Unit 3: Intermolecular Forces (IMF) and Properties (Simple Studies AP Chem Study Guide)

based on the unit 3 guide from https://www.simplestudies.org/groups/ap-chemistry

Amorphous Solids

Solids with particles that do not have a repeating lattice form, lacking a set melting point.

Barometer

An instrument used to measure atmospheric pressure.

Boiling

The process where bubbles are formed as liquid particles vaporize within the liquid.

Condensation

The process of a substance changing from a gas to a liquid.

Deposition

A phase change in which a substance changes directly from a gas to a solid.

Equilibrium

A state where trapped molecules reach a balance between evaporation and condensation.

Evaporation

When surface molecules gain enough energy to overcome intermolecular forces and change from liquid to gas.

Ionic Solids

Crystals composed of cations and anions; they are hard and brittle due to strong ionic bonds.

Intermolecular Attractions

Forces that determine the attraction between molecules.

Kinetic Molecular Theory

Theory stating that particles of matter are always in motion.

Melting Point

The temperature at which a solid becomes a liquid; equal to its freezing point.

Metallic Solids

Solids where electron clouds overlap, allowing free movement of electrons, highly conductive of heat and electricity.

Molecular Solids

Solids formed by covalently bonded molecules held together by weak intermolecular forces.

Network Covalent

A solid structure where atoms are bonded in a continuous network, resulting in hard, brittle crystals.

Phase Change

A transformation in the arrangement of molecules at constant temperature.

Pressure

The force exerted by gas particles when they collide with the walls of their container.

Temperature

The average kinetic energy of particles in a substance.

Sublimation

The transition of a substance directly from solid to gas without passing through the liquid phase.

Standard Atmosphere (atm)

A unit of pressure equivalent to 760 mm Hg.

Surface Tension

The tendency of liquids to minimize their surface area due to intermolecular interactions.

Volatility

A measure of how readily a substance vaporizes, influenced by temperature and intermolecular forces.

London Dispersion Forces

Weak intermolecular attractions caused by temporary polarities in molecules.

Dipole-Dipole Attractions

Forces that occur between polar molecules due to the attraction between positive and negative ends.

Hydrogen Bonds

Strong dipole attractions that occur when hydrogen bonds with highly electronegative atoms like F, O, or N.

Boyle's Law

P1V1 = P2V2 (Pressure is inversely proportional to volume at constant temperature).

Charles's Law

V1/T1 = V2/T2 (Volume is directly proportional to temperature at constant pressure).

Gay-Lussac's Law

P1/T1 = P2/T2 (Pressure is directly proportional to temperature at constant volume).

Combined Gas Law

(P1V1)/T1 = (P2V2)/T2 (Relates pressure, volume, and temperature variables for a gas).

Ideal Gas Law

PV = nRT (Relates pressure, volume, temperature, and amount of gas).

Dalton's Law of Partial Pressures

Ptotal = P1 + P2 + P3 + ... (Total pressure equals the sum of the individual partial pressures of a mixture of gases).