1. Unit 4 Section 2 Notes
Matter and Energy

2. Kinetic Theory of Matter:
Useful for seeing differences in the 3 common states of matter on earth: solid, liquid, and gas.

3. Kinetic Theory of Matter 3 Main Points
All matter is made of atoms and molecules which act like tiny particles that are always in motion.
The higher the temperature, the faster the particles move.
At the same temperature, heavier particles move slower than lighter particles.

4. Kinetic Theory
Using the Kinetic Theory of matter, explain why a balloon filled with helium goes flat faster than one filled with regular air.
According to the Kinetic Theory, at the same temperature, heavier particles move slower than lighter particles. Since oxygen & carbon dioxide are more massive than helium, they don’t escape out of the tiny microscopic holes as fast as helium.

6. Solids Solid: substances have a definite volume and definite shape.
Substances have a fixed position; no freedom to change positions
Particles are held closely together by strong chemical attractions
Definite melting point

7. Solids 2 Types of Solids:
Crystalline solids: particles have a regular, orderly arrangement; form a crystal lattice
Examples: salt (NaCl), sugar, diamond, quartz
Amorphous solids: particles don’t have a regular, orderly arrangement
Examples: rubber, glass

8. Crystal lattice

9. Diagram:

10. Liquid Liquid: substances have a definite volume but no definite shape
particles are closely packed, but can still slide past each other
Take the shape of their container
Particles are close but not as close as a solid
Particles can move randomly and spread on their own

11. Liquid
Diagram:

12. Viscosity: Viscosity: resistance of a fluid to flow
Determined by the attraction of particles: the stronger the attraction, the more viscous (thick) the liquid is.
Fluids with a high viscosity flow slowly, and fluids with a low viscosity flow quickly.
What is more viscous: apple juice or maple syrup?

13. Gas Gas: particles do not have a definite volume or shape.
Particles are in a constant state of motion and rarely stick together
Expand to fill available spaces
Free to spread in all directions from areas of high concentration to areas of low concentrations.
Example: scents of food or perfume
Have a low density

14. Gas
Diagram:

16. Gas Gases exert pressure
Pressure: force exerted per unit area of a substance
If there is too much pressure (too many helium particles) in a balloon, what happens?
A gas under pressure will escape the container if possible. Think about an air filled balloon that you let go.

17. Fluids Fluids: substances that can spread
Both liquids and gases can spread, so they are considered fluids.

18. States of Matter Video

19. Plasma
Plasma: does not have a definite shape or volume; considered to have the properties of fluids.
Most common state of matter in universe, but not on Earth
Makes up 99.9 % of the universe
Plasma is superheated gas and is a collection of free moving electrons and ions
Conducts electricity

20. Plasma Examples of natural plasma on earth: lightning fire
Aurora borealis
Artificial plasma on earth includes fluorescent lights

21. Energy Energy: the ability to change or move matter
Examples of energy or sources of energy:
heat, light, spring coiling, batteries
Energy must be added or removed to cause a change in state.

22. Energy Energy must be ADDED to melt or evaporate substances
Aluminum must be melted before it can be recycled
As aluminum particles gain heat, particles move faster and break away from fixed positions and become liquids: called melting

23. Energy
Energy must be RELEASED to make a gas become a liquid or solid again.
When H2O is a gas and molecules slow down the water vapor returns to a liquid (called condensation). When molecules slow down even more, the water goes to a solid (ice).

24. Energy Energy relationship between solid, liquid, and gas diagram:
Energy ABSORBED
Energy RELEASED

26. Important Note:
Changing the state of matter does NOT change the substance or mass.
Water, steam, and ice are all H2O: the only change is the nature of attraction between molecules

27. Phase Change Diagram: Solid Melting Sublimation Deposition Freezing
Condensation
Liquid
Gas
Vaporization

28. Phase Changes
Sublimation: change of a substance from a solid to a gas.
Deposition: change of a substance from a gas to a solid
Example: Water vapor without becoming liquid- this is how snow forms in clouds.

29. Atoms are constantly in motion.
As the temperature of an object increases,
The vibrations of atoms increases
The spacing of atoms increases
So, the volume of matter expands when the spacing increases.
A temperature increase results in a volume increase.

31. Law of Conservation of Mass
Law of Conservation of Mass states that Mass cannot be created or destroyed.
Example: Burning a match: consider what you start and end with.
Before Lab:

32. Trivia Question
Trivia Question: If mass cannot be created or destroyed, then why do we have to replace our tires when the rubber “wears away”?

33. Law of Conservation of Energy
Law of Conservation of Energy states that Energy cannot be created or destroyed.
Energy can be converted from one form to another.
Example: A wristwatch: from chemical energy to mechanical energy.