In the molecule of ${\mathrm{XeF}}_4$, hybridisation of ' $\mathrm{Xe}$ ' atom is

The Xenon Tetrafluoride (XeF4) molecule has a unique hybridization structure that contributes to its square planar geometry. To understand the XeF4 hybridization, let's break down the components and electron arrangement of the molecule.

Electron Pair Configuration

Xenon (Xe) in XeF4 forms bonds with four fluorine atoms. In its ground state, xenon has a total of eight valence electrons. These electrons undergo hybridization to form bonds with fluorine atoms.

The molecule of XeF4 has six electron pairs around the central xenon atom—four bonding pairs and two lone pairs. These lone pairs reside on the axis of the molecule, while the bonding pairs of electrons are positioned in the vertical surface. This arrangement leads to a repulsion between lone pair electrons and bond pair electrons, which distorts the geometry, resulting in a square planar shape.

Hybridization of Xenon in XeF4

The hybridization of the central xenon atom in XeF4 hybridization involves the mixing of one s-orbital, three p-orbitals, and two d-orbitals to form six sp³d² hybrid orbitals. These six orbitals are arranged in an octahedral geometry to minimize electron pair repulsion.

However, due to the presence of two lone pairs that occupy two of the positions on the axis, the resulting molecular geometry is not octahedral but square planar. This is because the lone pairs exert more repulsion on the bonding pairs, pushing the fluorine atoms into a planar arrangement.