Oxygen exists as a diatomic gas where as sulphur exists as otaatomic solid
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In s8 there is a crown like strucure involving all s atoms to a single disulfide bond formation with each other using 3py1,3pz1 electrons thus attaining stabilty.
There is a single bond between each pair of S atoms and two nonbonding electron pairs on each S atom.Thus, we see four electron domains around each S atom, and we would expect a tetrahedral electron-domaingeometry corresponding to sp3 hybridization.due to its bigger atomic size has stronger Vander Waal forces among atoms. So it forms a solid structure at room temperature. However, it forms Pπ-Pπ bonds but not so stable as oxygen. It is because of its size. Octasulfur forms several allotropes: α-Sulfur, β-sulfur, γ-sulfur, λ-sulfur.s-s bond angle is 106 degree.
Oxyzen is o8,where the size of o8 molecules are small,so the vanderwall forces,to gain stability oxyzen uses its last 2 electrons,2py1,2pz1 electrons,where one bond is sigma,another is pie bond. It lies at a straight line,bond angle 180 degree,again sp3 hybridization…
There is a single bond between each pair of S atoms and two nonbonding electron pairs on each S atom.Thus, we see four electron domains around each S atom, and we would expect a tetrahedral electron-domaingeometry corresponding to sp3 hybridization.due to its bigger atomic size has stronger Vander Waal forces among atoms. So it forms a solid structure at room temperature. However, it forms Pπ-Pπ bonds but not so stable as oxygen. It is because of its size. Octasulfur forms several allotropes: α-Sulfur, β-sulfur, γ-sulfur, λ-sulfur.s-s bond angle is 106 degree.
Oxyzen is o8,where the size of o8 molecules are small,so the vanderwall forces,to gain stability oxyzen uses its last 2 electrons,2py1,2pz1 electrons,where one bond is sigma,another is pie bond. It lies at a straight line,bond angle 180 degree,again sp3 hybridization…
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