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States of Matter

States of Matter. Common States of Matter. Gases What do you know about gases? Liquids What do you know about liquids? Solids What do you know about solids? States of matter phet. Kinetic Molecular Theory. The KMT relates the kinetic energy of molecules to states of matter.

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States of Matter

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  1. States of Matter

  2. Common States of Matter • Gases • What do you know about gases? • Liquids • What do you know about liquids? • Solids • What do you know about solids? • States of matter phet

  3. Kinetic Molecular Theory The KMT relates the kinetic energy of molecules to states of matter. Intro to KMT

  4. The Nature of Gases:Kinetic Molecular Theory (KMT) • Kinetic Energy: what is it? • Energy of a moving object: Ek = ½ mv2 • Assumptions of KMT as it applies to gases • Gas particles… 1. Have insignificant volume, (≈ 0) 2. Are in constant, random motion 3. Collisions are perfectly elastic 4. Do not attract or repel one another 5. Average Ek is proportional to absolute temp

  5. Movement of Gas Particles in a Container

  6. Gas Pressure • Pressure = Force/Area: • P = F/A • Gas pressure is the result of collision of gas particles with an object. • Why is there no pressure in a vacuum? • It is the sum of the force of collisions per unit area

  7. Atmospheric Pressure Atmospheric pressure is due to the force of atmospheric gases colliding with objects and weight of atmospheric gases.

  8. Barometer • Measures atmospheric pressure • Invented by Alejandro Torricelli • Patm presses down on the surface, forces Hg up into the tube

  9. Units of Pressure • Pascal (SI unit) Pa • Millimeters of Hg mmHg • Atmosphere atm • Torr torr • Conversion factors @ 25C: Know these! 1 atm = 760 mmHg = 760 torr = 101.3 kPa = 14.7 psi

  10. Converting Between Units of Pressure • Convert a pressure of 385 mmHg to kilopascals (kPa) • How would you do it? • 51.3 kPa

  11. Kinetic Energy & Temperature

  12. 13.2 The Nature of Liquids • Both liquids and gases are fluids, i.e. they can flow

  13. 13.2 The Nature of Liquids • Key difference from gases: • Molecules are close enough to have intermolecular forces of attraction • This is why liquids have a definite volume • But not close enough to fix them in place • This is why molecules of liquids can move past one another (flow) • Condensed matter: • Liquids and solids are known as condensed phases of matter

  14. Evaporation

  15. Evaporation • Vaporization: the conversion of a liquid to a gas or vapor • Evaporation: vaporization occurring at the surface of a liquid • During evaporation, molecules of liquid with sufficient KE “escape” in to the vapor phase • In a closed container, some molecules that escaped re-enter into the liquid phase (condense) • Eventually and equilibrium is reached where… • The rate of evaporation equals the rate of condensation • What would happen to the rate of evaporation when a liquid is heated? Why?

  16. 13.2 Vapor Pressure • Vapor pressure is a measure of the force exerted by a gas above a liquid. • States of matter phet

  17. Vapor Pressure • In a closed container, as molecules escape into the vapor phase, pressure builds • This is vapor pressure • At a certain pressure, the rate of vaporization equals the rate of condensation • This is an example of “dynamic equilibrium” • Then vapor pressure is constant

  18. Vapor Pressure • Depends upon the liquid • Depends upon temperature

  19. Vapor Pressure • Depends upon the liquid • Depends upon temperature

  20. Boiling Point • A liquid boils when the particles thoughout the liquid have enough KE to vaporize • This occurs when the vapor pressure of the liquid equals the external pressure on the liquid (e.g. atmospheric pressure) • This means that a liquid can boil at different temperatures, depending on the external pressure.

  21. Boiling Point & Normal Boiling Point • Normal boiling point is the boiling temperature when atmospheric pressure (Patm) = 1 atm • What is the normal BP for ethanol? • What is the BP for ethanol at Patm = 600 torr?

  22. 13.3 Solids • Crystal Structure • Simple cubic • Body centered cubic • Face centered cubic • Allotropes • Amorphous solids • Glasses

  23. Some Types of Unit Cells

  24. Allotropes • Allotropes are varying forms of an element • Example: oxygen (O2) and ozone (O3) • Example: allotropes of carbon

  25. Non-Crystalline Solids • Amorphous solids lack an ordered internal structure. • Examples: rubber, plastic, asphalt, glass

  26. 13.4 Changes of State • Vaporization/Condensation • Liquid ↔ Gas • Evaporation • Boiling • Vapor vs. Gas • Melting/Freezing • Liquid ↔ Solid • Solidification • Sublimation/Deposition • Solid ↔ Vapor • I2 (s) → I2 (g)

  27. Sublimation • Solid  Vapor • Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature. • Deposition • Vapor  Solid

  28. Phase Diagrams • Show pressure & temperature at which various states of matter exist for a given substance • Phase equilibrium exists along each line • Normal m.p./b.p. • Triple point • Critical point • Note negative slope for solid-liquid • Unique to water

  29. Phase Diagrams • A phase diagram is a graph that gives the conditions of temperature and pressure at which a substance exists as solid, liquid, and gas (vapor). • Lines represent pressures and temperatures at which two phases are in equilibrium

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