1. Phases & Behavior of Matter

2. Review Everything in the universe is either matter or energy.
Physical Science is the study of matter and energy.
Matter is anything that has mass and takes up space.

3. Kinetic Theory of Matter
All matter is composed of small particles (atoms).
These particles are in constant motion.
These particles are colliding with each other and the walls of their container.

4. Kinetic Energy Kinetic Energy is the energy of motion.
Temperature is the measurement of the KE in an object.
So, the more KE the higher the temp.
As the particles in an object gain KE, the temperature goes up.

5. Solids Particles are closely packed together. Most are geometric.
There are bonds between atoms/mol.
Rigid shapes.
Definite shape.
Definite volume.

6. Liquids Particles in a liquid have more KE than particles in a solid.
Liquid particles have enough KE to overcome the forces that hold them together.
The particles can now move past one another. (flow)
Definite volume
No Definite shape.
Viscosity

7. Gases fill their container.
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Gases
Gas particles have more KE than liquid particles.
They have enough energy to break all bonds and escape the liquid state.
No definite Shape
No definite Volume.
Gases fill their container.

9. Plasma Most common state of matter in the universe
Extremely high temperatures.
Contains positively and negatively charged particles

10. Artificially produced plasmas
Terrestrial plasmas
Lightning
Artificially produced plasmas
Those found in plasma displays, including TVs
Inside fluorescent lamps (low energy lighting), neon signs

12. Thermometers Work because of thermal expansion.
Because mercury expands and contracts uniformly, it was used in thermometers.

13. Gases exert pressure on their container

14. Pressure: The amt of force exerted per unit of area.
Gases exert pressure by colliding with things
Other particles of gas
Sides of the container
Objects within the area of the gas, like you. 

15. Boyle’s and Charles’ Law
Both deal with gases.
Boyle’s Law
As the volume decreases, the pressure increases.
Charles’ Law
As the temperature decrease, the volume of a gas decreases.

16. Boyle’s Law P1V1 = P2V2
If you decrease the volume, the pressure will increase ( no Δt)

18. Boyle’s Law P1 V1 = P2 V2 P1 V1 = P2 V2
A volume of helium occupies 11.0 L at 98.0 kPa. What is the new volume if the pressure drops to 86.2 kPa?
P1 V1 = P2 V2
(98.O kPa) (11.0 L) = (86.2 kPa) (V2)
(98.O kPa) (11.0 L) = (V2)
(86.2 kPa)
(V2)=12.5 L

19. Charles’ Law
If you increase the temperature, the volume will increase

20. Charles’ Law
V1/T1 = V2/T2

21. Charles’ Law

22. Charles’ Law V1 = T1 V2 T2 = V2 = 0.24 L
What would be the resulting volume of a 2.0 L balloon at 25.0˚C that was placed in a container of ice water at 3.0˚C?
V1 = T1 V2   T2
2.0 L V2
25.0˚C
3.0˚C =
V2 = 0.24 L

24. Viscosity
Resistance to flow