Question

(i)

Write Lewis structure of the following compound and show formal charge on each atom.

$HN{O}_3$

(ii)

Write Lewis structure of the following compound and show formal charge on each atom.

$N{O}_2$

(iii)

Write Lewis structure of the following compound and show formal charge on each atom.

$H_{2}S{O}_4$

Answer 1

The Lewis structure of the following compound and formal charge on each atom are as

$HN{O}_3$

Formal charge on an atom in a Lewis structure = [total number of valence electrons in free atom]-[total number of non-bonding (lone pairs) electrons]-$\frac{1}{2}$[total number of bonding or shared electrons]

Formal charge on H = 1 - 0 - $\frac{1}{2}\times$ 2 = 0

Formal charge on N = 5 - 0 - $\frac{1}{2}\times$ 8 = 1

Formal charge on O(1) = 6 - 4 - $\frac{1}{2}\times$ 4 = 0

Formal charge on O(2) = 6 - 4 - $\frac{1}{2}\times$ 4 = 0

Formal charge on O(3) = 6 - 6 - $\frac{1}{2}\times$ 2 = -1

(ii)

$N{O}_2$

Formal charge on an atom in a Lewis structure = [total number of valence electrons in free atom]-[total number of non-bonding (lone pairs) electrons]-$\frac{1}{2}$[total number of bonding or shared electrons]

Formal charge on O(1) = 6 - 4 - $\frac{1}{2}\times$ 4 = 0

Formal charge on N = 5 - 2 - $\frac{1}{2}\times$ 6 = 0

Formal charge on O(2)= 6 - 6 - $\frac{1}{2}\times$ 2 = -1

(iii)

$H_{2}S{O}_4$

Formal charge on H(1) or H(2) = 1 - 0 - $\frac{1}{2}\times$ 2 = 0

Formal charge on O(2) or O(3) = 6 - 4 - $\frac{1}{2}\times$ 4 = 0

Formal charge on O(1) or O(4) = 6 - 4 - $\frac{1}{2}\times$ 4 = 0

Formal charge on S = 6 - 0 - $\frac{1}{2}\times$ 12 = 0