BrCl Lewis structure

BrCl (bromine monochloride) has one bromine atom and one chlorine atom.

In the BrCl Lewis structure, there is a single bond between the bromine and chlorine atom, and on both bromine and chlorine atoms, there are three lone pairs.

Contents

Steps

To properly draw the BrCl Lewis structure, follow these steps:

#1 Draw a rough sketch of the structure
#2 Next, indicate lone pairs on the atoms
#3 Indicate formal charges on the atoms, if necessary

Let’s break down each step in more detail.

#1 Draw a rough sketch of the structure

• First, determine the total number of valence electrons

In the periodic table, both bromine and chlorine lie in group 17.

Hence, both bromine and chlorine have seven valence electrons.

Since BrCl has one bromine atom and one chlorine atom, so…

Valence electrons of one bromine atom = 7 × 1 = 7
Valence electrons of one chlorine atom = 7 × 1 = 7

And the total valence electrons = 7 + 7 = 14

• 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

We have to place the least electronegative atom at the center.

Since bromine is less electronegative than chlorine, assume that the central atom is bromine.

• And finally, draw the rough sketch

#2 Next, indicate lone pairs on the atoms

Here, we have a total of 7 electron pairs. And one Br — Cl bond is already marked. So we have to only mark the remaining six electron pairs as lone pairs on the sketch.

Also remember that bromine is a period 4 element, so it can keep more than 8 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atom is chlorine.

So for each atom, there are three lone pairs.

Mark the lone pairs on the sketch as follows:

#3 Indicate formal charges on the atoms, if necessary

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

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

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

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

Here, both bromine and chlorine atoms do not have charges, so no need to mark the charges.

In the above structure, you can see that the central atom (bromine) forms an octet. And the outside atom (chlorine) also forms an octet. Hence, the octet rule is satisfied.

Therefore, this structure is the stable Lewis structure of BrCl.

Next: BeI2 Lewis structure