Consider the following compounds:KO2, H2O2 and H2SO4The oxidation states of the underlined elements inthem are, respectively

Oxidation States in Compounds

In KO₂ (potassium superoxide), the superoxide ion (O₂^–) carries an overall –1 charge.

Since potassium (K) forms a +1 oxidation state, it balances the charge of the superoxide ion.

In hydrogen peroxide (H₂O₂), the compound contains a peroxide linkage (O₂^2–), where each oxygen atom has an oxidation state of –1 instead of the usual –2.

In sulfuric acid (H₂SO₄), the oxidation state of sulfur is determined by solving the equation for a neutral molecule:

2(+1) + S + 4(–2) = 0

Solving gives: 2 + S – 8 = 0 ⇒ S = +6

So, sulfur has an oxidation state of +6 in H₂SO₄.