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Chapter 13 Lecture
- 1. Bellwork -State Changes Waterexists on Earth as a liquid, a solid, and a vapor. As water cycles through the atmosphere, the oceans, and Earth’s crust, it undergoes repeated changes of state. You will learn what conditions can control the state of a substance. BELLWORK-name the following phase changes: a)Solid to liquid b) liquid to solid c)Liquid to gas d) gas to liquid e) Solid to gas
- 2. Melting - solidto liquid Freezing- liquid to solid Vaporization- liquid to gas Vapor- a gas that is usually a liquid at room temp Condensation- changing from a gas to a liquid
- 3. Chapter 13- Statesof Matter Intro to Gases The skunk releases its spray! Within seconds you smell that all-too-familiar foul odor. You will discover some general characteristics of gases that help explain how odors travel through the air, even on a windless day.
- 4. 13.1 The Kinetic MolecularTheory explains the behavior of gases.
- 6. The word kineticrefers to motion.
- 7. The word kineticrefers to motion. •The energy an object has because of its motion is called kinetic energy.
- 8. The word kineticrefers to motion. •The energy an object has because of its motion is called kinetic energy. • According to the kinetic theory, all matter consists of tiny particles that are in constant motion.
- 9.
- 10. Kinetic Molecular Theory:GASES • The particles in a gas are small, hard spheres with an insignificant volume.
- 11. Kinetic Molecular Theory:GASES • The particles in a gas are small, hard spheres with an insignificant volume. • The motion of gas particles is rapid, constant, and random.
- 12. Kinetic Molecular Theory:GASES • The particles in a gas are small, hard spheres with an insignificant volume. • The motion of gas particles is rapid, constant, and random. • All collisions between gas particles are perfectly elastic (no energy lost).
- 13. 13.1 Gas particles arein rapid, constant motion.
- 14. 13.1 Gas particles travelin straight-line paths. Gas particles move randomly.
- 15. 13.1 A gas fillsits container.
- 16. 13.1 Kinetic theory explainsgas pressure.
- 17. 13.1 Pressure = Force/Area A force is a push or a pull. Same force more less area area more pressure!
- 19. Which would youprefer? Why?
- 20. 13.1 Kinetic theory explainsgas pressure.
- 21. 13.1 Kinetic theory explainsgas pressure. Gas pressure is the force exerted by gas particles hitting the surface of an object.
- 22. 13.1 Kinetic theoryexplains gas pressure. Gas pressure can KILL!
- 24. An empty spacewith no particles and no pressure is called a vacuum.
- 25. Atmospheric pressure isthe pressure created by the earth’s gravitational pull on the gases in our atmosphere.
- 26. Gas pressure isexerted in all directions.
- 27. A barometer isa device that is used to measure atmospheric pressure.
- 28. Pressure Poem An emptywater bottle, closed tightly at high elevation, will be crushed by the atmosphere at sea level.
- 29. 13.1 Units of Pressure • The SI unit of pressure is the pascal (Pa). • One standard atmosphere (atm) is the atmospheric pressure at sea level.
- 30.
- 31.
- 32. 13.1 450 kPa x kPa
- 33. 13.1 atm 450 kPa x kPa
- 34. 13.1 1 atm 450 kPa x 101.3 kPa
- 35. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa
- 36. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa 450 kPa x
- 37. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa 450 kPa x kPa
- 38. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa mm Hg 450 kPa x kPa
- 39. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa 760 mm Hg 450 kPa x 101.3 kPa
- 40. 13.1 1 atm 450 kPa x = 4.4 atm 101.3 kPa 760 mm Hg = 3400mm Hg 450 kPa x 101.3 kPa
- 41.
- 42. Particles at agiven temperature have a wide range of kinetic energies. Most of the particles have kinetic energies in the middle of this range.
- 43. Particles at agiven temperature have a wide range of kinetic energies. Most of the particles have kinetic energies in the middle of this range.
- 44. Particles at agiven temperature have a wide range of kinetic energies. Most of the particles have kinetic energies in the middle of this range. Temperature measures Average Kinetic Energy
- 45. 13.1 The Kelvin temperatureof a substance is directly proportional to average kinetic energy.
- 46. 13.1 The Kelvin temperatureof a substance is directly proportional to average kinetic energy. The higher the kinetic energy, the higher the temperature.
- 47. 13.1 Two substances withthe same average kinetic energy are at the same temperature. Two substances at the same temperature have the same average kinetic energy.
- 48. 13.1 Absolute zero (0K, or –273.15°C) is the temperature at which the motion of particles theoretically stops.
- 49. 13.1 Absolute zero (0K, or –273.15°C) is the temperature at which the motion of particles theoretically stops. •Particles would have no kinetic energy at absolute zero.
- 50. 13.1 Absolute zero (0K, or –273.15°C) is the temperature at which the motion of particles theoretically stops. •Particles would have no kinetic energy at absolute zero. • Absolute zero has never been produced in the laboratory (and not for lack of trying!).
- 51. Bellwork- Kinetic Energy •Whatis kinetic energy? •How is average kinetic energy related to temperature? •Which has higher kinetic energy, an olympic size pool of water or a cup of hot coffee?
