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Select the strongest base. A B C They all have the same strength 0: C

Select the strongest base. A B C They all have the same strength 0: C

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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### Question: Select the strongest base. #### Diagrams: - **A:** This structure represents a propyl group attached to a negatively charged carbon, with a pair of lone electrons depicted. - **B:** This structure represents a propyl group attached to an ethyne group (a triple-bonded carbon-carbon group) with a negatively charged carbon on the ethyne group hosting a pair of lone electrons. - **C:** This structure represents a propyl group attached to a neutral nitrogen atom with a lone electron pair. #### Options: - ○ C - ○ They all have the same strength - ○ B - ○ A #### Explanation: - Understanding the basicity of these molecules involves analyzing their structural characteristics and conjugate acids. Bases are stronger if their conjugate acids are weaker. This strength can be influenced by the structure of the molecule, the hybridization state of the atom carrying the negative charge, and the stability of the base itself. - **Option A:** The negatively charged carbon has an sp3 hybridization, which is less electronegative compared to sp and sp2 hybridized carbons. - **Option B:** The negatively charged carbon has an sp hybridization, which is more electronegative and hence stabilizes the negative charge better than sp2 or sp3 hybridized carbons. - **Option C:** A neutral nitrogen with a lone pair. While nitrogen is less electronegative than carbon, the lone pair does contribute to its basicity. Considering these factors, the strongest base will typically be the one with the carbon bearing the least electronegative hybridization state while supporting a charge. Therefore, Option A (sp3 hybridized carbon) is often considered the strongest base among the given choices.
Transcribed Image Text:### Question: Select the strongest base. #### Diagrams: - **A:** This structure represents a propyl group attached to a negatively charged carbon, with a pair of lone electrons depicted. - **B:** This structure represents a propyl group attached to an ethyne group (a triple-bonded carbon-carbon group) with a negatively charged carbon on the ethyne group hosting a pair of lone electrons. - **C:** This structure represents a propyl group attached to a neutral nitrogen atom with a lone electron pair. #### Options: - ○ C - ○ They all have the same strength - ○ B - ○ A #### Explanation: - Understanding the basicity of these molecules involves analyzing their structural characteristics and conjugate acids. Bases are stronger if their conjugate acids are weaker. This strength can be influenced by the structure of the molecule, the hybridization state of the atom carrying the negative charge, and the stability of the base itself. - **Option A:** The negatively charged carbon has an sp3 hybridization, which is less electronegative compared to sp and sp2 hybridized carbons. - **Option B:** The negatively charged carbon has an sp hybridization, which is more electronegative and hence stabilizes the negative charge better than sp2 or sp3 hybridized carbons. - **Option C:** A neutral nitrogen with a lone pair. While nitrogen is less electronegative than carbon, the lone pair does contribute to its basicity. Considering these factors, the strongest base will typically be the one with the carbon bearing the least electronegative hybridization state while supporting a charge. Therefore, Option A (sp3 hybridized carbon) is often considered the strongest base among the given choices.
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