finctional group

Intermolecular Forces (IMFs)

The attractive or repulsive forces that arise between molecules, significantly weaker than intramolecular forces, but crucial in determining physical properties like melting point, boiling point, viscosity, and solubility.

Intramolecular Forces

The covalent or ionic bonds that hold atoms together within a molecule.

Dispersion Forces (London Dispersion Forces)

Universally present forces in all atoms and molecules, arising from instantaneous, temporary dipoles due to the constant motion of electrons, with strength increasing with molar mass and surface area.

Dipole-Dipole Forces

Forces occurring between polar molecules due to the electrostatic attraction between their permanent positive ($\delta+$) and negative ($\delta-$) ends.

Hydrogen Bonding

A special and particularly strong type of dipole-dipole interaction involving a hydrogen atom covalently bonded to a highly electronegative atom (F, O, or N) being attracted to an electron pair on an adjacent F, O, or N atom in another molecule.

Ion-Dipole Forces

Forces found in mixtures containing both ionic compounds and polar compounds, where the full charge of an ion interacts with the permanent dipole of a polar molecule.

Nonpolar covalent bond

A covalent bond characterized by an equal sharing of bonding electrons between two atoms with similar electronegativities, resulting in no significant partial charges.

Polar covalent bond

A covalent bond involving unequal sharing of bonding electrons between atoms with differing electronegativities, leading to the formation of partial positive ($\delta+$) and partial negative ($\delta-$) charges within the bond.

Ionic bond

A bond involving the complete transfer of one or more valence electrons from one atom to another, creating fully charged ions.

Electronegativity

A measure of an atom's ability to attract shared electrons in a covalent bond.