The compound which does not show paramagnetism is — Coordination Compounds Chemistry Question

💡 Solution & Explanation

# Identifying the Diamagnetic Compound I need to see the options to provide a complete solution. However, I'll explain the general approach: **Key Concept:** A compound is **paramagnetic** if it has unpaired electrons; **diamagnetic** if all electrons are paired. ## General Step-by-Step Method: 1. **Write the electron configuration** of the central atom and ligands 2. **Determine the geometry and crystal field splitting** (for coordination compounds) 3. **Count unpaired electrons:** - If unpaired electrons exist → Paramagnetic - If all electrons paired → Diamagnetic (non-paramagnetic) ## Common Examples: - $[Fe(CN)_6]^{4-}$ → All electrons paired → **Diamagnetic** - $[Fe(H_2O)_6]^{2+}$ → Unpaired electrons present → **Paramagnetic** - $Zn^{2+}$ complexes → Completely filled d-orbitals → **Diamagnetic** - $O_2$ → Two unpaired electrons → **Paramagnetic** **To provide the exact reasoning for option B, please share the four answer choices.** Then I can identify which compound has zero unpaired electrons and explain why it doesn't show paramagnetism.