Why does water show high boling points as compared to hydrogen sulphide? Given reason for answer.

Answer

N/a

Explanation

Water show high boiliong point as compared to hydrogen suliphide due to high electronegativity of oxygeb (EN = 3.5)Water undergoes extensive H- bonding as a result of which water exists as associated molecule.
`.......overset(delta^(+))(H) - underset(H)underset(|)overset(delta^(-))O.......overset(delta^(+))(H) - underset(H)underset(|)overset(delta^(-))O........overset(delta^(+))(H) - underset(H)underset(|)overset(delta^(-))O`
For breaking these hydrogen bond, a large amount of energy is needed and hence the boiliding point of `H_(2)O` is high.
Inother words, due to lower electronegativity of S (EN = 2.5), hydrogen sulphide do not undergo H- bonding . Consequently , `H_(2)S` exisit as discreter molecule and hecne its boiling do not point is much lower than that of `H_(2)O`. Thats why `H_(2)S` is a gas at room temperature.