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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).
