What is the molecular geometry of SF6?

The molecular geometry of SF6 (sulfur hexafluoride) is octahedral because it consists of a central sulfur atom surrounded by six fluorine atoms. In this geometry, the sulfur atom utilizes its six valence electrons to form six equivalent bonds with the fluorine atoms.

To achieve this arrangement, the electron pairs around the sulfur are organized to minimize repulsion according to VSEPR (Valence Shell Electron Pair Repulsion) theory. In an octahedral geometry, the bond angles between adjacent fluorine atoms are 90 degrees, and each fluorine atom occupies a vertex of the octahedron, allowing the sulfur atom to be at the center.

The symmetrical arrangement of the fluorine atoms ensures that the polar bonds formed do not create a net dipole moment, resulting in a nonpolar molecule. Thus, the octahedral molecular geometry is distinct and fitting for SF6 due to the presence of six bonded pairs of electrons and no lone pairs on the central atom.