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.
Like sulphur, oxygen does not show `+ 4` and `+6` oxidation states. The reason is

Options

A. That oxygen is a gas while sulphur is a solid
B. That oxygen has high ionisatio enthalpies in comparison to sulphur
C. That oxygen has high electron affinity in comparison to sulphur
D. That oxygen has no d-orbitals in its valence shell.

Answer

D