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Answer:
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.
