1. States of Matter Chapter 3 Section 1 states of matter
Section 2 behavior of gases
Section 3 changes of state

2. The Four States of Matter
Your textbook states that there are three states of matter but you will be responsible for learning about four states of matter…I am throwing in the 5th state just so you can dazzle your high school science teacher!
Solids
Liquids
Gases
Plasma

3. STATES OF MATTER Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles

4. Matter Matter is made of tiny particles.
Atoms - single element
Molecules -more than 1 type of element
Atoms and molecules are always in a state of motion (much like the St. Ann students) and are always bumping into each other

5. STATES OF MATTER SOLIDS
Particles of solids are tightly packed, vibrating about a fixed position.
Solids have a definite shape and a definite volume.
Heat

6. Solids Solids Definite Shape Definite Volume
Particles vibrate in fixed positions
Particles have low kinetic energy

7. Two Types of Solid Matter
Crystalline Solids
Long-range order
Repeating patterns
Think back to the 6 different crystalline structures you learned in the 6th grade
Ex. Iron, diamond, ice
Amorphous Solids
No long range order
Polymers, glass
Ex. Glass, rubber, wax
Sodium Chloride

8. STATES OF MATTER LIQUID
Particles of liquids are tightly packed, but are far enough apart to slide over one another.
Liquids have an indefinite shape and a definite volume.
Heat

9. Liquids Variable shape (takes the shape of the container)
Definite Volume
Particles can move around each other
Particles have medium Kinetic Energy

10. Unique characteristics of liquids
Surface tension- a force that acts on particles at the surface of a liquid
Remember the penny lab at the beginning of the year
Water has a high surface tension so forms droplets. Gas has a low surface tension and forms flat drops
Viscosity- liquid’s resistance to flow
Higher the attraction between the molecules, the more viscous the liquid
Think about pouring water vs honey

11. STATES OF MATTER GAS
Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite volume.
Heat

12. Gases Variable shape Variable volume (fills all space in a container)
Particles move about freely
Particles have high Kinetic Energy

13. Classifying Matter According to its State: Solid, Liquid, Gas
Water can exist as a solid, liquid or gas

14. Will everything just be a gas?
But what happens if you raise the temperature to super-high levels… between 1000°C and 1,000,000,000°C ?
Will everything just be a gas?

15. PLASMA NO! The 4th state of matter:
If the gas is made up of particles which carry an electric charge (“ionized particles”), but the entire gas as a whole has no electric charge, and if the density is not too high, then we can get
The 4th state of matter:
PLASMA

16. STATES OF MATTER 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
common state
of matter

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

18. 2. Lightning

19. 3. Aurora (Northern Lights)

20. 4. Neon lights

21. 5. Stars
Stars make up 99% of the total matter in the Universe. Therefore, 99% of everything that exists in the entire Universe is in the plasma state.

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

23. 6. Clouds of gas and dust around stars

24. 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

25. Will everything just be a frozen solid?
But now what happens if you lower the temperature way, way, down to 100 nano degrees above “Absolute Zero” (-273°C)
Will everything just be a frozen solid?

26. Not Necessarily!
In 1924 (82 years ago), two scientists, Albert Einstein and Satyendra Bose predicted a 5th state of matter which would occur at very very low temperatures.
Einstein
Bose +

27. Ketterle and his students
Finally, in 1995 (only 12 years ago!), Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time.
Ketterle and his students
The 5th state of matter:
Bose-Einstein Condensate
This 5th state of matter will not be on any St. Ann test but you will dazzle your high school science teacher if you know that a 5th state has been discovered!

28. To really understand Bose-Einstein condensate you need to know
Quantum Physics

29. In 2002, Ketterle and two other scientists received the highest award in science for discovering Bose-Einstein condensate:
The Nobel Prize

30. The five states of matter:
PLASMAS (only for low density ionized gases)
BOSE-EINSTEIN CONDENSATE
LIQUIDS
SOLIDS
GASES
Lower Temperature
Higher Temperature

31. Kinetic Theory Kinetic energy = energy an object has due to its motion
The faster an object is moving; the greater its kinetic energy.
Kinetic theory states that all particles of matter are in constant motion.

32. Classifying Matter According to its State: Kinetic Theory

33. 3-2 Behavior of Gases What's the Matter?
The three main states of matter that we meet daily are: gas, liquid, and solid.
Gases can be compressed, they expand to fill their containers. The volume of a gas is variable

34. In this room right now are millions of gas molecules and atoms colliding with the walls, the floor, your face and each other.
Can you feel it?

