BrF2- 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.

BrF2- lewis structure has an Bromine atom (Br) at the center which is surrounded by two Fluorine atoms (F). There is a single bond between the Bromine atom (Br) and each Fluorine atom (F). There is a -1 formal charge on the Bromine atom (Br).

If you haven’t understood anything from the above image of BrF2- lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of BrF2- ion.

So let’s move to the steps of drawing the lewis structure of BrF2- ion.

Steps of drawing BrF2- lewis structure

Step 1: Find the total valence electrons in BrF2- ion

In order to find the total valence electrons in BrF2- ion, 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 BrF2- ion

→ 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 BrF2- ion = valence electrons given by 1 bromine atom + valence electrons given by 2 fluorine atoms + 1 more electron is added due to 1 negative charge = 7 + 7(2) + 1 = 22.

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 ion is BrF2- ion 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 BrF2 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 BrF2 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 BrF2 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 BrF2- ion.

The BrF2- ion has a total 22 valence electrons and out of these, only 16 valence electrons are used in the above sketch.

So the number of electrons which are left = 22 – 16 = 6.

You have to put these 6 electrons on the central bromine atom in the above sketch of BrF2 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 BrF2.

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 the bromine atom (Br) as well as fluorine atoms (F) present in the BrF2 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 BrF2 molecule in the image given below.

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

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	–	4/2	–	6	=	-1
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the bromine (Br) atom has -1 charge and the fluorine atoms have 0 charges.

So let’s keep these charges on the respective atoms in the BrF2 molecule.

This overall -1 charge on the BrF2 molecule is represented in the image given below.

In the above lewis dot structure of BrF2- ion, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of BrF2- ion.

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:

P2 Lewis Structure	IBr2- Lewis Structure
PI3 Lewis Structure	NOBr Lewis Structure
ClF2- Lewis Structure	ClF4- Lewis Structure