Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A) : Both rhombic and monoclinic sulphur exist as $$S_8$$ while oxygen exists as $$O_2$$. Reason (R) : Oxygen forms $$p\pi - p\pi$$ multiple bonds with itself and other elements having small size and high electronegativity like C, N, which is not possible for sulphur. In the light of the above statements, choose the most appropriate answer from the options given below :

Assertion (A): Both rhombic and monoclinic sulphur exist as $$S_8$$ while oxygen exists as $$O_2$$.

This is correct. Both allotropes of sulphur (rhombic and monoclinic) contain $$S_8$$ molecules in a puckered ring structure, whereas oxygen naturally exists as $$O_2$$.

Reason (R): Oxygen forms $$p\pi - p\pi$$ multiple bonds with itself and other elements having small size and high electronegativity like C, N, which is not possible for sulphur.

The first part about oxygen forming $$p\pi - p\pi$$ bonds is correct. However, the statement "which is not possible for sulphur" is too absolute. Sulphur can form some degree of $$p\pi - p\pi$$ bonding in certain compounds (e.g., in SO$$_2$$, SO$$_3$$). The key distinction is that sulphur cannot form effective $$p\pi - p\pi$$ bonds with itself due to the larger size of 3p orbitals, which is why it forms $$S_8$$ rings with single bonds. Thus, the Reason as stated is not entirely correct.

Since (A) is correct but (R) is not correct, the answer is Option A.