BrCl2- 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.

BrCl2- lewis structure has an Bromine atom (Br) at the center which is surrounded by two Chlorine atoms (Cl). There is a single bond between the Bromine atom (Br) and each Chlorine atom (Cl). There is a -1 formal charge on the Bromine atom (Br).

If you haven’t understood anything from the above image of BrCl2- lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of BrCl2- ion.

So let’s move to the steps of drawing the lewis structure of BrCl2- ion.

Steps of drawing BrCl2- lewis structure

Step 1: Find the total valence electrons in BrCl2- ion

In order to find the total valence electrons in BrCl2- ion, first of all you should know the valence electrons present in the bromine atom as well as chlorine 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 chlorine using a periodic table.

Total valence electrons in BrCl2- 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 chlorine atom:

Chlorine is group 17 element on the periodic table. ^[2] Hence the valence electrons present in chlorine is 7.

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

Hence, 

Total valence electrons in BrCl2- ion = valence electrons given by 1 bromine atom + valence electrons given by 2 chlorine 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 BrCl2- ion and it contains bromine atom (Br) and chlorine atoms (Cl).

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

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

So here the bromine atom (Br) is the center atom and the chlorine atoms (Cl) are the outside atoms.

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

Now in the BrCl2 molecule, you have to put the electron pairs between the bromine atom (Br) and chlorine atoms (Cl).

This indicates that the bromine (Br) and chlorine (Cl) are chemically bonded with each other in a BrCl2 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 BrCl2 molecule, you can see that the outer atoms are chlorine atoms.

These outer chlorine 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 BrCl2- ion.

The BrCl2- 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 BrCl2 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 BrCl2.

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 chlorine atoms (Cl) present in the BrCl2 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 BrCl2 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 Chlorine (Cl) atom:
Valence electrons = 7 (because chlorine 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
Cl	=	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 chlorine atoms have 0 charges.

So let’s keep these charges on the respective atoms in the BrCl2 molecule.

This overall -1 charge on the BrCl2 molecule is represented in the image given below.

In the above lewis dot structure of BrCl2- ion, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of BrCl2- 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:

CF2S Lewis Structure	PI5 Lewis Structure
SO2F2 Lewis Structure	OPBr3 Lewis Structure
PH2- Lewis Structure	NS2 Lewis Structure