1. Make sure notebook is setup Friday Lab safety certificate due!
KINETIC THEORY
Unit 1
Baughman
Warm-up 8/28
Make sure notebook is setup
on the first left-side page (after you table of contents), answer the following:
What’s your opinion of the simulation as a safety review? Was it good/bad…ugly? Why?
reviewing your safety contract, list 5 things the simulation did not cover.
In complete sentences, tell me why you think the creators decided to leave those points of.
Would you?
Heads up for Friday:
Safety quiz!!!
Friday Lab safety certificate due!

2. KINETIC THEORY
Kinetic Theory states that the tiny particles in all forms of matter are in constant motion.
Kinetic refers to motion
Helps you understand the behavior of solid, liquid, and gas atoms/molecules as well as the physical properties
Provides a model behavior based off three principals
3 Principles of Kinetic Theory
All matter is made of tiny particles (atoms)
These particles are in constant motion
When particles collide with each other or the container, the collisions are perfectly elastic (no energy is lost)

3. STATES OF MATTER What is matter? 5 States of Matter
Anything that has mass
& takes up space
5 States of Matter
Solid
Liquid
Gas
Plasma
Bose-Einstein
Condensates

4. SOLIDS Particles are tightly packed and close together
Particles do move but not very much
Definite shape and definite volume (because particles are packed closely and do not move)
Most solids are crystals
Crystals are made of unit cells (repeating patterns)
The shape of a crystal reflects the arrangement of the particles within the solid

5. SOLIDS
Unit cells put together make a crystal lattice (skeleton for the crystal)
Crystals are classified into seven crystal systems: cubic, tetragonal, orthorhombic, monoclinic, triclinic, hexagonal, rhombohedral
Unit cell  crystal lattice  solid

6. SOLIDS Amorphous Solid: A solid with no defined shape (not a crystal)
A solid that lacks an ordered internal structure
Examples: Clay, PlayDoh, Rubber, Glass, Plastic, Asphalt
Allotropes:
Solids that appear in more than one form
2 or more different molecular forms of the same element in the same physical state (have different properties)
Example: Carbon
Powder = Graphite
Pencil “lead” = graphite
Hard solid = diamond

7. SOLIDS

8. SOLIDS www.wikipedia.org Allotropes of Carbon: a) diamond b) Graphite
c) lonsdaleite,
d)buckminsterfullerene (buckyball)
e) C540
f) C70
g) amorphous carbon
h) single-walled (buckytube)

9. LIQUIDS Particles are spread apart
Particles move slowly through a container
No definite shape but do have a definite volume
Flow from one container to another
Viscosity – resistance of a liquid to flowing
Honey – high viscosity
Water – low viscosity
Ex. Cats!
chemed.chem.purdue.edu/.../graphics

10. GASES Particles are very far apart Particles move very fast
No definite shape and No definite volume

11. PLASMA Particles are extremely far apart Particles move extremely fast
Only exists above 3000 degrees Celsius
Basically, plasma is a hot gas
When particles collide, they break apart into protons, neutrons, and electrons
Occurs naturally on the sun and stars

12. BOSE-EINSTEIN CONDENSATE
Particles extremely close together
Particles barely move
Only found at extremely cold temperatures
Basically Bose-Einstein is a cold solid
Lowest energy of the 5 states/phases of matter

13. GASES AND PRESSURE
Gas pressure is the force exerted by a gas per unit surface area of an object
Force and number of collisions
When there are no particles present, no collisions = no pressure = vacuum
Atmospheric Pressure is caused by a mixture of gases (i.e. the air)
Results from gravity holding air molecules downward in/on the Earth’s atmosphere; atmospheric pressure decreases with altitude, increases with depth
Barometers are devices used to measure atmospheric pressure (contains mercury)
Standard Pressure is average normal pressure at sea level
As you go ABOVE sea level, pressure is less
As you go BELOW sea level, pressure is greater

14. GASES AND PRESSURE Standard Pressure Values
At sea level the pressure can be recorded as:
14.7 psi (pounds per square inch)
29.9 inHg (inches of Mercury)
760 mmHg (millimeters of Mercury)
760 torr
1 atm (atmosphere)
kPa (kilopascals)
All of these values are EQUAL to each other:
29.9 inHg = kPa
760 torr = 760 mmHg
1 atm = 14.7 psi
and so on……….
Say hello to Factor Label Method & Dimensional Analysis!!!!!!!!!!!!

