Find the Oxidation Numbers H_2O_2

$H_{2} O_{2}$

Step 1

Since $H$ is in column $1$ of the periodic table, it will share $1$ electrons and use an oxidation state of $1$ .

$H = 2 (1) = 2$

Step 2

Since $O$ is in column $6$ of the periodic table, it will share $6$ electrons and use an oxidation state of $6$ .

$O = 2 (- 2) = - 4$

Step 3

This is the full list of oxidation states for this molecule.

$H = 2, O = - 4$