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Objectives

Explain the kinetic theory of matter. Distinguish among states of matter in terms of energy, properties, and particle arrangement. CLE 3202.1.8 Investigate the relationship among the pressure, temperature, and volume of gases and liquids.

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Objectives

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  1. Explain the kinetic theory of matter. • Distinguish among states of matter in terms of energy, properties, and particle arrangement. CLE 3202.1.8 Investigate the relationship among the pressure, temperature, and volume of gases and liquids. Knox County Performance Indicator: The student will be able to identify the four states of matter based on volume, shape, and particle arrangement. Objectives

  2. Kinetic Theory Explains how particles in matter behave. 16-1

  3. A. Sates of matter - solid, liquid, gas, plasma

  4. MATTER – anything that has mass and takes up space.

  5. 2. Kinetic Theory of Matter - explains how particles in matter behave.

  6. All matter is composed of small particles. • The particles are in constant, random motion. • Particles collide with each other and walls of their containers.

  7. 3. Thermal energy – total energy of a material’s particles; causes particles to vibrate in place.

  8. Average kinetic energy a. Temperature of the substance, or how fast the particles are moving; b. All particles move with kinetic energy when heat is added.

  9. c. The lower the temperature, the slower the particle motion. d. The higher the temperature, the faster they move.

  10. e. All states of matter expand and become less dense when heat is added.

  11. States of Matter

  12. Explain the kinetic theory of matter. • Distinguish among states of matter in terms of energy, properties, and particle arrangement. CLE 3202.1.8 Investigate the relationship among the pressure, temperature, and volume of gases and liquids. Knox County Performance Indicator: The student will be able to identify the four states of matter based on volume, shape, and particle arrangement. Objectives

  13. 5. Solid state – particles are closely packed together in a specific type of geometric arrangement.

  14. Definite shape, definite volume • Particles vibrate but do not move out of position. • Particles held close together by forces between them. • Examples: ___________

  15. Solids

  16. 6. Liquid state – a solid begins to liquefy at the melting point - the particles gain enough energy to overcome their ordered arrangement.

  17. No definite shape, but definite volume. • Liquid particle have more space between them allowing them to flow and take the shape of their container.

  18. C. Particles are held close together, but not attracted as strongly as particles in a solid, higher KE d. Example___________

  19. Liquids

  20. e. Energy required to reach the melting point is called heat of fusion.

  21. 7. Gaseous state –particles have enough energy to escape the attractive forces of the other particles

  22. No definite shape, no definite volume • Particles separate and move freely to fill the entire space of the container and can be squeezed into a smaller space.

  23. Gases

  24. c. Examples: ______ d. Heat of vaporization is the energy required for a liquid to change to a gas.

  25. e. At the boiling point, the pressure of the liquid’s vapor is equal to the pressure of the atmosphere, and that liquid becomes a gas.

  26. f. Gas particles spread evenly throughout their container in the process of diffusion.

  27. 8. Heating curve of a liquid – as a solid melts and a liquid vaporizes, the temperature remains constant; the temperature will increase after the attractive forces of the earlier state have been overcome.

  28. Plasma

  29. 9. Plasma state of matter consisting of extremely high-temperature gas with positively and negatively charged particles. (gas-like)

  30. Most common state of matter in the universe. • No definite shape, no definite volume. c. Examples:________

  31. Thermal Expansion – characteristic of materials that cause it to expand when heated and contract when cooled. 1. Most matter expands or increases in the size when the temperature increases. 2. The size of a substance will contract or decrease when the temperature decreases.

  32. 3. Expansion and contraction occur in most solids, liquids, and gases.

  33. 4.Water is an exception because it expands as it becomes a solid.

  34. Chart – Phases of Water

  35. Changing states of matter requires energy Changes of State

  36. Types of Solids Some substances do not react as expected when changing states.

  37. 1. Crystalline – has a repeating geometric shape Types of Solids

  38. 2. Amorphous solids – lack the tightly ordered structure found in crystals

  39. Thick liquid like substance with definite shape • Do not have definite temperature at which they change from solid to liquid • Ex. Glass, plastic

  40. Amorphous – will hold a definite shape

  41. Liquid crystals do not lose their ordered arrangement completely upon melting; used in liquid crystal displays in watches, clocks, calculators, and some notebook computers.

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