Warm Up: (5 minutes)
1. GET BINDERS OUT READY TO TAKE NOTES! (-5
FOR ANYONE NOT READY ONCE bell rings!)
2. We have learned about four states of matter, in
which of the following 3 states do particles
move the MOST  solids, liquids, or gases? (Do
not have to write question, but answer in
complete sentence).
3. What is the relationship between how fast these
particles move and the shape and volume this
state of matter has? (2 sentences) (Write question
and answer)
Announcements
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New TOP 10
Doughnuts Friday Morning
Quiz on Friday – States of Matter & Gas Laws
Grades – next class
TEDx Interviews today
Answer to DO NOW
• What is the relationship between how fast
these particles move and the shape and
volume this state of matter has? (2 sentences)
• Particles in a gas are well separated with no
regular arrangement/pattern. Gas particles
move freely/collide at high speeds.
GASES!
Get your notes set up:
1.Title: Gas Laws
2.Date your notes in top right
Kinetic Molecular Theory
• How particles in matter behave!
–All matter is composed of particles
–Particles are in constant motion
–Particles also collide with other
particles and may lose some
energy
SOLID
DO NOT NEED TO COPY, you already know!
•
•
•
•
•
Molecular Motion: Atoms vibrate in place
Packed closely together
Arranged in a geometric pattern
Heat Index: At its freezing point
Attraction: Very close together
LIQUID
DO NOT NEED TO COPY
• Molecular Motion: atoms able
to slide by one another
• Attraction: Still able to cling to
each other
• More kinetic energy
• To slip out of the solid state, the particles
had to gain in kinetic energy
• Heat Index: Melting Point –
when particles slip from a solid
to a liquid
PLASMA
DO NOT NEED TO COPY
• Most common state in the universe
• Positively charged particles
Molecular Motion: Moves extremely fast –
electrons are stripped off Electrically charged
GAS
• Molecular Motion: Freely floats around
• Attraction: No Attraction
• Will fill whatever container it is living in.
• Heat Index: Vaporization – when liquid becomes a
gas
– Must escape its attractive forces
Standards by ClayCo
• Just finished  SPS5a. Compare and contrast
the atomic/molecular motion of solids,
liquids, gases and plasmas.
• Now  SPS5b. Relate temperature, pressure,
and volume of gases to the behavior of gases.
• Enduring understanding 
For gaseous substances,
pressure, volume, and
temperature are
interdependent.
OBJECTIVES
• YOU will be able to identify Boyle’s Law,
Charles Law, & Guy-Lussac’s Law
• YOU will be able to relate temperature,
pressure, and volume to the behavior of
gases.
NEW VOCAB
• Today we are covering:
• Intermolecular attraction – The amount of "stick
togetherness"
• Temperature – intensity of heat
• Pressure - exertion of force upon a surface by an
object (force per unit of area)
• Specific Heat - amt of heat per unit mass required
to raise the temp by one degree Celsius
Gases- Pressure
Which balloon has HIGHER pressure?
Vote:
1
2
Gases- Pressure
What is it?
Pressure is the amount of force exerted on a container from within, it
is caused by gas particles colliding with each other.
Do MANY or FEW collisions cause a lot of pressure?
MANY, the more particles collide the more they Hit the walls of their
container, putting force on the walls
Does having MORE or FEWER particles cause many
collisions?
MORE, the more particles there are the more collisions there will be
Boyle’s Law
• Robert Boyle (1627 –
1691) British
• Decrease the volume of
the container of gas + a
constant temperature =
pressure of the gas will
increase
• Increase the volume of
the container of gas +
constant temperature =
pressure of gas will
decrease
Boyle’s Law
As the pressure of a gas
increases
the volume
of that gas decreases .
When Temperature is
constant.
(inversely proportional)
Pressure and Volume
(WHEN THE AMOUNT OF GAS IS CONSTANT)
Use arrow (up = increase, down = decrease) to
fill in the blanks under the diagram
V
P
V
P
Pressure and Volume
(WHEN THE AMOUNT OF GAS IS CONSTANT)
Use arrow (up = increase, down = decrease) to
fill in the blanks under the diagram
V
P
V
P
Boyles Law
P V =P V
1
1
2
2
Charles Law
• Jacques Charles (1746 –
1823) – French
• Volume of gases
increases with increasing
temperature as long as
pressure doesn’t change.
• Volume of gases
decreases with
decreased temperature
as long as pressure
doesn’t change.
Charles’s Law
As the temperature of a
gas increases the
volume of that gas
increases . The
pressure is constant.
(directly proportional)
Temperature
Temperature
Charles Law
V =V
T T
1
2
1
2
Guy-Lussac’s
Law
As the temperature of
a gas increases the
pressure of that gas
increases . When
volume is constant.
(directly proportional)
Temperature
Temperature
Guy Lussac’s Law
P =P
T T
1
2
1
2
Practice BOYLE
Prediction  solve
P1 = 20 atm
V1 = 1 L
P2 = 10 atm
V2 = ? (greater than or less than 1 L?)
Atm = atmospheric pressure (units of pressure)
Practice CHARLES
Prediction  solve
T1 = 300 K
V1 = 5 L
T2 = 150 K
V2 = ? (greater than or less than 5 L)
Practice GUY LUSSAC
Prediction  solve
P1 = 20 atm
T1 = 100 K
P2 = 80 atm
T2 = ? (greater than or less than 100 K)
Conclusion (2 min)
In your notes, write down your answer to this
question:
What does the set up of each equation tell us
about how those two variables affect each
other?
• Boyle's gas law states: the volume of a gas is
inversely proportional to the pressure of the
gas when temperature is held constant.
• Gay-Lussac's law states: @ constant volume,
the pressure of a gas is directly proportional to
its temperature.
• Charles' Law states: If the pressure of a gas
sample is kept constant, the volume of the
sample will vary directly with the temperature