Lewis Structure of KrCl4 (With 5 Simple Steps to Draw!)

Lewis Structure of KrCl4

I’m super excited to teach you the lewis structure of KrCl4 in just 5 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of KrCl4 molecule.

So, if you are ready to go with these 5 simple steps, then let’s dive right into it!

Lewis structure of KrCl4 contains four single bonds between the Krypton (Kr) atom and each Chlorine (Cl) atom. The Krypton atom (Kr) is at the center and it is surrounded by 4 Chlorine atoms (Cl). The Krypton atom has 2 lone pairs and all the Chlorine atoms have 3 lone pairs.

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of KrCl4).

5 Steps to Draw the Lewis Structure of KrCl4

Step #1: Calculate the total number of valence electrons

Here, the given molecule is KrCl4. In order to draw the lewis structure of KrCl4, first of all you have to find the total number of valence electrons present in the KrCl4 molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in KrCl4

  • For Krypton: 

Krypton is a group 18 element on the periodic table.

Hence, the valence electron present in krypton is also 8 (see below image).

  • For Chlorine:

Chlorine is a group 17 element on the periodic table.

Hence, the valence electron present in chlorine is 7 (see below image).

Hence in a KrCl4 molecule, 

Valence electrons given by Krypton (Kr) atom = 8
Valence electrons given by each Chlorine (Cl) atom = 7
So, total number of Valence electrons in KrCl4 molecule = 8 + 7(4) = 36

Step #2: Select the center atom

While selecting the atom, always put the least electronegative atom at the center. 

Here in the KrCl4 molecule, if we compare the krypton atom (Kr) and chlorine atom (Cl), then the krypton is less electronegative than chlorine.

So, krypton should be placed in the center and the remaining 4 chlorine atoms will surround it.

step 1

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of KrCl4 molecule, put the two electrons (i.e electron pair) between each krypton atom and chlorine atom to represent a chemical bond between them.

step 2

These pairs of electrons present between the Krypton (Kr) and Chlorine (Cl) atoms form a chemical bond, which bonds the krypton and chlorine atoms with each other in a KrCl4 molecule.

Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom

Don’t worry, I’ll explain!

In the Lewis structure of KrCl4, the outer atoms are chlorine atoms.

So now, you have to complete the octet on these chlorine atoms (because chlorine requires 8 electrons to have a complete outer shell).

step 3

Now, you can see in the above image that all the chlorine atoms form an octet.

Also, only 34 valence electrons of KrCl4 molecule are used in the above structure.

But there are total 36 valence electrons in KrCl4 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 36 – 32 = 4.

So let’s keep these four electrons (i.e 2 electron pairs) on the central atom.

step 4

Now, let’s move to the next step.

Step #5: Final step – Check the stability of lewis structure by calculating the formal charge on each atom

Now, you have come to the final step and here you have to check the formal charge on krypton atom (Kr) as well as each chlorine atom (Cl).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

step 5
  • For Krypton :
    Valence electron = 8 (as it is in group 18)
    Nonbonding electrons = 4
    Bonding electrons = 8
  • For Chlorine:
    Valence electron = 7 (as it is in group 17)
    Nonbonding electrons = 6
    Bonding electrons = 2
Formal charge=Valence electronsNonbonding electrons(Bonding electrons)/2

So you can see above that the formal charges on krypton as well as chlorine are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of KrCl4 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of KrCl4 represents the single bond ( | ). So the above lewis dot structure of KrCl4 can also be represented as shown below.

krcl4 lewis structure

Related lewis structures for your practice:
Lewis Structure of PS3-
Lewis Structure of SOF2
Lewis Structure of SeBr4
Lewis Structure of BrCl2-
Lewis Structure of CF2S 

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Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online learning platform that provides students with easily understandable explanations.

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