Sulphur show +4 and +6 oxidation stae in their compounds but oxygen can not show these oxidation states.

Explanation

Oxygen atom having `1s^2 2s^2 2p^4` configuration has tendency to gain or share two electrons in order to acquire nearest noble gas configuration. Due to high electronegativity, oxygen generally exhibits -2 oxdiation state e.g., in/`H_2 O`. Due to the non-availability of the vacant d-orbitals, oxygen does not show multiple oxidation states. However, other members of oxygen family show multiples oxidation states of +4 and +6. This is due to the promotion electrons s and p orbitals to vacant d-orbitals in the valence shell. The ground and excited states of sulphur atom are shown in the figure.