1. Molecular Kinetic Theory
S. Staron 2-11

2. KINETIC THEORY OF MATTER
ALL PARTICLES (ATOMS OR MOLECULES)OF MATTER ARE IN CONSTANT MOTION!
Kinetic – comes from Greek word meaning “to move”
Kinetic Energy – energy object has due to its motion

3. Separation Between Particles
Gases
separation between particles is very large compared to their size
there are no attractive or repulsive forces between the molecules
Liquids
particles are still far apart
but now they are close enough that attractive forces confine the material to the shape of its container
Solids
particles are so close that the forces of attraction confine the material to a specific shape.

4. USING THE KINETIC THEORY TO EXPLAIN BEHAVIOR OF MATTER
Gases
Particles in constant, random motion – allows gas to fill container
Motion of particles unaffected by other particles unless collision
Forces of attraction between particles can be ignored
Liquid
Particles can flow to new locations
Force of attraction between particles keeps them close
Solid
Particles vibrate around fixed locations due to stronger forces of attraction between particles

5. Particles are in Constant Motion
Each particle is in constant motion Gases: the movement of the particles is assumed to be random and free Liquids: the movement is somewhat constrained by the volume of the liquid Solids: the motion of the particles is severely constrained to a small area, in order for the solid to maintain its shape. The velocity of each particle determines its kinetic energy.

6. Collisions Transfer Energy
The numerous particles often collide with each other.
If a gas or liquid is confined in a container, the particles collide with the particles that make up the walls of a container.

7. Temperature
Temperature of an object or collection of matter is the average kinetic energy of the particles.
Faster moving particles - a higher
temperature.
A thermometer is used to measure the temperature
Puts it into temperature degrees instead of kinetic energy units.

8. Compare average KE of particles in 3 states of matter?
For a Given Substance:
Solid: low KE  slower speed  vibrate around fixed locations
Why? Particles “stuck” due to forces of attraction between particles
Liquid: greater KE than solid  greater speed  not “stuck” in place so can flow to new locations
Forces of attraction? Still there but not as strong
Gas: greater KE than liquid  even greater speed  particles can spread out far from each other
Forces of attraction? Very weak (can be ignored)

9. How is one state changed into another?
Energy is ABSORBED by the system from the surroundings  Endothermic Process
Energy is RELEASED by the system to the surroundings  Exothermic Process
This change in the state of matter is called a PHASE CHANGE

10. States of Matter State Movement speed Position Plasma Extremely fast –
so much energy that
electrons come off
All over
“Bumper cars”
Gas
Fast
(500 – 1000 m/s)
Liquid
Slower than in a gas
(~200 m/s)
Slide around each other
(Hallway full of people)
Solid
A. Crystalline solid (crystal)
B. Amorphous solid (glass)
No change of position
Vibrate in place
Stay in one place
A. Orderly arrangement
B. Not very ordered
BEC
Bose-Einstein Condensate VERY cold!
So close they act as one
big atom/molecule

11. States of Matter

12. Solids
The kinetic theory says solids are closely packed atoms or molecules (groups of atoms). Solids don’t have enough space between the particles to move around, but do have energy to vibrate in place.

13. Picture of a solid:

14. Liquids
The kinetic theory says liquids are closely packed atoms or molecules (groups of atoms), but do have enough energy to keep some amount of space between their particles.
Liquids do have enough space between them for particles to slide around each other, but not enough energy to overcome gravity.

15. Picture of a Liquid

16. Gas
The kinetic theory says gases are widely spaced atoms or molecules. Gases have a lot of space between the particles to move around.

17. Picture of a Gas

18. Equivalent Units
Many of the properties of gases can be measured in different ways. Conversion from one unit of pressure to another is very important. To achieve this there has to be a conversion factor to move from one unit to another. Here is a list of equivalent amounts of pressure:
1 atm
760 mmHg
76 cmHg
101.3 kPa
760 torr
29.92 inches Hg

19. General Properties of Gases
Gas particles can be monatomic (Ne), diatomic (N2), or polyatomic (CH4) – but they all have these characteristics:
1. Gases have mass.
2. Gases diffuse to fill their containers
uniformly and completely.
3. Gases diffuse and mix rapidly.
4. Gases exert pressure.
5. A gas’s pressure is dependent on its
temperature.

20. Gases are not dense, and fill up their containers.

21. The Kinetic Theory
The Kinetic Theory states that the tiny particles in all forms of matter are in constant motion.
This theory is used to explain the behaviors common among gases
There are 3 basic assumptions made by the Kinetic Theory as it applies to gases.

22. Large Separation Between Particles
Gas Separation between particles is very large compared to their size There are no attractive or repulsive forces between the molecules Liquid Particles are still far apart, but now are close enough that attractive forces confine the material to the shape of its container Solid Particles are so close that the forces of attraction confine the material to a specific shape.

23. Kinetic Theory Assumption 1: An “Ideal” Gas
A gas is composed of small hard particles.
The particles have an insignificant volume and are relatively far apart from one another.
There is empty space between particles.
There is no attractive or repulsive forces acting between particles.

24. Kinetic Theory Assumption 2: An “Ideal” Gas
The particles in a gas move in constant random motion.
Particles move in straight paths and are completely independent of each of other
A particle’s path is only changed by colliding with another particle or the sides of its container.

25. Kinetic Theory Assumption 3: An “Ideal” Gas
All collisions a gas particle undergoes are perfectly elastic.
No energy is lost from one particle to another, and the total kinetic energy remains constant.

26. Deviations from the “Ideal” Gas
1) Real molecules have volume.
The ideal gas consumes the entire amount of available volume. It does not account for the volume of the molecules themselves.
2) There are intermolecular forces.
An ideal gas assumes there are no attractions between molecules. In reality, attractions slow down the molecules and reduce the amount of collisions. (Otherwise a gas could not condense to become a liquid.)

27. Gas Compresses
Since one of the properties of a gas is compressibility, a gas at a certain volume can be compressed by applying more pressure.
The mass of the gas will remain unchanged.
Since the mass remains the same and the volume decreases, the density of the gas is greater.

28. If you squeeze a gas, its volume can be reduced considerably.

29. Example If the mass of the gas is .50 grams and the volume
of the gas is one liter then
the density of the gas is
.50 grams/liter.
However, if the gas is
compressed to only take up
one quarter of a liter then the
density will change to 2 g/l.

30. If I opened up a bag of popcorn in front of the class you would soon be able to smell it in the back.
The popcorn smell is a high- energy group of molecules in a gaseous state.
This property of gases spreading out until they have filled the room is called diffusion (spreading from an area of high concentration to one of low concentration).

31. It is because of all of the empty space between gas molecules that another gas molecule can pass between two of them until each gas is spread out over the entire container.

32. If the gases are in constant random motion the fact that they are moving and colliding with everything around them means they will mix with other gases uniformly.
This doesn’t happen at the same speeds for all gases though.
Some gases diffuse more rapidly then other gases – this is based on their size and their energy.