1. Chapter 16: Solids, Liquids, and Gases

2. Chapter 16 Overview Kinetic Theory A. States of Matter 1. Solids
2. Liquid
a. Melting point
b. Heat of Fusion
3. Gas
a. Boiling Point
b. Heat of Vaporization
4. Plasma
B. Thermal Expansion
Behavior of Gases
A. Pressure - pascal
B. Boyle’s Law
C. Charles’s Law

3. Kinetic Theory explanation of how particles in matter behave
All matter is composed of small particles.
These particles are in constant, random motion.
These particles are colliding with each other and the walls of their container.

4. Phases of Matter Phases The arrangement of particles
Motion of molecules
Definite shape?
Definite volume?
Solid
Packed tightly and
vibrate in place
Yes
Liquid
Able to slide past each other No
take the shape of the container
Gas
Bounce far apart

5. Phase Changes Phase Changes
From what Phase-to-Phase does change occur?
Point at which Phase Change occurs
Melting
Solid to Liquid
Melting point
Freezing
Liquid to Solid
Freezing point
Vaporization
Liquid to Gas
Boiling point
Condensation
Gas to Liquid
Condensation point
Sublimation
Solid to Gas
Sublimation point

6. Phase Change Diagram Heat of vaporization Heat of fusion Gas Liquid
Heat of Fusion: energy require to change a solid to a liquid
*heat absorbed
*no change in temp.
Heat of Vaporization: energy require to change a liquid to a gas
Gas
Heat of vaporization
Liquid
Heat of fusion
Solid

7. Thermal Expansion
Increase in the size of a substance when temperature increases.
Exception to the rule: WATER
Water expands as it cools.
Structure of Water

8. Gas Laws: Boyle’s, Charles’s, Gay-Lussac’s
Phases
Special Properties
Solid
*Crystals: particles are in regular repeating patterns
*Amorphous: solids that don’t have highly ordered structure like crystals – “without form”
Liquid
Viscosity: resistance to flow
Liquid crystals: start to flow during
melting phase but don’t lose all their
geometric order
Gas
Gas Laws: Boyle’s, Charles’s, Gay-Lussac’s

9. Gas Laws show relationship between pressure, temperature, and volume
Explanation
Boyle’s
As volume decreases, pressure increases.
Charles‘s
As temperature increases, volume increases.
Gay-Lussac’s
As temperature increases, pressure increases.

10. Which Gas Law is this?

11. Which Gas Law is this?

12. Graphing: Phase Changes

13. Lab: Four States of Matter Corrections to Lab Procedure:
1.            Put 5 ice cubes in a 150 mL beaker.
2.          Observe temperature every minute.
3.          Take 2 readings before putting beaker on hot plate.
4.          Put hot plate on medium until ice has completely melted
5.          Once ice has melted turn hot plate up to high.
6.          After boiling occurs, continue to record temperatures
every 1 minute for 2 minutes.

14. Lab: Pop Can and Gas Laws
Procedure:
1. Pour 5 mL of water into the pop can.
2. Put pop can on hot plate. Let it boil for 1 minute.
3. With tongs, put pop can upside down in beaker of COLD water.
Observations: (Describe what happened.)
Gas Law: (What Gas Law does this apply to?)
Conclusion: (Explain why the can behaved as it did according to the Gas Law.)

15. Lab: Gas Pressure and Volume