CH2 Lewis structure

CH₂ (methylene) has one carbon atom and two hydrogen atoms.

In the CH₂ Lewis structure, there are two single bonds around the carbon atom, with two hydrogen atoms attached to it, and on the carbon atom, there is one lone pair.

Alternative method: Lewis structure of CH₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, and hydrogen lies in group 1.

Hence, carbon has four valence electrons and hydrogen has one valence electron.

Since CH₂ has one carbon atom and two hydrogen atoms, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of two hydrogen atoms = 1 × 2 = 2

And the total valence electrons = 4 + 2 = 6

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

• Second, find the total electron pairs

We have a total of 6 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 = 6 ÷ 2 = 3

• Third, determine the central atom

Here hydrogen can not be the central atom. Because the central atom is bonded with at least two other atoms, and hydrogen has only one electron in its last shell, so it can not make more than one bond.

Hence, here we have to assume that the central atom is carbon.

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 3 electron pairs. And two C — H bonds are already marked. So we have to only mark the remaining one electron pair as a lone pair 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 hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell.

Always start to mark the lone pairs from outside atoms. Here, the outside atoms are hydrogens. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for carbon, there is one lone pair.

Mark the lone pair 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 hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

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

Final structure

The final structure of CH₂ (specifically the methylene radical) features a central carbon atom linked to two hydrogen atoms through single covalent bonds. In this arrangement, the carbon atom does not fulfill the octet rule, instead possessing only six electrons in its valence shell—four involved in bonding and two remaining as non-bonding electrons. Within this layout, each hydrogen atom achieves a stable duet. This configuration represents a highly reactive, short-lived intermediate rather than a stable molecule, as the carbon atom carries no formal charge but remains electron-deficient. Accordingly, this specific electronic distribution serves as the definitive and most accurate Lewis representation of methylene.

Next: HO₂^– Lewis structure