In which of the following compounds the oxidation state of...

In which of the following compounds the oxidation state of oxygen is other than $-2 ?$
(a) $\mathrm{H}_{2} \mathrm{O}_{2}$
(b) $\mathrm{O}_{2}$
(c) $\mathrm{O}_{2} \mathrm{~F}_{2}$
(d) $\mathrm{H}_{2} \mathrm{O}$

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Key Concepts

Oxidation States

Oxidation states indicate the hypothetical charge an atom would have if all bonds were completely ionic. This concept is essential for tracking electron transfer in redox reactions and for understanding the distribution of electrons within compounds.

Peroxides

Peroxides are a class of compounds where two oxygen atoms are bonded together, resulting in an oxidation state of -1 for each oxygen instead of the typical -2. This unique bonding leads to distinctive reactivity and chemical behavior compared to normal oxides.

Elemental Forms of Oxygen

Elemental oxygen, such as O2, exists in its pure state and carries an oxidation state of 0. This concept underlines that oxidation states are assigned based on compound formation, and elements in their standard state are usually considered to have an oxidation state of zero.

Oxyfluoride Compounds and Electronegativity Differences

In compounds where oxygen forms bonds with elements that are more electronegative, like fluorine, the oxidation state of oxygen can be different from its usual value. This alteration arises from the electronegativity differences which can cause the electron distribution to shift, resulting in oxidation states that deviate from the common -2.

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