Answer:
The structure is shown below.
Explanation:
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.
