1. Ch. 16 - Solids, Liquids, & Gases
MATTER
Ch Solids, Liquids, & Gases
I. States of Matter
Kinetic Molecular Theory
Four States of Matter
Thermal Expansion

2. A. Kinetic Molecular Theory
KMT
Tiny, constantly moving particles make up all matter.
The kinetic energy (motion) of these particles increases as temperature increases.
Temperature = AVERAGE kinetic energy of the particles in a system.
Heat = TOTAL kinetic energy of the particles.

3. B. Four States of Matter Solids
low KE - particles vibrate but can’t move around
definite shape & volume
crystalline - repeating geometric pattern (MOST solids)
amorphous - no pattern (e.g. glass, wax, obsidian) – it was frozen too fast to organize into crystals

4. B. Four States of Matter Liquids
higher KE - particles can move around but are still close together
indefinite shape
definite volume
Viscosity – resistance to flow.
Motor oil, syrup have high viscosity; water, gasoline lower viscosity
Heating the liquid reduces viscocity (warming syrup makes it flow easier)

5. B. Four States of Matter Gases
high KE (moving very fast) - particles can separate and move throughout container (99% empty space)
indefinite shape & volume

6. B. Four States of Matter Plasma
very high KE - particles collide with enough energy to break into charged particles (+/-)
gas-like, indefinite shape & volume
Stars (Sun), fluorescent light bulbs, TV tubes,
lightning
Most common state in the
universe

7. C. Thermal Expansion
Most matter expands when heated & contracts when cooled.
 Temp causes  KE. Particles collide with more force & spread out.
EX: thermostats (bimetallic strip) – two different metals, one contracts/expands more than the other.

8. Solid expansion, cont.
Expansion joints in bridges, concrete,etc.

9. Expansion of liquids
Alcohol or mercury in a (old style) thermometer expands with an increase in temperature.

10. Gas expansion Gases expand/contract the most of the states of matter.
EX. Hot-air balloons. Air expands, becomes less dense, rises.

11. Ch. 16 - Solids, Liquids, & Gases
MATTER
Ch Solids, Liquids, & Gases
II. Changes in State
Phase Changes
Heating Curves

12. melting point = freezing point
A. Phase Changes
** The temperature of a substance CAN NOT change during a phase change.
Melting
solid to liquid
Freezing
liquid to solid
melting point = freezing point

13. Vaporization (two types)
1. boiling - liquid to gas at the boiling point & throughout the liquid
2. evaporation - liquid to gas below the boiling point, but only at the surface

14. Condensation gas to liquid Sublimation
solid to gas without becoming a liquid in between
EX: dry ice, freeze drying, iodine

15. A. Phase Changes

16. B. Heating Curves Kinetic Energy Potential Energy motion of particles
related to temperature
Potential Energy
space between particles
related to phase changes

17. B. Heating Curves Gas - KE  Boiling - PE  Liquid - KE 
Melting - PE 
Solid - KE 

18. B. Heating Curves Heat of Fusion
energy required to change from solid to liquid
some attractive forces are broken

19. B. Heating Curves Heat of Vaporization
energy required to change from liquid to gas
all attractive forces are broken
EX: steam burns, sweating, and… the drinking bird
HEATING CURVE

20. Ch. 16 - Solids, Liquids, & Gases
MATTER
Ch Solids, Liquids, & Gases
III. Behavior of Gases
Pressure
Boyle’s Law
Charles’ Law

21. A. Pressure
Which shoes create the most pressure?

22. A. Pressure Key Units at Sea Level 101.3 kPa (kilopascal) 1 atm
760 mm Hg
14.7 psi

23. A. Pressure Barometer Manometer Atmospheric Pressure
Contained Pressure

24. A. Pressure Effect on Boiling Point
When atmospheric pressure decreases, the boiling point of a liquid decreases.
EX: high altitude cooking
Denver is 1 mile above sea level & water boils at 95o C;
on Mt. Everest (5.5 miles high) 71o C

25. Converting temperature units
K = 0C C = K – 273
What is the kelvin temperature of 20oC?
20 oC ___________ =
What is 20 K in celcius?
20 K _________ =

26. Boyle’s Law (temp constant)
Pressure and volume are inversely proportional. i.e. if one goes up the other goes down.
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

27. PV = kB P V
INVERSE

28. B. Boyle’s Law

29. V1=20 & P1 = 30 P2 = 120 V2= ? V1 P1 = V2 P2 (20)(30) = (V2)(120)

30. V1=50 & P1 = 30 V2 = 120 V1 P1 = V2 P2 (50)(30) = (120)(P2)

31. 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

32. C. Charles’ Law
When the temperature of a gas increases, its volume also increases (at constant pressure). V T
DIRECT

33. C. Charles’ Law

34. C. Charles’ Law -273°C or 0 K Absolute Zero - Temp at which...
the volume of a gas would equal zero.
all particle motion would stop.
-273°C or
0 K

35. Example #1 V1=20, T1 = 30, & T2 = 120

36. V1 = V2 T1 T2 20 = V /3 * 120 = V2 80 = V2

37. Example #2
V1=120, T1 = 30, & V2 = 300

38. V1 = V2 T1 T2 120 = T2 120 * T2 = 300 * * T2 = 9000 T2 = 75

39. Boyles (temperature constant) Charles (pressure constant)
Relating to Life
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”

40. Problems Boyles Law # V1 V2 P1 P2 1 30 15 ? 7 2 40 3 20 60 4 10 34 102
Charles Law # V1 V2 T1 T2 5 38
138 ? 69 6 15 20 45 7 30 13 8 76 17

41. Answers Boyles Law # V1 V2 P1 P2 1 30 15 3.5 7 2 40 3 8 20 60 4 10
2.35 34
102
Charles Law # V1 V2 T1 T2 5 38
138 19 69 6
6.67 15 20 45 7 30 65 13 8 76 17
8.5