The molecular geometry of xenon tetrafluoride (XeF4) is square planar.
This can be explained by looking at the structure of the molecule. Xenon (Xe) is a noble gas that can expand its octet due to the presence of d-orbitals. In XeF4, the xenon atom is central and is bonded to four fluorine atoms.
The electron pair geometry is octahedral because there are six regions of electron density around the xenon atom (four bonding pairs and two lone pairs). However, the presence of the two lone pairs distorts the geometry, resulting in a square planar shape.
In a square planar geometry, the four fluorine atoms are positioned at the corners of a square in one plane, while the lone pairs are situated above and below this plane. This arrangement minimizes the repulsion between the electron pairs according to VSEPR (Valence Shell Electron Pair Repulsion) theory.
Overall, understanding the molecular geometry of XeF4 helps in predicting its properties and how it interacts with other molecules.