ClF4- 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.

ClF4- lewis structure has an Chlorine atom (Cl) at the center which is surrounded by four Fluorine atoms (F). There are 4 single bonds between the Chlorine atom (Cl) and each Fluorine atom (F). There are 2 lone pairs on the Chlorine atom (Cl) and 3 lone pairs on all the four Fluorine atoms (F).

If you haven’t understood anything from the above image of ClF4- lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of ClF4- ion.

So let’s move to the steps of drawing the lewis structure of ClF4- ion.

Steps of drawing ClF4- lewis structure

Step 1: Find the total valence electrons in ClF4- ion

In order to find the total valence electrons in ClF4- ion, 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 ClF4- ion

→ 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 ClF4- ion = valence electrons given by 1 chlorine atom + valence electrons given by 1 fluorine atom + 1 more electron is added due to 1 negative charge = 7 + 7(4) + 1 = 36.

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 ion is ClF4- ion 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 ClF4 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 ClF4 molecule.

Step 4: Make the outer atoms stable

Now in this step, you have to check the stability of the outer atoms.

Here in the sketch of ClF4 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 ClF4- ion.

The ClF4- ion has a total 36 valence electrons and out of these, only 32 valence electrons are used in the above sketch.

So the number of electrons which are left = 36 – 32 = 4.

You have to put these 4 electrons on the central chlorine atom in the above sketch of ClF4 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 ClF4.

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 ClF4 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 ClF4 molecule in the image given below.

For Chlorine (Cl) atom:
Valence electron = 7 (because chlorine is in group 17)
Bonding electrons = 8
Nonbonding electrons = 4

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

Formal charge	=	Valence electrons	–	(Bonding electrons)/2	–	Nonbonding electrons
Cl	=	7	–	8/2	–	4	=	-1
F	=	7	–	2/2	–	6	=	0

From the above calculations of formal charge, you can see that the chlorine (Cl) atom has -1 charge, while the fluorine atom has 0 charge.

So let’s keep these charges on the respective atoms in the ClF4 molecule.

This overall -1 charge on the ClF4 molecule is represented in the image given below.

In the above lewis dot structure of ClF4- ion, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of ClF4- ion.

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:

CIF3 Lewis Structure	ClCN Lewis Structure
CH2S Lewis Structure	BrF4- Lewis Structure
AsF6- Lewis Structure	SCl6 Lewis Structure