CF3Cl Lewis structure

CF₃Cl (chlorotrifluoromethane) has one carbon atom, three fluorine atoms, and one chlorine atom.

In the CF₃Cl Lewis structure, there are four single bonds around the carbon atom, with three fluorine atoms and one chlorine atom attached to it, and on each fluorine and chlorine atom, there are three lone pairs.

Alternative method: Lewis structure of CF₃Cl

Rough sketch

• First, determine the total number of valence electrons

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

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

Since CF₃Cl has one carbon atom, three fluorine atoms, and one chlorine atom, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of three fluorine atoms = 7 × 3 = 21
Valence electrons of one chlorine atoms = 7 × 1 = 7

And the total valence electrons = 4 + 21 + 7 = 32

Learn how to find: Carbon valence electrons, Fluorine valence electrons, and Chlorine 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 fluorine and chlorine, assume that the central atom is carbon.

Therefore, place carbon in the center and fluorine and chlorine 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 fluorines and chlorines.

So for each fluorine and chlorine, 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 fluorine atom, formal charge = 7 – 6 – ½ (2) = 0

For each chlorine 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 CF₃Cl features a central carbon atom linked to three fluorine atoms and one chlorine atom through single covalent bonds. In this configuration, the carbon atom satisfies the octet rule by forming four total bonds, while each of the three fluorine atoms fulfills its octet by retaining three lone pairs alongside its single shared bond. Within this layout, the chlorine atom also reaches a stable octet by maintaining three lone pairs. This arrangement represents the most stable state for the molecule because it results in a formal charge of zero for every atom involved. Therefore, this specific electronic distribution serves as the definitive and most accurate Lewis representation of chlorotrifluoromethane.

Next: C₆H₁₂ Lewis structure

External video

• How to Draw the Lewis Structure for CF3Cl – YouTube • Wayne Breslyn