35. Pressure One property of gases is that they exert pressure.
The pressure exerted by the gas mixture we call air is called atmospheric pressure.
The atmosphere that surrounds Earth is a sea of air. It exerts a force on the surface of the planet.
Above you is a column of air that is exerting a force on you.
This pressure can be measured.
But why is air exerting pressure?

36. Pressure Pressure = the result of force distributed over an area
In a closed container, gases exert pressure when the particles of the gas collide with the walls of the container.

37. Compressibility Solids are incompressible Gases are compressible
Liquids are very slightly compressible – usually considered incompressible

38. Factors That Affect Gas Pressure
Temperature – raising temp. will increase pressure if volume of gas and # of particles are kept constant
Inc. in temp.  part. move faster  part. collide with walls more frequently  increased pressure

39. Volume – Decreasing volume of a gas causes an increase in pressure if the temp. and # of part. are constant
Decrease in vol.  less space  particles collide with walls more often  inc. pressure

40. Number of particles – increasing the number of particles of a gas will increase pressure if temp. and volume are constant
Inc. # of particles  particles collide with container more often  inc. pressure

41. Why is air pressure important?
Feel the pressure!!
Why is air pressure important?
It causes wind
Creates clouds and clear skies
Allows us to predict the weather

42. P1V1 = P2V2 Pressure and Volume Boyles Law
The volume of a gas is inversely proportional to its pressure
P1V1 = P2V2

43. Pressure and Volume: Boyles Law
Irish scientist Robert Boyle experimented with the relationship between pressure and volume of gases.
He set-up a J-shaped tube and added mercury to see what it did to the volume of a trapped gas.
As pressure increased volume decreases.

44. Pressure and Volume Boyles Law
If the volume is increased the gas particles collide with the walls of the container less often and the pressure is reduced.

45. Boyle’s Law

46. Boyle’s Law (temp constant)
A decrease in the volume of gas will result in an increase in pressure
An increase in the volume of gas will result in a decrease in pressure
V1P1 = V2P2

48. Volume and Temperature: Charles's Law
French physicist Jacques Charles was the first to fill a balloon with hydrogen gas and make a solo flight.
He showed that the volume of a gas increases when the temperature increases (at a constant pressure)

49. Volume and Temperature Charles’s Law
The volume of a gas is directly proportional to its Kelvin temperature at constant pressure V2 V1 = T1 T2

50. Charles’ Law

51. Charles’s Law pressure constant
Volume of a gas increases with increasing temperature
Volume of a gas decreases with decreasing temperature
V1 = V2
T T2

53. Principle- Use Boyles (temperature constant) Squeezing a balloon
Charles (pressure constant)
Why balloons decrease in size when kept in a cold room
Reason for statement on hair spray: “keep away from heat, contents under pressure”

54. Websites for additional help

55. 3-3 Changes of State
What would it take for matter to move from one state to another?

56. Melting and Freezing Melting Solid changes to liquid
Particles absorb energy (endothermic)
Particles become less orderly

57. Freezing Liquid changes to solid Particles release energy (exothermic)
Particles become more orderly

58. Vaporization and Condensation
Liquid changes into a gas
Particles absorb energy (endothermic)
Particles become LESS orderly and more free to move
2 types of vaporization
Evaporation – takes place at the surface of a liquid
Boiling – occurs when a liquid is heated to its boiling point

59. Condensation Gas changes to a liquid
Particles release or lose energy (exothermic)
Particles become MORE orderly

60. Sublimation and Deposition
Changing from a solid
directly to a gas
Energy is absorbed
(endothermic)
Deposition
Changing from a gas directly to a solid
Energy is released (exothermic)

61. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to liquid
Melting
Heat goes into the solid as it melts.
Liquid to solid
Freezing
Heat leaves the liquid as it freezes.

62. Description of Phase Change
PHASE CHANGES
Description of Phase Change
Term for Phase Change
Heat Movement During
Phase Change
Liquid to gas
Vaporization, which includes boiling and evaporation
Heat goes into the liquid as it vaporizes.
Gas to liquid
Condensation
Heat leaves the gas as it condenses.
Solid to gas
Sublimation
Heat goes into the solid as it sublimates.

63. Phase Changes Melting Going from Solid to Liquid Freezing
Going from Liquid to Solid
Vaporization
Going from Liquid to Gas
Condensation
Going from Gas to Liquid
Sublimation
Going from Solid to Gas

65. Phase Change Diagram