Vsepr & Hybridisation

Question

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.

Rank Guru

Vsepr & Hybridisation

Select the correct option:

Solution

🔒 Solution Hidden from View

More vsepr & hybridisation Practice Questions

Which statement about hydrogen bonding is correct?

Which statement best explains why PF5 is stable while NF5 is not?

Which set lists increasing bond length for the carbon–oxygen bonds?

Which pair correctly matches molecule with geometry?

The approximate bond angle in NH3 is:

About This Question