Timeline for Why are the boiling points of aldehydes less than those of ketones?
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6 events
| when toggle format | what | by | license | comment | |
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| Mar 1 at 8:18 | comment | added | Gaurav Sai Maddipati | How would electron donating groups increase polarity, this makes no sense. | |
| Mar 24, 2022 at 7:23 | comment | added | Balu | Considering that the carbon atom is positively polarised, why don't the electron donating groups reduce this polarization rather than increasing the polarization? | |
| S May 16, 2015 at 8:01 | history | suggested | user10259 | CC BY-SA 3.0 |
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| May 16, 2015 at 5:01 | review | Suggested edits | |||
| S May 16, 2015 at 8:01 | |||||
| Dec 21, 2013 at 11:57 | comment | added | Greg E. | Just a minor point: the comparison between acetaldehyde and acetone is not entirely fair, since acetone is also a heavier molecule, so its comparatively greater London dispersion forces will also come into play (albeit with a lesser degree of significance than difference in dipole moments). I think a better comparison would be between acetone and propanal, since that would be comparing molecules of the same size. Still, as the document Rauru Ferro linked to notes, the b.p. trend isn't entirely consistent. | |
| Dec 21, 2013 at 10:04 | history | answered | Devgeet Patel | CC BY-SA 3.0 |