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My understanding was that hydrogen bonding is much stronger than other dipole-dipole interactions since the dipole between hydrogen and O/F/N is much greater than other dipoles. However, the dipole between C and O in carbonyl is apparently greater than that of a hydroxy group in, say, an alcohol. Hydrogen bonding is still said to be stronger. Why is that?

heyhellohi2
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  • If it was just a dipole-dipole interaction there would be no reason to set it apart. – Mithoron Mar 08 '24 at 02:04
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    https://chemistry.stackexchange.com/questions/143419/why-hydrogen-bonds-are-stronger-than-van-der-waals-forces – Mithoron Mar 08 '24 at 02:07
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    https://chemistry.stackexchange.com/questions/5503/what-exactly-is-hydrogen-bonding-and-does-it-really-need-fluorine-oxygen-or-n – Mithoron Mar 08 '24 at 02:07

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