1. States of Matter
Chapter 13
of Matter Video

2. Kinetic Theory
Tiny particles in all forms of matter are in constant motion.
Temperature is related to the average kinetic energy of an object’s molecules.
High kinetic energy ~ Higher temperature
Low kinetic energy ~ Lower temperature
Molecules in Motion Applet

3. Temperature on the Kelvin Scale
Based on “Absolute Zero”
No negative values – all substances have energy (positive temperature)

4. Gas Particles farther apart than other forms of matter
Particles take up the volume of the container
Particles moving randomly in straight lines with “perfect elastic collisions”

5. Gas Pressure
The result of collisions of gas particles with the container walls
#collisions ~ gas pressure

6. Atmospheric Pressure Air molecules colliding with objects
cup

7. STP Measuring Pressure Standard Temperature = 0° Celsius
Standard Pressure Equivalents:
(measured at sea level, 0° Celsius)
1 atmosphere
101.3 kilopascals
760 mm Hg
760 torr
STP

8. The chart below illustrates how to interpret your barometer's inches of mercury reading. This provides a reasonably accurate forecast for the next 12 to 24 hours.
The Barometer
Invented by Evangelist Torricelli (1643)
What’s that weather man saying?
Does the barometric pressure
effect when the fish bite?

9. The monometer

10. Liquids Molecules are close together, touching
Liquids are not compressible
Intermolecular forces hold the molecules together loosely so that they can slip and slide around each other.
Need proof? Water Pours.

11. Evaporation
Molecules gain enough kinetic energy to “break away” or escape from intermolecular forces at the surface.
Why do we sweat?

12. Boiling
Tiny bubbles of vapor form inside the liquid due to increased kinetic energy.
The vapor pressure must be equal or greater than the air pressure to escape.
Water Boiling in a low g environment Video
Altitude changes and Boiling Temperatures
Cooking Under Pressure
Pressure cooking

13. Is boiling different than evaporation?
YES!!!!

14. Boiling Water with Ice Demo
How is it possible that the water boils when the flask is cooled?

15. Dynamic Equilibrium

16. Solids Particles are close together in fixed positions – only vibrate.
Solids are also not compressible.
Solids have stronger intermolecular forces
than liquids and gasses.

17. Solids Many solids form crystals. -repeating pattern or arrangement
of the particles (crystal lattice)
Other solids are amorphous & lack internal structure

18. Allotropes
Two or more different molecular forms of the same element.

19. Melting Point Temperature at which the solids turn to a liquid
The particles have enough kinetic energy to overcome the intermolecular force that holds them in place.
Ionic substances – high melting pts
Molecular substances – low melting pts

20. Sublimation
A solid changing to a vapor without passing through the liquid phase.
The solids vapor pressure is higher than the atmospheric pressure
Air fresheners Urinal Cakes Ice when very cold
Freeze Dried Products Dry Ice (Carbon dioxide)

22. Phase change diagram
vaporization
melting

23. Phase Diagrams
Example : Water
Triple Point

24. Plasma
State at which the kinetic energy is so high that the atom’s electrons are freed from the nucleus
Ionized state of an atom
Low temp plasma – 50,000 – 100,00 K
High temp plasma – 10,000,000+ K
Is this in my blood?
You ask about TVs?