Which of the following ions has the smallest radius? — Periodic Table and Periodicity Chemistry Question

💡 Solution & Explanation

I need to see the options to provide a complete answer. However, I can explain the general principle for determining which ion has the smallest radius: **Key Principle:** Ionic radius depends on: 1. **Nuclear charge (atomic number)** — higher charge → smaller radius 2. **Number of electrons** — more electrons → larger radius 3. **Charge of the ion** — higher positive charge → smaller radius; higher negative charge → larger radius **General Rules:** - For **isoelectronic ions** (same electron configuration), the ion with the highest nuclear charge has the smallest radius - Among **cations**, higher charge means smaller radius - Among **anions**, higher charge means larger radius **Example Logic:** If the options were something like $O^{2-}$, $F^-$, $Na^+$, $Mg^{2+}$: - All are isoelectronic (10 electrons) - $Mg^{2+}$ has the highest nuclear charge (12 protons) → **smallest radius** **To confirm option C is correct**, please provide the answer choices, and I'll explain specifically why C has the smallest radius and why the others are larger.