Chapter 21, Problem 21.15P

(a)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$ orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $5$

So, the total number of $\text{2p}$ orbital electrons is: $5\times 2=10$

(b)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$ orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $6$

So, the total number of $\text{2p}$ orbital electrons is: $6\times 2=12$

(c)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $2$

So, the total number of $\text{2p}$ orbital electrons is: $2\times 2=4$

(d)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $2$

So, the number of $\text{2p}$ orbital electrons is: $2\times 2=4$

There is an unpaired free-radical electron which is represented by a single dot. This unpaired free-radical electron will be in resonance with the $\text{2p}$ orbital electrons. So, additionally one electron has to be considered in the number of $\text{2p}$ orbital electrons.

Therefore, the total number of $\text{2p}$ orbital electrons is: $4+1=5$

(e)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $2$

So, the number of $\text{2p}$ orbital electrons is: $2\times 2=4$

There is a pair of electrons which is represented by two dots with a negative sign. This pair of electrons will be in resonance with the $\text{2p}$ orbital electrons. So, additionally 2 electrons have to be considered in the number of $\text{2p}$ orbital electrons.

Therefore, the total number of $\text{2p}$ orbital electrons is: $4+2=6$

(f)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $2$

So, the total number of $\text{2p}$ orbital electrons is: $2\times 2=4$

(g)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $3$

So, the total number of $\text{2p}$ orbital electrons is: $3\times 2=6$

(h)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $3$

So, the total number of $\text{2p}$ orbital electrons is: $3\times 2=6$

(i)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $3$

So, the total number of $\text{2p}$ orbital electrons is: $3\times 2=6$

(j)

Interpretation Introduction

Interpretation:

The number of $\text{2p}$ orbital electrons in each molecule or ion has to be stated.

Concept Introduction:

$2p$orbitals and their electrons:

There are three types of $\text{2p}$ orbitals such as ${\text{2p}}_{\text{x}},{\text{2p}}_{\text{y}}{\text{ and 2p}}_{\text{z}}$ orbitals. The bonding between two ${\text{2p}}_{\text{x}}$ orbitals will be $\text{π}$-bonding which result in the formation of double bond. Similarly, the bonding between two ${\text{2p}}_{\text{y}}$ orbitals will also be $\text{π}$-bonding which also result in the formation of double bond whereas the bonding between two ${\text{2p}}_{\text{z}}$ will be  $\text{σ}$ -bonding which result in the formation of single bond. Generally, a chemical bond is formed by the interaction of two electrons. So, a double bond formed by $\text{2p}$ orbitals will obviously hold two electrons.

Explanation of Solution

The given compound is shown here:

No. of double bonds: $3$

So, the number of $\text{2p}$ orbital electrons is: $3\times 2=6$

There are two pairs of electrons and each pair is represented by two dots with a negative sign. These two pair of electrons will be in resonance with the $\text{2p}$ orbital electrons. So, additionally four electrons have to be considered in the number of $\text{2p}$ orbital electrons.

Therefore, the total number of $\text{2p}$ orbital electrons is: $6+4=10$