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

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.