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What is the Hybridization of Sulphur Hexafluoride?

To determine the hybridization of sulphur hexafluoride we will look at the orbitals involved and the bonds that are formed during the combination of sulphur and fluorine molecules. The orbitals involved are 3s, 3p_y, 3p_y, 3p_z and 3dx²–^y2 and 3d_z². During the formation of SF₆, the sulphur atom which is the central atom in its ground state will have 3s²3p⁴ configuration. In the excited state, the electron pairs in 3s and 3px orbitals get unpaired and one out of each pair is promoted to vacant 3d_z² and 3d_x2-y2 orbitals. Now all these six orbitals (one 3s, three 3p and two 3d) which are half-filled get hybridized resulting in the formation of six sp³d² hybrid orbitals. Further, the sp³d² hybrid orbitals overlap with a 2p orbital of fluorine, and they form the S-F bond. sf6 hybridization

Important Points To Remember(sf6 hybridization)

• There are six hybrid orbitals formed.
• One 3s-orbital, three 3p-orbitals and two 3d-orbital take part in hybridization.
• The six sp³d² hybrid orbitals are projected towards the six corners of a regular octahedron.

SF4 Molecular Geometry And Bond Angles

SF6 molecular geometry will be octahedral because if we look at the structure sulphur hexafluoride has a central sulphur atom around which12 electrons or 6 electron pairs are present and there are no lone pairs. The F-S-F bonds are slated to be at 90 degrees. sf6 hybridization

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