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CH(3)COO^(-) (acetate ion) is more stabl...

`CH_(3)COO^(-)` (acetate ion) is more stable than `C_(2)H_(5)O^(-)` (ethoxide ion). Explain.

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To explain why the acetate ion (CH₃COO⁻) is more stable than the ethoxide ion (C₂H₅O⁻), we can analyze the structure and resonance stabilization of both ions. ### Step-by-Step Solution: 1. **Identify the Structures**: - The acetate ion (CH₃COO⁻) has a structure where the carbon atom is bonded to a carbonyl group (C=O) and a hydroxyl group (O-H). The negative charge is delocalized over the two oxygen atoms. - The ethoxide ion (C₂H₅O⁻) consists of an ethyl group (C₂H₅) attached to an oxygen atom with a negative charge. 2. **Acidity of Parent Acids**: - Acetate ion is derived from acetic acid (CH₃COOH), while ethoxide ion is derived from ethanol (C₂H₅OH). - Acetic acid is a stronger acid than ethanol. This is because acetic acid can stabilize the negative charge on the acetate ion through resonance. 3. **Resonance Stabilization**: - In the acetate ion, the negative charge can be delocalized between the two oxygen atoms. This delocalization is due to resonance structures that can be drawn, where the negative charge is shared between the two oxygens. - In contrast, the ethoxide ion does not have such resonance stabilization. The negative charge is localized on the oxygen atom, which does not benefit from any resonance. 4. **Comparison of Stability**: - The presence of resonance in the acetate ion allows it to distribute the negative charge over multiple atoms, leading to increased stability. - The ethoxide ion lacks this resonance stabilization, making it less stable compared to the acetate ion. 5. **Conclusion**: - Therefore, due to the ability of the acetate ion to stabilize its negative charge through resonance, it is more stable than the ethoxide ion, which does not have such stabilization.
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