Oxygen is a gas but sulphur a solid. Explain.

Explanation

Oxygen forms pr - pt multiple bonds . Due to small size and high electronegativity oxygen exists as diatomic `(O_(2))` molecules. These molecules are held together by weak Van der Waals. forces. Hence, `O_(2)` is a gas at room temperature. Sulphur because of its bigger size and lower electronegativity, prefers to form `S - S` single bonds . Further, because of stronger `S - S` single bond than `O- O` single bonds, sulphur has a much greater tendency for catenation than oxygen. Thus, sulphur because of its higher tendency for catenation and lower tendency for `ppi -ppi` multiple bonds, forms octaatomic `(S_(8))` molecules having eight - membered puckered ring structure, Because of bigger size, the forces of attraction holding the `S_(8)` molecules together are much stronger. Hence, sulphur is a solid at room temperature.