BrF Lewis structure

BrF (bromine monofluoride) has one bromine atom and one fluorine atom.

In BrF Lewis structure, there is a single bond between the bromine and fluorine atom, and on both bromine and fluorine atoms, there are three lone pairs.

Alternative method: Lewis structure of BrF

Rough sketch

• First, determine the total number of valence electrons

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

Hence, both bromine and fluorine have seven valence electrons.

Since BrF has one bromine atom and one fluorine atom, so…

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

And the total valence electrons = 7 + 7 = 14

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

• Second, find the total electron pairs

We have a total of 14 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 = 14 ÷ 2 = 7

• Third, determine the central atom

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

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 7 electron pairs. And one Br — F bond is already marked. So we have to only mark the remaining six 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 fluorine is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atom is fluorine.

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 bromine atom, formal charge = 7 – 6 – ½ (2) = 0

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

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

Final structure

The final structure of BrF involves a bromine atom connected to a fluorine atom through a single covalent bond. Within this layout, both the bromine and fluorine atoms satisfy the octet rule. The bromine atom retains three lone pairs, and the fluorine atom similarly maintains three lone pairs alongside the single shared bonding pair. This arrangement is the most stable because it results in formal charges of zero for both atoms, representing the most energetically favorable state for the molecule. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of bromine monofluoride.

Next: AlH₃ Lewis structure

External video

• BrF Lewis Structure: How to Draw the Lewis Structure for BrF (Bromine monofluoride) – YouTube • Wayne Breslyn

External links

• https://www.thegeoexchange.org/chemistry/bonding/Lewis-Structures/BrF-Lewis-structure.html
• https://lambdageeks.com/brf-lewis-structure/
• https://homework.study.com/explanation/draw-a-lewis-structure-for-brf-draw-the-molecule-by-placing-atoms-on-the-canvas-and-connecting-them-with-bonds-include-all-lone-pairs-of-electrons.html
• https://www.numerade.com/questions/draw-the-lewis-structure-for-brf-with-an-arrow-representing-the-dipole-moment-use-figure-65-to-estim/
• https://www.chegg.com/homework-help/questions-and-answers/part-draw-lewis-structure-brf-draw-molecule-placing-atoms-grid-connecting-bonds-include-lo-q5595105