XeF₄ has four Xe–F bonds and two lone pairs on xenon. Six electron domains are octahedral, and the two opposite lone pairs leave a square planar molecular geometry.
Xenon contributes 8 and four fluorines contribute 28.
Draw four Xe–F single bonds.
The four bonds use 8 electrons.
Complete fluorine octets.
Twelve fluorine lone pairs use 24 electrons.
Place the remaining four electrons on xenon.
They form two lone pairs.
Apply VSEPR.
The lone pairs occupy opposite positions in an octahedral domain arrangement, leaving four fluorines in a square plane.
Electron check
Four bonds use 8 electrons, fluorine lone pairs use 24, and xenon lone pairs use 4, totaling 36.
Angles and symmetry
Adjacent F–Xe–F angles are 90° and opposite fluorines are 180° apart. The symmetric square planar arrangement gives no net dipole in the idealized molecule.
Common mistakes
Drawing XeF4 tetrahedral because it has four fluorines.
Forgetting the two lone pairs on xenon.
Placing the xenon lone pairs next to each other instead of opposite.
Calling the electron geometry square planar; the electron geometry is octahedral.