15. GASES AND PRESSURE STP Standard Temperature and Pressure
Standard Pressure values are the values listed on the previous slides
Standard Temperature is 0°C or 273 K
If given in Fahrenheit, you must convert first!
°F = (9/5)°C + 32
°C = (5(°F-32)) / Remember order of operation rules
K = °C
°C = K – 273

16. What questions have we answered?
Using complete sentences, answer each of the following essential questions in your notebook. (You do NOT need to rewrite the question, but I should be able to tell what the question was by your answer.)
What is the kinetic theory of matter?
What are the characteristics of matter?
What are the 3 types of matter found extensively on Earth?
How do particles move in the different states of matter?

17. Friday 8/29 Standards of Measurement (p.19-25)
After quiz- Turn in ‘test’ & scantron (face-down) on front desk.
There will be NO TALKING/PHONES until EVERYONE is done with the quiz!
Get a textbook
Using p.19-25, create a table like the
one below with the data you find there.
Below your table, define the following terms:
heat of vaporization
heat of fusion
freezing
melting 
vaporization
condensation
evaporation
sublimation
deposition
Standards of Measurement (p.19-25)
Unit (name)
Unit (symbol)
What does it measure?
If units measure the same thing, what makes each unique?
Keep adding rows as needed… You WILL have more than this!

18. Warm-up Tues 9/2 Pick up a set of ‘States of Matter’ cards.
Match the properties to each state
Before we can go on…
Friday’s work needs to be completed.
You have 15min!
Below your table, define the following terms:
heat of vaporization
heat of fusion
freezing
melting 
vaporization
condensation
evaporation
sublimation
deposition
3. Using p.19-25, create a table like the one below with the data you find there.
Standards of Measurement (p.19-25)
Unit (name)
Unit (symbol)
What does it measure?
If units measure the same thing, what makes each unique?
Keep adding rows as needed… You WILL have more than this!

19. Warm-up Wed 9/4 Within 5min after the bell: Keep in mind…
Pick up Matter states ‘cards’ (If you haven’t already.)
Get your notebook & find your new ASSIGNED seat
Cut up cards, mix, & practice putting them back in order
Review our previous notes
Keep in mind…
Failure to do these tasks in a QUIET AND PROFESSIONAL MANNER will result in a Teacher Detention.
THIS IS YOUR WARNING!!!
Behave in a way that EARNS you the respect you feel you deserve!

20. keep out something to write with.
Pop Quiz!
Put your notes away, but
keep out something to write with.
On your answer sheet,
choose the correct response.
We will exchange, grade,
and discuss after.

21. Lab DEMO Instructions Review lab instructions as a class
In the meantime:
Changes of States diagram & Temperature Conversions
RECALL: Standard Temperature is 0°C or 273 K
If given in Fahrenheit, you must convert first!
°F = (9/5)°C + 32
°C = (5(°F-32)) / Remember order of operation rules
K = °C
°C = K – 273

22. Temperature Conversion Examples
What is the Celsius value for 65° Fahrenheit?
200°C is the same temperature as what value on the Fahrenheit scale?
Water boils at a temperature of 100°C. What would be the corresponding temperature for the Kelvin scale?
A substance has a melting point of 625 K. At what Celsius temperature would this substance melt?
Conversions from K to °F, or F to °K are rare, but possible. You can combine 2 formulas or use 2 steps.

23. Changes of States
2 Examples
Property Changes
from liquid to gas

24. Changes of States Key boiling solid liquid gas Property Changes
2 Examples
Heat of fusion
Heat of vaporization
boiling
evaporation
melting
vaporization
solid
liquid
gas
freezing
condensation
Sublimation
Ex. Dry ice
Property Changes
from liquid to gas
Decreased viscosity
Thermal expansion

25. Phase Change Diagram for Water
Warm-up Fri.: Where should our phase change terms go?