ClF5 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.

ClF5 lewis structure has a Chlorine atom (Cl) at the center which is surrounded by five Fluorine atoms (F). There are 5 single bonds between the Chlorine atom (Cl) and each Fluorine atom (F). There are 3 lone pairs on all the Fluorine atoms (F) and 1 lone pair on the Chlorine atom (Cl).

If you haven’t understood anything from the above image of ClF5 (chlorine pentafluoride) lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of ClF5.

So let’s move to the steps of drawing the lewis structure of ClF5.

Steps of drawing ClF5 lewis structure

Step 1: Find the total valence electrons in ClF5 molecule

In order to find the total valence electrons in a ClF5 (chlorine pentafluoride) molecule, first of all you should know the valence electrons present in 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 ClF5 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 ClF5 molecule = valence electrons given by 1 chlorine atom + valence electrons given by 5 fluorine atoms = 7 + 7(5) = 42.

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 ClF5 (chlorine pentafluoride) and it contains chlorine atom (Cl) and fluorine atoms (F).

You can see the electronegativity values of chlorine atom (Cl) and fluorine atom (F) in the above periodic table.

If we compare the electronegativity values of chlorine (Cl) and fluorine (F) then the chlorine atom is less electronegative.

So here the chlorine atom (Cl) is the center atom and the fluorine atoms (F) are the outside atoms.

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

Now in the ClF5 molecule, you have to put the electron pairs between the chlorine atom (Cl) and fluorine atoms (F).

This indicates that the chlorine (Cl) and fluorine (F) are chemically bonded with each other in a ClF5 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 ClF5 molecule, you can see that the outer atoms are fluorine atoms.

These outer fluorine atoms are forming an octet and hence they are stable.

Also, in step 1 we have calculated the total number of valence electrons present in the ClF5 molecule.

The ClF5 molecule has a total 42 valence electrons and out of these, only 40 valence electrons are used in the above sketch.

So the number of electrons which are left = 42 – 40 = 2.

You have to put these 2 electrons on the central chlorine atom in the above sketch of ClF5 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 ClF5.

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 ClF5 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 ClF5 molecule in the image given below.

For Chlorine (Cl) atom:
Valence electrons = 7 (because chlorine is in group 17)
Bonding electrons = 10
Nonbonding electrons = 2

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	–	10/2	–	2	=	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) atoms have a “zero” formal charge.

This indicates that the above lewis structure of ClF5 is stable and there is no further change in the above structure of ClF5.

In the above lewis dot structure of ClF5, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of ClF5.

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:

IF4- lewis structure	PBr3 lewis structure
NO2- Lewis Structure	CO3 2- Lewis Structure
NF2- Lewis Structure	SO4 2- Lewis Structure