ClF Lewis Structure in 5 Steps (With Images)

So you have seen the above image by now, right?

Let me explain the above image in short.

ClF lewis structure has one Chlorine atom (Cl) and one Fluorine atom (F) which contain a single bond between them. There are 3 lone pairs on both the Chlorine atom (Cl) as well as Fluorine atom (F).

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

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

Steps of drawing ClF lewis structure

Step 1: Find the total valence electrons in ClF molecule

In order to find the total valence electrons in a ClF molecule, first of all you should know the valence electrons present in the chlorine atom as well as fluorine 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 chlorine as well as fluorine using a periodic table.

Total valence electrons in ClF molecule

→ Valence electrons given by chlorine atom:

Chlorine is group 17 element on the periodic table. ^[1] Hence the valence electrons present in chlorine is 7.

You can see the 7 valence electrons present in the chlorine atom as shown in the above image.

→ Valence electrons given by fluorine atom:

Fluorine is group 17 element on the periodic table. ^[2] Hence the valence electron present in fluorine is 7.

You can see the 7 valence electrons present in the fluorine atom as shown in the above image.

Hence, 

Total valence electrons in ClF molecule = valence electrons given by 1 chlorine atom + valence electrons given by 1 fluorine atom = 7 + 7 = 14.

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.

Now here the given molecule is ClF. It has only two atoms, so you can select any of the atoms as a center atom.

Let’s assume the chlorine atom as a central atom.
(You should assume the less electronegative atom as a center atom).

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

Now in the ClF molecule, you have to put the electron pairs between the chlorine atom (Cl) and fluorine atom (F).

This indicates that the chlorine (Cl) and fluorine (F) are chemically bonded with each other in a ClF 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 atom.

Here in the sketch of ClF molecule, we have assumed the chlorine atom as a center atom. So the fluorine is the outer atom.

Hence you have to make the fluorine atom stable.

You can see in the below image that the fluorine atom is forming an octet and hence it is stable.

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

The ClF molecule has a total 14 valence electrons and out of these, only 8 valence electrons are used in the above sketch.

So the number of electrons which are left = 14 – 8 = 6.

You have to put these 6 electrons on the chlorine atom in the above sketch of ClF molecule.

Now let’s proceed to the next step.

Step 5: 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 ClF.

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 chlorine (Cl) atom as well as fluorine (F) atoms present in the ClF 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 ClF molecule in the image given below.

For Chlorine (Cl) atom:
Valence electrons = 7 (because chlorine is in group 17)
Bonding electrons = 6
Nonbonding electrons = 4

For Fluorine (F) atom:
Valence electrons = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
Cl	=	7	–	6/2	–	4	=	0
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the chlorine (Cl) atom as well as fluorine (F) atom has a “zero” formal charge.

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

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

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:

SO Lewis Structure	XeCl2 Lewis Structure
SeF2 Lewis Structure	C2F2 Lewis Structure
XeCl4 Lewis Structure	AlBr3 Lewis Structure