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?

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The bond energy of HF molecules is greater than in other hydrogen halides.

There is strong hydrogen bonding between HF molecules.

The effect of nuclear shielding is much reduced in fluorine which polarises the HF molecule.

The electronegativity of fluorine is much higher than for other elements in the group.

answer is A.

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Detailed Solution

HF forms strong intermolecular H-bonding due to high electronegativity of F. Hence, the boiling point of HF is abnormally high.

Boiling points of other hydrogen halides gradually increase from HCl to HI due to increase in size of halogen atoms from HCl to HI which consequently increases the magnitude of van der Waals forces.

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