Discuss the shape of `SF_6`

Explanation

Ground state electronic configuration of sulphur (Z=16) is as follows.
`S(Z=16) : (Ne)^(10) 3s^2 3p_x^2 3p_y^1 3p_z^1`
To form six S-F bonds in `SF_6`, two electrons, one each form 3s and 3p subshell are promoted to 3d-subshell followed by `sp^3 d^2`-hybridised to give six equivalent half filled orbitals. These six half filled hybridised orbitals overlap with the half filled p-orbitals of six fluorine atoms. As hybridisation is `sp^3 d^2` and there is no lone pair the shape of the `SF_6` molecule is octahedral with F-S-F bond angle of `90^@`. In `SF_6` all the bonds are of equal length and the F-S-F bond angles are `90^@` each, hence in `SF_6` all the SF bonds are equivalent.