is ${109.5}^0$

Explanation of Solution

To find: The bond angle of the given molecule

Given molecule is

${\text{SnH}}_4$.

Lewis structure of the given molecule is drawn below.

${\text{SnH}}_4$ Contains five atoms. Here the central atom tin atom does not have any lone pair of electrons. It is a ${\text{AB}}_4$ type molecule. Since there is no lone pair on the central atom, to minimize the repulsion, they form a tetrahedral geometry. So the bond angle between two atoms is ${109.5}^0$.