Chapter 3

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Chapter 3 States of Matter
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3.1 Solids, Liquids, and Gases

• Solids
• Definite Shape
• Definite Volume
• Particles vibrate in fixed positions
• Particles have low kinetic energy

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• Liquids
• Variable shape (takes the shape of the container)
• Definite Volume
• Particles can move around each other
• Particles have medium Kinetic Energy

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• Gases
• Variable shape
• Variable volume (fills all space in a container)
• Particles move about freely
• Particles have high Kinetic Energy

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• Plasma
• Exists only at extremely high temperatures
• 99 of the matter in the UNIVERSE is plasma
• Stars are plasma
• Bose-Einstein Condensate
• Exists only at extremely low temperatures
• Groups of atoms behave as a single particle

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Kinetic Theory

• Kinetic energy energy an object has due to its
  motion
• The faster an object is moving the greater its
  kinetic energy.
• Kinetic theory states that all particles of
  matter are in constant motion.
• View animation on visual concepts CD

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3.2 The Gas Laws

• Pressure the result of force distributed over
  an area
• More CollisionsMore Pressure
• In a closed container, gases exert pressure when
  the particles of the gas collide with the walls
  of the container.

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Factors That Affect Gas Pressure

• Temperature raising temp. will increase
  pressure if volume of gas and of particles are
  kept constant
• Inc. in temp. ? part. move faster ? part. collide
  with walls more frequently ? increased pressure

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• Volume Decreasing volume of a gas causes an
  increase in pressure if the temp. and of part.
  are constant
• Decrease in vol. ? less space ? particles collide
  with walls more often ? inc. pressure

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• Number of particles increasing the number of
  particles of a gas will increase pressure if
  temp. and volume are constant
• Inc. of particles ? particles collide with
  container more often ? inc. pressure

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Gas Laws

• Charles Law volume of a gas is DIRECTLY
  PROPORTIONAL to temperature
• Inc. Temp. x2 ? Inc. Vol. x2
• V1 V2
• T1 T2

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• Boyles Law volume of a gas is INVERSELY
  PROPORTIONAL to pressure
• Inc. Vol. x2 ? Dec. pressure by ½
• P1V1 P2V2

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• The Combined Gas Law relates temperature,
  volume and pressure of a gas.
• P1V1 P2V2
• T1 T2

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3.3 Phase Changes

• Phase change reversible physical change that
  occurs when a substance changes from one state of
  matter to another
• Temperature of a substance DOES NOT CHANGE during
  a phase change.
• Energy is either absorbed or released during a
  phase change.
• Endothermic energy is absorbed
• Exothermic energy is released

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Melting and Freezing

• Melting
• Solid changes to liquid
• Particles absorb energy (endothermic)
• Particles become less orderly

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• Freezing
• Liquid changes to solid
• Particles release energy (exothermic)
• Particles become more orderly

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Vaporization and Condensation

• Vaporization
• Liquid changes into a gas
• Particles absorb energy (endothermic)
• Particles become LESS orderly and more free to
  move
• 2 types of vaporization
• Evaporation takes place at the surface of a
  liquid
• Boiling occurs when a liquid is heated to its
  boiling point

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• Condensation
• Gas changes to a liquid
• Particles release or lose energy (exothermic)
• Particles become MORE orderly

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Sublimation and Deposition

• Sublimation
• Changing from a solid
• directly to a gas
• Energy is absorbed
• (endothermic)
• Deposition
• Changing from a gas directly to a solid
• Energy is released (exothermic)

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Phase Change Diagram