Question

Association of molecules in water is due to:
a.Hydrogen bonding
b.Covalent bonding
c.Ionic bonding
d.Van der waals force

Answer 1

Hint: A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form. Ionic bonds are formed by the electrostatic force of attraction between oppositely charged ions, whereas covalent bonds are formed by the sharing of electrons. Chemical bonds come in a variety of strengths; there are "strong bonds" or "primary bonds" like covalent, ionic, and metallic connections, as well as "weak bonds" or "secondary bonds" like dipole–dipole interactions, the London dispersion force, and hydrogen bonding.

Complete answer:
A dipole interaction is the attraction force between water molecules. The hydrogen atoms form an extremely polar connection with the very electronegative oxygen atom. One molecule's partly positive hydrogen atom attracts the oxygen atom of a neighbouring water molecule. H is linked to the more electronegative O atom in water. One water molecule's H atom creates a hydrogen bond with another water molecule's O atom. The second water molecule's hydrogen atom establishes a hydrogen connection with the third water molecule's O atom. This leads to the formation of a bond with water molecules. Hydrogen bonding is responsible for the association of molecules in water.
A hydrogen bond (or H-bond) is an electrical attraction between a hydrogen (H) atom covalently linked to a more electronegative atom or group and another electronegative atom containing a single pair of electrons—the hydrogen bond acceptor (Ac). The solid line signifies a polar covalent link, while the dotted or dashed line denotes the hydrogen bond in such an interacting system. The second-row elements nitrogen (N), oxygen (O), and fluorine (F) are the most common donor and acceptor atoms (F).

Hence option a is correct.

Note:
A molecule of water in the liquid or solid state may establish up to four hydrogen bonds with adjacent molecules due to its polarity. In most liquids, hydrogen bonds are roughly ten times stronger than the Van der Waals force, which pulls molecules together. Water's melting and boiling temperatures are significantly greater than those of other similar substances like hydrogen sulphide because of this.