1. http://www.harcourtschool.com/ac tivity/states_of_matter/
Section 16.1
tivity/states_of_matter/ 1

2. Physical Change 2 IDENTITY DOES NOT CHANGE!!
a change in size, shape, or state of matter
All phase changes are physical changes!!
may or may not involve energy changes and color changes 2

4. Distillation
Separating a mixture through evaporating a liquid and re- condensing its vapor.
Vapors from the liquid with the lowest boiling point form first and are condensed and collected 4

5. 5

6. Chemical Change
change in identity-
changes the COMPOUND or SUBSTANCE

7. Kinetic Theory Explains how particles in matter behave
All matter is composed of small particles
Particles are in constant random motion
Particles collide with each other and the walls of their containers constantly
Produces pressure 7

8. Kinetic energy Total energy of a material’s Particles
causes the particles to vibrate
KE - energy of motion
Low KE in solids
High KE in gases
Higher temperatures- more vibration 8

9. Average KE = Temperature Of a substance
or how fast the particles are moving
Lower in Solids,  Higher in Liquids  Highest in Gases 9

10. -273 ˚C Particle Motion Only temp at which No particle motion
Absolute zero
0 K (kelvin)
-273 ˚C 10

11. 11

12. Solids
particles have strong attraction for each other, preventing motion – held in rigid structure
Particles are closely arranged in a specific type of geometric arrangement
Crystal structure
definite shape and volume 12

13. Solids- particles are closely packed
Geometric arrangement of particles in a solid- determines chemical & physical properties of a solid
Solids- particles are closely packed 13

14. Melting Different solids melt in different ways:
Amorphous -solid that softens and gradually turns into a liquid over a large temperature range – don’t form crystals
Ex. Glass, rubber, cotton candy, plastic, Coal 14

15. 15

16. Crystalline solids- have set geometric structure-melt at a set temperature
Water, NaCl (table salt), Diamond, Graphite, Sugar 16

17. 17

18. Liquids Indefinite shape Definite volume
Take the shape of their container 18

19. Liquids
Particles have more space between them allowing them to Flow and take the shape of their container.
Particles of a liquid have more KE than particles of a solid 19

20. Buoyancy
The ability of a fluid (liquid or a gas) to exert an upward force on an object immersed in it
The 2 forces acting on any object in a fluid are Weight Force and Buoyant Force 20

21. Buoyant force is equal to the object’s weight
When object FLOATS
Buoyant force is equal to the object’s weight 21

22. Viscosity
A Fluid’s resistance to flow 22

23. Viscosity is different for different fluids because structure of fluids differs
If moving particles don’t pull others into motion, liquid has high viscosity (slow flowing) 23

24. If moving particles do pull others into motion, liquid has low viscosity (flow easily)24

25. How does Temperature affect Viscosity?
Viscosity is greater when the substance is Cold
particles move slower and transfer energy slower
Ex. Syrup that’s Cold vs. micro-waved syrup 25

26. Gas
particles have enough energy that they have escaped the attractive forces that held them in liquid state 26

27. Gas Indefinite volume and indefinite shape
Takes shape and volume of container 27

28. Particle Motion - Gas
Particles of a gas- have enough KE to overcome the attractions between them completely
Spread and fill the container completely 28

29. Diffusion-spreading of particles throughout a container until they are uniformly distributed29

30. 30

31. Plasma
Gas-like state of matter consisting of positive and negative particles
Most common state of matter in universe 31

32. Changes in State of matter
Also called phase changes.
All are physical changes!!!

33. From solid to liquid in solids, particles move slowly
Heat is added- particles move faster
When have enough KE (moving fast enough), they overcome the attractive forces between the particles and escape the solid 33

34. Liquid State A solid begins to liquefy at the Melting Point-
temperature at which a solid begins to liquefy.
As the particles gain enough energy to over come their ordered arrangement
Liquid State 34

35. At what temperature does water freeze
At what temperature does water freeze? At what temperature does water melt?
The temperature at which a substance melts  Melting point, is the same as the temperature at which it freezes
Melting pt. = Freezing pt.

36. Liquid to gas
Some particles of a liquid move faster than others and escape the attractive forces of other particles- allows them to enter the gas phase
Call this Evaporation
Can occur below its BP 36

37. Boiling- the Temp. at which the Pressure of a vapor in the liquid is equal to the external Pressure acting on the surface of the liquid 37

38. 38

39. Boiling pt and Pressure
Lower external pressure like on a mountain means lower boiling point
Higher external pressure like at sea level means higher boiling point 39

40. 40

41. What is sublimation? When a substance skips the liquid state.
Goes straight from a solid to a gas
Ex. Dry Ice

42. THERMAL EXPANSION
Increase in the size of a substance with the temperature increases.
Size of substance will decrease when temp decreases
Expansion and Contraction occur in most Solids, Liquids and Gases 42

44. For Example: Thermometers
energy is added
particles of the liquid move faster & farther apart
forces fluid upward through the thermometer 44

45. higher temperature = expansion = lower density = rises
Hot air balloons rise
higher temperature = expansion = lower density = rises 45

46. Analyzing Heating Curves

47. Heating Curve D E C B A
A- SOLID is being heated- energy is used to increase temperature
It is still a solid, just getting hotter or colder. 47

48. D E C B A
B- Phase Change- heat of fusion - melting point – energy is used to overcome attractions b/w particles 48

49. Heat of fusion-
the amount of energy required to change a substance from the solid phase to the liquid phase at its melting point 49

50. Substance is still a liquid only getting hotter or colder
C-liquid is heated up- heat energy is used to increase temperature of liquid
Substance is still a liquid only getting hotter or colder 50

51. D E C B A
D- Phase change (liq to gas- heat of vaporization- boiling point- energy is used to overcome attractions 51

52. Heat of vaporization- amount of energy required to overcome the pressure at the surface of the liquid  Liquid to a Gas
Energy needed to boil
Phase change from Liquid to Vapor 52

53. D E C B A
E – vapor or gas is being heated- energy is used to increase temperature of Vapor 53

54. Water- Essential to Life on Earth!!
Has “+” and “–” regions
Decrease in temperature-particles get closer together
“-” from one particle attracts to “+” of other molecule
Most Dense at 4 °C 54

55. Water Empty spaces in ice are greater than those in water
Ice is less dense than water
Different from all other substances  Water expands from liquid to solid! 55

56. Why might this occur??

57. 57