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Which of the following is the weakest base? O fluoride anion, F2 O bromide anion, Br? O chloride anion, CIa O iodide anion, I?

Which of the following is the weakest base? O fluoride anion, F2 O bromide anion, Br? O chloride anion, CIa O iodide anion, I?

Organic Chemistry
Organic Chemistry
8th Edition
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Chapter4: Acids And Bases
Section: Chapter Questions
Problem 4.10P: Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow...
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Title: Understanding Basic Bases: Halide Anions --- **Question: Which of the following is the weakest base?** - Fluoride anion, \( \text{F}^- \) - Bromide anion, \( \text{Br}^- \) - Chloride anion, \( \text{Cl}^- \) - Iodide anion, \( \text{I}^- \) --- This question aims to test your understanding of the relative basicity of halide anions. Halides are a group of anions derived from halogens, which include fluorine, chlorine, bromine, and iodine. In aqueous solutions, these anions can act as bases, but their ability to accept protons (H⁺) varies. **Factors to Consider:** 1. **Electronegativity:** Fluorine is the most electronegative element, making the fluoride anion less likely to share its electrons compared to other halides, hence acting as a weaker base. 2. **Polarizability:** As you move down the group (from F to I), the anions become larger and more polarizable. This increases their ability to stabilize additional charges, usually indicating stronger bases. By analyzing these factors, one can determine which anion acts as the weakest base in the given options.
Transcribed Image Text:Title: Understanding Basic Bases: Halide Anions --- **Question: Which of the following is the weakest base?** - Fluoride anion, \( \text{F}^- \) - Bromide anion, \( \text{Br}^- \) - Chloride anion, \( \text{Cl}^- \) - Iodide anion, \( \text{I}^- \) --- This question aims to test your understanding of the relative basicity of halide anions. Halides are a group of anions derived from halogens, which include fluorine, chlorine, bromine, and iodine. In aqueous solutions, these anions can act as bases, but their ability to accept protons (H⁺) varies. **Factors to Consider:** 1. **Electronegativity:** Fluorine is the most electronegative element, making the fluoride anion less likely to share its electrons compared to other halides, hence acting as a weaker base. 2. **Polarizability:** As you move down the group (from F to I), the anions become larger and more polarizable. This increases their ability to stabilize additional charges, usually indicating stronger bases. By analyzing these factors, one can determine which anion acts as the weakest base in the given options.
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