CCl2F2 Lewis structure

CCl₂F₂ (dichlorodifluoromethane) has one carbon atom, two chlorine atoms, and two fluorine atoms.

In the CCl₂F₂ Lewis structure, there are four single bonds around the carbon atom, with two chlorine atoms and two fluorine atoms attached to it, and on each chlorine and fluorine atom, there are three lone pairs.

Alternative method: Lewis structure of CCl₂F₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, and both chlorine and fluorine lie in group 17.

Hence, carbon has four valence electrons, both chlorine and fluorine have seven valence electrons.

Since CCl₂F₂ has one carbon atom, two chlorine atoms, and two fluorine atoms, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of two chlorine atoms = 7 × 2 = 14
Valence electrons of two fluorine atoms = 7 × 2 = 14

And the total valence electrons = 4 + 14 + 14 = 32

Learn how to find: Carbon valence electrons, Chlorine valence electrons, and Fluorine valence electrons

• Second, find the total electron pairs

We have a total of 32 valence electrons. And when we divide this value by two, we get the value of total electron pairs.

Total electron pairs = total valence electrons ÷ 2

So the total electron pairs = 32 ÷ 2 = 16

• Third, determine the central atom

We have to place the least electronegative atom at the center.

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

Therefore, place carbon in the center and chlorine and fluorine on either side.

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 16 electron pairs. And four bonds are already marked. So we have to only mark the remaining twelve electron pairs as lone pairs on the sketch.

Also remember 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.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are chlorines and fluorines.

So for each chlorine and fluorine, there are three lone pairs, and for carbon, there is zero lone pair because all twelve electron pairs are over.

Mark the lone pairs on the sketch as follows:

Formal charge

Use the following formula to calculate the formal charges on atoms:

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

For carbon atom, formal charge = 4 – 0 – ½ (8) = 0

For each chlorine atom, formal charge = 7 – 6 – ½ (2) = 0

For each fluorine atom, formal charge = 7 – 6 – ½ (2) = 0

Here, the atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of CCl₂F₂ features a central carbon atom linked to two chlorine atoms and two fluorine atoms through single covalent bonds. In this arrangement, the carbon atom satisfies the octet rule by forming four total bonds, while each of the four halogen atoms also fulfills its octet by retaining three lone pairs alongside its single shared bond. Within this layout, every atom achieves a complete valence shell without the need for multiple bonds or expanded octets. This configuration represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of dichlorodifluoromethane (also known as Freon-12).

Next: P₄ Lewis structure

External video

• CCl2F2 Lewis Structure: How to Draw the Lewis Structure for CCl2F2 – YouTube • Wayne Breslyn

External links

• https://lambdageeks.com/ccl2f2-lewis-structure/
• https://topblogtenz.com/cf2cl2-lewis-structure-molecular-geometry-and-polar-or-nonpolar/
• https://www.chemistryscl.com/general/dichlorodifluoromethane-CCl2F2-lewis-structure/index.php
• https://oneclass.com/homework-help/chemistry/7028769-ccl2f2-lewis-structure.en.html