HBrO4 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.

HBrO4 lewis structure has a Bromine atom (Br) at the center which is surrounded by three Oxygen atoms (O) and one O-H group. There are 3 double bonds between the Bromine atom (Br) & Oxygen atom (O) and the rest other atoms have a single bond.

If you haven’t understood anything from the above image of HBrO4 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of HBrO4.

So let’s move to the steps of drawing the lewis structure of HBrO4.

Steps of drawing HBrO4 lewis structure

Step 1: Find the total valence electrons in HBrO4 molecule

In order to find the total valence electrons in a HBrO4 molecule, first of all you should know the valence electrons present in hydrogen atom, bromine atom as well as oxygen 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 hydrogen, bromine as well as oxygen using a periodic table.

Total valence electrons in HBrO4 molecule

→ Valence electrons given by hydrogen atom:

Hydrogen is group 1 element on the periodic table. ^[1] Hence the valence electron present in hydrogen is 1.

You can see that only 1 valence electron is present in the hydrogen 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.

→ Valence electrons given by oxygen atom:

Oxygen is group 16 element on the periodic table. ^[3] Hence the valence electrons present in oxygen is 6.

You can see the 6 valence electrons present in the oxygen atom as shown in the above image.

Hence, 

Total valence electrons in HBrO4 molecule = valence electrons given by 1 hydrogen atom + valence electrons given by 1 bromine atom + valence electrons given by 4 oxygen atoms = 1 + 7 + 6(4) = 32.

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.

(Remember: If hydrogen is present in the given molecule, then always put hydrogen outside.)

Now here the given molecule is HBrO4 and it contains hydrogen atom (H), bromine atom (Br) and oxygen atoms (O).

So as per the rule we have to keep hydrogen outside.

Now, you can see the electronegativity values of bromine atom (Br) and oxygen atom (O) in the above periodic table.

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

So here the bromine atom (Br) is the center atom and the oxygen atoms (O) are the outside atom.

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

Now in the HBrO4 molecule, you have to put the electron pairs between the oxygen (O) & hydrogen (H) atom and between the oxygen (O) & bromine (Br) atoms.

This indicates that these atoms are chemically bonded with each other in a HBrO4 molecule.

Step 4: Make the outer atoms stable

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

Here in the sketch of HBrO4 molecule, you can see that the outer atoms are hydrogen and oxygen atoms.

These hydrogen and oxygen atoms are forming a duplet and octet respectively and hence they are stable.

Also, in step 1 we have calculated the total number of valence electrons present in the HBrO4 molecule.

The HBrO4 molecule has a total 32 valence electrons and all these valence electrons are used in the above sketch of HBrO4.

Hence there are no remaining electron pairs to be kept on the central atom.

So 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 bromine atom (Br) is stable or not.

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

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

And hence the central bromine atom is stable.

Now let’s proceed to the final step to check whether the lewis structure of HBrO4 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 HBrO4.

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 hydrogen (H) atom, bromine (Br) atom as well as oxygen (O) atoms present in the HBrO4 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 HBrO4 molecule in the image given below.

For Hydrogen (H) atom:
Valence electron = 1 (because hydrogen is in group 1)
Bonding electrons = 2
Nonbonding electrons = 0

For Bromine (Br) atom:
Valence electrons = 7 (because bromine is in group 17)
Bonding electrons = 8
Nonbonding electrons = 0

For Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 2
Nonbonding electrons = 6

For Oxygen (O) atom (of O-H group):
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
H	=	1	–	2/2	–	0	=	0
Br	=	7	–	8/2	–	0	=	+3
O	=	6	–	2/2	–	6	=	-1
O (of OH group)	=	6	–	4/2	–	4	=	0

From the above calculations of formal charge, you can see that the bromine (Br) atom has +3 charge and the three oxygen (O) atoms have -1 charges.

Because of this reason, the above obtained lewis structure of HBrO4 is not stable.

So we have to minimize these charges by shifting the electron pairs towards the bromine atom.

After shifting the electron pairs from oxygen atoms to bromine atom, the lewis structure of HBrO4 becomes more stable.

In the above lewis dot structure of HBrO4, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of HBrO4.

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:

TeF5- Lewis Structure	SeCl6 Lewis Structure
SeBr2 Lewis Structure	HCP Lewis Structure
TeF6 Lewis Structure	SeF5- Lewis Structure