Xenon tetrafluoride, XeF4, is a colorless solid. Give the...

Xenon tetrafluoride, $\mathrm{XeF}_{4}$, is a colorless solid. Give the Lewis formula for the $\mathrm{XeF}_{4}$ molecule. What is the hybridization of the xenon atom in this compound? What geometry is predicted by the VSEPR model for this molecule?

Key Concepts

Lewis Structure

The Lewis structure of a molecule represents the arrangement of valence electrons among the atoms. For a molecule like XeF4, the xenon atom is placed at the center and forms bonds with four fluorine atoms. Xenon uses four of its valence electrons to form single bonds with the fluorine atoms, and the remaining electrons appear as two lone pairs on xenon. This structure helps illustrate not only the bonding connections but also the locations of nonbonding electrons which are essential in predicting molecular geometry.

Hybridization

Hybridization explains how atomic orbitals mix to form new hybrid orbitals for bonding. In XeF4, the xenon center has a total of six electron pairs (four bonding pairs from the Xe-F bonds and two lone pairs), which requires six hybrid orbitals. This mix results in an sp3d2 hybridization, where one s, three p, and two d orbitals combine. The hybridization concept accounts for the molecule’s ability to expand its octet reaching beyond the typical eight electrons.

VSEPR Theory

The VSEPR (Valence Shell Electron Pair Repulsion) theory is used to predict the three-dimensional shape of molecules based on electron pair repulsions. In XeF4, with six regions of electron density around the xenon atom (an octahedral arrangement), the molecule adopts an octahedral electron pair geometry. However, the two lone pairs occupy positions opposite one another, minimizing repulsion, which results in the molecular shape being square planar. This arrangement specifically accounts for the observed geometry of XeF4.

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