Numford
Hybridisation

Hybridisation of XeF₂

Xe is sp³d hybridised (hybridization by the VSEPR count): 2 sigma bonds and 3 lone pairs give a linear shape, bond angle 180°.

FXeF
  • Xe
  • F
  • lone pair

XeF₂Xenon difluoride

Linear

AB₂E₃: 2 bond pairs, 3 lone pairs

  • Hybridisationsp³d
  • Bond angle180°
  • Polaritynon-polar

Why this shape

  1. Xe has 8 valence electrons. It uses two in two single bonds to F, so six are left as three lone pairs.
  2. Steric number = two sigma bonds + three lone pairs = 5, so Xe is sp³d hybridised.
  3. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With three lone pairs in place of atoms, the atoms make a linear shape.
  4. All three lone pairs take the equatorial positions, 120 degrees apart, and the two bonds point up and down.
  5. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 180°.
  6. The bond dipoles cancel in the symmetric linear shape, so XeF₂ is non-polar.

Lewis structure

22 valence electrons
XeFF

Formal charges: none

Working

Why this hybridisation and shape

  1. Xe has 8 valence electrons. It uses two in two single bonds to F, so six are left as three lone pairs.
  2. Steric number = two sigma bonds + three lone pairs = 5, so Xe is sp³d hybridised.
  3. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With three lone pairs in place of atoms, the atoms make a linear shape.
  4. All three lone pairs take the equatorial positions, 120 degrees apart, and the two bonds point up and down.
  5. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 180°.
  6. The bond dipoles cancel in the symmetric linear shape, so XeF₂ is non-polar.

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

Hybridisation of XeF2: quick answers

What is the hybridisation of XeF2?

Xe has 8 valence electrons. It uses two in two single bonds to F, so six are left as three lone pairs. Steric number = two sigma bonds + three lone pairs = 5, so Xe is sp³d hybridised.

What is the shape of XeF2 and its bond angle?

Linear, with a bond angle of 180 degrees. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With three lone pairs in place of atoms, the atoms make a linear shape. All three lone pairs take the equatorial positions, 120 degrees apart, and the two bonds point up and down. The lone pairs balance each other, so the bonds are not pushed out of place and the angle stays at 180°.

Is XeF2 polar or non-polar?

Non-polar. The bond dipoles cancel in the symmetric linear shape, so XeF₂ is non-polar.

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