Chapter 10, Problem 10.36QP

(a)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of new set of hybrid orbitals which have equivalent energies.  The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

$\begin{array}{l}\text{σ-bond}\Rightarrow \text{forms}\text{by}\text{head-to-head}\text{overalp}\text{of}\text{atomic}\text{orbitals}.\\ \text{π-bond}\Rightarrow \text{forms}\text{by}\text{lateral}\text{overalp}\text{of}\text{atomic}\text{orbitals}\end{array}$

• If the carbon atom is bonded with four $\text{σ-}\text{bonds}$, then it is $s{p}^3$ hybridized carbon atom.
• If the carbon atom is bonded with three $\text{σ-sigma}\text{bond}$ and one $\text{π-bond}$, then it is $s{p}^2$hybridized carbon atom.
• If the carbon atom is bonded with two $\text{σ-}\text{bond}$ and two $\text{π-bonds}$, then it is $sp$hybridized carbon atom.

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

(b)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

$\begin{array}{l}\text{σ-bond}\Rightarrow \text{forms}\text{by}\text{head-to-head}\text{overalp}\text{of}\text{atomic}\text{orbitals}.\\ \text{π-bond}\Rightarrow \text{forms}\text{by}\text{lateral}\text{overalp}\text{of}\text{atomic}\text{orbitals}\end{array}$

• If the carbon atom is bonded with four $\text{σ-}\text{bonds}$, then it is $s{p}^3$ hybridized carbon atom. 
• If the carbon atom is bonded with three $\text{σ-sigma}\text{bond}$ and one $\text{π-bond}$, then it is $s{p}^2$hybridized carbon atom.
• If the carbon atom is bonded with two $\text{σ-}\text{bond}$ and two $\text{π-bonds}$, then it is $sp$hybridized carbon atom.

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

(c)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of new set of hybrid orbitals which have equivalent energies.  The various types of atomic orbitals are: s, p, and d orbitals.  Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

$\begin{array}{l}\text{σ-bond}\Rightarrow \text{forms}\text{by}\text{head-to-head}\text{overalp}\text{of}\text{atomic}\text{orbitals}.\\ \text{π-bond}\Rightarrow \text{forms}\text{by}\text{lateral}\text{overalp}\text{of}\text{atomic}\text{orbitals}\end{array}$

• If the carbon atom is bonded with four $\text{σ-}\text{bonds}$, then it is $s{p}^3$ hybridized carbon atom. 
• If the carbon atom is bonded with three $\text{σ-sigma}\text{bond}$ and one $\text{π-bond}$, then it is $s{p}^2$hybridized carbon atom.
• If the carbon atom is bonded with two $\text{σ-}\text{bond}$ and two $\text{π-bonds}$, then it is $sp$hybridized carbon atom.

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

(d)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

$\begin{array}{l}\text{σ-bond}\Rightarrow \text{forms}\text{by}\text{head-to-head}\text{overalp}\text{of}\text{atomic}\text{orbitals}.\\ \text{π-bond}\Rightarrow \text{forms}\text{by}\text{lateral}\text{overalp}\text{of}\text{atomic}\text{orbitals}\end{array}$

• If the carbon atom is bonded with four $\text{σ-}\text{bonds}$, then it is $s{p}^3$ hybridized carbon atom. 
• If the carbon atom is bonded with three $\text{σ-sigma}\text{bond}$ and one $\text{π-bond}$, then it is $s{p}^2$hybridized carbon atom.
• If the carbon atom is bonded with two $\text{σ-}\text{bond}$ and two $\text{π-bonds}$, then it is $sp$hybridized carbon atom.

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below:

(e)

Interpretation Introduction

Interpretation:

The hybrid orbitals of the carbon atoms in the given molecule have to be found.

Concept Introduction:

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The valency of carbon atom is four, which means it can make four bonding with the other atoms.

There are two major types of bonding:

$\begin{array}{l}\text{σ-bond}\Rightarrow \text{forms}\text{by}\text{head-to-head}\text{overalp}\text{of}\text{atomic}\text{orbitals}.\\ \text{π-bond}\Rightarrow \text{forms}\text{by}\text{lateral}\text{overalp}\text{of}\text{atomic}\text{orbitals}\end{array}$

• If the carbon atom is bonded with four $\text{σ-}\text{bonds}$, then it is $s{p}^3$ hybridized carbon atom. 
• If the carbon atom is bonded with three $\text{σ-sigma}\text{bond}$ and one $\text{π-bond}$, then it is $s{p}^2$hybridized carbon atom.
• If the carbon atom is bonded with two $\text{σ-}\text{bond}$ and two $\text{π-bonds}$, then it is $sp$hybridized carbon atom.

Explanation of Solution

In the given molecule, the hybrid orbitals of each carbon atom are shown below: