Water $(H_2O)$ is a liquid while hydrogen sulfide $(H_2S)$ is a gas. This is due to:

Use the information and data given below to answer the questions $(a)$ to $(c)$. Stronger intermolecular forces result in higher boiling point.
Strength of London forces increases with the number of electrons in the molecule.
Boiling points of $HF, HCl, HBr$ and $HI$ are $293 \ K, 189 \ K, 200 \ K$ and $238 \ K$ respectively.
$(a)$ Which type of intermolecular forces are present in the molecules $HF, HCl, HBr$ and $HI$?
$(b)$ Looking at the trend of boiling points of $HCl, HBr$ and $HI$,explain out of dipole-dipole interaction and London interaction,which one is predominant here.
$(c)$ Why is the boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?

The boiling point of $CH_3OH$ (methanol) is greater than that of $CH_3SH$ (methyl thiol) because

Identify the type of hydrogen bonding in the following substances: Ice,Water,Liquid Ammonia,$o$-Nitrophenol,$p$-Nitrophenol.

The variation of the boiling points of the hydrogen halides is in the order $HF > HI > HBr > HCl$. What explains the higher boiling point of hydrogen fluoride?

Which among the following compounds does $NOT$ form intermolecular hydrogen bonding?