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CH 3- States of Matter 2
What makes up matter?
What is the difference between a solid, a
liquid, and a gas?
What kind of energy do all particles of
matter have?
Kinetic theoryKinetic Theory
3 Parts
1. All matter is made of tiny particles.
2. These tiny particles are always in motion.
The higher the temperature, the faster the particles move.
3. At the same temperature, more massive (heavier) particles move slower
Animation
CH 3- States of Matter 3
� Kinetic Molecular Theory:
� This motion is different for the 3 states of matter.
Copyright © 2010 Ryan P. Murphy
6
State the three parts of Kinetic Theory
Kinetic theory
CH 3- States of Matter 4
States of Matter
When a substance changes from one phase of matter to another, the identify of the substance does NOT change. • Water freezes to a
solid and melts to a liquid, but it is still just water.
States of MatterMicroscopic view of matter
CH 3- States of Matter 5
• Activity! Describing Solid-Liquid-Gas
– Please fill out the following spreadsheet and then
collect data.
– Find it or write (?)
Solid Liquid Gas
Volume L*W*H
Shape
Mass
Copyright © 2010 Ryan P. Murphy
• Activity! Describing Solid-Liquid-Gas
– Possible Answers!
Solid Liquid Gas
Volume
Shape
Mass
Copyright © 2010 Ryan P. Murphy
Easy to find –
in ml or cm3
Many different forms. Easy to mold.
Generally Heavy / Weigh in grams
Easy to find.
Easy to find. Use graduated cylinder – ml
Takes shape of the container.
Generally Heavy / Weigh in grams.
Difficult to find in a classroom ����.
No Shape ����
Lighter in mass / Harder to weigh in a classroom ����
CH 3- States of Matter 6
SOLIDS
•Solids have a definite shape and
volume
•The particles are held closely together
by strong attractions
•Packed close together
•Vibrate in place.
•Don’t flow
States of Matter
Characteristics of Solids
_______ have a rigid
structure.
– They do not need
a container to
maintain shape.
But they can still
________ in
place.
Solids
vibrate
Fill in the blanks
CH 3- States of Matter 7
Characteristics of Solids
Definite volume and a definite shape.
Particles are packed close together in relatively fixed positions.
Particles are held by strong attractive forces between them.
Particles vibrate about in a fixed position.
LIQUIDS
States of Matter
1. Has a definite volume but no definite shape.• Volume remains the same, but shape changes.
2. Take shape of container.
3. Particles are held close together but can
flow freely.
4. The particles in a liquid move much faster
than in a solid. • This allows the particles of a liquid to temporarily
overcome the attractive forces between them.
Characteristics of Liquids
CH 3- States of Matter 8
________ can fill the
bottom of their container.
Particles are close
together, but not as close
as particles in a
_________.
Liquids
solid
CH 3- States of Matter 9
Characteristics of Liquids
Definite volume and not definite shape.
Particles are close together
Takes shape of container
Particles flow freely and slide past each other
GASES
States of Matter
Characteristics of Gases
CH 3- States of Matter 10
A ______ expands to fill any available
space.
–_______ can exert pressure on their
container.
gas
Gases
•These particles are approximately 10 times farther apart than those of a liquid or solid.
Characteristics of Gases
Gases
Gases
Gases
Attractive forces
between gas
particles are much
weaker than those in
liquids and solids.
Particles move very
rapidly and are at
great distance from
one another.
No definite
shape nor
definite volume.
CH 3- States of Matter 11
PLASMA
States of Matter
Characteristics of Plasma
Ionized gas that emits electrons.
High-energy plasma collides
with gas particles.
• Plasmas are similar to gases but have some properties
that are different.• Example: plasmas conduct electric current, while gases do
NOT!
• The glow of fluorescent light is caused by artificial plasma
which is formed by passing electric currents through gases.
PLASMA
States of Matter
CH 3- States of Matter 12
Energy is the ability to change or move matter, or to do work.
The energy of motion is called kinetic energy
Because atoms and molecules are always in motion, all particles of matter have kinetic energy.
Energy’s Role
CH 3- States of Matter 13
Energy’s Role
Which is a solid,
which is a liquid,
and which is a gas?
