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Why is the boiling point of \mathrm{\mathrm{H}_2 \mathrm{O}} higher than the boiling point of \mathrm{\mathrm{HF}}, even though fluorine is more electronegative than oxygen?

Option: 1

The hydrogen bonds in \mathrm{H}_2 \mathrm{O} are stronger than the hydrogen bonds in \mathrm{HF}.
 


Option: 2

Each \mathrm{H}_2 \mathrm{O} molecule can form four intermolecular hydrogen bonds, while each \mathrm{HF} molecule can only form two.
 


Option: 3

The molecules of \mathrm{H}_2 \mathrm{O} are more polarizable than the molecules of \mathrm{HF}.
 


Option: 4

Both (1) and (2) are correct.


Answers (1)

best_answer

The strength of a hydrogen bond is determined by the coulombic interaction between the lone-pair electrons of the electronegative atom and the hydrogen nucleus. Fluorine is more electronegative than oxygen, and so we would expect a stronger hydrogen bond to exist in liquid \mathrm{HF} than in \mathrm{H}_2 \mathrm{O}. But boiling point of \mathrm{HF} is lower than that of water because each \mathrm{H}_2 \mathrm{O} takes part in four intermolecular hydrogen bonds. Therefore, the forces holding the molecules together are stronger in \mathrm{H}_2 \mathrm{O} than in \mathrm{HF}.

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Divya Prakash Singh

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