Would you expect the hydrides of $N$,$O$ and $F$ to have lower boiling points than the hydrides of their subsequent group members? Give reasons.

(N/A) Based on molecular masses,the boiling points of $NH_{3}$,$H_{2}O$ and $HF$ would be expected to be lower than those of the hydrides of their subsequent group members (e.g.,$PH_{3}$,$H_{2}S$,$HCl$).
However,due to the high electronegativity of $N$,$O$ and $F$ atoms,these hydrides exhibit strong intermolecular hydrogen bonding.
This hydrogen bonding leads to molecular association,which significantly increases the energy required to vaporize these substances.
Consequently,the boiling points of $NH_{3}$,$H_{2}O$ and $HF$ are actually higher than those of the hydrides of their subsequent group members.