The hybridization of SF4 is sp3d2 type. Just to describe the compound in brief, Sulfur Hexafluoride is a type of greenhouse gas which is colourless, odourless, non-toxic and non-flammable. It is also an inorganic and a non-polar gas. Normally, SF6 can be prepared by exposing or combining S8 with F2. Now we will look at how the hybridization takes place.
|Name of the Molecule||Sulfur Hexafluoride|
What is the Hybridization of Sulfur Hexafluoride?
To determine the hybridization of sulfur 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, 3py, 3py, 3pz and 3dx2–y2 and 3dz2. 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 3dz2 and 3dx2-y2 orbitals. Now all these six orbitals (one 3s, three 3p and twp 3d) which are half-filled get hybridised 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.
Important Points To Remember
- 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 sulfur hexafluoride has a central sulfur 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.