Answer :
The formal charges on each nitrogen atom in the N₃⁻ ion are zero.
To calculate the formal charges on each nitrogen atom in the N₃⁻ ion, we need to determine the valence electron distribution and assign formal charges based on the number of electrons each nitrogen atom possesses.
The Lewis structure for the N₃⁻ ion can be represented as follows, with a triple bond between the three nitrogen atoms:
N≡N-N⁻
To calculate the formal charges, we follow these steps:
Determine the valence electrons for each atom:
Nitrogen (N) has 5 valence electrons.
Calculate the number of electrons each nitrogen atom possesses:
Each nitrogen atom in the ion is directly bonded to two other nitrogen atoms and has one lone pair of electrons.
The central nitrogen atom:
It is bonded to two nitrogen atoms, so it shares two electrons in each bond (2 × 2 = 4 electrons).
It has one lone pair of electrons (2 electrons).
The two terminal nitrogen atoms:
Each is bonded to one nitrogen atom, so it shares one electron in the bond (1 electron).
Each has two lone pairs of electrons (4 electrons).
Calculate the formal charge for each nitrogen atom:
Formal charge = Valence electrons - Non-bonding electrons - (1/2) * Bonding electrons
The formal charge for each nitrogen atom is as follows:
Central nitrogen atom:
Formal charge = 5 - 2 - (1/2) * 4 = 0
Terminal nitrogen atoms:
Formal charge = 5 - 4 - (1/2) * 1 = 0
Therefore, the formal charges on each nitrogen atom in the N₃⁻ ion are zero.
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