Question

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

$HN{O}_3,N{O}_2,H_{2}S{O}_4$

Answer 1

Lewis dot structure of $HN{O}_3$ and formal charges on $HN{O}_3$



Formal charge $=[V.E-U.E-\frac{1}{2}(S.E\left)\right]$

where,

$V.E=Totalnumberofvalenceelectrons$

$U.E=Totalnumberofunsharedelectrons$

$U.E=Totalnumberofsharedelectrons$

Lewis dot structure of $N{O}_2$ and formal charges on $N{O}_2$



Formal charge on oxygen $\left(1\right)$

$=6-6\frac{1}{2}\left(2\right)=-1$

Formal charge on oxygen $\left(2\right)$

$=6-4\frac{1}{2}\left(4\right)=-0$

Formal charge on nitrogen

$=5-1\frac{1}{2}\left(6\right)=-+1$

Lewis dot structure of $H_{2}S{0}_4$ and formal charges on $H_{2}S{0}_4$



Formal charge on oxygen $1\text{and}4$

$=6-4\frac{1}{2}\left(4\right)=-0$

Formal charge on oxygen $2\text{and}3$

$=6-4\frac{1}{2}\left(4\right)=-0$

Formal charge on hydrogen $1\text{and}2$

$=1-0\frac{1}{2}\left(2\right)=-0$

Formal charge on sulphur

$=6-0\frac{1}{2}\left(12\right)=-0$