Passage-IV :
Sulphur and rest of the elements of group 16 are less electronegative than oxygen. Therefore, their atoms cannot take up 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 shell. As a result, they can show +4 and +6 oxidation states shell.
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 ionization 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

Explanation

Due to the absence of vacant d-orbitals oxygen forms only stable compounds in valency of 2.