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.
The nature of the compounds of sulphur having +4 oxidation state is :

Options

A. act as oxidizing agents
B. act as reducing agents
C. act as oxidizing as well as reducing agents
D. cannot be predicted

Answer

C

Explanation

It is in intermediate oxidation state it may increase (or) decrease. Therefore it act as oxidizing agent and also reducing agent.