Question

What factors affect hydrogen bonding?

Answer 1

Hint : Hydrogen bonding is the forming of hydrogen bonds, which are a kind of attractive intermolecular force caused by the dipole-dipole interaction between a hydrogen atom bound to a strongly electronegative atom and another highly electronegative atom nearby. Hydrogen, for example, is covalently bound to the more electronegative oxygen atom in water molecules. As a result of dipole-dipole interactions between the hydrogen atom of one water molecule and the oxygen atom of another water molecule, hydrogen bonding occurs in water molecules.

Complete Step By Step Answer:
Hydrogen bonding is a key element in deciding the 3D structures and properties of synthetic and natural proteins. The ice's crystal structure is strongly influenced by hydrogen bonding, resulting in an open hexagonal lattice.
Extensiveness – A molecule with more hydrogen bonds can form more hydrogen bonds with neighbouring molecules, so severing more hydrogen bonds per molecule takes more energy, and the melting/boiling point is lower.
Polarity - If the extension is the same, we can calculate hydrogen bond strength by comparing H-F, H-O, and H-N bond polarity.
The below are the conditions for hydrogen bonding:
An extremely electronegative atom must be compared to the hydrogen atom in the molecule. The polarisation of a molecule is proportional to its electronegativity.
The electronegative atom should be tiny in size. The stronger the electrostatic attraction, the smaller the size.

Note :
When a hydrogen atom is bound to a strongly electronegative atom in a molecule, it absorbs the mutual pair of electrons further, making one end of the molecule slightly negative and the other slightly positive. The negative end of one molecule absorbs the positive end of the other, resulting in the formation of a weak bond. The hydrogen bond is the name for this kind of bond.