Given below are two statements :
Statement (I) : Oxygen being the first member of group 16 exhibits only -2 oxidation state.
Statement (II) : Down the group 16 stability of +4 oxidation state decreases and +6 oxidation state increases.
In the light of the above statements, choose the most appropriate answer from the options given below :

Solution

Chemistry ma’am · 4 steps

Test each claim against one real compound: OF₂ breaks the first, inert pair effect breaks the second.

1. Check Statement I. Oxygen does show -2 most often, but not only -2. In peroxides such as H₂O₂ it is -1, in superoxides such as KO₂ it is -1/2, and with fluorine it turns positive: +2 in OF₂ and +1 in O₂F₂. So Statement I is incorrect.
2. Inert pair effect. Going down group 16, the ns² pair holds on more tightly and takes part in bonding less and less. So the lower state, +4, becomes more stable, and the higher state, +6, becomes less stable.

   Element	Preferred positive state	Example
   S	+6 is stable	SF₆, H₂SO₄
   Se	+4 gaining ground	SeO₂ is stable, SeO₃ is a strong oxidiser
   Te, Po	+4 favoured	TeO₂, PoO₂

3. Check Statement II. Statement II states the trend backwards. Down the group, +4 stability increases and +6 stability decreases, so Statement II is incorrect.
4. So. Both statements are incorrect, which is option (b).

The idea to keep. Down groups 13 to 16, the inert pair effect makes the lower oxidation state more stable. Oxygen is only -2 in most compounds: peroxides, superoxides and fluorides break that pattern.

Answer from the NTA final answer key. Solution by PrepWiser.