1. It’s what the world is made of.
Matter:
It’s what the world is made of.
Here are some notes

2. What is matter?
Matter is anything that has mass and takes up space.

3. States of Matter
A. The Kinetic Theory
1. All matter is composed of small particles (atoms, molecules, or ions).
2. They are in constant, random motion.
3. They constantly collide with each other and with the walls of their container.

4. Classification Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles

5. Solid

6. Solids Solids have definite shape and definite volume.
Solids have mass.
Solids take up space.
Do not take the shape of the container in which it’s placed

7. Particles in Solids: Are packed tightly together
Have very little energy
Vibrate in place

8. Liquid

9. Liquids
Liquids take the shape of their container and have definite volume.
Liquids have mass.
Liquids take up space.

10. Particles in Liquids: Are loosely packed
Have medium energy levels and particles flow around each other but they don’t have enough energy to move far apart

11. Gas

12. Gases
Gases spread out to fill the entire space given and do not have definite volume.
Gases have mass.
Gases take up space.

13. Particles in Gases:
Move freely
Have LOTS of energy

14. Particle Properties Phase Distance Energy Motion Shape Volume Solid
Tight
Little
Vibrates
Definite
Liquid
Close
Moderate
Sliding
Indefinite
Gas
Far apart
A lot
Free

15. Activity: States of Matter
Slide 125 / 166
Activity: States of Matter
"Watch different types of molecules form a solid, liquid, or gas.
Add or remove heat and watch the phase change!"
Click the picture above to access the web activity.

16. Plasma Lightning is a plasma.
Used in fluorescent light bulbs and Neon lights.
Plasma is a lot like a gas, but the particles are electrically charged.

17. PLASMA A plasma is an ionized gas.
A plasma is a very good conductor of electricity and is affected by magnetic fields.
Plasmas, like gases have an indefinite shape and an indefinite volume.
Plasma is the most common state of matter

18. STATES OF MATTER LIQUID PLASMA SOLID GAS
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place
Close together with no regular arrangement.
Vibrate, move about, and slide past each other
Well separated with no regular arrangement.
Vibrate and move freely at high speeds
Has no definite volume or shape and is composed of electrical charged particles

19. Some places where plasmas are found…
1. Flames

20. 2. Lightning

21. 3. Aurora (Northern Lights)

22. The Sun is an example of a star in its plasma state

24. What would it take for matter to move from one state to another?
STATES of matter?
What would it take for matter to move from one state to another?

25. Energy determines the state!

26. Add or Subtract Energy. . .
When energy is added, endothermic, particles move faster!
When energy is taken away, exothermic, particles move slower!

27. Energy Transfer
Heat – Transfer of thermal energy between substances that are at different temperatures. Always transfers from warmer substance to cooler substance.
Endothermic – process or reaction in which the system absorbs energy from the surroundings in the form of heat (object gets hotter)
Exothermic- process or reaction in which the system releases energy into the surroundings in the form of heat (object gets colder)

28. Phase Changes
Melting
Freezing
Vaporization
Condensation
Sublimation
Deposition

29. Melting The change from solid to liquid
When a solid gains heat or energy, molecules move father apart
Endothermic change

30. Freezing The change from liquid to solid
When a liquid loses heat energy, molecules move closer together
Exothermic change
Sub Zero

31. Vaporization The Change from a liquid to a gas
Liquid gains heat or energy - endothermic
Evaporation
Vaporization at the surface of a liquid

32. Condensation The change of a substance from a gas or vapor to a liquid
Gas loses heat or energy - exothermic

33. Sublimation
To change phase from a solid to gas without becoming a liquid – endothermic change

34. Deposition
To change phase from a gas to a solid without becoming a liquid – exothermic change
When water vapor touches something below its freezing point, it changes from a gas to a solid

35. Deposition
Sublimation

36. Deposition

37. Kinetic Molecular Model of Water
At 100°C, water becomes water vapor, a gas. Molecules can move randomly over large distances.
Between 0°C and 100 °C, water is a liquid. In the liquid state, water molecules are close together, but can move about freely.
Below 0°C, water solidifies to become ice. In the solid state, water molecules are held together in a rigid structure.

38. Endothermic Exothermic
Energy must be added to cause melting or evaporation
Energy is transferred in all changes of state
Phase Diagram
Segment A demonstrates the increase of heat causing increasing vibration. Segment B demonstrates the increase in heat energy without a corresponding rise in temperature until the phase change is complete. Segment C has the temperature rising again and the liquid particles moving faster, but not fast enough to change state. Segment D demonstrates again an increase in heat energy without a corresponding rise in temperature until the phase change is complete. Phase changes are accompanied by increases in heat energy but not by increases in temperature. The heat energy that is absorbed is used to overcome forces that hold the particles of the substance together.
Evaporation can regulate body temperature Cool a restaurant patio and Dry the side walk after a spring shower.

39. Melting Point Temperature at which a solid changes to a liquid.
Aluminum M.P. = 660ºC
0ºC for water at sea level

40. Freezing Point Temperature at which a liquid changes to a solid
Water F.P. = 0ºC at sea level

41. Boiling Point Temperature a liquid boils at.
B.P. of a liquid is related to pressure above it.
Water BP = 100ºC
Table Salt BP = 1413ºC
Diamond BP = 4200ºC
the temperature at which a liquid becomes a gas below the surface At high altitudes liquids boil at lower temperatures

42. Graphing a Phase Change

43. Conservation of Matter
Law of
Conservation of Matter
There is no observable change in the quantity of matter during a chemical reaction or a physical change.
In other words, matter cannot be created nor destroyed. It is just converted from one form to another
Definition of Conservation of matter.