Chapter 10, Problem 10.10P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of ${\text{HNO}}_3$$\left({\text{HONO}}_2\right)$ is to be drawn.

Concept introduction:

The steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that the octet of each atom is satisfied.

Step 5: Convert the lone pair into a bond pair if required.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted into another by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of ${\text{HAsO}}_4^{2-}\left({\text{HOAsO}}_3^{2-}\right)$ is to be drawn.

Concept introduction:

The steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that the octet of each atom is satisfied.

Step 5: Convert the lone pair into a bond pair if required.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.