1. Chapter 13
States of Matter

2. States of Matter matter classified as one of these physical states
solids,
liquids and
gases.
4th state of matter—plasma: does not occur naturally on Earth except in the form of lightning bolts.

3. States of Matter

4. States of Matter
The physical state of a sub is a physical property of that sub.
Other physical properties:
m.p., b.p., heat conductivity, electricity conductivity, color, crystal shapes, hardness etc.

6. Solids A solid is a physical state matter that has definite shape and
definite vol.
e.g.Wood, Fe, paper, and sugar

7. Solids particles tightly and orderly packed.
When heated, expands slightly
fixed position (particles just vibrate)
Definite shape
Not conform to shape of container

8. Solid
Particle Movement
Examples

9. Liquids A liquid is a state of matter that flows (fluids)
constant volume, and
takes the shape of its container.
e.g. liquids : H2O, blood, and Hg.
Particles
not rigidly held in place
less closely packed than those in a solid:
able to move past each other.
move much faster than (s)

10. Liquids allows a (l) to flow and take the shape of its container
may not completely filled the container because definite volume.

11. Liquids 
Because of the way the particles of a (l) are packed, (l) are virtually incompressible.
Like (s), (l) tend to expand when heated.

12. Liquid
Examples
Particle Movement

13. Gases A (g) is a state of matter that flows (fluid)
to conform to the shape of its container and
fills the entire vol.
Particles
very far apart (compressible)
moving very fast (high KE)

14. Gases
Gas: a sub that is naturally in the gaseous state at room temp.(oxygen gas)
Vapor:the gaseous state of a sub that is a (s) or a (l) at room temp. (water vapor)
e.g. steam is a vapor because at room temp water exists as a (l). (steam is invisible)

15. Gas
Particle Movement
Examples

16. Gases subs can change physical states e.g. water changes to steam
condensation:
vaporization:
evaporation:
*melting—not involving gas
sublimation:

17. Ice at -60°C (Ice) temp increasing All vapor All water (l) vaporizing
water(l) temp increasing
(d)
(100°C)
Temp increasing
All ice 0°C
(c)
Boiling water & vapor at 100°C
melting
All water(l) 0°C
(b)
(0°C)
Ice+water 0°C
(a)
(Ice) temp increasing
Ice at
-60°C

18. Heating curve of water

19. Kinetic Energy and Temperature
Absolute zero (0 K, or –273°C)
temp at which the motion of particles theoretically ceases.
Particles would have no KE.
Absolute zero has never been produced in the lab. (on earth)

20. Gases Kinetic Theory for gases
The theory makes the assumptions about the size, motion, and energy of (g) particles.

21. Kinetic Theory and a Model for Gases
kinetic → motion.
Kinetic Energy
energy an object has because of its motion.
all matters (of different physical states) consist of tiny particles that are in constant motion.

22. Kinetic Theory for Gases
Assumptions for gases
(1)Particles in a (g) are separated by empty spaces.
(2) vol of the empty space is much > than the total vol of the (g) particles.
total vol of particles ≈ 0.
(3) Since (g) particles are far apart and are so light → inter-molecular attractive forces ≈ 0.

23. Kinetic Theory for Gases
(4) (g) particles are in constant, random motion in a straight line until they bump into something (another particle or the side of a container); only change direction; continue to move …
(5) All collisions among particles in a (g) are perfectly elastic.
An elastic collision
A collision in which KE is transferred w/o loss from one particle to another.

24. Particle Energy Temperature
a measure of the average KE of the particles in a sample of matter.
At higher temp
gas particles absorbed heat energy
higher KE → move faster
higher pressure (gases)??
At a given temp, all (g) have the same average KE.

25. Particle Energy The velocity of a particle includes both its speed and
its direction.
Each particle in a sample containing only one (g) will have the same mass but not the same velocity.

