XeO2 Lewis Structure & Characteristics: 11 Complete Facts

XeO2 Lewis structure can be defined as an informative study on internal structure of the compound. Let us find the various facts about this Lewis structure.

XeO2 Lewis structure is the design of electronic arrangement of the compound. This compound is clearly consisting one of the noble gases that is Xenon. Therefore, the facts about compound are going to be interesting regarding the electron sharing methods between two Oxygen atom and Xenon.

As Xe is a noble gas it has filled electronic configuration with 8 electrons in its last electronic valance shell. Each oxygen molecule undergoes electron-sharing process by grabbing four electrons from Xe and drives them to create bonds with each other and generates a well-figured Lewis structure. Let us broadly discuss the characteristics of XeO2.

How to draw XeO2 Lewis structure

Drawing XeO2 Lewis structure would follow few easy and acquirable steps. Let us describe the steps below:

Step 1: Calculating number of valence electrons in Xenon and Oxygen atoms

The number of valence electrons in Xe and two Oxygen atoms helps to identify the stability of atoms. Depending on the number of valence electrons, the necessity of electrons in element are identified. Number of valence electrons supports the elements to gain or leave electrons from its last energy level.

Step 2: Finding the needs of electrons in each atom

The need of valence electron in Xenon is not significant as I has filled valence shell. Xenon is one of the most stable elements in periodic table. Nevertheless, each of the Oxygen atoms needs two electrons in last energy level to gain the similar stability as neon (their nearest noble gas).

Step 3: Identifying number and type of bonds

XeO2 Lewis structure has two double bonds. That the total number of sigma bond is 2 and totals number of pi bonds is 2. This is due to the sharing of 2 electrons is encouraged by Xenon in the compound for each of the Oxygen atom.

Step 4: Highlighting the centre atom

Xenon is the chosen centre atom for the compound as it joins in bonding with an appearance of single atom. Even after being more electronegative than Xenon, Oxygen cannot take place in the centre. Xenon is the most stable element so it is perfect suitor of that position.

Step 5: Recognising presence of lone pairs and extra electrons

XeO2 Lewis structure holds the elements with lone pairs. Xenon has two lone pairs left in it after making bonds with 2 Oxygen atom. Both the oxygen are similar and they and have 2 lone pairs in each as well. This lone pairs effective display their existence in the compound that would be described later.

XeO2 Lewis structure resonance

Resonance is a special feature that is found in some specific compound that have extra electron or Pi bonds in the compound. Let us find resonance in XeO2 is effective or not.

XeO2 Lewis structure resonance comes from its intact composition of two double bond and six lone pairs. Both the ligands are attached with centre atom with one pi bond and one sigma bond, therefore, there is no chance to flip or alter the pi bond on other side.  There is no resonating structure of XeO2.

xeo2 lewis structure
XeO2 Lewis structure resonance from Wikipedia

All the valence shells are filled in the Xenon dioxide. Therefore, it does not allow to make any resonating structure. No negative charge exists in xenon dioxide. Therefore, there is no resonating structure appears in case of XeO2.

XeO2 Lewis structure shape

Shape of Xenon dioxide can be defined by studying its Lewis structure in detail. Let us recognise the shape of XeO2 and reason behind possessing that shape.

The shape of XeO2 Lewis structure is bent. This could be linear shaped compound but the internal effect o lone pairs and presence of pi bonds makes the structure bent.  The compound deviated from its ideal bond angle.

The geometry of XeO2 is tetrahedral. This geometric shape is defined by recognising the position of lone pairs in the compound. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the compound feels high lone pair–lone pair and lone pair-bond pair repulsion which gives it bent shape.

XeO2 Lewis structure formal charge

Formal charge calculation is needed to identify the state of compound regarding its charge and electron holding capacity. Let us calculate the formal charge of Xenon dioxide.

Formal charge of XeO2 Lewis structure can be calculated with a simple formula. Formal charge = number of valence electrons – number of nonbonding electrons – number of electron shared (number of bonding electrons/2)

ElementsNumber of valence electronsNumber of nonbonding electronsNumber of electron sharedFormal charge
Xe844/2 = 2(8-4-2) = +2
O1642/2 = 1(6-4-1) = +1
O2642/2 = 1(6-4-1) = +1
Formal charge of XeO2[+2- (+1+1)] = 0
Formal charge calculation of XeO2 Lewis structure

XeO2 Lewis structure angle

Angle of a structure refers to the bond angle between centre atom and its ligands. The facts about bond angle of Xenon dioxide is described below.

