XeCl2 Lewis structure

XeCl₂ (xenon dichloride) has one xenon atom and two chlorine atoms.

In the XeCl₂ Lewis structure, there are two single bonds around the xenon atom, with two chlorine atoms attached to it, and each atom has three lone pairs.

Alternative method: Lewis structure of XeCl₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, xenon lies in group 18, and chlorine lies in group 17.

Hence, xenon has eight valence electrons and chlorine has seven valence electrons.

Since XeCl₂ has one xenon atom and two chlorine atoms, so…

Valence electrons of one xenon atom = 8 × 1 = 8
Valence electrons of two chlorine atoms = 7 × 2 = 14

And the total valence electrons = 8 + 14 = 22

Learn how to find: Chlorine valence electrons

• Second, find the total electron pairs

We have a total of 22 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 22 ÷ 2 = 11

• Third, determine the central atom

We have to place the least electronegative atom at the center.

Since xenon is less electronegative than chlorine, assume that the central atom is xenon.

Therefore, place xenon in the center and chlorines on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 11 electron pairs. And two Xe — Cl bonds are already marked. So we have to only mark the remaining nine electron pairs as lone pairs on the sketch.

Also remember that xenon is a period 5 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are chlorines.

So for each atom, there are three lone pairs.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For xenon atom, formal charge = 8 – 6 – ½ (4) = 0

For each chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, both xenon and chlorine atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of XeCl₂ consists of a central xenon atom connected to two chlorine atoms through single covalent bonds. In this configuration, the xenon atom utilizes an expanded valence shell to accommodate ten electrons, which include two bonding pairs and three lone pairs. Each chlorine atom satisfies the octet rule by maintaining three lone pairs alongside its single shared bond. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for all atoms involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of xenon dichloride.

Next: KrF₄ Lewis structure

External video

• A step-by-step explanation of how to draw the XeCl2 Lewis Dot Structure (Xenon Dichloride) – YouTube • Wayne Breslyn