The States of Matter

1. The States of Matter Chapter 16

2. Kinetic Theory Explanation of how particles in matter behave.

3. Kinetic Theory Assumptions All matter made of small particles. Particles are in constant, random motion. Particles collide with each other and the walls of the container. (Energy lost by particles during their collisions)

4. Characteristics of Solids Definite shape. Definite volume. Slow moving. Not enough kinetic energy to overcome their attractive forces to flow.

5. Solids Crystalline- geometric shape (snow flakes) Amorphous- no shape (glass and plastic)

6. Let’s see a solid at a molecular Level!

7. Crystalline structure of a solid What kind of shape is a grain of salt? Look at a grain of salt under a magnifying glass. What shape is the salt? Are all salt grains this shape? Why do you think they are this shape?

8. Liquids Indefinite shape. Definite volume. Medium speed. Flow because there is enough kinetic energy for the particles to overcome their attractive forces.

9. Lets see a liquid at the molecular level! http://www.harcourtschool.com/activity/states_of_matter/

10. Gases Indefinite shape. Indefinite volume. Greatest kinetic energy (enough to overcome the attractive forces completely).

11. Lets see a Gas at a molecular level!

12. Animations of Phases… http://mutuslab.cs.uwindsor.ca/schurko/animations/phasescontainers/phasescontainer.html

14. Melting Point The point where a solid begins to liquefy. The amount of energy needed to change a solid to a liquid is called the Heat of Fusion.

15. Vaporization When a liquid becomes a gas. The amount of energy needed to make a liquid become a gas at its boiling point is called the Heat of Vaporization.

16. 2 Types of Vaporization Evaporation Boiling Actually is a third type called sublimation (solid into gas--skips liquid phase).

17. At A and C, the temperature is rising because the kinetic energy is increasing. At B and D, energy is being used to overcome the particle bonds, no increase in temperature.

18. Viscosity Another property of a fluid that determines its tendency to flow (how “thick” it is). Soda vs. toothpaste

19. Diffusion Spreading of particles throughout a given volume until they are uniformly spread.

20. Plasma Consists of positively and negatively charged particles. Indefinite volume and shape. Found in stars, auroras, lightning bolts, neon and fluorescent tubes. MOST abundant state of matter in the universe.

21. Thermal Expansion An increase in the size of a substance when its temperature is increased. Occurs in solids, liquids, and gases. Water is an exception!

22. Lesson 16.2 Properties of Fluids

23. Fluids All gases and liquids are fluids because they flow.

24. Buoyancy Ability of a fluid to exert an upward force on an object immersed in it. Buoyant force = object weight, object will float Buoyant force less than object’s weight, object will sink

25. Archimedes’ Principle The buoyant force on an object is equal to the weight of the fluid that is displaced by the object. An object will float as long as the weight of the fluid being displaced is greater than or equal to the weight of the object.

26. Density Mass per unit volume An object with a density less than the fluid it is in will float.

27. Pascal’s Principle Pressure is force per unit area. Principle: Pressure applied to a fluid is transmitted unchanged through the fluid.

28. Bernoulli’s Principle As the velocity of a fluid increases, the pressure decreases.

29. Lesson 16.3 Behavior of gases

30. Boyle’s Law As the pressure on a gas increases, the volume will decrease, provided that the temperature stays the same.

31. Charles’s Law The volume of a gas will increase with increasing temperature provided that the pressure stays the same.