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States of Matter

Chapter 8. States of Matter. 8.1 Solids, Liquids, Gases. States of Matter - the physical forms in which a substance can exist Solid – ex. ice Liquid Gas Plasma – positively and negatively charged particles Most common in universe. 8.1 Solids, Liquids, Gases. Particles of Matter

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States of Matter

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  1. Chapter 8 States of Matter

  2. 8.1 Solids, Liquids, Gases • States of Matter- the physical forms in which a substance can exist • Solid – ex. ice • Liquid • Gas • Plasma – positively and negatively charged particles • Most common in universe

  3. 8.1 Solids, Liquids, Gases • Particles of Matter • Matter is made up of tiny particles called atoms and molecules. • Atoms and molecules are always in motion bumpinginto each other.

  4. 8.1 Solids, Liquids, Gases • Solid-the state of matter that has a definiteshape and volume • particles are packed closely together • Particles only vibrate in place.

  5. 8.1 Solids, Liquids, Gases Two types of solids: • Crystalline- These solids have an orderly arrangement of particles in a repeating pattern. • Examples include iron, diamond, ice, crystal • Amorphous- These solids do not have a special arrangement. • Examples include glass, rubber, wax.

  6. 8.1 Solids, Liquids, Gases • Liquid-the state of matter that has a definitevolume but takes the shape of its container • particles are close together • Particles slide past one another. .

  7. 8.1 Solids, Liquids, Gases Liquids have several properties that make them unique. • Surface tension-an uneven force that acts on the particles at the surface of a liquid. • This causes some particles to form spherical drops like beads. • Water has a high surface tension while rubbing alcohol has a low surface tension. • Viscosity-a measurement of a liquid’s resistance to flow • The stronger the attractions between the molecules, the more viscous the liquid is. • Honey has a high viscosity. • Water has a low viscosity.

  8. 8.1 Solids, Liquids, Gases • Gas- the state of matter that has no definite shape or volume • particles are far apart • Particles move independently. • Vapor is the gas state of asubstance that is normally asolid or liquid at room temperature

  9. 8.1 Solids, Liquids, Gases

  10. 8.2 Changes in State • Change of state- the change of a substance from one physical form to another • ALL STATE CHANGES ARE PHYSICAL CHANGES. • Particles of a substance have different amounts of energy depending on the state of the substance. • The amount of energy is determined by how close the particles are • Solids – low energy • Liquids – medium • Gases – high • YOU MUST ADD OR REMOVE ENERGY TO CHANGE STATES.

  11. 8.2 Changes in State • Melting • Freezing • Vaporization (evaporation) 4. Condensation 5. Sublimation 6. Deposition

  12. 8.2 Changes in State Melting: Solid to Liquid • Melting- change in state from solid to liquid. • Adding energy to ice raisesits temperature. • As the temperature increases, the particles energy increases • When a certain temperature is reached the substance melts • Ex. At 0°C ice melts • Melting is endothermic- energy is gained by the substance

  13. 8.2 Changes in State • Melting Point - The temperature at which a substance changes from a solid to a liquid. • Melting point is a physical property. • Different substances have different melting points.

  14. 8.2 Changes in State Freezing: Liquid to Solid • Freezing- change in state from a liquid to solid. • Freezing point-The temperature at which liquid changes into a solid. Freezing is the reverse of melting, so they occur at the same temperature. • Any solid is in the frozen state! • Freezing isexothermic- • energy isremovedfrom the substance

  15. 8.2 Changes in State Vaporization: Liquid to Gas • Vaporization- change in state form a liquid to gas. • Evaporation is vaporization that occurs only at the surface of a liquid • Boiling is the change of a liquid to a gas (vapor) throughout the whole liquid • Boiling point- temperature at which a substance boils • Vaporization requires addingenergyso it is endothermic Evaporation Boiling

  16. 8.2 Changes in State Effects of Pressure on Boiling Point • Water boils at 100ºC, but only at sea level because of atmospheric pressure. • Atmospheric pressure is caused by the gases that make up the atmosphere. • The higher you go above sea level, the fewer air particles there are above you so atmospheric pressure is less. • In Denver, the mile high city, water boils at 94o C.

  17. 8.2 Changes in State Condensation: Gas to Liquid • Condensation- change of state from a gas to liquid. • Energy must be removed - exothermic • Condensation point-temperature at which a substance goes from a gas to a liquid. Condensation is the reverse of vaporization, so they occur at the same temperature.

