STATES OF
MATTER
CHAPTER 3
KONICHEK
DOES IT REALLY MATTER?
 I. Classification of matter
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A. solids-definite shape and volume
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1. atoms are in an exact positions—just sit
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and vibrate
B. Liquid- no definite shape, but a definite
volume.- Takes the shape of its container(fluid)
2. atoms flow around each other
C. Gas(- No definite shape or volume.
3. atoms move freely- takes shape of its
container(fluid)
STATES OF MATTER
SOLIDS
•Particles of solids are
tightly packed, vibrating
about a fixed position.
•Solids have a definite
shape and a definite
volume.
Heat
STATES OF MATTER
LIQUID
 Particles of liquids are
tightly packed, but are
far enough apart to
slide over one
another.
 Liquids have an
indefinite shape and a
definite volume.
Heat
STATES OF MATTER
GAS
 Particles of gases
are very far apart
and move freely.
 Gases have an
indefinite shape
and an indefinite
volume.
Heat
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II. Other states of matter
A. Plasma- exist at very high temperatures
1. stars, Lightning
2. Most abundant form of matter in the
universe( stars)
B. Bose-Einstein condensate- Exist at very low
temperatures
1. temperatures near 0 Kelvin
2. All the electrons fall to the lowest
III. Kinetic Theory of matter
A. Describes how matter behaves
B. Basic assumptions
1.matter is made of particles
constantly in motion.
2.The particles are constantly
colliding with each other without losing
energy(perfect elastic collisions)
3. the temperature depends upon the
average Ke of the particles
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C. Motion in gases- Very random
1.Average velocity is 1600Km/hr.
2. Very little attraction between particles.
D. The constant motion of gases allow them
to fill the container of any shape or volume.
E. Explaining the Behavior of liquids.
 1. Average velocity is much slower than
gases.
 2. particles are closer together.
 3. the forces of attraction, and molecular
motion explain the behavior of liquids.Liquids take the volume of the container,
and can flow
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PRESSURE’S ON!!!!
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IV. Pressure- Force per unit area
A. P=F/A( units: N/m2 = Pascal)
1. Kilopascal(Kpa) = 1000 pa
B. Caused by collisions of particles
on the wall of the container.
V. Factors which affect gas pressure
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A. Temperature-raises the average ke
of the particles.
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1. Raising temp of a gas will increase
the pressure if the volume is kept
constant.
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B. Volume-Reducing the volume of a
gas increases the pressure if the temp and
number of particles are constant.
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C. Particles- Increasing the number of
particles will increase pressure if temp and
volume are constant
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VI. Gas laws:
A. Charles Law- the volume of a gas is directly
proportional to the temperature (Kelvin), if Pressure
and number of particles is constant.
1. V1/T1=V2/t2
B. Boyles law-The volume is inversely
proportional to the pressure of a Gas.
1. P1V1=P2V2
• VII. Phase Changes.- A reversible physical
change from one state to another.
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A.Melting,freezing,vaporization,
condensation,deposition, sublimation
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B. Temperature always remains
constant during a phase change.
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VIII. Energy and Phase changes.
A. Energy is either absorbed or released.
1. endothermic- absorbing energy( melting
ice to water)
a. heat of fusion of water- the amount of
heat necessary for 1 g of ice to melt into 1 g of
water at the same temp
1. 334j/g
2. Exothermic- Energy is released(freezing
of water to ice)
• IX. Melting and freezing
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A. melting- The force of attraction
between particles is diminished because
their overall energy content has increased.
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1.moving farther apart
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B. freezing- the force of attraction is
increasing because the overall energy
content of the particle is decreasing
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1. moving closer together
PHASE CHANGES
Description of
Phase Change
Solid to
liquid
Term for Phase
Change
Melting
Liquid to
Freezing
solid
Heat Movement During
Phase Change
Heat goes into
the solid as it
melts.
Heat leaves the
liquid as it
freezes.
X. Vaporization and condensation
A. Vaporization-Endothermic
1. the liquid has absorbed enough heat to
become a gas.
2. heat of vaporization- The amount of heat
necessary to change 1 g of a liquid to 1 g of a
solid at the same temperature( water 2260j/g)
3. takes place at the surface of the liquid.
PHASE CHANGES
Description of
Phase Change
Term for Phase
Change
Heat Movement During
Phase Change
Vaporization,
Liquid to
which includes Heat goes into the
gas
boiling and
liquid as it vaporizes.
evaporation
Heat leaves the gas
Gas to liquid Condensation
as it condenses.
Heat goes into the
Solid to gas Sublimation
solid as it sublimates.
• B. Evaporation- when a gas gains enough
energy at temperatures far below boiling to
escape from a liquid.
• C. Boiling-Takes place throughout the
entire liquid.
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1. temp doesn’t rise during boiling
• D. Condensation- when a gas becomes a
liquid
STATES OF MATTER
SOLID
Tightly packed, in
a regular pattern
Vibrate, but do not
move from place
to place
LIQUID
Close together
with no regular
arrangement.
Vibrate, move
about, and slide
past each other
GAS
Well separated
with no regular
arrangement.
Vibrate and move
freely at high
speeds
PLASMA
Has no definite
volume or shape
and is composed
of electrical
charged particles
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XI Sublimation and deposition
A. Sublimation- The process of going directly
from a solid to a gas
1. Endothermic Rx
2. dry Ice, ice Cubes in the freezer
B. Deposition- when a gas vapor goes
directly into a solid state.
1. Water vapor on a cold Plate of Glass