1. Chemistry: Chapter 13
States of Matter

2. Kinetic Molecular Theory (KMT)
accounts for the behavior of atoms and molecules that make up matter.
KMT is based on idea that particles of matter are always in motion and upon these 5 assumptions…

3. Kinetic Molecular Theory (KMT)
1. Gases consist of large numbers of tiny particles that are far apart relative to size
2. Collisions between gas particles and between particles and container walls are elastic collisions
Elastic collisions: no net loss of kinetic energy

4. Kinetic Molecular Theory (KMT)
3. Gas particles are in continuous, rapid, random motion, and therefore possess kinetic energy (energy of motion)
4. There are no forces of attraction between gas particles
5. The temperature of a gas depends on the average kinetic energy of the particles of the gas

5. The Nature of Gases a. Gases have no definite shape or volume
b. Gases have fluidity (the ability to flow)
c. Gases have low density
d. Gases have compressibility

6. The Nature of Gases
e. Diffusion: spontaneous mixing of the particles of two substances caused by their random motion

7. The Nature of Gases
f. Effusion: a process by which gas particles pass through a tiny opening

8. The Nature of Gases
g. Ideal gas: a hypothetical gas that perfectly fits all the assumptions of the kinetic molecular theory.
h. Real gas: a gas that does not behave completely according to the assumptions of the kinetic molecular theory

9. Properties of Liquids A. Liquids have definite volume,
but no definite shape
B. Relatively high density
(100s of times denser than gases)
C. Relative Incompressibility
D. Ability to diffuse (slower than gases)

10. Properties of Liquids
E. Surface tension: a force that tends to pull adjacent parts of a liquid’s surface together
thereby decreasing surface area to the smallest possible size.

11. Properties of Liquids F. Capillary action:
the attraction of the surface of a liquid to the surface of a solid

12. Properties of Liquids G. Vaporization: a liquid changes to a gas
H. Evaporation: particles escape from the surface of a nonboiling liquid and enter the gaseous state

13. Properties of Liquids
I. Freezing (or solidification): a liquid changes to a solid by removal of energy as heat
J. Condensation: a gas changes to a liquid

14. Properties of Solids A. There are two types of solids:
1. Crystalline solids: consist of crystals, which are substances in which the particles are arranged in an orderly, geometric, repeating pattern
2. Amorphous solids: the particles are arranged randomly

15. Properties of Solids
B. Solids have a definite shape and a definite volume
C. Have a definite melting point: the temperature at which as solid becomes as liquid
D. Melting: a solid changes to a liquid by the addition of energy as heat

16. Properties of Solids E. Solids have high density and incompressibility
F. Solids have low rates of diffusion
G. Sublimation: solid changes directly to a gas
H. Deposition: a gas changes directly to a solid

17. Changes of State and Equilibrium
 A. Equilibrium: a dynamic condition in which two opposing changes occur at equal rates in a closed system
B. Volatile liquids: liquids that evaporate readily

18. Changes of State and Equilibrium
C. Molar Enthalpy of Vaporization ∆Hv: the amount of energy as heat that is needed to vaporize one mole of liquid at the liquid’s boiling point at constant pressure
D. Molar Enthalpy of Fusion ∆Hf : the amount of energy as heat required to melt one mole of solid at the solid’s melting point

19. Changes of State and Equilibrium

20. Phase Diagrams (graph of pressure versus temperature)

21. Phase Diagrams (graph of pressure versus temperature)
A. Triple point: indicates the temperature and pressure at which the solid, liquid, and vapor of a substance coexist at equilibrium
B. Critical point: indicates the critical temperature and critical pressure
C. Critical temperature Tc: the temperature above which the substance cannot exist in the liquid state
D. Critical pressure Pc: the lowest pressure at which the substance cannot exist as a liquid at the critical temperature

22. Phase Diagrams (graph of pressure versus temperature)

23. Water
A. Structure is bent

24. Water
B. Water molecules in solid and liquid states are linked by hydrogen bonding

25. Water C. Liquid water is denser than solid water (why?)
D. High molar enthalpy of vaporization

26. Metal + Water  Metal Hydroxide + Hydrogen
Reactions with Water
Production of a Base
Bases contain hydroxide: OH–
Metal + Water  Metal Hydroxide + Hydrogen
Li H2O 
Be H2O 

27. Reactions with Water Production of a Base Bases contain hydroxide: OH–
Metal Oxide + Water  Metal Hydroxide
K2O H2O 
CaO H2O 

28. Reactions with Water Production of an Acid
Acids contain hydrogen, written first, and usually a polyatomic ion: H+
Nonmetal Oxide + Water  Acid
SO H2O 
SO H2O 
CO H2O 
C2O H2O 

29. Reactions with Water Synthesis and Decomposition of Water
Hydrogen + Oxygen  Water
Water  Hydrogen + Oxygen

30. Reactions with Water Decomposition of a Hydrate
Hydrate  Ionic Compound + Water
Cu2SO4•7H2O heat
Fe(MnO4)3•3H2O heat
Au2(Cr2O7)3•8H2O heat