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Why only fluorine, oxygen and nitrogen can form hydrogen-bonds with the hydrogen of another molecule?

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    $\begingroup$ That's a common misconception, that is thoroughly incorrect. $\endgroup$
    – Mithoron
    Commented Apr 26, 2018 at 17:35

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No, that's not necessary. Amongst the strongest hydrogen bonds are formed by $\ce{ N, O, F}$ because of their high electronegativity.

There's evidence that the ions $\ce{Cl-, I-, Br- }$ form hydrogen bonds that are much stronger than those of the covalently bonded atoms

$\ce{Cl}$ can form weak hydrogen bonds, but $\ce{Br}$ and $\ce{I}$ form very weak bonds if at all.

A sulfur atom can also function as weak acceptor., but the $\ce{SH-}$ ion forms much stronger bonds.

Hydrogen bonding has been directly observed between a negatively charged carbon and an $\ce{-OH}$ group in the same molecule

Isocyanides' ($\ce{R- N+ #C- }$) carbon atom can also act as an acceptor (forming a rather strong Hydrogen bond).


Reference: March's Advanced Organic Chemistry, Chapter 3: Bonding weaker than Covalent

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  • $\begingroup$ Just to avoid future confusion: the NOF hydrogen bonds are not necessarily stronger than others either. $\endgroup$ Commented Apr 26, 2018 at 19:02
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    $\begingroup$ I think they are, why not? @LinearChristmas . Other atoms form hydrogen bonding but the strongest is formed by N O F atoms... $\endgroup$
    – user43021
    Commented Apr 27, 2018 at 1:10
  • $\begingroup$ @santimirandarp While many strong and common hydrogen bonds are formed with NOF, it is not a sufficient criterion of assigning superiority when comparing strengths of two hydrogen bonds. In other words: while many strong H-bonds are indeed of the NOF variety, there are still cases where others are stronger. One must still carry out meticulous experiments, or perform accurate calculations to make such assignments. See my earlier comment on another question for a concrete example. $\endgroup$ Commented Apr 27, 2018 at 20:43

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