Use the information and data given below to answer the question (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 point of `HF, HCl, HBr` and `HI` are 293 K, 189 K, 206 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 boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest ?

Explanation

From the information and data given in the question, we concluded that
In HCl, HBr and HI, dipole-dipole and London forces are present because molecules possess permanent dipole. In HF dipole-dipole. London forces and hydrogen bonding are present.