Phase Changes
Solid to liquid
melting
P1xV1=P2xV2
Boyle‘s Law
Inter Forces
across multiple
Higher in liquids because particles are held together
Density
A solid who’s atoms, ions, or molecules are arranged in an order, geometric, 3d lattice
Crystalline Solids
Liquid to solid
freezing
V1/T1=V2/T2
Charle’s Law
Within
Requires enormous pressure, produces volume change
Compression
the temperature at which a crystalline solid becomes a liquid
melting point
Liquid to gas
evaporation
P1/T1=P2/T2
Gay-Lussac’s Law
Weak forces that result from temporary shifts in the density of electrons in electron clouds
Dispersion Forces
Less fluid than gases
Fluidity
The temperature at which a liquid changes to a gas
Boiling point
Gas to liquid
condensation
P1xV1/T1=P2xV2/T2
Combined Gas Law
Attractions between oppositely charged regions of polar molecules
dipol-dipole forces
Inward pull of particles
surface tension
A measure of the average kinetic energy
Temperature
Solid to gas
sublimation
PV=nRT
Ideal Gas Law
A special type of dipole-dipole attraction that occurs between molecules containing Hydrogen
Hydrogen Bonds
Movement up a narrow glass tube.
Capillary Action
no kinetic energy is lost when gas particles collide with each other or with the walls of their container
Elastic