1. States of Matter

2. Kinetic Theory—an explanation of how particles in matter behave. 3 assumptions of kinetic theory: 1. All matter is made of small particles 2. Particles are in constant, random motion 3. Particles collide with each other & the walls of their container. Thermal Energy—total energy of a material’s particles Kinetic (particles move) & Potential Temperature is the average kinetic energy of particles or how fast particles move

3. Kinetic Theory & States of Matter Solid State The particles of a solid are closely packed together. Most solids have a specific geometric arrangement (crystal). Solids have a definite shape and volume.

4. Liquid State Melting point—the temp. that a solid begins to liquefy. Heat of Fusion—energy required to melt Particles have more KE than a solid—they move faster. Particles can slide past each other, so they flow. Have a definite volume, but no definite shape.

5. Gas State Boiling Point—temp. when a liquid becomes a gas Heat of Vaporization—energy required to change liquid to gas Gas particles have enough KE to overcome the attractions between them. Have no definite shape or volume. Diffusion—gas particles spread out to fill their container

6. States of Matter

7. Heating curve

8. Plasma State Plasma—positive and negative particles at very high temperatures. High temps force the electrons to be pulled off of atoms All stars consist of plasma. Plasma is also found in lightning, neon light tubes, and auroras.

10. Daniel Bernoulli

11. Bernoulli’s Principle Bernoulli’s Principle—as the velocity of a fluid increases, the pressure exerted by the fluid decreases. (Fluid can be liquid or gas) Describes how people could build a machine that flies Airplane wings were designed to reduce pressure above the wings.

12. Bernoulli’s Principle Bernoulli’s Principle explains why a shower curtain pushes in. Ping pong ball in waterPing pong ball in water

14. Gas Laws Boyle’s Law—when volume of a gas is decreased, pressure is increased (& vice versa) as long as temperature is constant. The equation for Boyle’s Law is P 1 V 1 = P 2 V 2 The subscript 1 is initial (or before), and the 2 is final (after) The unit for pressure is kilopascals (kPa) & the unit for volume is liters (L). http://www.youtube.com/watch?v=q6- oyxnkZC0 http://www.youtube.com/watch?v=q6- oyxnkZC0 Underwater balloon

15. Charles’ Law The volume of a gas increases as temperature increases (and vice versa) The equation for Charles’ Law is V 1 = V 2 T 1 T 2 Temperature must be in Kelvin. K = °C + 273

16. Temperature/Pressure Law The pressure of a gas increases as temperature increases (& vice versa) This is why you should keep pressurized spray canisters away from heat. P 1 = P 2 T 1 T 2 Temp must be in Kelvin again