Draw the Lewis structure for CH3N 2CH3N2 . Draw the molecule by placing atoms on the grid and connecting them with bonds. Show the formal charges of all nonhydrogen atoms in the correct structure. Include all lone pairs of electrons.

The Lewis structure of a molecule is done bt putting the atoms with their valence electrons, and then done the bonds (with lines) to the atoms be with 8 electrons.

The formal charge is a way to quantify the valence electrons, and it can be calculated by:

FC = X - (Y + Z/2)

Where X is the number of the valence electrons of the neutral atom, Y is the number of lone electrons, and Z is the number of shared electrons. As close to 0 is the formal charge of the atoms, as stable is the structure, and, if FC < 0, the negative charge must be in the most electronegative element.

C has 4 valence electrons (group 14), H has 1 valence electrons, and N has 5 valence electrons (group 15). So, each carbon will do 4 bonds, each hydrogen 1 bond, and each nitrogen, 3 bonds. The Lewis structure is shown in the figure below.

The formal charge of the carbon and the nitrogens will be:

C = 4 - ( 0 + 8/2) = 0

First N = 5 - (2 + 6/2) = 0

Second N = 5 - (3 + 4/2) = 0

So, it's the most stable structure.