Question
Why does water show high boiling point as compared to hydrogen sulphide? Give reasons for your answer.
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Answer
In water $\mathrm{H}_2 \mathrm{O}$ there is electrostatic attraction between partially positive hydrogen of one atom with partial negative oxygen (highly electronegative) of another atom which produces dipole-dipole interactions resulting hydrogen bonding. As these hydrogen bonds are strong in water, it requires high energy to break the bonds with high boiling point of 373 K .
While in hydrogen sulphide $\mathrm{H}_2 \mathrm{S}$, even though there are intermolecular forces of attraction between atoms, hydrogen bonding is not present. Hence the $\mathrm{H}_2 \mathrm{S}$ requires less energy to break the bonds with low boiling point of 213 K .
While in hydrogen sulphide $\mathrm{H}_2 \mathrm{S}$, even though there are intermolecular forces of attraction between atoms, hydrogen bonding is not present. Hence the $\mathrm{H}_2 \mathrm{S}$ requires less energy to break the bonds with low boiling point of 213 K .
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