- 52. 13.2 Substances that canflow are referred to as fluids. Both liquids and gases are fluids.
- 53. 13.2 The intermolecular attractions (IMFs)are counteracted by motion of molecules. Together they determine the physical properties of liquids. High IMFs promote a solid state High temps (motion) promote a gas state.
- 54. 13.2 If the liquid is not boiling it is called evaporation.
- 55. 13.2 When aliquid converts to a gas it is called vaporization. If the liquid is not boiling it is called evaporation.
- 56. 13.2 When aliquid converts to a gas it is called vaporization. If the liquid is not boiling it is called evaporation.
- 57. 13.2 When aliquid converts to a gas it is called vaporization. If the liquid is not boiling it is called evaporation.
- 58. 13.2 In a closedcontainer, evaporated molecules collect as a vapor above any liquid. Vapor pressure is the force exerted by a gas above a liquid.
- 59. During evaporation, onlymolecules with a certain minimum kinetic energy can escape from the surface of the liquid.
- 60. During evaporation, onlymolecules with a certain minimum kinetic energy can escape from the surface of the liquid.
- 61. During evaporation, onlymolecules with a certain minimum kinetic energy can escape from the surface of the liquid. Evaporation is a cooling process because the molecules with the highest kinetic energy escape.
- 62. 13.2 In an opencontainer, molecules that evaporate can escape from the container.
- 63. Some evaporated moleculeswill condense back into a liquid.
- 64. Some evaporated moleculeswill condense back into a liquid.
- 65. Some evaporated moleculeswill condense back into a liquid. A dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium when the rate of evaporation equals the rate of condensation.
- 67.
- 68. DYNAMIC EQUILIBRIUM For each molecule that evaporatesa different molecule returns to the liquid.
- 69. DYNAMIC EQUILIBRIUM For each molecule that evaporatesa different molecule returns to the liquid. SAME RATES!!
- 71.
- 72. DYNAMIC EQUILIBRIUM Equilibrium- The amount of liquidand vapor do not change.
- 73. DYNAMIC EQUILIBRIUM Equilibrium- The amount of liquidand vapor do not change. Dynamic- There is a constant turnover of particles.
- 74. 13.2 Vapor pressure increaseswith Temperature.
- 76. The particles haveincreased kinetic energy, so more particles will have the minimum energy needed to escape the liquid.
- 77. When a liquidis heated to a temperature at which particles throughout the liquid have enough kinetic energy to vaporize, the liquid begins to boil.
- 78. Liquids boil whentheir vapor pressure exceeds the pressure pushing down on the liquid (usually atmospheric pressure).
- 79.
- 81. Boiling Point andPressure Changes
- 82. Boiling Point andPressure Changes Because a liquid boils when its vapor pressure is equal to the external pressure, liquids don’t always boil at the same temperature.
- 83. Boiling Point andPressure Changes Because a liquid boils when its vapor pressure is equal to the external pressure, liquids don’t always boil at the same temperature. • At high altitudes, atmospheric pressure is low, so water boils cooler and food needs longer to cook.
- 84. Boiling Point andPressure Changes Because a liquid boils when its vapor pressure is equal to the external pressure, liquids don’t always boil at the same temperature. • At high altitudes, atmospheric pressure is low, so water boils cooler and food needs longer to cook. • A pressure cooker increases the boiling point so food cooks fast.
- 85. Altitude and BoilingPoint
- 86. The normal boilingpoint is the boiling point of a liquid at atmospheric pressure (1 atm or 101.3 kPa)
- 88.
- 89. Solids keep theirshape because their particles are in fixed positions.
- 90. In a crystallinesolid, the particles are in an orderly, repeating, three-dimensional pattern called a crystal lattice. ionic compound elemental metal
- 91. 13.3 When an elementcan make more than one structure, the different forms are called allotropes.
- 92. 13.3 When an elementcan make more than one structure, the different forms are called allotropes. •Allotropes have different properties because their structures are different.
- 93. 13.3 When an elementcan make more than one structure, the different forms are called allotropes. •Allotropes have different properties because their structures are different. • Only a few elements have allotropes.
- 94. 13.3 Carbon’s allotropes arediamond and graphite
- 95. Non-Crystalline Solids Anamorphous solid lacks an ordered internal structure. • Rubber, plastic, asphalt, and glass are amorphous solids.
- 96. Non-Crystalline Solids Anamorphous solid lacks an ordered internal structure. • Rubber, plastic, asphalt, and glass are amorphous solids.
- 97. Quartz is crystallizedSiO2 Glass is amorphous SiO2
- 98. Non-Crystalline Solids Quartz iscrystallized SiO2 Glass is amorphous SiO2
- 99. Non-Crystalline Solids An amorphous solid lacks an ordered internal structure. Quartz is crystallized SiO2 Glass is amorphous SiO2
- 100. Non-Crystalline Solids An amorphous solid lacks an ordered internal structure. •A glass has cooled to a rigid state without crystallizing. Quartz is crystallized SiO2 Glass is amorphous SiO2
- 101.
- 102. 13.4 The change ofa substance from a solid to a vapor without passing through the liquid state is called sublimation. Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature.
- 103. 13.4 The change ofa substance from a solid to a vapor without passing through the liquid state is called sublimation. Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature.