(C) The boiling point of $H_2O$ is significantly higher than that of $H_2S$ because $H_2O$ molecules exhibit intermolecular hydrogen bonding,whereas $

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(C) The boiling point of $H_2O$ is significantly higher than that of $H_2S$ because $H_2O$ molecules exhibit intermolecular hydrogen bonding,whereas $H_2S$ molecules do not form hydrogen bonds due to the lower electronegativity of sulfur compared to oxygen.

Class 11 Chemistry Chemical Bonding and Molecular Structure Hydrogen bonding

Medium

The difference in the $B.P.$ of $H_2O$ $(100 \ ^oC)$ and $H_2S$ $(-42 \ ^oC)$ is explained by:

A
Vander Waal's forces
B
Covalent bond
C
Hydrogen bond
D
Ionic bond

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Class 11

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Chemical Bonding and Molecular Structure

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Hydrogen bonding

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The difference in the $B.P.$ of $H_2O$ $(100 \ ^oC)$ and $H_2S$ $(-42 \ ^oC)$ is explained by:

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The dominant intermolecular force that must be overcome to convert liquid methanol to its vapour is

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