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Why SnCl(2) is more ionic than SnCl(4) ?...

Why `SnCl_(2)` is more ionic than `SnCl_(4)` ?

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To understand why \( \text{SnCl}_2 \) is more ionic than \( \text{SnCl}_4 \), we can analyze the properties of the cations and anions involved, particularly focusing on their charges and sizes. ### Step-by-Step Solution: 1. **Identify the Cation and Anion**: - In \( \text{SnCl}_2 \), the cation is \( \text{Sn}^{2+} \) and the anion is \( \text{Cl}^- \). - In \( \text{SnCl}_4 \), the cation is \( \text{Sn}^{4+} \) and the anion is \( \text{Cl}^- \). ...
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