Lewis structure of CCl2F2

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The Lewis structure of CCl₂F₂ contains four single bonds, with carbon in the center, and two chlorines and two fluorines on either side. There are three lone pairs on each chlorine atom and each fluorine atom, and the carbon atom does not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of CCl₂F₂.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

• Let’s calculate the total number of valence electrons

We know that… carbon is a group 14 element, and both chlorine and fluorine are the group 17 elements. Hence, carbon has four valence electrons, and both chlorine and fluorine have seven valence electrons.

Now CCl₂F₂ has one carbon atom, two chlorine atoms, and two fluorine atoms.

So the total number of valence electrons = valence electrons of carbon atom + (valence electrons of chlorine atom × 2) + (valence electrons of fluorine atom × 2)

Therefore, the total number of valence electrons = 4 + 14 + 14 = 32

• Now decide the central atom

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for carbon, chlorine, and fluorine as follows:

Electronegativity value of carbon = 2.55
Electronegativity value of chlorine = 3.16
Electronegativity value of fluorine = 3.98

Obviously, carbon is less electronegative than chlorine and fluorine. Hence, assume that carbon is the central atom.

So now, put carbon in the center and chlorines and fluorines on either side. And draw the rough skeleton structure for the Lewis structure of CCl₂F₂ something like this:

Also read: How to draw Lewis structure of HSO₄^– (5 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since carbon is surrounded by two chlorines and two fluorines, use eight electrons to show four chemical bonds as follows:

Also read: How to draw Lewis structure of C₂H₂Cl₂ (5 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 32 valence electrons. And in the above structure, we have already used eight valence electrons. Hence, twenty-four valence electrons are remaining.

Two valence electrons represent one lone pair. So twenty-four valence electrons = twelve lone pairs.

Note that both (carbon and fluorine) are the period 2 elements, so they can not keep more than 8 electrons in their last shell. And chlorine is a period 3 element, so it can keep more than 8 electrons in its last shell.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are chlorines and fluorines, so each chlorine and each fluorine will get three lone pairs. And the central atom (carbon) will not get any lone pair, because all twelve lone pairs are used.

So the Lewis structure of CCl₂F₂ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (carbon), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of C₂^2- (5 steps)

#4 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

• For carbon atom

Valence electrons = 4
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 4 – 0 – ½ (8) = 0

• For each chlorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

• For each fluorine atom

Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 7 – 6 – ½ (2) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of CCl₂F₂ looks something like this:

In the above structure, you can see that the formal charges of all atoms are zero. Therefore, this is the stable Lewis structure of CCl₂F₂.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

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Related

• Lewis structure of HSO₄^–
• Lewis structure of C₂H₂Cl₂
• Lewis structure of C₂^2-
• Lewis structure of SeO₃^2-
• Lewis structure of P₄

External links

• CCl2F2 Lewis Structure in 6 Steps (With Images) – Pediabay
• Draw the Lewis structure for CCl2F2 (carbon is the central atom) – Homework.Study.com
• How do you find the Lewis structure for CCl2F2? – Quora
• Dichlorodifluoromethane (CCl2F2) Lewis Structure and Steps of Drawing – Chemistry School
• CF2Cl2 Lewis structure, Molecular geometry, and Polar or nonpolar – Topblogtenz
• Draw a Lewis structure for CCl2F2, one of the compounds responsible for the depletion of stratospheric ozone – Numerade
• CCl2F2 (Dichlorodifluoromethane) Oxidation Number – ChemicalAid
• What is the Lewis structure for dichlorodifluoromethane, CCl2F2? – OneClass
• Draw a Lewis structure for CCl2F2 – Bartleby
• What is the molecular geometry for CCl2F2? – Quizlet