Question

B.P of \[{{\text{H}}_{\text{2}}}\text{O (10}{{\text{0}}^{\text{o}}}\text{C) }\!\!~\!\!\text{ }\] and \[{{\text{H}}_{\text{2}}}\text{S (- 4}{{\text{2}}^{\text{o}}}\text{C) }\!\!~\!\!\text{ }\] explained by:
A van der Waal's forces
B Covalent bond
C Hydrogen bond
D Ionic bond

Answer 1

Hint: The temperature at which a liquid's vapour pressure equals the pressure around it and the liquid transforms into a vapour is known as the boiling point of a substance. A liquid's boiling point varies depending on the atmospheric pressure in the area. The boiling point depends on the inter-particles force of attaction between particles of any substance.

Complete step-by-step answer:A hydrogen atom that is bound to a highly electronegative atom and another highly electronegative atom that is close by interact with one another to form hydrogen bonds, which are an unique kind of attractive intermolecular interactions. This process is known as hydrogen bonding.

Due to the additional energy required to break these bonds, the molecule with hydrogen bonds has a high melting and boiling point.
The presence of hydrogen bonding accounts for the particularly high boiling point of hydrogen fluoride among the halogen acids.
At room temperature, \[{{\text{H}}_{\text{2}}}\text{O}\] is a liquid but \[{{\text{H}}_{\text{2}}}\text{S}\], \[{{\text{H}}_{\text{2}}}\text{Se}\], and \[{{\text{H}}_{\text{2}}}\text{Te}\] are all gases. Water's boiling point is higher than that of other chemicals because hydrogen bonds create links between its molecules.
Because hydrogen bonds exist in \[\text{N}{{\text{H}}_{\text{3}}}\] but not in \[\text{P}{{\text{H}}_{\text{3}}}\], ammonia has a higher boiling point than $PH_3$.
Because ethanol contains hydrogen bonds, it has a greater boiling point than diethyl ether.
Because \[{{\text{H}}_{\text{2}}}\text{O}\] creates hydrogen bonds but \[{{\text{H}}_{\text{2}}}\text{S}\] does not, \[{{\text{H}}_{\text{2}}}\text{O}\] has a higher B.P than \[{{\text{H}}_{\text{2}}}\text{S}\].

Option ‘C’ is correct

Additional Information: Hydrogen bonds create a cage-like structure of water molecules in the case of solid ice. In actuality, each water molecule is tetrahedrally connected to four other water molecules. As opposed to when they are in a liquid condition, the molecules are not as tightly packed. This cage-like structure compresses when the ice melts, bringing the molecules even closer together. As a result, the volume reduces and the density rises for a given mass of water. As a result, at 273 K, ice is less dense than water. Ice floats because of this.

Note: The small size and high electronegativity of oxygen among group 16 elements, helps in formation of strong hydrogen bonds. The hydrogen bonding in water is stronger than ammonia and hydrogen fluoride due to hydrogen bonding water is liquid at room temperature.