Why is dioxygen a gas but sulphur a solid?

(N/A) Oxygen has a smaller atomic size compared to sulphur. Due to its small size,it can effectively form $p\pi-p\pi$ multiple bonds to exist as a discrete $O_2$ molecule. The intermolecular forces in $O_2$ are weak van der Waals forces,which result in it being a gas at room temperature.
On the other hand,sulphur has a larger atomic size and does not form stable $S=S$ double bonds. Instead,it forms single $S-S$ bonds and exists as a puckered $S_8$ ring structure. These large $S_8$ molecules are held together by stronger van der Waals forces,making sulphur a solid.