The **Lewis structure of BrCl _{3}** contains three single bonds, with bromine in the center, and three chlorines on either side. There are three lone pairs on each chlorine atom, and two lone pairs on the bromine atom.

## Steps

By using the following steps, you can easily draw the Lewis structure of BrCl_{3}.

#1 Draw skeleton

#2 Show chemical bond

#3 Mark lone pairs

#4 Calculate formal charge and check stability (if octet is already completed on central atom)

Let’s one by one discuss each step in detail.

### #1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

- Let’s calculate the total number of valence electrons

We know that… both bromine and chlorine are the group 17 elements. Hence, both bromine and chlorine have **seven** valence electrons.

Now BrCl_{3} has one bromine atom and three chlorine atoms.

So the total number of valence electrons = valence electrons of bromine atom + (valence electrons of chlorine atom × 3)

Therefore, the **total number of valence electrons** = 7 + 21 = 28

- Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for bromine and chlorine as follows:

Electronegativity value of bromine = 2.96

Electronegativity value of chlorine = 3.16

Obviously, bromine is less electronegative than chlorine. Hence, assume that **bromine is the central atom**.

So now, put bromine in the center and chlorines on either side. And draw the rough skeleton structure for the Lewis structure of BrCl_{3} something like this:

**Also read:** How to draw Lewis structure of CSe_{2} (5 steps)

### #2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since bromine is surrounded by three chlorines, use six electrons to show **three chemical bonds** as follows:

**Also read:** How to draw Lewis structure of BeBr_{2} (4 steps)

### #3 Mark lone pairs

As calculated earlier, we have a total of 28 valence electrons. And in the above structure, we have already used six valence electrons. Hence, twenty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-two valence electrons = **eleven lone pairs**.

Note that bromine is a period 4 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.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are chlorines, so each chlorine will get three lone pairs. And the central atom (bromine) will get two lone pairs.

So the Lewis structure of BrCl_{3} looks something like this:

In the above structure, you can see that the octet is completed on the central atom (bromine), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

**Also read:** How to draw Lewis structure of XeO_{2}F_{2} (5 steps)

### #4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

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

Collect the data from the above structure and then, write it down below as follows:

- For
**bromine**atom

Valence electrons = 7

Nonbonding electrons = 4

Bonding electrons = 6

Formal charge = 7 – 4 – ½ (6) = 0

- For
**each chlorine**atom

Valence electrons = 7

Nonbonding electrons = 6

Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of BrCl_{3} looks something like this:

In the above structure, you can see that the formal charges of both (bromine and chlorine) are zero. Therefore, this is the **stable Lewis structure of BrCl _{3}**.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

## Related

- Lewis structure of CSe
_{2} - Lewis structure of BeBr
_{2} - Lewis structure of XeO
_{2}F_{2} - Lewis structure of AlBr
_{3} - Lewis structure of N
_{2}O_{5}

## External links

- BrCl3 Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Techiescientist
- Drawing the Lewis Structure for BrCl3 – The Geoexchange
- Brcl3 lewis structure, Characteristics:13 Must To Know Facts – Lambda Geeks
- BrCl3 Lewis Structure in 5 Steps (With Images) – Pediabay
- BrCl3 Lewis Structure (Bromine Trichloride) – Pinterest
- What is the orbital hybridization in BrCl3? – Socratic
- Draw the Lewis structure for BrCl3 – Homework.Study.com
- Draw the Lewis structure for BrCl – Chegg
- Draw the Lewis structure for BrCl3. What are the approximate bond angles about the central atom? – Brainly
- What is the lewis structure for BrCl3? – OneClass
- What is the hybridization and geometry of BrCl3? – Quora
- Draw the Lewis structure for BrCl3 – Course Hero
- What is the molecular shape of BrCl3? – Answers
- BrCl3 (Bromine Trichloride) Oxidation Number – ChemicalAid

Deep

Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.