CCl2 Lewis structure

CCl₂ (dichlorocarbene) has one carbon atom and two chlorine atoms.

In CCl₂ Lewis structure, there are two single bonds around the carbon atom, with two chlorine atoms attached to it. Each chlorine atom has three lone pairs, and the carbon atom has one lone pair.

Alternative method: Lewis structure of CCl₂

Rough sketch

• First, determine the total number of valence electrons

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

Hence, carbon has four valence electrons and chlorine has seven valence electrons.

Since CCl₂ has one carbon atom and two chlorine atoms, so…

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

And the total valence electrons = 4 + 14 = 18

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

• Second, find the total electron pairs

We have a total of 18 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 = 18 ÷ 2 = 9

• Third, determine the central atom

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

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

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 9 electron pairs. And two C — Cl bonds are already marked. So we have to only mark the remaining seven electron pairs as lone pairs on the sketch.

Also remember that carbon is a period 2 element, so it can not keep more than 8 electrons in its 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.

So for each chlorine, there are three lone pairs, and for carbon, there is one lone pair.

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 – 2 – ½ (4) = 0

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

Here, both carbon and chlorine atoms do not have charges, so no need to mark the charges.

Final structure

The final structure of CCl₂ contains a central carbon atom linked to two chlorine atoms through single covalent bonds. In this layout, the carbon atom does not complete a full octet but instead maintains six valence electrons, which comprise two bonding pairs and one lone pair. Within this arrangement, each chlorine atom successfully satisfies the octet rule by retaining three lone pairs alongside its single shared bond. This configuration represents the most stable state for the neutral 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 dichlorocarbene.

Next: SF₅Cl Lewis structure

External video

• How to Draw the Lewis Dot Structure for CCl2: Dichlorocarbene – YouTube • Wayne Breslyn

External links

• https://homework.study.com/explanation/draw-and-explain-the-lewis-structure-for-ccl2.html