KrCl4 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.

KrCl4 lewis structure has Krypton atom (Kr) at the center which is surrounded by four Chlorine atoms (Cl). There are 4 single bonds between the Krypton atom (Kr) and each Chlorine atom (Cl). There are 2 lone pairs on the Krypton atom (Kr) and 3 lone pairs on all the four Chlorine atoms (Cl).

If you haven’t understood anything from the above image of KrCl4 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of KrCl4.

So let’s move to the steps of drawing the lewis structure of KrCl4.

Steps of drawing KrCl4 lewis structure

Step 1: Find the total valence electrons in KrCl4 molecule

In order to find the total valence electrons in a KrCl4 molecule, first of all you should know the valence electrons present in krypton atom as well as chlorine 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 krypton as well as chlorine using a periodic table.

Total valence electrons in KrCl4 molecule

→ Valence electrons given by krypton atom:

Krypton is a group 18 element on the periodic table. ^[1] Hence the valence electrons present in krypton is 8.

You can see the 8 valence electrons present in the krypton atom as shown in the above image.

→ Valence electrons given by chlorine atom:

Chlorine is group 17 element on the periodic table. ^[2] 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.

Hence, 

Total valence electrons in KrCl4 molecule = valence electrons given by 1 krypton atom + valence electrons given by 4 chlorine atoms = 8 + 7(4) = 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 molecule is KrCl4 and it contains krypton atom (Kr) and chlorine atoms (Cl).

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

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

So here the krypton atom (Kr) is the center atom and the chlorine atoms (Cl) are the outside atoms.

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

Now in the KrCl4 molecule, you have to put the electron pairs between the krypton atom (Kr) and chlorine atoms (Cl).

This indicates that the krypton (Kr) and chlorine (Cl) are chemically bonded with each other in a KrCl4 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 KrCl4 molecule, you can see that the outer atoms are chlorine atoms.

These outer chlorine 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 KrCl4 molecule.

The KrCl4 molecule 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 krypton atom in the above sketch of KrCl4 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 KrCl4.

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 krypton (Kr) atom as well as chlorine (Cl) atoms present in the KrCl4 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 KrCl4 molecule in the image given below.

For Krypton (Kr) atom:
Valence electrons = 8 (because krypton is in group 18)
Bonding electrons = 8
Nonbonding electrons = 4

For Chlorine (Cl) atom:
Valence electron = 7 (because chlorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6

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

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

This indicates that the above lewis structure of KrCl4 is stable and there is no further change in the above structure of KrCl4.

In the above lewis dot structure of KrCl4, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of KrCl4.

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:

PS3- Lewis Structure	SOF2 Lewis Structure
SeBr4 Lewis Structure	BrCl2- Lewis Structure
CF2S Lewis Structure	PI5 Lewis Structure