The bond angle of XeO2 Lewis structure should be 109.5°. In accordance with the ideal bond angle of tetrahedral geometry, XeO2 bond angle differs. Bond angle of Xenon dioxide deviates from its ideal bond angle due to Lone-pair-bond pair repulsion. Bent shape of XeO2 does not make it ideally shaped compound.

XeO2 bond angle varies according to the increase and decrease in repulsion. It is obvious that the compound cannot regulate repulsion factor and cannot achieve the ideal bond angle.

XeO2 Lewis structure octet rule

Octet rule is the key factor that drives Lewis elements to share electrons with each other. An interesting fact about octet rule, works behind formation of XeO2 is given below.

XeO2 Lewis structure follows octet rule to generate bonds. This rule says, each atom must have 8 electrons in its last energy level to achieve ultimate stability. Xe already have 8 electrons and for having the same each of the Oxygen atoms borrows 2 electrons from Xe and makes double bonds with it.

Octet rule is found to be driving force for making the elements share or transfer their electrons. It can be said that for satisfying octet state oxygen takes help of Xenon. Being an ideal compound and complete octet Xenon shares its electrons with oxygen partially.

XeO2 Lewis structure lone pairs

Calculating number of lone pairs in compounds is important, This feature defines the internal effect on bonding and shape of compounds. Fact about lone pairs is evaluated below:

XeO2 Lewis structure has total 6 lone pairs. After binding the centre atom, Xenon holds 2 lone pairs. Each of the oxygen atom makes similar bond with Xenon so both of them holds two lone pairs. The lone pairs of Oxygen atoms make the difference in this compound from others.  

In Xenon dioxide, the lone pairs of Oxygen molecules are arranged in dissimilar way. This effects on the bond of the compound and creates a unique structure of compound. This lone pairs are strongly influential in the physical properties of this compound.

XeO2 valence electrons

Valence electron calculation is highly important factor, which activates the drawing the Lewis structure of XeO2. Let us calculate the number of valence electron in XeO2 below.

  • Number of valence electrons in Xenon = 8
  • Number of valence electrons in each of the oxygen atoms = 6
  • Total number of valence electrons in two Oxygen atoms = (6*2) = 12
  • Total number of valence electron in XeO2 = (8+12) = 20

Octet rule works accordingly with the quantity of valence electrons in compound. This factor is related to the octet rule. In order to gain or lose electron for 8 electrons in total the calculation of valence electrons is the most significant job.

XeO2 hybridization

Hybridisation is a major factor that activates the knowledge about changed structure of compound after sharing electrons. Let us find the Hybridisation of XeO2.

Hybridisation of Xe in XeO2 Lewis structure is found as sp3. This is an controversial approach as Xe is found here as a hypervalent atom. As the geometric shape of the compound is found as tetrahedral and this kind of geometry had sp3 hybridisation, the hybridisation of XeO2 is predicted as sp3.

Is XeO2 polar or nonpolar?

Polarity can be found for XeO2 by studying the presence of internal effects again. This fact would broadly discussed here.

XeO2 Lewis structure is polar. As the shape of XeO2 is bent and bond angle is deviated from its ideal state, its polarity is found with as specific amount of dipole movement. Two diploes of XeO2 compound are not cancelled out anyway which makes it polar.

This fact also face a controversial argument. Some chemists use to say that the lone pairs of XeO2 can be out in opposite to each other which would derive it as nonpolar compound. This makes the debate according to the exact amount of dipole moment in Xenon dioxide and this is a exceptional compound in chemistry.

Why and how XeO2 is Polar?

Reason of calling XeO2 Lewis structure polar is quite interesting. Let us identify this factor describing the way XeO2 behaves as a polar compound below.

XeO2 is polar due to the tetrahedral geometry and bent shape of the compound. VSEPR theory has identified that the lone pairs of the compound cannot be put in opposite to each other. Lone pairs of oxygen create dissimilar tension in each dipole of XeO2 and it is polar by a specific amount of dipole moment.


XeO2 Lewis structure has been found as an informative subject. It has given several important chemical ideas about bent shape and deviation of bond angle due to lone pair-bond pair repulsion. The article has provided knowledge about octet rule and other related factor with bond formation of compounds.

Sarnali Mukherjee

Hi.....I am Sarnali Mukherjee, a graduate from the University of Calcutta. I love to teach and share knowledge on chemistry. I have gradually gained interest in article writing since one year ago. I would love to acquire more knowledge on my subject in the future. Let's connect through LinkedIn: https://www.linkedin.com/in/sarnali-mukherjee-921b59231

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