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Chapter 3 – States of Matter

Chapter 3 – States of Matter. 3.1 Solids, Liquids, and Gases. Solids Definite Shape Definite Volume Particles vibrate in fixed positions Particles have low kinetic energy. Liquids Variable shape (takes the shape of the container) Definite Volume Particles can move around each other

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Chapter 3 – States of Matter

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  1. Chapter 3 – States of Matter

  2. 3.1 Solids, Liquids, and Gases • Solids • Definite Shape • Definite Volume • Particles vibrate in fixed positions • Particles have low kinetic energy

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

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

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

  6. 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

  7. 3.2 The Gas Laws • Pressure = the result of force distributed over an area • More Collisions=More Pressure • In a closed container, gases exert pressure when the particles of the gas collide with the walls of the container.

  8. 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

  9. 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

  10. 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

  11. Gas Laws • Charles’ Law – volume of a gas is DIRECTLY PROPORTIONAL to temperature • Inc. Temp. x2  Inc. Vol. x2 V1 = V2 T1 T2

  12. Boyle’s Law – volume of a gas is INVERSELY PROPORTIONAL to pressure • Inc. Vol. x2  Dec. pressure by ½ P1V1 = P2V2

  13. Combined Gas Law • The Combined Gas Law – relates temperature, volume and pressure of a gas. • Formula: P1V1 = P2V2 T1 T2

  14. 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

  15. Melting and Freezing • Melting • Solid changes to liquid • Particles absorb energy (endothermic) • Particles become less orderly

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

  17. 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

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

  19. 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)

  20. Phase Change Diagram

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