SF4 has four bonded atoms and one lone pair. The five electron pairs around sulphur adopt trigonal bipyramidal geometry in which one position is occupied by a lone pair. This lone pair finds a position that minimizes the number of 90^o repulsions it has with bonding electron pairs. It occupies an equatorial position with two 90^o repulsions. The bonded electrons occupy the axial and equatorial positions. The axial S-F bonds are bent slightly away from the lone pair. Hence, all the bonds in SF4 are not equivalent.

SF6 Sulfur Hexafluoride. Sulfur hexafluoride has 12 electrons around the central sulfur atom. This means there are six electron pairs arranged in an octahedral shape with 90° F-S-F bond angles. There are no lone pairs.