Calculate the formal charge on the indicated atom in each of the following molecules or ions. Some molecules may have more than one possible resonance structure, each resulting in a different possible formal charge on the indicated atom. In such cases, supply both unique formal charge values separated by commas. Part Cnitrogen in NO2If there is more than one answer, separate them by commas.

Formal charge for the first resonance structure of NO₂; first Oxygen = 0, N = +1, second Oxygen = -1

Formal charge for the second resonance structure of NO₂; first Oxygen = -1, N = +1, second Oxygen = 0

Explanation:

The formal charge of an atom in a molecule is the assumed charge the atom would have if the electrons in the bonds are redistributed evenly between the atoms.

Formal charge = valence electrons - (non-bonding electrons) - (bonding electrons / 2).

For NO₂ molecule, the formal charges for the atoms are as follows;

First Oxygen atom = 6 - 4 - 4/2 = 0

For Nitrogen = 5 - 1 - 6/2 = +1

For the second Oxygen atom = 6 - 6 - 2/2 = -1.

Overall charge = 0 + (+1) + (-1) = 0

For the second resonance structure,

First Oxygen atom = 6 - 6 - 2/2 = -1

For Nitrogen = 5 - 1 - 6/2 = +1

For the second Oxygen atom =  6 - 4 - 4/2 = 0

Overall charge = (-1) + (+1) + (0) = 0

Note: Where resonance structures for atoms or ions exist, the formal charges of each of the respective atoms or ions are calculated according.