Chapter 3 States of Matter
plasma
Gases
Liquids
Solids
Bose-Einstein
Condensate
http://www.colorado.edu/physics/2000/bec/what_it_looks_like.html
BUT...99% of the matter in the universe is
PLASMA! (often 10 million degrees Celsius):
the Fourth State of Matter!
Plasma= "Super Hot and Super Excited Atoms"!
Examples of plasma = in stars, lightning, "Northern
Lights"... and artificially made plasma in fluorescent
bulbs and neon lights
And yes, there is a Fifth State of Matter (discovered in
YOUR lifetime! 1995!):
The Bose-Einstein Condensate (BEC), a group of atoms that
gets so cold (near but not at Absolute Zero) that they clump
together to form a "Superatom" blob!
BEC = "Super Cold and Super Unexcited Atoms"
3.1 Venn
Diagram
3.1 Solids, Liquids, and Gases 3.1.1
Matter can be classified as:
solid - if it has a definite shape and definite volume (definite meaning
it does not take the shape or volume of its container)
liquid - if it has a definite volume, but no definite shape (takes the
3.1.10
shape of its container) 3.1.4
gas - if it has neither a definite shape nor definite volume (takes the
volume and shape of its container) 3.1.5 3.1.7
plasma - extremely high temperatures (will discuss later) 3.1.8
Bose-Einstein condensate - extremely low temperatures 3.1.9
Why and how does matter exist in these different states?
Kinetic-Molecular Theory of Matter
-kinetic energy: energy an object has due to its motion 3.1.11
-kinetic comes from Greek "to move"
-the faster an object moves, the more kinetic energy it has (95 mph
fastball has more kinetic energy than a 94 mph fastball)
-Kinetic Theory of Matter states that all matter is in constant motion 3.1.12
http://www.plasmas.org/E-4phases2.jpg
Behavior of states of matter
-forces of attraction exist between particles in all types of matter 3.1.13
-total kinetic energy does not change in matter
-individual atoms' kinetic energy may change, but total remains
constant
Gases
-particles are far apart and moving too fast for attractive forces to influence
the path of particles
-particles move in straight-line paths until they collide with container or
other particles
-average speed of particles in a gas at room temperature is about 1,600
km/h
-the constant motion of a gas allows it to fill a container
Kinetic Theory as applied to gases:
a. particles in a gas are in constant, random motion
b. the motion of one particle is unaffected by the motion of other
particles unless they collide 3.1.14
c. forces of attraction among particles in a gas can be ignored under
ordinary conditions
Liquids
-particles are more closely packed and are affected by attractive forces of
other particles
-a "tug of war" exists between the constant motion of particles and the
3.1.16 3.1.17
attraction among particles
-liquids can take shape of container because particles can flow to new
locations
-liquids still have definite volumes due to the attraction between the
particles
3.1.6
3.1.3 3.1.18
3.2 Fun with dry ice!
3.2 The Gas Laws
Pressure is a force over an area 3.2.1
-force is measured in Newtons (N)
-area is measured in square meters (m2)
-the SI shorthand for N/m2 is Pa (pascal), so you express
pressure with the unit Pa
3.2.2
Factors that affect pressure 3.2.4
-as T  P  (if volume and number of particles are kept
constant) e.g. car tires 3.2.5 & 6
-as V P  (if temperature and number of particles are
constant) e.g. inhaling 3.2.7
-as n  P  (if temperature and volume are kept constant)
e.g. inflating tires 3.2.8
Let's look at these relationships more closely
1. What relationship does the line describe?
(As gas temperature ____, gas volume _____)
2. Why is part of
the line solid and
part dashed?
3. At what
temperature will
the volume equal
zero?
Charles Law:
The volume of a gas
is directly
proportional to the
temperature of the
gas in Kelvins:
Problem 1: If a gas has a
volume of 50 ml at 10 K,
calculate its volume at 20 K.
50 ml
10 K
V2
20 K
(50 ml)(20 K) = (10 K) (V2)
(50 ml)(20 K) = V2
10 K
100 ml = V2
TODAY'S BALLOON LAB WILL PUT
CHARLES LAW RIGHT TO WORK!
Your balloon exposed to 5 different temperatures:
HOT water (almost boiling!)
Warm water from the tap
Room temperature
Cold water from the tap
COLD dry ice in the cooler
1. How do you measure the volume of a balloon?
(What do you need to know?)
2. How do you measure the circumference of a
balloon? (What "tools" do you need?)
P1V1 = P2V2
Boyle's Law: P1V1 = P2V2
Q: A gas has a volume of 5.0 L at a
pressure of 50 kPa. What happens to the
volume if the pressure is increased to 125
kPa? The temperature doesn't change.
A: 2.0 L
Charles Law
-states the volume of a gas is directly proportional to its
temperature in kelvins (P and n are constant) 3.2.9 &11
-temperature must be in kelvins
-experimental data are the basis for the value of absolute zero
(Figure 13) 3.2.10
V1/T1=V2/T2
Boyle's Law
-states the volume of a gas is inversely proportional to its
pressure (T and n are constant)
P1V1=P2V2
3.2.13
Combined Gas Law
P1V1/T1=P2V2/T2
3.2.14
Math practice on Wkbk page 68 for Tuesday
A. Hand back tests
B. Collect Space Labs
C. Finish 3.2 Notes and demos
-balloon lab
-pop can demo and blow up bottle
D. PDB phase change lab
-3.3 notes
E. Test next Tuesday
Solid naphthalene is slowly heated to melt it.
1. What is the temperature from 4 to 7 minutes?
2. What is happening to the naphthalene from 4-7
minutes? How do you know?
Red Arrows = Exo or Endo?
Blue Arrows = Exo or Endo?
What about evaporation? Why does water turn to a
gas below the vaporization (boiling) point?