Hybridization of XeF6 is sp^3 d^ 3according to vsepr theory molecules Which are AB6L ( means 6 bp and 1 lp but here we can consider the 1 e- as lp)type have pentagonal bipyramid - geometry but shape is distorted.

The hybridization of XeF6 is sp3d3. To understand this, let's break down the concept step by step:

Hybridization:
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form hybrid orbitals. These hybrid orbitals have different shapes and energies compared to the original atomic orbitals. Hybridization occurs when there is a need for the atoms to form bonds in a molecule.

XeF6:
XeF6 is the chemical formula for xenon hexafluoride. It consists of one xenon (Xe) atom and six fluorine (F) atoms bonded together. Xenon is a noble gas, which means it typically does not form compounds easily. However, with fluorine, it forms a compound due to the high electronegativity difference between the two elements.

Electronic Configuration:
The atomic number of xenon is 54, and its electronic configuration is [Kr] 5s2 4d10 5p6. Fluorine, on the other hand, has an atomic number of 9 and an electronic configuration of 1s2 2s2 2p5.

Formation of Bonds:
In XeF6, xenon forms covalent bonds with each of the six fluorine atoms. Each fluorine atom contributes one electron to form a single bond with xenon. This results in the formation of six sigma bonds.

Valence Shell Electron Pair Repulsion (VSEPR) Theory:
According to the VSEPR theory, electron pairs in the valence shell of an atom repel each other and try to stay as far apart as possible. This leads to the arrangement of electron pairs around the central atom in a way that minimizes repulsion.

Hybridization of XeF6:
In XeF6, xenon has eight valence electrons. To accommodate all six fluorine atoms and minimize electron pair repulsion, xenon undergoes sp3d3 hybridization.

Explanation:
The s and p orbitals of xenon (5s, 5p, and 5d orbitals) hybridize to form six sp3d3 hybrid orbitals. Each of these hybrid orbitals overlaps with a 2p orbital of a fluorine atom, resulting in the formation of six sigma bonds.

The geometry of XeF6 is octahedral, where the six fluorine atoms are positioned around the central xenon atom, forming a regular octahedron. The six hybrid orbitals are directed towards the six corners of the octahedron, ensuring maximum separation and minimizing repulsion.

In conclusion, the hybridization of XeF6 is sp3d3, where xenon forms six sigma bonds with fluorine atoms using six hybrid orbitals.