Vsepr & Hybridisation

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Formal charge on oxygen in the nitrate ion (NO3−) using a structure with one double bond and two single bonds is:

RankGuru · Accepted Answer

1. **Formal Charge (FC) Formula**: $FC = [V] - [L] - \frac{1}{2}[S]$, where $V=$ valence electrons, $L=$ lone pair electrons, and $S=$ shared (bonding) electrons.
2. **O with Single Bond**:
   - Valence $V = 6$.
   - Lone pair electrons $L = 6$ (3 lone pairs).
   - Shared electrons $S = 2$.
   - $FC = 6 - 6 - (2/2) = -1$.
3. **O with Double Bond**:
   - Valence $V = 6$.
   - Lone pair electrons $L = 4$ (2 lone pairs).
   - Shared electrons $S = 4$.
   - $FC = 6 - 4 - (4/2) = 0$.
4. **Conclusion**: In the Lewis structure, each **single-bonded Oxygen** has a formal charge of **$-1$**. The nitrate ion has two such oxygens.

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