1. States of Matter Ch

2. Solids Have an orderly arrangement and fixed location of particles
Particles “vibrate” in place, so they do not flow
When heat (energy) is added, particles “vibrate” faster and begin to spread apart (melt)
Most are crystalline (rigid), some are amorphous (lack an internal structure)
Examples of amorphous solids: rubber, glass

3. Liquids
Intermolecular attractions reduce movement of particles (more dense than gas)
Vaporization: turning liquid to gas
Evaporation: surface particles only
Is a cooling process (sweat)
Boiling: particles throughout liquid
Vapor pressure = atmospheric pressure (BP)
Higher altitudes=lower bp

4. Gases
Kinetic Theory:
Particles are small, hard spheres with an insignificant volume
Most of particles is rapid, constant, and random
All collisions are perfectly elastic (energy is transferred without loss)
Gas Pressure: caused by collisions with an object
SI unit: pascal (Pa)
Standard Pressure: 1 atm = 760 mmHg = kPa