AsBr3 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.

AsBr3 lewis structure has an Arsenic atom (As) at the center which is surrounded by three Bromine atoms (Br). There are 3 single bonds between the Arsenic atom (As) and each Bromine atom (Br). There is 1 lone pair on the Arsenic atom (As) and 3 lone pairs on all three Bromine atoms (Br).

If you haven’t understood anything from the above image of AsBr3 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of AsBr3.

So let’s move to the steps of drawing the lewis structure of AsBr3.

Steps of drawing AsBr3 lewis structure

Step 1: Find the total valence electrons in AsBr3 molecule

In order to find the total valence electrons in AsBr3 molecule, first of all you should know the valence electrons present in arsenic atom as well as bromine 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 arsenic as well as bromine using a periodic table.

Total valence electrons in AsBr3 molecule

→ Valence electrons given by arsenic atom:

Arsenic is a group 15 element on the periodic table. ^[1] Hence the valence electrons present in arsenic is 5.

You can see the 5 valence electrons present in the arsenic atom as shown in the above image.

→ Valence electrons given by bromine atom:

Bromine is a group 17 element on the periodic table. ^[2] 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.

Hence, 

Total valence electrons in AsBr3 molecule = valence electrons given by 1 arsenic atom + valence electrons given by 3 bromine atoms = 5 + 7(3) = 26.

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 AsBr3 and it contains arsenic atom (As) and bromine atoms (Br).

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

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

So here the arsenic atom (As) is the center atom and the bromine atoms (Br) are the outside atoms.

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

Now in the AsBr3 molecule, you have to put the electron pairs between the arsenic atom (As) and bromine atoms (Br).

This indicates that the arsenic (As) and bromine (Br) are chemically bonded with each other in a AsBr3 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 AsBr3 molecule, you can see that the outer atoms are bromine atoms.

These outer bromine 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 AsBr3 molecule.

The AsBr3 molecule has a total 26 valence electrons and out of these, only 24 valence electrons are used in the above sketch.

So the number of electrons which are left = 26 – 24 = 2.

You have to put these 2 electrons on the central arsenic atom in the above sketch of AsBr3 molecule.

Now let’s proceed to the next step.

Step 5: Check the octet on the central atom

In this step, you have to check whether the central arsenic atom (As) is stable or not.

In order to check the stability of the central arsenic (As) atom, we have to check whether it is forming an octet or not.

You can see from the above picture that the arsenic atom is forming an octet. That means it has 8 electrons.

And hence the central arsenic atom is stable.

Now let’s proceed to the final step to check whether the lewis structure of AsBr3 is stable or not.

Step 6: 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 AsBr3.

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 arsenic (As) atom as well as bromine (Br) atoms present in the AsBr3 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 AsBr3 molecule in the image given below.

For Arsenic (As) atom:
Valence electrons = 5 (because arsenic is in group 15)
Bonding electrons = 6
Nonbonding electrons = 2

For Bromine (Br) atom:
Valence electrons = 7 (because bromine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
As	=	5	–	6/2	–	2	=	0
Br	=	7	–	2/2	–	6	=	0

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

This indicates that the above lewis structure of AsBr3 is stable and there is no further change in the above structure of AsBr3.

In the above lewis dot structure of AsBr3, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of AsBr3.

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:

TeO3 Lewis Structure	TeO2 Lewis Structure
SbH3 Lewis Structure	KrCl4 Lewis Structure
PS3- Lewis Structure	SOF2 Lewis Structure