Amongst the following the number of oxide(s) which are paramagnetic in nature is Na O, KO , NO , N O — Chemical Bonding Chemistry Question

💡 Solution & Explanation

**Step 1: Identify what makes an oxide paramagnetic** An oxide is paramagnetic if it contains unpaired electrons. Use electron configuration and Lewis structures to determine unpaired electrons. **Step 2: Analyze each oxide** - **Na₂O**: Na⁺ and O²⁻ ions. O²⁻ has all paired electrons. **Diamagnetic** - **KO₂**: Superoxide ion O₂⁻ contains one unpaired electron. **Paramagnetic** ✓ - **NO**: Odd number of electrons (7 total). Has 1 unpaired electron. **Paramagnetic** ✓ - **N₂O**: Linear molecule with all paired electrons. **Diamagnetic** - **ClO₂**: Odd number of electrons (23 total). Has 1 unpaired electron. **Paramagnetic** ✓ - **NO₂**: Odd number of electrons (23 total). Has 1 unpaired electron. **Paramagnetic** ✓ - **SO₂**: Even electrons, all paired. **Diamagnetic** - **Cl₂O**: Even electrons, all paired. **Diamagnetic** **Step 3: Count paramagnetic oxides** KO₂, NO, ClO₂, and NO₂ are paramagnetic. Therefore, the answer is 4.