Why hydrogen peroxide acts as oxidising as well as reducing agent?

PLACEHOLDER ANSWER - the answer is an explanation. In $$\text{H}_2\text{O}_2$$, oxygen has oxidation state $$-1$$, between its lowest state $$-2$$ (in $$\text{H}_2\text{O}$$) and $$0$$ (in $$\text{O}_2$$). It can be reduced to $$-2$$, acting as an oxidising agent (for example it oxidises $$\text{I}^-$$ to $$\text{I}_2$$), or oxidised to 0, acting as a reducing agent (for example with acidified $$\text{KMnO}_4$$, releasing $$\text{O}_2$$).