1. Chapter 16 – SOLIDS, LIQUIDS & GASES

2. Section 1 – KINETIC THEORY

3. States of Matter
GAS
SOLID
                        
                       
                       
LIQUID

4. The Kinetic Theory Explains how particles behave
All matter is made of small particles
These particles are in constant, random motion
Particles collide with each other & with the walls of containers
                             

5. Total energy of a material’s particles
                               
Thermal Energy
Causes particles to vibrate in place

6. Average Kinetic Energy = temperature of a substance
                
How fast the particles are moving
The the temp, the slower the motion

7. Solid State of Matter
Particles closely packed together in specific geometric arrangement
                                  
                            

8. Liquid State of Matter
Liquids flow and take the shape of their container
Solids begin to liquefy at the melting point as particles gain energy to overcome arrangement
                                  
                            
Heat of FUSION

9. Gaseous State of Matter
Gases spread evenly throughout their container (diffusion)
When a liquid has enough energy to escape the attractive forces of other particles
                                  
                                     
                            

10. Gaseous State of Matter
Heat of Vaporization
Energy changing a liquid to a gas
At the boiling point –
Pressure of the liquid’s vapor =
the presure of the atmosphere
                                  
                                     
                           
                            

11. Heating Curve of a Liquid Melting Point & Freezing Point
                              
                                
Melting Point & Freezing Point
Boiling Point

12. Plasma State of Matter High temperature gas
Balanced positively and negatively charged particles
Most abundant state
                                  
                            

13. Happens in most solids, liquids & gases
Thermal Expansion
Increase in the size due to an increase in temperature
If temp then size
Happens in most solids, liquids & gases
Water is an exception – it expands
as it becomes a solid!

14. Exceptions – these do not act as expected -
Liquid Crystals
Amorphous Solids

15. AMORPHOUS SOLIDS Lack tight ordered structure
No definite temperature for change from solid to liquid.
Glass, ceramic & plastics

16. LIQUID CRYSTALS Don’t completely lose ordered arrangement upon melting
Used in LCD’s
Watches, clocks, notebook computers & TV’s

17. Properties of Fluids Chapter 16 - 2

18. Buoyant Force
Buoyancy = the ability of a fluid to exert an upward force on an object immersed in it.
Buoyant Force – the supporting force on an immersed object
If force = weight, object will…
If force is less than weight, object will…
FLOAT
SINK

19. The older one b/c he displaces more water.
Archimedes’ Principle
The buoyant force on an object is equal to the weight of the water displaced by the object
Which has a higher buoyant force, a baby in a bath tub or a 40 year old person?
The older one b/c he displaces more water.

20. D = m / v
Density…
Objects will float if their density is less that the density of the fluid it is placed in
Why do ships float???

21. Pascal’s Principle
Pressure applied to a fluid is transmitted throughout the fluid.
What are some everyday examples of this?
Toothpaste tubes, balloon animals

22. Bernoulli’s Principle
As velocity of a fluid increases, the pressure exerted by the fluid decreases.
The faster air flows over the wings. What do we know about the pressure above the wing?
It’s lower!

23. Viscosity = resistance to flow
Different structures cause different tendencies to flow
Particles “pull” other particles with them increasing the flow
As temperature increases, viscosity decreases allowing for easier flow
Ex: Honey has a higher viscosity than water, b/c it does not flow as easily.

24. Sec. 16.3
Behavior of Gases

25. Pressure : SI Unit = Pascals (Pa) Pressure = Force/Area
Collisions of particles in air result in atmospheric pressure – Highs and Lows in weather
Particles colliding with walls of a container create GAS pressure

26. Why does this balloon stay inflated?
The particles in air striking the balloon’s walls forces them outward.

27. British scientist, Robert Boyle
1. Boyle’s Law – relates pressure and volume
British scientist, Robert Boyle
At a constant temp, volume of gas decreases as pressure increases. (inverse relationship)
P1V1 = P2V2
Why does a weather balloon expand as it rises in the atmosphere?

28. French scientist, Jacques Charles
2. Charle’s Law – relates volume and temp
French scientist, Jacques Charles
At a constant pressure, volume increases as temp increases. (direct relationship)
V1T2 = V2T1
Explain this using Kinetic Theory of Matter.

29. 3. Gay-Lussac’s Law – relates pressure and temp
At a constant volume, as temp increases, pressure increases. (what kind of relationship is this?)
T1P2 = T2P1
Explain what will happen to a canister that says “keep away from heat” if placed in a heated area?