Geometry of XeF4
XeF4 has a square planar geometry with a bond angle of 90 degrees. It means that the molecule has four fluorine atoms and one lone pair on the central xenon atom, and all the atoms lie in the same plane.

Hybridization of XeF4
The hybridization of XeF4 is sp3d2. It means that the central xenon atom has five hybrid orbitals that are formed from the mixing of one 5s, three 5p, and two 5d orbitals.

Explanation
The xenon atom in XeF4 has eight valence electrons, out of which six electrons are used for forming bonds with the four fluorine atoms. The remaining two electrons occupy one of the hybrid orbitals as a lone pair. The hybridization of the xenon atom is sp3d2, which means that it has five hybrid orbitals.

The hybridization of the xenon atom is explained as follows:

- The 5s orbital of xenon mixes with three 5p orbitals to form four sp3d hybrid orbitals. These hybrid orbitals have a trigonal bipyramidal geometry.
- The two remaining 5d orbitals of xenon participate in hybridization to form two new hybrid orbitals. These hybrid orbitals are perpendicular to the plane of the four sp3d hybrid orbitals and are oriented along the z-axis.

Thus, the hybridization of XeF4 is sp3d2, and the geometry is square planar. The lone pair on the central xenon atom is responsible for the deviation of the bond angle from the ideal 90 degrees.