Gas
Solid
Liquid
CH 3- States of Matter 14
• Identify as a Solid, Liquid, Gas, Plasma
Copyright © 2010 Ryan P. Murphy
CH 3- States of Matter 19
Chapter 3.2 Changes of State
• What happens when a substance changes
from one state of matter to another?
• What happens to mass and energy during
physical and chemical changes?
Energy and Changes of State
– The identity of a substance does not change during a change in state
– The ability to change or move matter
• As you add energy to a liquid, the temperature
goes up separating molecules
– Some changes of state require energy
• Melting, evaporation and sublimation
CH 3- States of Matter 20
• The change of state from a liquid to a gas
Energy and Changes of State
• Boiling Point- The temperature
at which a liquid boils.
• The temperature of boiling water is
100oC on the celsius scale and 212oF
on the Fahrenheit scale.
• The temp in the room is about 22°C
and 70°F.
• Are the following temperatures hot or
cold?
65°F
CH 3- States of Matter 21
• The process in which a solid changes
directly into a gas
Sublimation
Ex. Dry ice (Carbon dioxide in the solid
form) changes directly from a solid to a gas
Video Clip
Melting Point• The temperature at which a substances
changes from solid to liquid.
• Melting point depends on the pressure.
32 degrees F
0 degrees C
CH 3- States of Matter 22
• Energy is released in some changes of
state
– Freezing and condensation
Name the physical phase
change
Copyright © 2010 Ryan P. Murphy
Freezing
Melting
Sublimation
Evaporation
Condensation
CH 3- States of Matter 23
Solid Liquid Gas
sublimation
Freezing Condensation
Melting Boiling or
evaporation
CH 3- States of Matter 24
47
Look at the vertical lines.
What is the energy doing if it is not increasing the temperature?
Why are the arrows on each side of the graph the same length?
En
erg
y o
f S
ys
tem
CH 3- States of Matter 25
• Please sketch the following into your
notes
Copyright © 2010 Ryan P. Murphy
What is the name of the first
electricity detective?
Sherlock Ohms
Joke of the Day
CH 3- States of Matter 26
Copyright © 2010 Ryan P. Murphy
Energy
Energy
Su
blim
atio
n
De
po
sitio
n
Copyright © 2010 Ryan P. Murphy
CH 3- States of Matter 27
• The temperature of a substance does not
change during a change of state.– For example, if you add energy to ice at 0oC,
the temperature will NOT rise until all of the ice has melted.
– When energy is added – Move up a step.
– When energy is removed – Go down a step.
Heat added
Tem
pera
ture
(oC
)
0
100
MeltingIce
Water
Water VaporBoiling
Copyright © 2010 Ryan P. Murphy
CH 3- States of Matter 28
• Latent Heat: The energy absorbed or
released when a substance changes its
physical state.
Heat added
Tem
pera
ture
(oC
)
0
100
MeltingIce
Water
Water VaporBoiling
Latent Heat
Latent Heat
Copyright © 2010 Ryan P. Murphy
• Mass cannot be created or destroyed.
• Matter can change form, and turn into
different forms, but the TOTAL mass stays
the same.
• Gas has mass!
Conservation of Mass and Energy
CH 3- States of Matter 29
The Law of conservation of energy
• Energy cannot be created or destroyed.
– Energy can convert from one form to another, but the TOTAL energy, before and after the change, is the same.
Conservation of Mass and Energy
• In any physical or chemical change, matter is
neither created nor destroyed
– Matter can be changed from one form to another.
Copyright © 2010 Ryan P. Murphy
Heat
Law Conservation of Matter
Conservation of Mass and Energy
CH 3- States of Matter 30
• Law Conservation of Matter
Copyright © 2010 Ryan P. Murphy
Chapter 3.3 Fluids• How do fluids exert pressure?
• What force makes a rubber duck float in a bathtub?
• What happens when pressure in a fluid changes?
• What affects the speed of a fluid in motion?
CH 3- States of Matter 31
Fluids• A nonsolid state of matter in which the atoms
or molecules are free to move past each other.
• Liquids and gases are fluids, because their particles can move past each other.
• Pressure is the amount of force exerted on a given area of surface.
• Fluids exert pressure evenly in all directions. How does the pressure change if you remove
some of the air?
Pressure
CH 3- States of Matter 32
• The SI unit of pressure is the pascal.
