My textbook says:
The Oxygen atom of other molecules links to form coordinate covalent bond with H-atom using lone pair.
Now I am confused. Is H-bonding coordinate covalent bond?
My textbook says:
The Oxygen atom of other molecules links to form coordinate covalent bond with H-atom using lone pair.
Now I am confused. Is H-bonding coordinate covalent bond?
"In a way yes". However, rather than starting from nomenclature to get facts, do the vice versa. Otherwise and again "in a way", they could be seen as permanent dipole-dipole interactions, too.
Hydrogen bonds have energy of about a tenth as compared to covalent bonds. So they are considerably weaker but still stronger than other intermolecular interactions.
Thus, they have a special, energetically intermediate, status that was given a name.
How much one goes into quantum mechanical description (the partially donated lone pair is in a deformed orbital between the X and the H)* or if one stops at considering a pure electrostatical attraction between partial and essentially point-like charges as done in not too advanced courses I do not know in details. I guess it depends on how deep one want to go with the description.
But the experimental facts are as I have described above.
*https://www.tandfonline.com/doi/full/10.1080/23746149.2018.1428915 is an example.