Kinetic Molecular Theory and Properties of Matter

These flashcards cover key concepts, terms, and definitions related to Kinetic Molecular Theory, states of matter, intermolecular forces, physical properties of liquids, solids, solutions, concentration units, and important formulas.

Kinetic Molecular Theory (KMT)

A theory stating that matter is made up of tiny particles in constant random motion.

Compressibility

The ability of a substance to decrease in volume under pressure; gases are the easiest to compress.

Phase

A homogeneous, physically distinct, and uniform part of a system.

Intermolecular Forces (IMF)

Forces between molecules that are weaker than intramolecular forces.

Intramolecular Forces

Forces within a molecule, such as chemical bonds.

London Dispersion Force

The weakest intermolecular force, present in all molecules, dominant in nonpolar molecules.

Dipole–Dipole Force

An intermolecular force that occurs between polar molecules.

Hydrogen Bonding

A strong intermolecular force that occurs when hydrogen is bonded to nitrogen, oxygen, or fluorine.

Ion–Dipole Force

An intermolecular force between ions and polar molecules, such as salt in water.

Boiling Point

The temperature at which a liquid becomes gas; higher intermolecular forces result in a higher boiling point.

Surface Tension

A measure of the elastic force at the surface of a liquid, affected by intermolecular forces.

Viscosity

A measure of a fluid's resistance to flow; higher intermolecular forces result in higher viscosity.

Cohesion

The attraction between molecules of the same substance.

Adhesion

The attraction between molecules of different substances.

Crystalline Solids

Solids with a definite crystal lattice and sharp melting points, such as salt and ice.

Amorphous Solids

Solids without a definite shape or melting point that break unpredictably, such as glass.

Solution

A homogeneous mixture that exists in one phase.

Solvent

The substance present in greater amount in a solution.

Solute

The substance present in lesser amount in a solution.

Molarity (M)

A concentration unit defined as moles of solute per liter of solution.

Molality (m)

A concentration unit defined as moles of solute per kilogram of solvent.

Mole Fraction

The ratio of moles of a component to the total moles in a solution.