Calculate the formal charge of the central N in the molecule -N=N-O:.

1. Determine the number of valence electrons of nitrogen from the periodic table.
2. Calculate the formal charge using the formula:
\[
\text{Formal Charge} = (\text{Valence Electrons}) - (\text{Non-bonding Electrons}) - \frac{1}{2}(\text{Bonding Electrons})
\]
3. Enter the formal charge, including the magnitude and sign.

Part B:
Calculate the formal charge of the leftmost N in the molecule -N=N-O:.

Follow the same steps as above to determine the formal charge for the leftmost nitrogen.

The formal charge of an atom in a molecule can be calculated by subtracting the number of valence electrons of the atom in its isolated state from the sum of nonbonding electrons and one-half of the bonding electrons associated with that atom. For the central N in the molecule -N=N-õ, the valence electron of N is 5. Assuming that the bonding electrons are equally shared, the central N is connected to 3 bonding electrons and has 1 nonbonding electron. Therefore, the formal charge of the central N is calculated as follows:

Formal charge = #valence electrons (neutral atom) - #nonbonding electrons - 1/2(#bonding electrons)

Formal charge = 5 - 1 - 1.5 = 2.5

The magnitude of the formal charge is 2.5 and the sign is positive.