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 point of HF, HCl, HBr and HI are 293 K, 189 K, 206 K and 238 K respectively.
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.

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 ?

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 ?

The boiling points of HF, HCl, HBr and HI follow the order

Arrange the following in the decreasing order of their boiling points HF, HCl, HBr