The total number of lone pair present in XeF4

XeF4 is the chemical formula for xenon tetrafluoride, which is a colorless crystalline substance. It is composed of a xenon atom bonded to four fluorine atoms. To determine the number of lone pairs present in XeF4, we need to understand its molecular structure and electron arrangement.

Molecular Structure of XeF4
XeF4 has a square planar molecular geometry, meaning it has a central xenon atom surrounded by four fluorine atoms in a flat square arrangement. The xenon atom is located in the center, and the four fluorine atoms are positioned around it, with a bond angle of 90 degrees.

Electron Arrangement in XeF4
Xenon (Xe) has a total of 54 electrons. In its ground state, it has the electron configuration of [Kr] 5s2 4d10 5p6. To form XeF4, xenon undergoes hybridization to form four sp3d2 hybrid orbitals. These hybrid orbitals are formed by mixing one s orbital, three p orbitals, and two d orbitals. Each of these hybrid orbitals forms a sigma bond with a fluorine atom, resulting in four sigma bonds.

Lone Pairs in XeF4
Lone pairs are electron pairs that are not involved in bonding. In XeF4, there are two lone pairs present on the central xenon atom. These lone pairs occupy two of the sp3d2 hybrid orbitals, while the other four hybrid orbitals form sigma bonds with the four fluorine atoms.

Summary
In summary, XeF4 has a square planar molecular geometry with a central xenon atom bonded to four fluorine atoms. It has two lone pairs of electrons on the xenon atom, occupying two of the sp3d2 hybrid orbitals. These lone pairs are not involved in bonding and contribute to the overall electronic configuration and properties of XeF4.