XeF4 Lewis Structure| Lewis Dot Structure

XeF4 Lewis structure

Xenon tetrafluoride is a chemical compound having the chemical formula XeF4.It is formed by the reaction of xenon with fluorine. Xenon tetrafluoride is a white-colored solid compound with a square planar shape. Xenon tetrafluoride is non polar and has zero dipole moment.

XeF4 Lewis structure

According to VSEPR theory in xenon tetrafluoride, the xenon center has two lone pairs. White crystalline colorless solid and sublimes at 115.7 ℃.

Xenon tetrafluoride is formed by the reaction of Xe with fluorine.

Xe + 2F2 → XeF4

This is an exothermic reaction releasing 251 KJ/mole energy.

Lewis Structure of XeF4 :

XeF4 Lewis structure

Xenon tetrafluoride consist of Xenon noble gas. As we know that noble gases do not share electrons to any other atom. But xenon is different. The electronic configuration of xenon is ;

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

5th energy level of the orbital consists of s,p, d, f. Xenon has only completely filled s and p. The coming force from outside the electrons from p moves into d orbital. And then these moving electrons participate in bond formation. So as for drawing Lewis’s structure, Xenon is a noble gas and is expected to more than 8 electrons form outside.

For this problem.

We will use the number of valence electrons and valence shell electronic configuration of electrons of each atom to help in drawing the right Lewis structure.

By obtaining the following:

  1. valence electrons
  2. Electron configuration
XeF4 Lewis structure

Valence electrons of XeF4 :

This can be given out by sum up of valence electrons of each atom in the compound. First of all list down atoms present and the total number of atoms in the compound. AS we know that in xenon tetrafluoride there is 1 xenon and four fluorine. And from the periodic table, we get the valence electrons of each atom.

AtomNo.of atomvalence esub-total

So xenon has 8 electrons and fluorine has 7 electrons so the total number of electrons is 36 electrons.

Electron Configuration:

The electronic configuration of xenon tetrafluoride is;

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

In xenon tetrafluoride, the xenon is a less electronegative atom so it is considered a central atom. First of all, we draw single bonds between the central atom and terminals fluorine atoms. Then we draw the remaining unpaired electrons of each atom according to their number of valence electrons. Now after this we have to check the stability of xenon tetrafluoride the fluorine must follow the octet rule. Fluorine must have 8 electrons. There is no lone pair.

Dipole moment in XeF4 :

XeF4 geometry

By knowing dipole moment helps to determine the position of atoms attached with the central atom is correct or not. For dipole moment between Xenon and Fluorine, it helps us pull xenon towards fluorine because fluorine is more electronegative in nature. Between the central atom and its lone pair direction of the dipole moment will favor in pointing the lone pair. The geometry is square planar.

Imagine a plane on the y-axis perpendicular to the plane in the x-axis. The lone pairs are present in the plane on the y-axis. Fluorine atoms are in the perpendicular plane on the x-axis. The lone pair pulls xenon atoms towards them at equal force. Fluorine atoms also pull the xenon atom towards them in opposite direction and with the same amount of force.

This results in zero dipole moment.


Xenon tetrafluoride contains xenon as the central atom and it is the place where hybridization takes place. Valence shell of atom contains 6 electrons in 5p orbital. Whereas there are 2 electrons in 5s orbital. There is no electrons present in f and d orbitals.

AS we discussed earlier that in xenon tetrafluoride the two electrons in 5p orbital becomes excited and move to 5d orbitals in order to fill empty or vacant space. And after this the remaining 4 unpaired electrons form sp3d2 hybridization in which there is two unpaired electrons in 5p orbital and 2 in 5d orbital. A sigma bond is formed so xenon tetrafluoride has sp3d2 hybridization.

Points to be noted:

  • In xenon tetrafluoride the central atom constitute 6 electron pairs in which 2 are lone pair electrons.
  • So hybridization is because 2 electrons shifted from p to d which results into formation of sigma bond with fluorine.

Molecular geometry:

As xenon tetrafluoride has two lone pair electrons. According VSEPR theory the net electronic repulsion will be decreases. And in this way the get a stable state. For this the lone pairs lie in perpendicular plane in an octahedral arrangement that are opposite from each other. And the bond angle is 90 degree. So that’s why xenon tetrafluoride has square planar geometry.

XeF4 bond angle

Polarity of XeF4 :

Xenon tetrafluoride is non polar molecule. As we discussed that there is square planar geometry and net dipole moment is zero across the molecule. So there is uniform charge distribution and no polarization across xenon tetrafluoride.

Mo diagram of XeF4 :

First of all that MO diagram of any molecule explain chemical bonds in a given molecule with the help of molecular orbital theory. MO diagram helps to determine existence of molecules. This determine strength of bonds and electronic transitions.

In xenon tetrafluoride there is square planar geometry. And there is 1.95A° distance between xenon and fluorine. It is explained through valence bond theory that there is 2 non bonding electrons that jumps from p orbital to d orbital in order to fill vacant space. 4 half filled orbitals form covalent bonds with half filled 2p orbitals of fluorine atom in structure.

Xenon tetrafluoride there is 2 lone pairs and four bond pairs.

XeF4 MO diagram

Uses of XeF4:

It is used in finding traces of silicon metal that is contaminated to rubber.

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