  18. 8.2 Changes in State Sublimation: Solid to Gas • Sublimation- the change from a solid to a gas without being a liquid • Dry ice (carbon dioxide) • The substance must gain a lot of energy for this to occur, therefore it is endothermic.

  19. 8.2 Changes in State Deposition: Gas to Solid • Deposition: the change from a gas to a solid without being a liquid • Frost • Deposition is an exothermicchange because a lot energy must be removed.

  20. 8.2 Changes in State Change in temperature vs. Change in state • Change of temperature versus change of state • When energy is added… • Either the temperature changes • OR the state changes • Not both!

  21. 8.2 Changes in State Change in temperature vs. Change in state • When substances gain or lose energy, the temperature will change or remain the same. • As the temperature rises, the particles gain energy. • Once the particles have enough energy, the state will change. • At this point the temperature will remain until the state change is complete. • Boiling water will remain at 100oC until it all evaporates.

  22. 8.2 Changes in State Change in temperature vs. Change in state

  23. 8.2 Changes in State What’s happing in a phase change diagram? • When you add heat to a solid… • …thetemperatureincreases until the melting point • You still add heat… • …the temperature stays while the solid melts • You now add heat to a liquid… • …the temperature increases until the boiling point • You still add heat… • …the temperature stays while the liquid vaporizes • You now add heat to a gas… • …thetemperaturewill just keep increasing!

  24. 8.2 Changes in State

  25. Partner Share • Neatly and in your own words, Write at least 8 lines describing the difference between boiling and evaporation. Be sure to give an example of where there may be different boiling points for the same substance.

  26. 8.3 Behavior of Gases • The kinetic molecular theory is an explanation of how particles in matter behave • Small particles make up all matter • Particles are in constant, randommotion • Particles collide with other particles, other objects, an the walls of their container • Noenergyis lost when particles collide • Describing Gas Behavior • Gases behave differently from solids and liquids. • Gases have large amounts of empty space between molecules.

  27. 8.3 Behavior of Gases • What factors affect how gases behave? • Temperature • Volume • Pressure

  28. 8.3 Behavior of Gases Temperature of Gases • Temperatureis a measure of how fast the particles in an object are moving around. • The faster the particles move, the more energy they have • On a hot day, particles move faster and hit the inside walls of a balloonmore often. Thus, increasing energy and pushing on the walls. • On a cold day, particles have less energy They do not push very hard on the walls of the balloon.

  29. 8.3 Behavior of Gases Volume • Volume is the amount of space that an object takes up • Volume of a gas depends on its container • Decrease volume…increase pressure • Increase volume…decrease pressure

  30. 8.3 Behavior of Gases 8.3 Behavior of Gases 8.3 Behavior of Gases Pressure • Pressure is the amount of force exerted per area on a surface • A basketball is very firmcompared to a beach ball • It has a greater pressure. • The beach ball has a much lower pressure.

  31. 8.3 Behavior of Gases • Gas behavior laws • Boyle’s Law • Involves volume and pressure • Charles’s Law • Involves temperature and volume • Guy-Lussac’s Law • Involves temperature and pressure

  32. Section 3: The Behavior of Gases • What is Boyle’s Law? • Boyle’s Law states that pressure of a gas increases if the volume decreases and pressure of a gas decreases if the volume increases, when temperature is constant • Inverse = oppositerelationship • So… • As pressure increases,volume decreases • As pressure decreases,volume increases • Think: Boyle is the vice president (VP)(volume, pressure)

  33. Section 3: The Behavior of Gases • Boyle’s Law

  34. Section 3: The Behavior of Gases • What is Charles’s Law? • Charles’s Law states that for a fixed amount of gas at a constant pressure, the volume of gas changes in the same way that the temperature changes • So… • As temperature increases, volume increases • As temperature decreases, volume decreases • Think: Charlie Brown is on TV (Temperate and volume)

  35. Section 3: The Behavior of Gases • Charles’s Law

  36. Section 3: The Behavior of Gases • What is Guy Lussac’s Law? • Guy Lussac’s Law states that for a fixed amount of gas at a constant volume, the pressure of gas changes in the same way that the temperature changes • So… • As temperature increases, pressure increases • As temperature decreases, pressure decreases • Think: G lives in a TP (Temperate and pressure)

  37. Section 3: The Behavior of Gases Volume constant • Guy Lussac’s Law Volume constant

  38. Gas Behavior Laws

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