Which of the oxidation state(s) is/are shown by the element sulphur?

Having a high electronegativity, oxygen. In most of its metallic oxides, it exhibits a -2 oxidation state, which indicates that it gains 2 electrons. Oxygen does not have room for unpaired electrons because it is tiny and lacks d-orbitals. A +2 oxidation state in ${\mathrm{OF}}_2$, a +1 oxidation state in ${\mathrm{O}}_2{\mathrm{F}}_2$, and a -1 oxidation state in hydrogen peroxide are examples of exceptions, though (${\mathrm{H}}_2{\mathrm{O}}_2$ ). Sulfur Oxidation State
The size of sulphur is larger. It can expand its valency because its third d-orbital is vacant. Sulfur exhibits a -2 oxidation state in addition to +2, +4, and +6 oxidation states, the latter two of which are the most frequent.