Transcript Solids, Liquids & Gases

State Standard: Students know each
element has distinct properties and
structure. Students know the states of
matter depend on molecular structure.
Students know chemical reactions
rearrange the molecular structure of
molecules.
I. States of Matter
 A. Solids
 Definite shape and volume
 Particles packed closely together
 Tightly fixed in one position
 Particles can only vibrate
 Types
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Crystalline Solids
Amorphous Solids
Solid Video
 Eureka Solids Video
Crystalline Solids
 Regular repeating
pattern
 Create crystals
 Melts at specific T°
Amorphous Solids
 Particles not arranged
in pattern
 NO distinct melting
point
 May become soft
 May change into
another substance
B. Liquids
 Definite volume, no shape
 Particles packed close, but move freely
 Particles can collide and move past one another
 Fluid or substance that flows
Liquid Video
 Eureka Liquid
Properties of Liquids
 Surface tension: inward pull of molecules near the
surface to be closely packed together
 Viscosity: resistance to flow or movement
 High viscosity: slow movement
 Low viscosity: move fast
Properties of Liquids
C. Gases
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Type of fluid
Change volume easily
Particles squeezed together or spread apart
Particles move in all directions
No shape
No volume
More energy
More motion
What am I?
What are the particle arrangements?
D. Plasma
 1. gas to plasma
 a. sun or stars
 b. lighting
 2. Properties
 a. glow brightly
Conducting electricity
3. Particles
a. ionized gas

-exposure to heat & radiation
free e- and + charged protons
from nucleus
b. Lack electrons in valence
shell
c. respond 2 electric &
magnetic fields
II. Changes of State
 A. Changes between Solids & Liquids
 Change in thermal energy = change in molecular
motion

Particles vibrate enough to break free of position
 Liquids contain more thermal energy than solids
 Melting occurs due to temperature
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Changes with air pressure
 Freezing: molecules slow in motion and become
fixed in a position
 Physical Changes: melting & freezing
B. Changes between Liquid &Gas
 Vaporization
 Particles in liquid gain
energy to form gas
 Examples: evaporation or
boiling
 Evaporation
 Only occurs at surface
 Boiling
 Occurs below and at
surface
 Forms bubbles that rise
and move to surface
 Boiling point= T° at which
liquid boils
 Changes with air pressure
 Condensation
 Reverse of vaporization
 Warm air meets a cool
surface
 Loss of thermal energy
 Motion of particles decreases
 Physical change

reversible
C. Changes between Solid & Gas
 Sublimation: surface particles of solid gain energy
to form gas
 Freedom of particle motion increases
 Solid absorbs thermal energy
 Example: dry ice aka solid carbon dioxide
 Absorbs surrounding thermal energy
 Changes to gas and cools water vapor in air
III. Behavior of Gases
 A. Measuring Gases
1. Volume
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Measured in cubic meters, milliliters, liters
Gas moves and fills space of container
2. Temperature
 atoms constantly moving
 Temp. measure of average energy of motion
3. Pressure
 particles collide due to movement
 particles create outward push on container
 particles move from high pressure to low
pressure
 P measured in pascals
Gases
 Condensation and Evaporation
Temperature and Volume
 Charles’ Law
 Volume of gas
changes with T°
 Cold T°= less
volume
 Hot
temperature =
greater volume
 Charles' Law
Pressure and Volume
 Boyle’s Law
 Measured volume of
gas at different
pressures
 Pressure of gas at
constant temperature
the volume decreases
 Pressure on gas
decreased the volume
increases
Boyle’s Law
Graphing Boyle’s Law
Pressure and Temperature
 Increased temperature = increased pressure
 Particles with more energy collide and move
faster creating more force
 All particle movement sum is net force