Lewis structure of XeF₂
22 valence electrons. Two Xe-F single bonds, with three lone pairs on Xe, so Xe has 10 electrons around it (an expanded octet).
Lewis structure
22 valence electronsFormal charges: none
Why this shape
- 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.
- 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°.
- The bond dipoles cancel in the symmetric linear shape, so XeF₂ is non-polar.
How to draw it
- Count the valence electrons: Xe 8 + 2 × F 7 = 22 valence electrons, 11 pairs.
- Put Xe in the middle and join it to the two outer atoms with single bonds.
- Give each outer atom lone pairs until it has an octet (H needs only two electrons), then put any electrons left over on the central atom.
- Result: two Xe-F single bonds, with three lone pairs on Xe, so Xe has 10 electrons around it (an expanded octet).
- Formal charge = valence electrons − lone pair electrons − number of bonds. Here: none.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Lewis structure of XeF2: quick answers
How many valence electrons are in XeF2?
Xe 8 + 2 × F 7 = 22 valence electrons, 11 pairs.
What are the formal charges in the Lewis structure of XeF2?
Every atom has a formal charge of zero.
How many lone pairs are in the Lewis structure of XeF2?
9 in all, 3 of them on the central Xe.