Question

What are the intermolecular forces in water?

Answer 1

Hint: Water is the only substance that we come across as a solid, a liquid, and a gas on a regular basis. It is a solid at low temperatures, with individual molecules bound into a hard structure. The average kinetic energy of the molecules increases as the temperature rises, increasing the pace at which they move.

Complete answer:
Hydrogen bonds, dipole-induced dipole forces, and London dispersion forces all exist in water. Polar OH bonds exist in water. The negative O atoms attract the positive H atoms in adjacent molecules, forming a hydrogen bond, which is an extremely powerful sort of dipole-dipole interaction. Water possesses dipole-induced dipole and London dispersion forces because it has hydrogen bonds. The greatest force is hydrogen bonds, although other forms of intermolecular attraction are also present. Hydrogen bonding can be intermolecular (between two molecules) or intramolecular (between two molecules) (occurring among parts of the same molecule). The energy of a hydrogen bond can range from 1 to 40 kcal/mol, depending on the nature of the donor and acceptor atoms that make up the bond, their shape, and the surrounding environment. This makes them a little stronger than a van der Waals interaction but not quite as strong as completely covalent or ionic connections. This kind of connection may be found in both inorganic and organic compounds, such as water and DNA and proteins. Many of the unusual physical and chemical characteristics of N, O, and F compounds are due to the hydrogen bond. Water's high boiling point (100 °C) is due to intermolecular hydrogen bonding, as opposed to the other group 16 hydrides, which have significantly weaker hydrogen bonds. The secondary and tertiary architectures of proteins and nucleic acids are partially due to intramolecular hydrogen bonding. It also plays a crucial function in the structure of synthetic and natural polymers.

Note:
The hydrogen bond is similar to the dihydrogen bond, which is likewise an intermolecular bonding contact that involves hydrogen atoms. These structures have been known for a long time and crystallography has described them well; nonetheless, their connection to the traditional hydrogen bond, ionic bond, and covalent bond is still unknown. In nonmetallic atoms, the hydrogen bond is defined by a proton acceptor, which is a lone pair of electrons. These proton acceptors might be pi-bonds or metal complexes in some circumstances. A metal hydride, on the other hand, acts as a proton acceptor in the dihydrogen bond, resulting in a hydrogen-hydrogen interaction.