How to work it out
- Central atom: Xe, with 8 valence electrons.
- Add 1 for each H or halogen around it: 4. O and S add nothing.
- Steric number = ½ × (8 + 4) = 6.
- 5 atoms are bonded, so 6 − 5 = 1 lone pair.
- 6 electron pairs → sp³d², octahedral arrangement; the lone pairs make the shape square pyramidal.
Why XeOF₄ has this shape
Five bonds and one lone pair give a square pyramid, with O at the top and the lone pair underneath the square of F atoms.
XeOF₄ is polar: its shape means the bond dipoles don't cancel.
Other molecules with the same square pyramidal shape: BrF₅, IF₅.
Hybridization of common molecules
| Molecule or ion | Hybridization | Shape | Lone pairs |
|---|---|---|---|
| XeF₄ | sp³d² | Square planar | 2 |
| XeF₂ | sp³d | Linear | 3 |
| XeF₆ | sp³d³ | Distorted octahedral | 1 |
| XeO₃ | sp³ | Trigonal pyramidal | 1 |
| XeOF₄ | sp³d² | Square pyramidal | 1 |
| SF₄ | sp³d | See-saw | 1 |
| SF₆ | sp³d² | Octahedral | 0 |
| ClF₃ | sp³d | T-shaped | 2 |
| BrF₃ | sp³d | T-shaped | 2 |
| BrF₅ | sp³d² | Square pyramidal | 1 |
| IF₅ | sp³d² | Square pyramidal | 1 |
| IF₇ | sp³d³ | Pentagonal bipyramidal | 0 |
| PCl₅ | sp³d | Trigonal bipyramidal | 0 |
| PCl₃ | sp³ | Trigonal pyramidal | 1 |
| NH₃ | sp³ | Trigonal pyramidal | 1 |
| H₂O | sp³ | Bent (V-shaped) | 2 |
| CH₄ | sp³ | Tetrahedral | 0 |
| BF₃ | sp² | Trigonal planar | 0 |
| BeCl₂ | sp | Linear | 0 |
| CO₂ | sp | Linear | 0 |
| SO₂ | sp² | Bent (V-shaped) | 1 |
| SO₃ | sp² | Trigonal planar | 0 |
| H₂S | sp³ | Bent (V-shaped) | 2 |
| NH₄⁺ | sp³ | Tetrahedral | 0 |
| H₃O⁺ | sp³ | Trigonal pyramidal | 1 |
| NO₃⁻ | sp² | Trigonal planar | 0 |
| NO₂⁺ | sp | Linear | 0 |
| CO₃²⁻ | sp² | Trigonal planar | 0 |
| SO₄²⁻ | sp³ | Tetrahedral | 0 |
| ClO₄⁻ | sp³ | Tetrahedral | 0 |
| I₃⁻ | sp³d | Linear | 3 |
| ICl₄⁻ | sp³d² | Square planar | 2 |
| PF₆⁻ | sp³d² | Octahedral | 0 |
| SnCl₂ | sp² | Bent (V-shaped) | 1 |
Questions students ask
What is the hybridization of XeOF₄?
sp³d². The central Xe has 6 electron pairs around it: 5 bonds and 1 lone pair.
What is the shape of XeOF₄?
Square pyramidal. The electron pairs are arranged octahedral, but the 1 lone pair is not counted in the shape.
What is the bond angle in XeOF₄?
about 91°, smaller than the ideal octahedral angle because lone pairs repel the bonds more.
Is XeOF₄ polar or nonpolar?
XeOF₄ is polar: its shape means the bond dipoles don't cancel.