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Considering the hydrogen atoms highlighted in red in the two compounds shown below, which is more acidic and why? -H VS. B -H A is the stronger acid because its conjugate base is stabilized by resonance. B is the stronger acid because its conjugate base is stabilized by resonance. A is the stronger acid because the carbon atom bearing the highlighted proton is sp² hybridized. B is the stronger acid because the carbon atom bearing the highlighted proton is sp3 hybridized.

Considering the hydrogen atoms highlighted in red in the two compounds shown below, which is more acidic and why? -H VS. B -H A is the stronger acid because its conjugate base is stabilized by resonance. B is the stronger acid because its conjugate base is stabilized by resonance. A is the stronger acid because the carbon atom bearing the highlighted proton is sp² hybridized. B is the stronger acid because the carbon atom bearing the highlighted proton is sp3 hybridized.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The image is a question from an educational practice module on the topic "3.4 Brønsted-Lowry Acidity: Factors Affecting the Stability of Anions." Title: Considering the hydrogen atoms highlighted in red in the two compounds shown below, which is more acidic and why? There are two chemical structures labeled "A" and "B." Each structure has a hydrogen atom highlighted in red. Below the structures, there are answer options: - A is the stronger acid because its conjugate base is stabilized by resonance. - B is the stronger acid because its conjugate base is stabilized by resonance. - A is the stronger acid because the carbon atom bearing the highlighted proton is sp² hybridized. - B is the stronger acid because the carbon atom bearing the highlighted proton is sp³ hybridized. There are buttons labeled "Save for Later" and "Submit Answer" at the bottom. **Explanation:** The question asks you to compare the acidity of two hydrogen atoms in different compounds based on their structural features and the stability of their conjugate bases. The options suggest thinking about resonance stabilization and hybridization of the carbon atom to which the hydrogen is attached.
Transcribed Image Text:The image is a question from an educational practice module on the topic "3.4 Brønsted-Lowry Acidity: Factors Affecting the Stability of Anions." Title: Considering the hydrogen atoms highlighted in red in the two compounds shown below, which is more acidic and why? There are two chemical structures labeled "A" and "B." Each structure has a hydrogen atom highlighted in red. Below the structures, there are answer options: - A is the stronger acid because its conjugate base is stabilized by resonance. - B is the stronger acid because its conjugate base is stabilized by resonance. - A is the stronger acid because the carbon atom bearing the highlighted proton is sp² hybridized. - B is the stronger acid because the carbon atom bearing the highlighted proton is sp³ hybridized. There are buttons labeled "Save for Later" and "Submit Answer" at the bottom. **Explanation:** The question asks you to compare the acidity of two hydrogen atoms in different compounds based on their structural features and the stability of their conjugate bases. The options suggest thinking about resonance stabilization and hybridization of the carbon atom to which the hydrogen is attached.
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