General Chemistry 2: Intermolecular Forces and States of Matter

A set of vocabulary flashcards to help review key concepts about intermolecular forces and the properties of liquids and solids as discussed in General Chemistry 2.

Kinetic Molecular Model

A model that describes the behavior of molecules in liquids and solids, emphasizing the proximity of molecules and the strength of attractive forces among them.

Intermolecular Forces

Attractive forces between two molecules that are weaker than ionic and covalent bonds, acting at short-range distances.

London Dispersion Force (LDF)

The weakest intermolecular force arising from temporary changes in electron density, causing temporary dipoles in adjacent atoms.

Dipole-Dipole Force (DDF)

An intermolecular force resulting from the electrostatic interaction between molecules that have permanent dipoles.

Hydrogen Bond

A strong type of dipole-dipole force occurring when hydrogen is bonded to highly electronegative atoms like fluorine, oxygen, or nitrogen.

Ion-Dipole Force

An attractive force between an ion (cation or anion) and a polar molecule, dependent on the magnitude of the ion's charge and the net dipole moment of the polar molecule.

Compressibility

The measure of how much the volume of a substance decreases under pressure; gases are highly compressible while liquids and solids are less so.

Density in States of Matter

A measure of mass per volume; solids have higher densities than liquids, which in turn have higher densities than gases.

Phase

A state of matter that has uniform composition and appearance; examples are solid, liquid, and gas.

Condensed Phases

Phases of matter (liquids and solids) where molecules are close together, leading to significant attractive forces.