Understanding Hybridisation of XeO₂F₂: Xenon Dioxide Difluoride

Xenon Dioxide Difluoride (XeO₂F₂) is also known as difluoro(dioxo)xenon. It has one xenon atom bonded to two fluorine atoms and two oxygen atoms. It’s a good example of sp³d hybridisation in inorganic chemistry. The compound also expands its octet.

Let us understand how hybridisation happens in XeO₂F₂. Read on to learn how it leads to its bonding and molecular shape.

What is the Hybridisation of XeO₂F₂?

Xenon Dioxide Difluoride consists of one central xenon atom, which is bonded to fluorine atoms and oxygen atoms. In all, it also has one lone pair of electrons. In order to form these bonds and follow the principle of expanded octet, xenon undergoes sp3d hybridisation.

Breakdown of XeO₂F₂ Hybridisation

XeO₂F₂ has a see-saw shape. The lone pairs take up equatorial positions, leading the fluorine atoms to take the axial positions. The VSEPR Theory explains all this structure.

Here is a complete understanding of its hybridisation.

Electronic Configuration of Xenon

Atomic number of xenon: 54

The ground state of xenon :

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶

Only has zero unpaired electron → insufficient to form four bonds

Excited state configuration:

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p3 5d3

Now, six unpaired electrons → enough to form bonds

And, now we can have space for lone pair also

Ground state vs excited state orbital diagram

Formation of Hybrid Orbitals

sp³d hybridisation occurs when 1 s orbital, 3 p orbitals, and 1 d orbital mix to form equivalent hybrid orbitals.
The result:
→ 5 sp³d hybrid orbitals on the xenon atom
→ These accommodate lone pairs and are used to form bonds between atoms.

Bond Formation in Xenon Dioxide Difluoride

The xenon atom uses:

2 sp³d hybrid orbitals to form a σ bond with oxygen (in the Xe=O )
2 sp³d hybrid orbitals to form a σ bond with fluorine
1 sp³d hybrid orbital holds the lone pair of electrons

Result:

2 Xe–F σ bond
2 Xe–O σ bond
2 Xe=O π bonds
1 Lone Pair
Hybridisation type: sp³d
Geometry: See-saw

Geometry of Xenon Dioxide Difluoride

Details At A Glance

Property	Details
Molecule	Xenon Dioxide Difluoride (XeO₂F₂)
Hybridisation	sp³d
Geometry	Trigonal Bipyramidal (distorted)
Bond angle	<120° (equatorially) and <90° (axially)
Bonding	4 σ bonds (2 Xe–F, 2 Xe–O) + 2 π bonds (Xe=O)
Unhybridised Orbitals	0 (all involved in hybridisation)
Xenon valency satisfied?	Yes, by having expanded octet with 10 electrons around it

Formal Charge in XeO₂F₂

To determine if the Lewis structure of XeO₂F₂ is stable, we calculate the formal charge on each atom using the formula:

Formal charge = Valence electrons – (Lone pair electrons + ½ × Bonding electrons)

Step-by-step for each atom:

Xenon (Xe) :

Valence electrons: 8
Lone pairs: 1 (2 electrons)
Bonding electrons: 12
(4 from two Xe–F bonds and 8 from two Xe=O bonds)

Formal charge = 8 – (2 + ½×12) = 8 – (2 + 6) = 8 – (8) = 0

Oxygen (O) – each

Valence electrons: 6
Lone pairs: 2 (4 electrons)
Bonding electrons: 4 (1 Xe=O bond)

Formal charge = 6 – (4 + ½×4) = 6 – (4 + 2) = 6 – (6) = 0

Fluorine (F) – each

Valence electrons: 7
Lone pairs: 3 (6 electrons)
Bonding electrons: 2 (1 Xe–F)

Formal charge = 7 – (6 + ½×2) = 7 – (6 + 1) = 7 – (7) = 0

Thus, all atoms in XeO₂F₂ have zero formal charge, which concludes and confirms that the Lewis structure is stable and correct.

Summing Up

Xenon in XeO₂F₂ forms 6 bonds: 2 with fluorine and 4 with oxygen (2 σ and 2 π). XeO₂F₂ has a distorted trigonal bipyramidal geometry and ends up having a see-saw-like structure.

Frequently Asked Questions

Q1. Why does xenon undergo hybridisation in XeO₂F₂?

To form 4 single bonds with F and O and also accommodate 1 lone pair, xenon forms multiple bonds, promotes electrons, and uses d orbitals for bonding.

Q2. How many σ and π bonds are present in XeO₂F₂?

There are 4 σ bonds and 2 π bonds in total.

Q3. What is the shape of Xenon Dioxide Difluoride?

Distorted trigonal bipyramidal (See-saw), due to the presence of a lone pair.

Q4. Is XeO₂F₂ polar or non-polar?

Polar, as the molecule has asymmetrical distribution of charge due to lone pairs.

Q5. What are some uses of Xenon Dioxide Difluoride in our daily lives?

Xenon Dioxide Difluoride, under specific conditions, can be synthesized by the reaction of xenon with oxygen difluoride (OF₂).