The **Lewis structure of BrF _{5}** contains five single bonds, with bromine in the center, and five fluorines on either side. There are three lone pairs on each fluorine atom, and one lone pair on the bromine atom.

## Steps

By using the following steps, you can easily draw the Lewis structure of BrF_{5}:

#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)

Letâ€™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.

- Letâ€™s calculate the total number of valence electrons

We know thatâ€¦ both bromine and fluorine are the group 17 elements. Hence, both bromine and fluorine have **seven** valence electrons.

Now BrF_{5} has one bromine atom and five fluorine atoms.

So the total number of valence electrons = valence electrons of bromine atom + (valence electrons of fluorine atom Ã— 5)

Therefore, the **total number of valence electrons** = 7 + 35 = 42

- 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 fluorine as follows:

Electronegativity value of bromine = 2.96

Electronegativity value of fluorine = 3.98

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

So now, put bromine in the center and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of BrF_{5} something like this:

**Also read:** How to draw Lewis structure of BrF_{3} (4 steps)

### #2 Show chemical bond

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

**Also read:** How to draw Lewis structure of HF (4 steps)

### #3 Mark lone pairs

As calculated earlier, we have a total of 42 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, thirty-two valence electrons are remaining.

Two valence electrons represent one lone pair. So thirty-two valence electrons = **sixteen lone pairs**.

Note that bromine is a period 4 element, so it can keep more than 8 electrons in its last shell. And fluorine is a period 2 element, so it can not 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 fluorines, so each fluorine will get three lone pairs. And the central atom (bromine) will get one lone pair.

So the Lewis structure of BrF_{5} 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 IF_{5} (4 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 – Â½ 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 = 2

Bonding electrons = 10

Formal charge = 7 – 2 – Â½ (10) = 0

- For
**each fluorine**atom

Valence electrons = 7

Nonbonding electrons = 6

Bonding electrons = 2

Formal charge = 7 – 6 – Â½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of BrF_{5} looks something like this:

In the above structure, you can see that the formal charges of both (bromine and fluorine) are zero. Therefore, this is the **stable Lewis structure of BrF**** _{5}**.

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

## Related

- Lewis structure of BrF
_{3} - Lewis structure of HF
- Lewis structure of IF
_{5} - Lewis structure of SCl
_{2} - Lewis structure of ClF
_{3}

## External links

- Drawing the Lewis Structure for BrF5 – The University of Maryland
- Brf5 Lewis Structure, Characteristics:13 Must To Know Facts – Lambda Geeks
- BrF5 Lewis Structure in 5 Steps (With Images) – Pediabay
- BrF5 lewis structure, molecular geometry, bond angle, polarity, electrons – Topblogtenz
- BrF5 Lewis Structure, Geometry – Kemicalinfo
- BrF5 Lewis Structure, Molecular Structure, Hybridization, Bond Angle and Shape – Geometry of Molecules
- BrF5 Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Techiescientist
- BrF5 Lewis Dot Structure (Bromine Pentafluoride) – Pinterest
- Chemical Bonding: BrF5 Lewis Structure – The Geoexchange
- How to draw BrF5 Lewis Structure? – Science Education and Tutorials
- Molecular Geometry of BrF5 [with video and free study guide] – AceOrganicChem
- Draw the Lewis structure for BrF5 – Homework.Study.com
- Bromine Pentafluoride, BrF5 Molecular Geometry & Polarity – Tutor-Homework.com
- For the molecule BrF5, draw the Lewis structure, arrangement, geometry/shape, and hybridization for non-hydrogen atoms? – Chegg
- What is the Lewis structure for BrF5? – Brainly
- brf5 lewis structure molecular geometry – Quizlet
- BrF5 Geometry and Hybridization – Chemistry Steps
- Draw the Lewis structure for BrF5 – Numerade
- Explain in detail if Bromine Pentafluoride (BrF5) has resonance structures? – Wyzant

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.