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 MATTER SOLIDS Particles of solids are tightly packed, vibrating about a fixed position. Solids have a definite shape and a definite volume. Heat

4. 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

5. STATES OF MATTER GAS  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 II. Other states of matter A. Plasma- exist at very high temperatures A. Plasma- exist at very high temperatures 1. stars, Lightning 1. stars, Lightning 2. Most abundant form of matter in the universe( stars) 2. Most abundant form of matter in the universe( stars) B. Bose-Einstein condensate- Exist at very low temperatures B. Bose-Einstein condensate- Exist at very low temperatures 1. temperatures near 0 Kelvin 1. temperatures near 0 Kelvin 2. All the electrons fall to the lowest quantum level 2. All the electrons fall to the lowest quantum level

7. III. Kinetic Theory of matter A. Describes how matter behaves A. Describes how matter behaves B. Basic assumptions B. Basic assumptions 1.matter is made of particles constantly in motion. 1.matter is made of particles constantly in motion. 2.The particles are constantly colliding with each other without losing energy(perfect elastic collisions) 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 3. the temperature depends upon the average Ke of the particles

8. C. Motion in gases- Very random C. Motion in gases- Very random 1.Average velocity is 1600Km/hr. 1.Average velocity is 1600Km/hr. 2. Very little attraction between particles. 2. Very little attraction between particles. D. The constant motion of gases allow them to fill the container of any shape or volume. D. The constant motion of gases allow them to fill the container of any shape or volume.

9. E. Explaining the Behavior of liquids. E. Explaining the Behavior of liquids. 1. Average velocity is much slower than gases. 1. Average velocity is much slower than gases. 2. particles are closer together. 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 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/m 2 = 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. V 1 /T 1 =V 2 /t 2 B. Boyles law-The volume is inversely proportional to the pressure of a Gas. 1. P 1 V 1 =P 2 V 2

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 Description of Phase Change Term for Phase Change Heat Movement During Phase Change Solid to liquid Melting Heat goes into the solid as it melts. Liquid to solid Freezing Heat leaves the liquid as it freezes.

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 Description of Phase Change Term for Phase Change Heat Movement During Phase Change Liquid to gas Vaporization, which includes boiling and evaporation Heat goes into the liquid as it vaporizes. Gas to liquidCondensation Heat leaves the gas as it condenses. Solid to gasSublimation Heat goes into the solid as it sublimates.

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

21. STATES OF MATTER SOLID LIQUID GAS PLASMA 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

22. XI Sublimation and deposition XI Sublimation and deposition A. Sublimation- The process of going directly from a solid to a gas A. Sublimation- The process of going directly from a solid to a gas 1. Endothermic Rx 1. Endothermic Rx 2. dry Ice, ice Cubes in the freezer 2. dry Ice, ice Cubes in the freezer B. Deposition- when a gas vapor goes directly into a solid state. B. Deposition- when a gas vapor goes directly into a solid state. 1. Water vapor on a cold Plate of Glass 1. Water vapor on a cold Plate of Glass