BrCl_{5} has **one bromine** atom and **five chlorine** atoms.

In BrCl_{5} Lewis structure, there are five single bonds around the bromine atom, with five chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the bromine atom has one lone pair.

## Steps

Use these steps to correctly draw the BrCl_{5} Lewis structure:

#1 First draw a rough sketch

#2 Mark lone pairs on the atoms

#3 Calculate and mark formal charges on the atoms, if required

Let’s discuss each step in more detail.

### #1 First draw a rough sketch

- First, determine the total number of valence electrons

In the periodic table, both bromine and chlorine lie in group 17.

Hence, both bromine and chlorine have **seven** valence electrons.

Since BrCl_{5} has one bromine atom and five chlorine atoms, so…

Valence electrons of one bromine atom = 7 × 1 = 7

Valence electrons of five chlorine atoms = 7 × 5 = 35

And the **total valence electrons** = 7 + 35 = 42

Learn how to find: Bromine valence electrons and Chlorine valence electrons

- Second, find the total electron pairs

We have a total of 42 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** = 42 ÷ 2 = 21

- Third, determine the central atom

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

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

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

- And finally, draw the rough sketch

### #2 Mark lone pairs on the atoms

Here, we have a total of 21 electron pairs. And five Br — Cl bonds are already marked. So we have to only mark the remaining sixteen electron pairs as lone pairs on the sketch.

Also remember 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.

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 bromine, there is **one** lone pair.

Mark the lone pairs on the sketch as follows:

### #3 Calculate and mark formal charges on the atoms, if required

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

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

For **bromine** atom, formal charge = 7 – 2 – ½ (10) = 0

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

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

In the above structure, you can see that the central atom (bromine) forms an octet. And the outside atoms (chlorines) also form an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the **stable Lewis structure** of BrCl_{5}.

**Next:** CFCl_{3} Lewis structure

## External links

- https://lambdageeks.com/brcl5-lewis-structure/
- https://homework.study.com/explanation/find-the-number-of-electron-pairs-number-of-lone-pairs-electronic-geometry-molecular-geometry-and-lewis-structure-for-brcl5.html
- https://www.chegg.com/homework-help/questions-and-answers/draw-lewis-structure-brcl5-give-electron-domain-geometry-molecular-geometry-molecule-q9002031
- https://www.numerade.com/ask/question/draw-a-lewis-structure-for-brcl5-what-is-the-molecular-geometry-around-the-central-atom-in-the-lewis-structure-39165/

Deep

Learnool.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.