Numford
Hybridisation

Hybridisation of XeF₄

Xe is sp³d² hybridised (hybridization by the VSEPR count): 4 sigma bonds and 2 lone pairs give a square planar shape, bond angle 90°.

FFXeFF
  • Xe
  • F
  • lone pair

XeF₄Xenon tetrafluoride

Square planar

AB₄E₂: 4 bond pairs, 2 lone pairs

  • Hybridisationsp³d²
  • Bond angle90°
  • Polaritynon-polar

Why this shape

  1. Xe has 8 valence electrons. It uses four in four single bonds to F, so four are left as two lone pairs.
  2. Steric number = four sigma bonds + two lone pairs = 6, so Xe is sp³d² hybridised.
  3. Six electron pairs point to the corners of an octahedron (octahedral electron geometry). With two lone pairs in place of atoms, the atoms make a square planar shape.
  4. The two lone pairs sit opposite each other, 180 degrees apart, so their repulsion is least and the four bonds lie in a square.
  5. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 90°.
  6. The bond dipoles cancel in the symmetric square planar shape, so XeF₄ is non-polar.

Lewis structure

36 valence electrons
XeFFFF

Formal charges: none

Working

Why this hybridisation and shape

  1. Xe has 8 valence electrons. It uses four in four single bonds to F, so four are left as two lone pairs.
  2. Steric number = four sigma bonds + two lone pairs = 6, so Xe is sp³d² hybridised.
  3. Six electron pairs point to the corners of an octahedron (octahedral electron geometry). With two lone pairs in place of atoms, the atoms make a square planar shape.
  4. The two lone pairs sit opposite each other, 180 degrees apart, so their repulsion is least and the four bonds lie in a square.
  5. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 90°.
  6. The bond dipoles cancel in the symmetric square planar shape, so XeF₄ is non-polar.

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

Hybridisation of XeF4: quick answers

What is the hybridisation of XeF4?

Xe has 8 valence electrons. It uses four in four single bonds to F, so four are left as two lone pairs. Steric number = four sigma bonds + two lone pairs = 6, so Xe is sp³d² hybridised.

What is the shape of XeF4 and its bond angle?

Square planar, with a bond angle of 90 degrees. Six electron pairs point to the corners of an octahedron (octahedral electron geometry). With two lone pairs in place of atoms, the atoms make a square planar shape. The two lone pairs sit opposite each other, 180 degrees apart, so their repulsion is least and the four bonds lie in a square. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 90°.

Is XeF4 polar or non-polar?

Non-polar. The bond dipoles cancel in the symmetric square planar shape, so XeF₄ is non-polar.

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