HBrO Lewis structure

HBrO (hypobromous acid) has one hydrogen atom, one bromine atom, and one oxygen atom.

In HBrO Lewis structure, there are two single bonds around the oxygen atom, with one bromine atom and one hydrogen atom attached to it. The bromine atom has three lone pairs, and the oxygen atom has two lone pairs.

Alternative method: Lewis structure of HBrO

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, hydrogen lies in group 1, bromine lies in group 17, and oxygen lies in group 16.

Hence, hydrogen has one valence electron, bromine has seven valence electrons, and oxygen has six valence electrons.

Since HBrO has one hydrogen atom, one bromine atom, and one oxygen atom, so…

Valence electrons of one hydrogen atom = 1 × 1 = 1
Valence electrons of one bromine atom = 7 × 1 = 7
Valence electrons of one oxygen atom = 6 × 1 = 6

And the total valence electrons = 1 + 7 + 6 = 14

Learn how to find: Hydrogen valence electrons, Bromine valence electrons, and Oxygen valence electrons

• Second, find the total electron pairs

We have a total of 14 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 14 ÷ 2 = 7

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Now we have to choose the central atom from bromine and oxygen. Place the least electronegative atom at the center.

Since bromine is less electronegative than oxygen, the central atom should be bromine, right?

But if we place bromine in the center and hydrogen and oxygen outside, and calculate the formal charge, then we do not get the formal charges on atoms closer to zero.

And the structure with the formal charges on atoms closer to zero is the best Lewis structure.

Hence, here we have to assume that the central atom is oxygen.

Therefore, place oxygen in the center and hydrogen and bromine on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 7 electron pairs. And two bonds are already marked. So we have to only mark the remaining five electron pairs as lone pairs on the sketch.

Also remember that hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell. Bromine is a period 4 element, so it can keep more than 8 electrons in its last shell. And oxygen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are bromine and hydrogen. But no need to mark on hydrogen, because hydrogen already has two electrons.

So for bromine, there are three lone pairs, and for oxygen, there are two lone pairs.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

For hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For bromine atom, formal charge = 7 – 6 – ½ (2) = 0

For oxygen atom, formal charge = 6 – 4 – ½ (4) = 0

Here, the atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of HBrO features a central oxygen atom connected to one hydrogen atom and one bromine atom through single covalent bonds. In this configuration, the oxygen atom satisfies the octet rule by forming two single bonds and maintaining two lone pairs. Within this layout, the bromine atom also fulfills its octet by forming a single bond with oxygen and retaining three lone pairs. The hydrogen atom reaches its stable duet state by sharing its only electron with the oxygen atom. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for all atoms involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of hypobromous acid.

Next: IO₂^– Lewis structure

External links

• https://www.showme.com/sh/?h=QiVsB6W
• https://www.chegg.com/homework-help/questions-and-answers/determine-lewis-structure-following-acid-hbro-orient-molecule-left-end-worry-unbonded-elec-q86333143