In hybridization of XeF4 (Xenon Tetrafluoride), there are actually two hybridizations that take place. Xe is sp2d2 hybridized and F is sp3 hybridized.
|Name of the Molecule||Xenon Tetrafluoride|
|Bond Angle||90o or 180o|
What is the Hybridization of Xenon Tetrafluoride?
In xenon tetrafluoride, the hybridization takes place in the central atom which is Xenon (Xe). If we look at the valence shell of Xe there are a total of six electrons in the 5p orbital and two electrons in the 5s orbital. If we observe the 5th orbital then there are the d orbital and f orbital which no electrons are present. In the formation of XeF4, two of the 5p orbital electrons which are in excited state move to fill the vacant 5 d orbitals. As a result, there are 4 unpaired hybridized electrons which include 2 in 5p and 2 in 5d orbitals. This results in sp2d2 hybridization.
In the case of fluorine, four F atoms bond with these four half filled orbitals. These fluorine atoms will then be placed on either side of the central atom.
Important Points To Remember
- The central atom has 6 electron groups out of which two are lone pair electrons.
- The hybridization in Xenon is d2sp2 because there is a migration of two electrons of p to d orbital which results in the formation of sigma bond with F.
- The steric numbers of fluorine are all 4 meaning it is sp3 hybridised.
XeF4 Molecular Geometry And Bond Angles
XeF4 consists of two lone pair electrons. Now if we follow the VSEPR theory, the bond pair electrons and lone pair electrons experience repulsion between them. With this, they will acquire a stable state. The lone pairs of Xenon lie in the perpendicular plane in an octahedral arrangement. Therefore, XeF4 molecular geometry is square planar.
The bond angles are 90o or 180°. The lone pairs lie on the opposite sides of the molecule basically at 180° from each other.