Question

Hydrogen bonds are the strongest type of

dipole-dipole force.
It occurs when a strongly electronegative
element has a hydrogen attached:
name 3 examples

Answer 1

Hydrogen bonds are very strong intermolecular attractive forces. Three examples of hydrogen bonding include water, ammonia, and hydrogen fluoride.

Step-by-step explanation:

A hydrogen bond is an intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule. Hydrogen bonds are very strong compared to other dipole interactions. The strength of a typical hydrogen bond is about 5% of that of a covalent bond.

Three examples of hydrogen bonding include:

1. Water: In water, hydrogen bonds form between the oxygen atom of one water molecule and the hydrogen atom of another water molecule.
2. Ammonia: In ammonia (NH3), hydrogen bonds form between the hydrogen atom and the lone pairs on the nitrogen atom.
3. Hydrogen fluoride: In hydrogen fluoride (HF), hydrogen bonds form between the hydrogen atom and the fluorine atom.