Chapter 1, Problem 42P

(a)

Interpretation Introduction

Interpretation:

The approximate bond angle for $\text{C-N-C}$ in ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}{\text{N}}^{\text{+}}{\text{H}}_{\text{2}}$ should be predicted.

Concept introduction:

• 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.
• Cylindrically symmetrical bonds are called sigma ($\sigma$) bonds; side to side overlap of parallel p orbital forms a pi ($\pi$) bond.
• 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 more s character 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.

(b)

Interpretation Introduction

Interpretation:

The approximate bond angle for $\text{C-O-H}$ in ${\text{CH}}_{\text{3}}\text{OH}$ should be predicted.

Concept introduction:

• 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.
• Cylindrically symmetrical bonds are called sigma ($\sigma$) bonds; side to side overlap of parallel p orbital forms a pi ($\pi$) bond.
• 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 more s character 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.

(c)

Interpretation Introduction

Interpretation:

The approximate bond angle for $\text{C-N-H}$ in ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}\text{NH}$ should be predicted.

Concept introduction:

• 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.
• Cylindrically symmetrical bonds are called sigma ($\sigma$) bonds; side to side overlap of parallel p orbital forms a pi ($\pi$) bond.
• 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 more s character 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.

(d)

Interpretation Introduction

Interpretation:

The approximate bond angle for $\text{C-N-C}$ in ${\left({\text{CH}}_{\text{3}}\right)}_{\text{2}}\text{NH}$ should be predicted.

Concept introduction:

• 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.
• Cylindrically symmetrical bonds are called sigma ($\sigma$) bonds; side to side overlap of parallel p orbital forms a pi ($\pi$) bond.
• 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 more s character 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.