Felix Castory
Jun 23
Why ethylamine is more basic than methylamine?
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ChatGPT
Jun 23
Ethylamine is more basic than methylamine because the ethyl group in ethylamine is larger and more electron-donating than the methyl group in methylamine. This means that the lone pair of electrons on the nitrogen atom in ethylamine is more readily available for donation to a proton, making it a stronger base. Additionally, the ethyl group can stabilize the resulting positive charge on the nitrogen atom through inductive effects, further increasing the basicity of ethylamine compared to methylamine.
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Google Gemini AI
Jun 23
Ethylamine is more basic than methylamine due to the following reasons:
1. Inductive Effect: In ethylamine, the ethyl group (-CH2-CH3) is more electron-donating than the methyl group (-CH3) in methylamine. This is because the ethyl group has more C-H bonds, which are less electronegative than the C-N bond in the methyl group. The electron-donating nature of the ethyl group stabilizes the positive charge on the nitrogen atom in the conjugate acid of ethylamine, making it more likely to dissociate and form hydroxide ions (OH-), thus increasing its basicity.
2. Steric Effect: The ethyl group in ethylamine is larger than the methyl group in methylamine. This steric bulk hinders the approach of protons (H+) to the nitrogen atom, making it more difficult for methylamine to form its conjugate acid. In contrast, the smaller methyl group in methylamine allows for easier protonation, resulting in a lower basicity compared to ethylamine.
3. Solvent Effects: Ethylamine is typically encountered in aqueous solutions, where water molecules can interact with the amino group through hydrogen bonding. These hydrogen bonds stabilize the free amino group, making it less likely to accept protons and lowering its basicity. However, the larger ethyl group in ethylamine shields the amino group from hydrogen bonding more effectively than the methyl group in methylamine. This reduced hydrogen bonding allows ethylamine to retain more of its basic character in aqueous solutions.
In summary, the electron-donating inductive effect of the ethyl group, its steric hindrance, and the reduced solvent effects in ethylamine all contribute to its increased basicity compared to methylamine.
1. Inductive Effect: In ethylamine, the ethyl group (-CH2-CH3) is more electron-donating than the methyl group (-CH3) in methylamine. This is because the ethyl group has more C-H bonds, which are less electronegative than the C-N bond in the methyl group. The electron-donating nature of the ethyl group stabilizes the positive charge on the nitrogen atom in the conjugate acid of ethylamine, making it more likely to dissociate and form hydroxide ions (OH-), thus increasing its basicity.
2. Steric Effect: The ethyl group in ethylamine is larger than the methyl group in methylamine. This steric bulk hinders the approach of protons (H+) to the nitrogen atom, making it more difficult for methylamine to form its conjugate acid. In contrast, the smaller methyl group in methylamine allows for easier protonation, resulting in a lower basicity compared to ethylamine.
3. Solvent Effects: Ethylamine is typically encountered in aqueous solutions, where water molecules can interact with the amino group through hydrogen bonding. These hydrogen bonds stabilize the free amino group, making it less likely to accept protons and lowering its basicity. However, the larger ethyl group in ethylamine shields the amino group from hydrogen bonding more effectively than the methyl group in methylamine. This reduced hydrogen bonding allows ethylamine to retain more of its basic character in aqueous solutions.
In summary, the electron-donating inductive effect of the ethyl group, its steric hindrance, and the reduced solvent effects in ethylamine all contribute to its increased basicity compared to methylamine.
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Anonymous
Jun 23
Soba bolchstan k sab se bar darya
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