# 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.

Contents

## Steps

Use these steps to correctly draw the BrF 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 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

• 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

### #2 Mark lone pairs on the atoms

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:

### #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 – 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.

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

Therefore, this structure is the stable Lewis structure of BrF.

Next: AlH3 Lewis structure