Chapter 1.14, Problem 36P

(a)

Interpretation Introduction

Interpretation:

The orbitals used in bonding and the angles in the given compounds should be described.

Concept introduction:

Lewis structure:

• A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.
• The bond angle depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angle.
• For example, ${\text{sp}}^3$ carbon have bond angle of ${109.5}^0$, ${\text{sp}}^2$ carbon have bond angle of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angle of  ${\text{180}}^{\text{0}}$.
• The bond angle increases the s character in the orbital increases.
• The more s characters in the orbital, the shorter the bond.
• The more s characters in the orbital, the stronger the bond.
• The more s characters in the orbital, the larger the bond angle.
• A $\text{π}$ bond is weaker than a $\text{σ}$ bond.

Bond angle:

It is the angle formed between three atoms across at least two bonds.

(b)

Interpretation Introduction

Interpretation:

The orbitals used in bonding and the angles in the following compounds should be described.

Concept introduction:

 Lewis structure:

• A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.
• The bond angle depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angle.
• For example, ${\text{sp}}^3$ carbon have bond angle of ${109.5}^0$, ${\text{sp}}^2$ carbon have bond angle of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angle of  ${\text{180}}^{\text{0}}$.
• The bond angle increases the s character in the orbital increases.
• The more s characters in the orbital, the shorter the bond.
• The more s characters in the orbital, the stronger the bond.
• The more s characters in the orbital, the larger the bond angle.
• A $\text{π}$ bond is weaker than a $\text{σ}$ bond.

Bond angle:

It is the angle formed between three atoms across at least two bonds.

(c)

Interpretation Introduction

Interpretation:

The orbitals used in bonding and the angles in the following compounds should be described.

Concept introduction:

Lewis structure:

• A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.
• The bond angle depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angle.
• For example, ${\text{sp}}^3$ carbon have bond angle of ${109.5}^0$, ${\text{sp}}^2$ carbon have bond angle of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angle of  ${\text{180}}^{\text{0}}$.
• The bond angle increases the s character in the orbital increases.
• The more s characters in the orbital, the shorter the bond.
• The more s characters in the orbital, the stronger the bond.
• The more s characters in the orbital, the larger the bond angle.
• A $\text{π}$ bond is weaker than a $\text{σ}$ bond.

Bond angle:

It is the angle formed between three atoms across at least two bonds.

(d)

Interpretation Introduction

Interpretation:

The orbitals used in bonding and the angles in the following compounds should be described.

Concept introduction:

Lewis structure:

• A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.
• The bond angle depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angle.
• For example, ${\text{sp}}^3$ carbon have bond angle of ${109.5}^0$, ${\text{sp}}^2$ carbon have bond angle of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angle of  ${\text{180}}^{\text{0}}$.
• The bond angle increases the s character in the orbital increases.
• The more s characters in the orbital, the shorter the bond.
• The more s characters in the orbital, the stronger the bond.
• The more s characters in the orbital, the larger the bond angle.
• A $\text{π}$ bond is weaker than a $\text{σ}$ bond.

Bond angle:

It is the angle formed between three atoms across at least two bonds.

(e)

Interpretation Introduction

Interpretation:

The orbitals used in bonding and the angles in the following compounds should be described.

Concept introduction:

Lewis structure:

• A structure that shows the bonding between atoms of a molecule and lone pair of electron that may present in the molecule is called as Lewis structure.
• The bond angle depends on the orbital used by Carbon to form the bond.
• The greater the amount of s characters in the orbital, the larger the bond angle.
• For example, ${\text{sp}}^3$ carbon have bond angle of ${109.5}^0$, ${\text{sp}}^2$ carbon have bond angle of ${\text{120}}^{\text{0}}$, and $\text{sp}$ carbon have bond angle of  ${\text{180}}^{\text{0}}$.
• The bond angle increases the s character in the orbital increases.
• The more s characters in the orbital, the shorter the bond.
• The more s characters in the orbital, the stronger the bond.
• The more s characters in the orbital, the larger the bond angle.
• A $\text{π}$ bond is weaker than a $\text{σ}$ bond.

Bond angle:

It is the angle formed between three atoms across at least two bonds.