Among $NH_{3}$,$H_{2}O$,and $HF$,which would you expect to have the highest magnitude of hydrogen bonding and why?

(B) The extent of hydrogen bonding depends on the electronegativity of the atom and the number of hydrogen atoms available for bonding.
Although fluorine is the most electronegative,the actual order of the extent of hydrogen bonding is $H_{2}O > HF > NH_{3}$.
In $H_{2}O$,each oxygen atom has two lone pairs and two hydrogen atoms,allowing it to form a three-dimensional network structure. This results in the highest magnitude of hydrogen bonding.
In $HF$,there is only one hydrogen atom per fluorine atom,which limits the bonding to a linear chain structure.
In $NH_{3}$,nitrogen has only one lone pair,which limits its ability to form extensive hydrogen bonds compared to water and $HF$.