INTERMOLECULAR FORCE Meaning and
Definition
-
Intermolecular force refers to the attractive forces that exist between molecules in a substance. These forces play a crucial role in determining the physical properties of substances, such as their boiling point, melting point, and viscosity.
There are several types of intermolecular forces, including van der Waals forces, hydrogen bonding, and dipole-dipole interactions. Van der Waals forces are the weakest intermolecular forces and are present in all molecules. They arise due to temporary fluctuations in electron density that cause temporary or induced dipoles in neighboring molecules, resulting in a weak attraction between them.
Hydrogen bonding occurs when a hydrogen atom in one molecule is attracted to a highly electronegative atom, such as oxygen, nitrogen, or fluorine, in a nearby molecule. This type of intermolecular force is stronger than van der Waals forces and gives rise to unique properties in substances such as water.
Dipole-dipole interactions occur between polar molecules, where the positive end of one molecule is attracted to the negative end of another molecule. These forces are stronger than van der Waals forces but weaker than hydrogen bonding.
Overall, intermolecular forces determine the physical state, stability, and behavior of substances. They are responsible for the cohesive forces that hold molecules together, and understanding them is essential in fields such as chemistry, materials science, and biochemistry.
Etymology of INTERMOLECULAR FORCE
The word "intermolecular" comes from the Latin roots "inter", meaning "between" or "among", and "molecula", meaning "a small mass or particle". The word "force" comes from the Latin word "fortis", meaning "strong". In physics and chemistry, "intermolecular forces" refer to the attractive or repulsive forces that exist between molecules. These forces are responsible for the physical properties of substances, such as boiling and melting points.
