HBrO 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.

HBrO (or HOBr) lewis structure has an Oxygen atom (O) at the center which is surrounded by one Hydrogen atom (H) and one Bromine atom (Br). There is a single bond between the Hydrogen (H) & Oxygen (O) atom as well as between the Oxygen (O) & Bromine (Br) atom.

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

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

Steps of drawing HBrO lewis structure

Step 1: Find the total valence electrons in HBrO molecule

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

Total valence electrons in HBrO 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 HBrO molecule = valence electrons given by 1 hydrogen atom + valence electrons given by 1 oxygen atom + valence electrons given by 1 bromine atom = 1 + 6 + 7 = 14.

Step 2: Prepare the rough sketch

To draw the rough sketch of HOBr (or HBrO) molecule, just look at its chemical formula only. You can see that there is an oxygen atom (O) at the center and it is surrounded by hydrogen atom (H) and bromine atom (Br) on either side.

So let’s draw a rough sketch for the same.

(Note: Here we have kept the oxygen atom at the center and not bromine. If you keep the bromine atom at the center, then the final lewis structure will not be stable. Hence the oxygen is kept at the center.)

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

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

This indicates that these atoms are chemically bonded with each other in a HBrO 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 HBrO molecule, you can see that the outer atoms are hydrogen atom and bromine atom.

These hydrogen and bromine 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 HBrO molecule.

The HBrO molecule has a total 14 valence electrons and out of these, only 10 valence electrons are used in the above sketch.

So the number of electrons which are left = 14 – 10 = 4.

You have to put these 4 electrons on the central oxygen atom in the above sketch of HBrO 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 oxygen atom (O) is stable or not.

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

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

And hence the central oxygen atom is stable.

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

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, oxygen (O) atom as well as bromine (Br) atom present in the HBrO 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 HBrO 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 Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4

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

From the above calculations of formal charge, you can see that the hydrogen (H) atom, oxygen (O) atom as well as bromine (Br) atom have a “zero” formal charge.

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

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

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:

About author

Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.

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