Sulphur and rest of the elements of group `16` are less electronegative than oxygen, Therefore, their atoms cannot take electrons easily. They can acquire `ns^2 np^6` configuration by sharing two electrons with the atoms of other elements and thus, exhibit `+2` oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the `p` and s-orbitals of the same shell. As a result, they can show `+4` and `+ 6` oxidation states.
Oxygen exhibits `+2` oxidation state in

Options

A. `OF_2`
B. `H_2O`
C. `Cl_2O`
D. `H_2O_2`

Answer

A

Explanation

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