Lewis Structure of C2Cl4 (With 6 Simple Steps to Draw!)

Lewis Structure of C2Cl4

Ready to learn how to draw the lewis structure of C2Cl4?


Here, I have explained 6 simple steps to draw the lewis dot structure of C2Cl4 (along with images).

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of C2Cl4 contains one double bond between the two Carbon (C) atoms and a single bond between Carbon (C) & Chlorine (Cl) atoms. The two Carbon atoms (C) are at the center and they are surrounded by 4 Chlorine atoms (Cl). All the four 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 C2Cl4).

6 Steps to Draw the Lewis Structure of C2Cl4

Step #1: Calculate the total number of valence electrons

Here, the given molecule is C2Cl4. In order to draw the lewis structure of C2Cl4, first of all you have to find the total number of valence electrons present in the C2Cl4 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 C2Cl4

  • For Carbon:

Carbon is a group 14 element on the periodic table. [1]

Hence, the valence electrons present in carbon is 4 (see below image).

  • For Chlorine:

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

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

Hence in a C2Cl4 molecule, 

Valence electrons given by each Carbon (C) atom = 4
Valence electron given by each Chlorine (Cl) atom = 7
So, total number of Valence electrons in C2Cl4 molecule = 4(2) + 7(4) = 36

Step #2: Select the center atom

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

(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table). [3]

Here in the C2Cl4 molecule, if we compare the carbon atom (C) and chlorine atom (Cl), then carbon is less electronegative than chlorine.

So, both the carbon atoms 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 C2Cl4 molecule, put the two electrons (i.e electron pair) between the carbon-carbon atoms and carbon-chlorine atoms to represent a chemical bond between them.

step 2

These pairs of electrons present between the Carbon atoms as well as between the Carbon and Chlorine atoms form a chemical bond, which bonds these atoms with each other in a C2Cl4 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 C2Cl4, 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 C2Cl4 molecule are used in the above structure.

But there are total 36 valence electrons in C2Cl4 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 36 – 34 = 2.

So let’s keep these two electrons (i.e 1 electron pair) on the central atom.

step 4

Now, let’s move to the next step.

Step #5: Check whether the central atom has octet or not. If it does not have an octet, then convert the lone pair into double bond or triple bond

In this step, we have to check whether the central atoms (i.e two carbon atoms) have an octet or not. 

In simple words, we have to check whether the central Carbon (C) atoms has 8 electrons or not.

step 5

As you can see from the above image, one carbon atom has 8 electrons, while the other carbon atom has only 6 electrons. So this carbon atom does not fulfill the octet rule.

Now, in order to fulfill the octet of this carbon atom, we have to convert the lone pair into a double bond.

step 6

Now you can see from the above image that both the central carbon atoms are having 8 electrons. So they fulfill the octet rule and both the carbon atoms are stable.

Step #6: 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 carbon atoms (C) as well as chlorine atoms (Cl).

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

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

step 7
  • For Carbon:
    Valence electrons = 4 (as it is in group 14)
    Nonbonding electrons = 0
    Bonding electrons = 8
  • For Chlorine:
    Valence electrons = 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 carbon as well as chlorine are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of C2Cl4 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of C2Cl4 represents the single bond ( | ). So the above lewis dot structure of C2Cl4 can also be represented as shown below.

c2cl4 lewis structure

Related lewis structures for your practice:
Lewis Structure of CF3Cl
Lewis Structure of PF3Cl2
Lewis Structure of C2H4Cl2
Lewis Structure of HClO4
Lewis Structure of SeS2 

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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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