What is the Lewis structure of CH3NO2?

The Lewis structure of CH₃NO₂ (methyl nitrite) can be represented by following these steps:

1. Count the total valence electrons: Carbon (C) has 4, Hydrogen (H) has 1 (and there are 3 H’s), Nitrogen (N) has 5, and Oxygen (O) has 6 (with 2 O’s). So, the total is:
   4 (C) + 3 (H) + 5 (N) + 2 × 6 (O) = 24 valence electrons.
2. Arrange the atoms: We place the carbon atom in the center, surrounded by three hydrogen atoms and a nitrogen atom attached to it. The nitrogen atom bonds with the two oxygen atoms.
3. Distribute the electrons: Start by placing a single bond between C and each H, C and N, and N and each O. After creating these bonds, distribute the remaining electrons to satisfy the octet rule for N and O. Each O needs to have a total of 8 electrons in its outer shell, which may involve creating double bonds.

The final Lewis structure looks like this:

   H   H
    |   |
H - C - N = O
       | 
       O

In this structure, the nitrogen atom forms a double bond with one oxygen and a single bond with the other oxygen, while carbon is bonded to three hydrogens and one nitrogen. This configuration accounts for all 24 valence electrons and gives each atom a complete outer shell.