"An intermolecular force (IMF) (or secondary force) is the force that mediates interaction between molecules, including the electromagnetic forces of attraction or repulsion which act between atoms and other types of neighboring particles, e.g. atoms or ions."
The attractive or repulsive forces between molecules.
Electronegativity: The tendency of an atom to attract shared electrons towards itself.
Polarity: A measure of how equally or unequally the electrons are shared in a covalent bond.
Dipole-dipole forces: The attractive forces between polar molecules due to the positive and negative ends of their dipoles aligning.
Hydrogen bonding: A type of dipole-dipole interaction where a hydrogen atom is covalently bonded to a highly electronegative atom and interacts with another highly electronegative atom in a different molecule.
Ion-dipole forces: The attraction between an ion and a polar molecule.
London dispersion forces: The attraction between instantaneous dipoles that arise due to temporary fluctuations in electron distribution.
Surface tension: The tendency of liquids to minimize their surface area in order to reduce energy.
Cohesion: The intermolecular attraction between molecules of the same substance.
Adhesion: The intermolecular attraction between two different substances.
Viscosity: The resistance of a liquid to flow.
Boiling point: The temperature at which a liquid turns into a gas.
Melting point: The temperature at which a solid turns into a liquid.
Phase changes: The processes that occur during the transformation between different states of matter.
Intermolecular potential energy: The energy that is required to break the intermolecular forces between molecules.
Clausius-Clapeyron equation: A mathematical equation that relates the changes in temperature and pressure to changes in the boiling point of a substance.
Vapor pressure: The pressure exerted by a gas in equilibrium with its liquid or solid phase.
Critical temperature and pressure: The maximum temperature and pressure at which a gas can be condensed into a liquid phase.
Solubility: The ability of one substance (the solute) to dissolve in another substance (the solvent).
Solutions and their properties: The physical and chemical properties of solutions, and how they differ from pure substances.
Van der Waals forces: A general term for all intermolecular forces, including dipole-dipole, hydrogen bonding, and London dispersion forces.
Van der Waals forces: These are the weakest intermolecular forces that exist between neutral atoms or molecules. There are two types of Van der Waals forces: London dispersion forces and dipole-dipole forces. London dispersion forces are caused by temporary dipoles that are induced in nonpolar molecules, while dipole-dipole forces are caused by permanent dipoles in polar molecules.
Hydrogen bonds: Hydrogen bonding is a special type of dipole-dipole force that exists between a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and a neighboring highly electronegative atom. Hydrogen bonds are relatively strong, and they are responsible for many of the unique properties of water and biological molecules like DNA and proteins.
Ionic bonds: An ionic bond is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. This type of bond is typically formed between a metal and a non-metal. Ionic bonds are quite strong, and they are a major factor in determining the structure and properties of many salts and other ionic compounds.
Covalent bonds: Covalent bonds are formed when two atoms share a pair of electrons. These bonds can be polar or nonpolar, depending on the electronegativity difference between the atoms involved. Covalent bonds are relatively strong, and they are responsible for the structure and properties of many molecules.
Metallic bonds: Metallic bonds are formed between positively charged metal ions and their surrounding delocalized electrons. These bonds are responsible for the unique properties of metals, such as their high electrical conductivity and malleability.
Dipole-induced dipole forces: Dipole-induced dipole forces exist between a permanent dipole in a polar molecule and an induced dipole in a neighboring nonpolar molecule. These forces are weaker than dipole-dipole forces but stronger than London dispersion forces.
Ion-induced dipole forces: Ion-induced dipole forces exist between an ion and an induced dipole in a neighboring nonpolar molecule. These forces are much weaker than ionic bonds but stronger than London dispersion forces.
"Intermolecular forces are weak relative to intramolecular forces – the forces which hold a molecule together."
"For example, the covalent bond, involving sharing electron pairs between atoms, is much stronger than the forces present between neighboring molecules."
"The first reference to the nature of microscopic forces is found in Alexis Clairaut's work Théorie de la figure de la Terre, published in Paris in 1743."
"Other scientists who have contributed to the investigation of microscopic forces include: Laplace, Gauss, Maxwell, and Boltzmann."
"Attractive intermolecular forces are categorized into the following types: Hydrogen bonding, Ion–dipole forces and ion–induced dipole forces, Van der Waals forces – Keesom force, Debye force, and London dispersion force."
"Information on intermolecular forces is obtained by macroscopic measurements of properties like viscosity, pressure, volume, temperature (PVT) data."
"The link to microscopic aspects is given by virial coefficients and Lennard-Jones potentials."
"Both sets of forces are essential parts of force fields frequently used in molecular mechanics."
"The electromagnetic forces of attraction or repulsion which act between atoms and other types of neighboring particles, e.g. atoms or ions."
"For example, the covalent bond, involving sharing electron pairs between atoms, is much stronger than the forces present between neighboring molecules."
"The link to microscopic aspects is given by virial coefficients and Lennard-Jones potentials."
"Attractive intermolecular forces are categorized into the following types: Hydrogen bonding..."
"Attractive intermolecular forces are categorized into the following types: ...Van der Waals forces – Keesom force, Debye force, and London dispersion force."
"Information on intermolecular forces is obtained by macroscopic measurements of properties like viscosity, pressure, volume, temperature (PVT) data."
"Measurements of properties like viscosity, pressure, volume, and temperature (PVT) data serve as key indicators of intermolecular forces."
"An intermolecular force (IMF) (or secondary force) is the force that mediates interaction between molecules, including the electromagnetic forces of attraction or repulsion."
"Intramolecular forces – the forces which hold a molecule together, are stronger than intermolecular forces."
"Other scientists who have contributed to the investigation of microscopic forces include: Laplace, Gauss, Maxwell, and Boltzmann."
"Both sets of forces are essential parts of force fields frequently used in molecular mechanics."