why is dioxygen a gas but sulphur a solid?
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Answered by
11
Intermolecular forces plays a major role
in oxygen due to weak vanderwaal forces it remains as gas but in sulphur there is no strong bonding as they are covalent bonds and exist as puckered S8 structure
other reason would be that substance with high melting and boiling points usually exists as solid at room temperature
in oxygen due to weak vanderwaal forces it remains as gas but in sulphur there is no strong bonding as they are covalent bonds and exist as puckered S8 structure
other reason would be that substance with high melting and boiling points usually exists as solid at room temperature
Answered by
15
Hey !!
It is because of its small size, oxygen is capable of forming pπ - pπ bond and exists as diatomic O₂ molecule. The intermolecular forces in oxygen are weak van der Waals force, due to which it is a gas at room temperature. On the other hand, sulphur, due to its larger size prefers to form S - S single bond and exist as octaatomic S₈ molecule puckered ring structure. Because of larger size the force of attraction holding the S₈ molecules together are much stronger. Hence sulphur is a solid at room temperature.
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