Lewis Dot Structure For Hbr

Then yous have seen the higher up image by now, right?

Let me explain the in a higher place image in short.

HBr (hydrogen bromide) lewis structure has ane Hydrogen atom (H) and one Bromine atom (Br) which contain a single bond between them. In that location are 3 lone pairs on the Bromine atom (Br).

If you haven't understood annihilation from the in a higher place image of HBr (hydrogen bromide) lewis structure, then merely stick with me and you lot volition become the detailed stride by step explanation on drawing a lewis structure of HBr.

Then let'southward move to the steps of drawing the lewis structure of HBr.

Steps of drawing HBr lewis structure

Pace 1: Find the full valence electrons in HBr molecule

In society to find the total valence electrons in HBr (hydrogen bromide) molecule, first of all you should know the valence electrons present in a single hydrogen cantlet likewise as bromine cantlet.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)

Here, I'll tell yous how yous can hands find the valence electrons of hydrogen as well as bromine using a periodic table.

Total valence electrons in HBr molecule

→ Valence electrons given by hydrogen cantlet:

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

You tin can see that only i valence electron is present in the hydrogen atom as shown in the above image.

→ Valence electrons given past bromine atom:

Bromine is a grouping 17 chemical element on the periodic tabular array. Hence the valence electrons nowadays in bromine is vii.

You can encounter the 7 valence electrons present in the bromine atom as shown in the above paradigm.

Hence,

Total valence electrons in HBr molecule = valence electrons given by 1 hydrogen atom + valence electrons given by 1 bromine atom = 1 + vii = 8.

Step 2: Select the central atom

For selecting the eye atom, you have to retrieve that the atom which is less electronegative remains at the center.

Now the given molecule is HBr (hydrogen bromide). It has only two atoms, so you lot can select whatever of the atoms equally a center cantlet.

Allow's assume the bromine cantlet equally a fundamental atom (Because we have to keep hydrogen outside in whatsoever lewis structure).

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

Now in the HBr molecule, you accept to put the electron pairs betwixt the hydrogen atom (H) and bromine atom (Br).

This indicates that the hydrogen (H) atom and bromine (Br) cantlet are chemically bonded with each other in a HBr molecule.

Pace 4: Make the outer atoms stable. Place the remaining valence electrons pair on the cardinal atom.

Now in this stride, yous have to check the stability of the outer atom.

Here in the sketch of HBr molecule, we have assumed the bromine atom as a center atom. Then the hydrogen is the outer atom.

Hence you have to make the hydrogen atom stable.

Yous can meet in the beneath image that the hydrogen atom is forming a duplet and hence it is stable.

As well, in footstep 1 nosotros take calculated the total number of valence electrons nowadays in the HBr molecule.

The HBr molecule has a total viii valence electrons and out of these, just 2 valence electrons are used in the in a higher place sketch.

So the number of electrons which are left = 8 – 2 = vi.

You have to put these vi electrons on the bromine atom in the above sketch of HBr molecule.

Now let'due south keep to the next step.

Step 5: Cheque the octet on the central atom

In this stride, y'all have to cheque whether the central bromine cantlet (Br) is stable or non.

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

Yous can see from the to a higher place 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'south proceed to the final pace to bank check whether the lewis construction of HBr is stable or not.

Step six: Cheque the stability of lewis structure

Now y'all have come up to the final step in which you accept to bank check the stability of lewis structure of HBr.

The stability of lewis construction can be checked by using a concept of formal charge.

In short, now yous take to find the formal charge on hydrogen (H) atom as well as bromine (Br) atoms nowadays in the HBr molecule.

For calculating the formal charge, y'all take to use the post-obit 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 HBr molecule in the epitome given below.

For Hydrogen (H) atom:
Valence electron = i (because hydrogen is in group one)
Bonding electrons = two
Nonbonding electrons = 0

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

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
H	=	one	–	2/two	–	0	=	0
Br	=	7	–	two/2	–	vi	=	0

From the to a higher place calculations of formal charge, you can see that the hydrogen (H) atom equally well as bromine (Br) atom has a "nothing" formal accuse.

This indicates that the higher up lewis structure of HBr is stable and in that location is no further modify in the above structure of HBr.

In the above lewis dot structure of HBr, y'all can also represent each bonding electron pair (:) as a single bond (|). By doing and then, you volition become the following lewis structure of HBr.

I hope you have completely understood all the to a higher place steps.

For more than practise and better understanding, you lot tin can try other lewis structures listed beneath.

Effort (or at least Come across) these lewis structures for better understanding: