BrF3 Lewis Structure in 6 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

BrF3 lewis structure has a Bromine atom (Br) at the center which is surrounded by three Fluorine atoms (F). There are 3 single bonds between the Bromine atom (Br) and each Fluorine atom (F). There are 2 lone pairs on the Bromine atom (Br) and 3 lone pairs on all three Fluorine atoms (F).

If you haven’t understood anything from the above image of BrF3 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of BrF3.

So let’s move to the steps of drawing the lewis structure of BrF3.

Steps of drawing BrF3 lewis structure

Step 1: Find the total valence electrons in BrF3 molecule

In order to find the total valence electrons in a BrF3 molecule, first of all you should know the valence electrons present in the bromine atom as well as fluorine atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I’ll tell you how you can easily find the valence electrons of bromine as well as fluorine using a periodic table.

Total valence electrons in BrF3 molecule

→ Valence electrons given by bromine atom:

Bromine is a group 17 element on the periodic table. ^[1] Hence the valence electrons present in bromine is 7.

You can see the 7 valence electrons present in the bromine atom as shown in the above image.

→ Valence electrons given by fluorine atom:

Fluorine is group 17 element on the periodic table. ^[2] Hence the valence electron present in fluorine is 7.

You can see the 7 valence electrons present in the fluorine atom as shown in the above image.

Hence, 

Total valence electrons in BrF3 molecule = valence electrons given by 1 bromine atom + valence electrons given by 3 fluorine atoms = 7 + 7(3) = 28.

Step 2: Select the central atom

For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.

Now here the given molecule is BrF3 (bromine trifluoride) and it contains bromine atom (Br) and fluorine atoms (F).

You can see the electronegativity values of bromine atom (Br) and fluorine atom (F) in the above periodic table.

If we compare the electronegativity values of bromine (Br) and fluorine (F) then the bromine atom is less electronegative.

So here the bromine atom (Br) is the center atom and the fluorine atoms (F) are the outside atoms.

Step 3: Connect each atoms by putting an electron pair between them

Now in the BrF3 molecule, you have to put the electron pairs between the bromine atom (Br) and fluorine atoms (F).

This indicates that the bromine (Br) and fluorine (F) are chemically bonded with each other in a BrF3 molecule.

Step 4: Make the outer atoms stable. Place the remaining valence electrons pair on the central atom.

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of BrF3 molecule, you can see that the outer atoms are fluorine atoms.

These outer fluorine atoms are forming an octet and hence they are stable.

Also, in step 1 we have calculated the total number of valence electrons present in the BrF3 molecule.

The BrF3 molecule has a total 28 valence electrons and out of these, only 24 valence electrons are used in the above sketch.

So the number of electrons which are left = 28 – 24 = 4.

You have to put these 4 electrons on the central bromine atom in the above sketch of BrF3 molecule.

Now let’s proceed to the next step.

Step 5: Check the stability of lewis structure

Now you have come to the final step in which you have to check the stability of lewis structure of BrF3.

The stability of lewis structure can be checked by using a concept of formal charge.

In short, now you have to find the formal charge on bromine (Br) atom as well as fluorine (F) atoms present in the BrF3 molecule.

For calculating the formal charge, you have to use the following formula;

Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons

You can see the number of bonding electrons and nonbonding electrons for each atom of BrF3 molecule in the image given below.

For Bromine (Br) atom:
Valence electrons = 7 (because bromine is in group 17)
Bonding electrons = 6
Nonbonding electrons = 4

For Fluorine (F) atom:
Valence electrons = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
Br	=	7	–	6/2	–	4	=	0
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the bromine (Br) atom as well as fluorine (F) atom has a “zero” formal charge.

This indicates that the above lewis structure of BrF3 is stable and there is no further change in the above structure of BrF3.

In the above lewis dot structure of BrF3, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of BrF3.

I hope you have completely understood all the above steps.

For more practice and better understanding, you can try other lewis structures listed below.

Try (or at least See) these lewis structures for better understanding:

IF5 lewis structure	HNO3 lewis structure
SCN- lewis structure	ClF3 lewis structure
Cl2 lewis structure	HF lewis structure