This is not at all an anwer, but the discussion above pointed to the 2011 IUPAC definition of hydrogen bonds, which I did not know about:

The hydrogen bond is an attractive interaction between a hydrogen atom from a molecule or a molecular fragment X–H in which X is more electronegative than H, and an atom or a group of atoms in the same or a different molecule, in which there is evidence of bond formation.

That definition paper from Pure and Applied Chemistry is accompanied by a technical report that gives history, examples, etc.

This is not at all an anwer, but the discussion above pointed to the 2011 IUPAC definition of hydrogen bonds, which I did not know about:

The hydrogen bond is an attractive interaction between a hydrogen atom from a molecule or a molecular fragment X–H in which X is more electronegative than H, and an atom or a group of atoms in the same or a different molecule, in which there is evidence of bond formation.

That definition paper from Pure and Applied Chemistry is accompanied by a technical report that gives history, examples, etc.

So, while hydrogen bonds are most well known for fluorine (FH-F), oxygen (OH-O) and nitrogen (NH-N) (and permutations), there is a huge zoo of other examples (e.g. reaction intermediates for proton transfers, etc) where this definition applies, and they include most of the periodic table except the electropositive metals.

(Any hydrogen bond of course also works with deuterium, just the stability and reaction dynamics are in most cases slightly different.)