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. The nature of the compounds of sulphur having `+4` oxidation state isA. Act as oxidising agentsB. Acts as reducing agentsC. Act as oxidising as well as reducing agentsD. Cannot be predicted

Sulphur and rest of the elements of group `16` are less electronegativ

1.	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. The nature of the compounds of sulphur having `+4` oxidation state isA. Act as oxidising agentsB. Acts as reducing agentsC. Act as oxidising as well as reducing agentsD. Cannot be predicted
Answer» Correct Answer - C Compound of sulphur in oxidation state `+4` can reduce as well as oxidise and hence behave as oxidising agent and reducing agent.