# How do you draw the Lewis Structures of each of the following acids? These structures, like most acids, have each H attached to one of the oxygens.

## ${H}_{2} S {O}_{4}$ $H I {O}_{2}$

Sep 22, 2016

You have $\text{iodous and sulfuric acids}$.

#### Explanation:

Sulfuric acid is easy: $H O - S {\left(= O\right)}_{2} \left(O H\right)$, we have a $S \left(V I +\right)$ oxidation state. Alternatively, I could represent this as HO-""^(2+)S(-O)_2^(-)(OH).

For $\text{iodous acid}$ I have a formal ${I}^{I I I +}$ oxidation state:

$O = I - O H$

This is an unstable beasty, and I don't think it has ever been isolated.