XeCl3- Lewis structure

XeCl₃^– (xenon trichloride) has one xenon atom and three chlorine atoms.

In the XeCl₃^– Lewis structure, there are three single bonds around the xenon atom, with three chlorine atoms attached to it, and each atom has three lone pairs.

Also, there is a negative (-1) charge on the xenon atom.

Alternative method: Lewis structure of XeCl₃^–

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 XeCl₃^– has one xenon atom and three chlorine atoms, so…

Valence electrons of one xenon atom = 8 × 1 = 8
Valence electrons of three chlorine atoms = 7 × 3 = 21

Now the XeCl₃^– has a negative (-1) charge, so we have to add one more electron.

So the total valence electrons = 8 + 21 + 1 = 30

Learn how to find: Chlorine valence electrons

• Second, find the total electron pairs

We have a total of 30 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 = 30 ÷ 2 = 15

• 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 15 electron pairs. And three Xe — Cl bonds are already marked. So we have to only mark the remaining twelve 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 chlorine, there are three lone pairs, and for xenon, 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 (6) = -1

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

Here, the xenon atom has a charge, so mark it on the sketch as follows:

Final structure

The final structure of XeCl₃^– consists of a central xenon atom connected to three chlorine atoms through single covalent bonds. In this configuration, the xenon atom utilizes an expanded valence shell to accommodate twelve electrons, which include three 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 is the most stable because it results in a -1 formal charge on the central xenon atom, while each chlorine atom retains a formal charge of zero. Consequently, this specific electronic distribution serves as the definitive and most accurate Lewis representation of XeCl₃^–.

To properly represent this as a polyatomic ion, the entire Lewis structure is enclosed within square brackets. The overall charge of 1- is then written as a superscript outside the brackets at the top right, reflecting the presence of an additional electron beyond the total valence count of the neutral atoms.

Next: POF₃ Lewis structure

External video

• How to Draw the Lewis Dot Structure for XeCl3-: Xenon trichloride anion – YouTube • Wayne Breslyn