Intermolecular forces

Intermolecular Forces

Intermolecular forces (pronunciation: /ˌɪntərməˈlɛkjʊlər ˈfɔːrsɪz/) are the forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions). They are weaker than intramolecular forces, the forces which keep a molecule together.

Etymology

The term "intermolecular force" comes from the prefix "inter-", meaning "between" or "among", and "molecular", relating to or consisting of molecules. The word "force" is derived from the Latin word "fortis", meaning strong. Thus, "intermolecular forces" refers to the forces between or among molecules.

Types of Intermolecular Forces

There are three major types of intermolecular forces:

1. London dispersion forces: These are the weakest intermolecular force and occur between all types of molecules, whether ionic or covalent—polar or nonpolar. The more electrons a molecule has, the stronger its dispersion forces are.

1. Dipole-dipole forces: These forces act between the positive end of one polar molecule and the negative end of another polar molecule. Dipole-dipole forces are stronger than London dispersion forces.

1. Hydrogen bonds: This is a special type of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom. It is the strongest type of intermolecular force.

Related Terms

• Molecule
• Atom
• Ion
• Intramolecular forces
• London dispersion forces
• Dipole-dipole forces
• Hydrogen bonds

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