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Sulfur in SF4 is in the +4 oxidation state, with two of its six valence electrons forming a lone pair. According to VSEPR theory, SF4 has a see-saw structure with sulfur at the center and one of the three equatorial positions occupied by the lone pair, giving it two types of fluorine ligands - two axial and two equatorial. In contrast, SF6 has sulfur in the +6 oxidation state with no remaining nonbonding electrons, so it adopts a symmetrical octahedral structure and is extraordinarily inert chemically unlik

Author

iitsivaiah

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EN