1 / 23

Phases of Matter

Phases of Matter. Kinetic Theory. All matter is made of atoms and molecules that act like tiny particles. These tiny particles are always in motion. The higher the temp., the faster the particles move.

hera
Download Presentation

Phases of Matter

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Phases of Matter

  2. Kinetic Theory • All matter is made of atoms and molecules that act like tiny particles. • These tiny particles are always in motion. The higher the temp., the faster the particles move. • At the same temp., more massive (heavier) particles move slower than less massive (lighter) particles.

  3. SOLIDS • Definite shape? • YES • Definite volume? • YES • Molecules in a solid are tightly packed and constantly vibrating.

  4. LIQUIDS • Definite shape? • NO • Definite volume? • YES • Some liquids flow more easily than others. The resistance of a liquid to flow is called viscosity. • Honey has a high viscosity compared to water.

  5. GASES • Definite shape? • NO • Definite volume? • NO • The particles in a gas are spread very far apart, but can be compressed by pumping them into a restricted volume.

  6. Phase Changes • Changes in phase are examples of physical changes. • Melting: solid  liquid • Freezing: liquid  solid • Vaporization: liquid  gas • Condensation: gas  liquid • Sublimation: solid  gas

  7. GAS Vaporization Condensation Deposition Sublimation LIQUID Melting Melting Freezing SOLID Changes of State

  8. ENERGY TRANSFERS!!! • ENERGY is the ability to change or move matter. • Energy is ABSORBED when substances melt or evaporate. • NOTE: our bodies cool down when our sweat evaporates. • Energy is RELEASED when substances freeze or condense.

  9. Melting • The change of state from solid to liquid. • Energy (heat) is absorbed by the substance that is melting.

  10. Freezing • The change of state from liquid to solid. Opposite of melting. Energy (heat) is released by the substance undergoing freezing.

  11. Evaporation • The change of state at the surface of a liquid as it passes to a vapor. This results from the random motion of molecules that occasionally escape from the liquid surface. • Energy (heat) is absorbed by the liquid (Cooling of the liquid results) • Can happen at any temperature

  12. Condensation • The change of state from gas to liquid. The opposite of evaporation. • Energy (heat) is released by the liquid (Warming of the liquid results)

  13. Boiling • Change from state from a liquid to a gas. • Occurs throughout the liquid. • boiling point/temperature is determined by pressure • Energy (heat) is absorbedby the liquid.

  14. Phase Change Graph *Boiling & freezing points depend on the pressure.

  15. Water at normal pressure (1 atm): • For water at normal (every day) pressures: • Melting/freezing point: • Condensing/boiling point: 0 oC (32oF) 100 oC (212oF) Label the points & temperatures on your graph.

  16. Change the pressure  Change the Boiling Point

  17. Phase Diagrams • a phase diagram shows the equilibria pressure-temperature relationship among the different phases of a given substance

  18. WATER Carbon Dioxide C AD = AB = AC =

  19. C meltingcurve AD = AB = AC =

  20. C meltingcurve sublimationcurve AD = AB = AC =

  21. C vaporpressurecurve meltingcurve sublimationcurve AD = AB = AC =

  22. C A triple point = Point ______ The point at which all 3 phases of a substance (solid, liquid, gas) can coexist at equilibrium. D critical point = Point ______ The combination of critical temperature and critical pressure. • critical temp = temp. above which a gas cannot be liquefied. (H2O=374ºC) • critical pressure = press. required to liquefy a gas at its critical temperature. (H2O=218 atm)

  23. Conditions for H2O on other planets…

More Related