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STATES OF MATTER CHAPTER 3

STATES OF MATTER CHAPTER 3. KONICHEK. DOES IT REALLY MATTER?. I. Classification of matter A. solids-definite shape and volume 1. atoms are in an exact positions—just sit and vibrate

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STATES OF MATTER CHAPTER 3

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  1. STATES OF MATTER CHAPTER 3 KONICHEK

  2. DOES IT REALLY MATTER? • I. Classification of matter • A. solids-definite shape and volume • 1. atoms are in an exact positions—just sit 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)

  3. STATES OF MATTERSOLIDS • Particles of solids are tightly packed, vibrating about a fixed position. • Solids have a definite shape and a definite volume. Heat

  4. STATES OF MATTERLIQUID • 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

  5. STATES OF MATTERGAS • Particles of gases are very far apart and move freely. • Gases have an indefinite shape and an indefinite volume. Heat

  6. 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 quantum level

  7. 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

  8. 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.

  9. 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

  10. PRESSURE’S ON!!!! • 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.

  11. V. Factors which affect gas pressure • A. Temperature-raises the average ke of the particles. • . 1. Raising temp of a gas will increase the pressure if the volume is kept constant. • B. Volume-Reducing the volume of a gas increases the pressure if the temp and number of particles are constant. • C. Particles- Increasing the number of particles will increase pressure if temp and volume are constant

  12. 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

  13. VII. Phase Changes.- A reversible physical change from one state to another. • A.Melting,freezing,vaporization, condensation,deposition, sublimation • B. Temperature always remains constant during a phase change.

  14. 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)

  15. IX. Melting and freezing • A. melting- The force of attraction between particles is diminished because their overall energy content has increased. • 1.moving farther apart • B. freezing- the force of attraction is increasing because the overall energy content of the particle is decreasing • 1. moving closer together

  16. PHASE CHANGES

  17. 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.

  18. PHASE CHANGES

  19. 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. • 1. temp doesn’t rise during boiling • D. Condensation- when a gas becomes a liquid

  20. STATES OF MATTER LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

  21. 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

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