– One pascal (1 Pa) is the force of one newton exerted over an area of one square meter (1N/m2).
• The newton is the SI unit of force.
Pressure
Pressure = forcearea
P = FA
Blaise Pascal
• Buoyancy is the force with which a more dense fluid pushes a less dense fluid substance upward.
• All fluids exert an upward buoyant force on matter.
• Archimededs’ principle is used to find buoyant force.
Buoyant Force
How does this relate to me?
–Buoyancy tells me whether or
not an object will float.
CH 3- States of Matter 33
Archimedes Principle
• The buoyant force on an object in a fluid
is an upward force that equals the weight
of the fluid that the object displaces.
Buoyant Force
66
Archimedes Principle
• Explains why a steel ship
floats!
CH 3- States of Matter 34
Density
• An object will float or sink based on its density.
• You can determine if a substance will float or sink by comparing densities.
Buoyant Force
Pascal’s Principle
• A change in pressure at any point in an enclosed fluid
will be transmitted equally to all parts of the fluid.
P=force/ area
Hydraulic devices are based on Pascal’s Principle.
CH 3- States of Matter 35
How does this relate to me?
Viscosity tells me how
thick a liquid or gas is.
Fluids In Motion
• Fluids move faster through small areas than through larger areas.
• Rates at which they flow also varies.
• Viscosity is the resistance of a fluid to flow.
Which has a greater
viscosity? Water or honey
Stronger attraction between particles, the more viscous
70
CH 3- States of Matter 37
Chapter 3.4 Behavior of Gases
• What are some properties of gases?
• How can you predict the effects of
pressure, temperature, and volume
changes on gases?
Think about this…….
The gas in the toy balloon expands outward, as shown below. After this expansion, does the pressure of the gas
a. increase?
b. decrease?
c. remain unchanged?
The temperature of the water vapor in the pressure cooker increases. Does the pressure of the gasa. increase?b. decrease?c. remain unchanged?
Volume goes up
Pressure goes down
Temperature increases
Pressure increases
CH 3- States of Matter 38
Properties of Gases
• Have low densities and are
compressible.
• Mostly empty space.
• Gases fill containers
uniformly and completely.
• Gases diffuse and mix
rapidly.
• The gas laws will help you understand
and predict the behavior of gases in
specific situations.
• Boyle’s Law (relates pressure to volume)
• Gay-Lussac’s Law (relates pressure to temperature)
• Charles’s Law (relates temperature to volume)
Gases Laws
CH 3- States of Matter 39
Boyle’s Law
Robert Boyle (1627-1691). Son of Earl of Cork, Ireland.
• Boyle’s law relates the pressure of a gas to its volume.
• For a constant temperature, as the pressure goes up the volume goes down.
• As the volume goes up the pressure goes down.
Gases Laws
Pressure Volume
Temperature is constant
• A bicycle pump is an
example.
• As the volume of the
air trapped in the
pump is reduced, its
pressure goes up, and
air is forced into the
tire.
Gases Laws
Boyle’s Law
CH 3- States of Matter 40
(pressure1) (volume1) = (pressure2) (volume2)
P1V1 = P2V2
Gases Laws
Boyle’s Law
The gas in a balloon has a volume of 7.5 L at 100.0 kPa. In the atmosphere,
the has expands to a volume of 11 L. Assuming a constant temperature, what
is the final pressure in the balloon?
V1 =
P1=
V2 =
P2 = ?
V1 = 7.5 L
P1= 100.0 kPa
V2 = 11 L
P2 = ?
P1V1 = P2V2
P2= P1V1
V2
P2= (100.0 kPa)(7.5 L)
11 L
P2= 68 kPa
• Relates gas pressure to temperature.
• The pressure of a gas increases as the
temperature increases.
• If the volume of the gas does not change.
The pressure decreases as the
temperature decreases.
Gases Laws
Gay-Lussac’s Law
Volume is constant
Pressure Temperature
P lower in winter than summer
CH 3- States of Matter 41
• Charles’s law relates temperature to volume.
• For a fixed amount of gas at a constant pressure, the volume of the gas increases as the gas’s temperature increases.
• Likewise, the volume of the gas decreases as the gas’s temperature decreases.
Gases Laws
Charle’s Law
Pressure is constant
Volume Temperature
Charles’s Law