1. Solid phase (s): Strong attractive forces hold particles in fixed location. Regular definite geometric shape; crystalline Liquid phase (l): Particles have mobility; sufficient attractive forces to give liquids a definite volume. Gaseous phase (g): Particles have minimal attractive forces holding them together. No definite volume or shape.
States of Matter

2. Aim: How can one interpret the heating curve for a substance?
The structure and arrangement of particles and their interactions determine the physical state of a substance at a given temperature and pressure.
The three phases of matter (solids, liquids, and gases) have different properties.

3. Vocabulary
Temperature: A measure of the average kinetic energy of its particles. (°C or K)
Heat: a measure of the amount of energy transferred from one substance to another. (J)
Heat of fusion: The amount of heat needed to convert a unit mass of a substance from solid to liquid at its melting point. (Hf)
Heat of vaporization: The amount of heat needed to convert a unit mass of a substance from its liquid phase to its vapor phase at constant temperature. (Hv)

4. Phase Changes
Fusion: Melting; when particles have enough potential energy to break foa’s holding them together.
Freezing: liquid to solid (solidification)
Vaporization: Boiling; When particles have enough kinetic energy to enter the gas phase.
Condensation: gas to liquid
Sublimation: solid to gas
Deposition: gas to solid