locate the atom, and indicate the charge on the atom in the lewis structure.

Explanation:

Step1: Count valence electrons

N has 5 valence - electrons, O has 6 valence - electrons. In the given structure, the total number of valence electrons considered for the calculation of formal charges should match the expected number for the species.

Step2: Calculate formal charge of N

The formula for formal charge (FC = V - N_{l.p.}- \frac{1}{2}N_{b.p.}), where (V) is the number of valence electrons of the neutral atom, (N_{l.p.}) is the number of non - bonding (lone - pair) electrons, and (N_{b.p.}) is the number of bonding electrons. For N, (V = 5), (N_{l.p.}=0), and (N_{b.p.}=8). So, (FC_N=5 - 0-\frac{8}{2}=+ 1).

Step3: Calculate formal charge of double - bonded O

For the double - bonded O, (V = 6), (N_{l.p.}=4), (N_{b.p.}=4). So, (FC_{O_{(double - bonded)}}=6 - 4-\frac{4}{2}=0).

Step4: Calculate formal charge of single - bonded O

For the single - bonded O, (V = 6), (N_{l.p.}=6), (N_{b.p.}=2). So, (FC_{O_{(single - bonded)}}=6 - 6-\frac{2}{2}=-1).

Answer:

The nitrogen atom has a charge of + 1, the double - bonded oxygen atom has a charge of 0, and the single - bonded oxygen atom has a charge of - 1.