CH2N2 Lewis structure

CH₂N₂ (diazomethane) has one carbon atom, two hydrogen atoms, and two nitrogen atoms.

In the CH₂N₂ Lewis structure, there is a double bond between the carbon and nitrogen atom. The carbon atom is attached with two hydrogen atoms, and the nitrogen atom is attached with one other nitrogen atom. And on the right nitrogen atom, there are two lone pairs.

Also, there is a negative (-1) charge on the right nitrogen atom, and a positive (+1) charge on the left nitrogen atom.

Alternative method: Lewis structure of CH₂N₂

Rough sketch

• First, determine the total number of valence electrons

In the periodic table, carbon lies in group 14, hydrogen lies in group 1, and nitrogen lies in group 15.

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

Since CH₂N₂ has one carbon atom, two hydrogen atoms, and two nitrogen atoms, so…

Valence electrons of one carbon atom = 4 × 1 = 4
Valence electrons of two hydrogen atoms = 1 × 2 = 2
Valence electrons of two nitrogen atoms = 5 × 2 = 10

And the total valence electrons = 4 + 2 + 10 = 16

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

• Second, find the total electron pairs

We have a total of 16 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 = 16 ÷ 2 = 8

• 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.

Now we have to choose the central atom from carbon and nitrogen. Place the least electronegative atom at the center.

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

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

• And finally, draw the rough sketch

Lone pair

Here, we have a total of 8 electron pairs. And four bonds are already marked. So we have to only mark the remaining four electron pairs as lone pairs on the sketch.

Also remember that both (carbon and nitrogen) are the period 2 elements, so they can not keep more than 8 electrons in their 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 and nitrogens. But no need to mark on hydrogen, because each hydrogen has already two electrons.

So for left nitrogen, there are two lone pairs, for right nitrogen, there are three lone pairs, and for carbon, there is zero lone pair because all four 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 (6) = +1

For each hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For left nitrogen atom, formal charge = 5 – 2 – ½ (4) = +1

For right nitrogen atom, formal charge = 5 – 6 – ½ (2) = -2

Here, both carbon and nitrogen atoms have charges, so mark them on the sketch as follows:

The above structure is not a stable Lewis structure because both carbon and nitrogen atoms have charges. Therefore, reduce the charges (as below) by converting lone pairs to bonds.

Convert a lone pair of the right nitrogen atom to make a new N — N bond with the left nitrogen atom as follows:

In the above structure, you can see that the central atom (carbon) doesn’t form an octet. Hence, the octet rule is not satisfied.

Therefore, again convert a lone pair of the left nitrogen atom to make a new C — N bond with the carbon atom. Also, we have to again check whether there are charges on atoms or not.

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 hydrogen atom, formal charge = 1 – 0 – ½ (2) = 0

For left nitrogen atom, formal charge = 5 – 0 – ½ (8) = +1

For right nitrogen atom, formal charge = 5 – 4 – ½ (4) = -1

Here, both nitrogen atoms have charges, so mark them on the sketch as follows:

Final structure

The final structure of CH₂N₂ consists of a central carbon atom linked to two hydrogen atoms and an inner nitrogen atom, which is then connected to a terminal nitrogen atom. In this layout, the carbon atom forms single covalent bonds with both hydrogen atoms and a double bond with the inner nitrogen atom, while the two nitrogen atoms are joined by a double bond to satisfy the octet rule. Within this arrangement, the inner nitrogen atom achieves four bonds and carries no lone pairs, resulting in a formal charge of +1, while the terminal nitrogen atom maintains two lone pairs alongside its double bond, resulting in a formal charge of -1. This configuration represents the most stable state for the molecule because the carbon atom carries a formal charge of zero and every atom (excluding hydrogen) successfully fulfills the octet rule. Thus, this specific electronic distribution serves as the definitive and most accurate Lewis representation of diazomethane.

Next: SiBr₄ Lewis structure

External video

• CH2N2 Lewis Structure: How to Draw the Lewis Structure for CH2N2 – YouTube • Wayne Breslyn

External links

• https://techiescientist.com/ch2n2-lewis-structure/
• https://chemistry.stackexchange.com/questions/32528/what-is-the-correct-lewis-structure-of-diazomethane
• https://lambdageeks.com/ch2n2-lewis-structure/
• https://oneclass.com/homework-help/chemistry/2103350-draw-the-lewis-structure-inclu.en.html