26. Gas Pressure (1) Gas pressure
When (g) particles collide with the walls of their container, they exert pressure on the walls. (pressure depends on the mass of (g) )
Pressure is force (N) per unit area (m2). --N/m2
Vacuum
An empty space with no (g) particles and no
pressure. (no collision)
Atmospheric pressure
pressure exerted by the particles in the atm that surrounds Earth.

27. Gas Pressure (5) The SI unit of pressure is the pascal (Pa).
One standard atmosphere (atm) is the pressure required to support 760 mm of Hg in a Hg barometer at 25°C.
Barometer …..
= 1 torr

28. Gas Pressure (4)
A barometer is a device that is used to measure atm pressure.

29. Phase Changes that Require Energy (2)
vapor
If a sub is usually a (l) at room temp (as water is), the (g) phase.
Vaporization
the process by which a (l)changes into a (g) or vapor.
Evaporation
vaporization occurs only at the surface of a (l) at any temperature (not boiling)

30. Phase Changes condensation ↔ vaporization sublimation↔ deposition
freezing ↔ melting

31. Fluidity Fluids: (l) and (g) Fluidity is the ability to flow.
(l) are less fluid than (g).

32. Liquid-vapor Equilibrium
Sealed container
evaporation
Evaporation and condensation
equilibrium
At Eqm, Rate (l)→ (g) = rate (g)→ (l)
Evaporation rate = Condensation Rate

33. Solids Liquids Gases volume Shape density Position of particles
compressibility
Inter-molecular attraction
Particle motion
Space between particles
KE of particles
Arrangement of particles

34. melting↔freezing
Vaporization↔condensation
Sublimation↔deposition

35. Phase Diagrams
Triple point Critical point

36. Phase Changes on phase diagram
Sublimation↔deposition Melting (fusion)↔freezing Vaporization↔condensation

37. CST example 1
In a sealed bottle that is half full of water, eqm will be attained when water molecules
A cease to evaporate.
B begin to condense.
C are = in # for both the (l) and the (g) phase.
D evaporate and condense at = rate

38. CST problem 2
Under the same conditions of pressure and temperature, a liquid differs from a gas because of the molecules of the liquid
A have no regular arangement
B are in constant motion
C have stronger forces of attraction between
them.
D take the shape of the container they are in.

39. CST problem 3
Methane (CH4) gas diffuses through air because the molecules are
A moving randomly.
B dissolving quickly.
C traveling slowly.
D expanding steadily

40. CST problem 4
When someone standing at one end of a large room opens a bottle of vinegar, it may take several minutes for a person at the other end to smell it. Gas molecules at room temperature move at very high velocities, so what is responsible for the delay in detection of the vinegar?
A the increase in the airspace occupied by vinegar molecules
B the chemical rxn with nerves, which is slower than other sensory process
C attractive forces between the air and vinegar molecules
D random collisions between the air and vinegar molecules

41. CST problem 5
If the attractive forces among (s) particles are less than the attractive forces between the (s) and a (l), the (s) will
A probably form a new precipitate as its crystal
lattice is broken and re-formed.
B be unaffected because attractive forces
within the crystal lattice are too strong for the
dissolution to occur.
C begin the process of melting to form a (l).
D dissolve as particles are pulled away from
the crystal lattice by the (l) molecules.

42. CST problem 6
The random molecular motion of a substance is greatest when the substance is
A condensed.
B a liquid.
C frozen
D a gas

43. A water at 0°C is colder than (l) nitrogen and freezes.
CST problem 7
The boiling point of (l) nitrogen is 77 K. It is observed that ice forms at the opening of a container of (l) nitrogen. The BEST explanation for this observation is
A water at 0°C is colder than (l) nitrogen and freezes.
B the nitrogen boils and then cools to form a (s) at the opening of the container.
C water trapped in the (l) nitrogen escapes and freezes.
D the water vapor in the air over the opening of the (l) nitrogen freezes out.

45. The End