2. CHAPTER 12 SOLIDS, LIQUIDS, AND GASES HONORS CHEMISTRY

3. Section 12.1 Gases The Kinetic-Molecular Theory Kinetic-molecular theory explains the different properties of solids, liquids, and gases. The kinetic-molecular theory describes the behavior of matter in terms of particles in motion.

4. Gases consist of small particles separated by empty space. Gas particles are too far apart to experience significant attractive or repulsive forces.

5. Gas particles are in constant, random motion. An elastic collision is one in which no kinetic energy is lost.elastic collision

6. Kinetic energy of a particle depends on mass and velocity. Temperature is a measure of the average kinetic energy of the particles in a sample of matter. Temperature

7. Great amounts of space exist between gas particles. Compression reduces the empty spaces between particles. Expansion increases the empty space between particles.

8. Explaining the Behavior of Gases Gases easily flow past each other because there are no significant forces of attraction. Diffusion is the movement of one material through another. Diffusion Effusion is a gas escaping through a tiny opening.

9. Gas Pressure Pressure is defined as force per unit area. Pressure Gas particles exert pressure when they collide with the walls of their container. Simulation: Gas Properties

10. Air Pressure The particles in the earth’s atmosphere exert pressure in all directions called air pressure (atmospheric pressure). There is less air pressure at high altitudes because there are fewer particles present, since the force of gravity is less.

11. Air Pressure Air pressure may be measured using several possible units: – Atm – mm Hg – Torr – Pascals (Pa) – Kilopascals (kPa) – psi

12. Air Pressure Air pressure conversion factors: 1.00 atm = 760. mm Hg = 760. Torr = 101 325 Pascals (Pa) = 101.325 Kilopascals (kPa) = 14.7 psi

13. Gas Pressure Dalton’s law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases of the mixture. Dalton’s law of partial pressures P total = P 1 + P 2 + P 3 +...P n

14. Section 12.3 Liquids and Solids Liquids Forces of attraction keep molecules closely packed in a fixed volume, but not in a fixed position. Liquids are much denser than gases because of the stronger intermolecular forces holding the particles together. Large amounts of pressure must be applied to compress liquids to very small amounts.

15. Fluidity is the ability to flow and diffuse; liquids and gases are fluids. Viscosity is a measure of the resistance of a liquid to flow and is determined by the type of intermolecular forces, size and shape of particles, and temperature. Viscosity Surface Tension is a measure of the inward pull by particles in the interior (explains why H 2 O beads up and how insects walk on H 2 O)

16. Solids Solids contain particles with strong attractive intermolecular forces. Particles in a solid vibrate in a fixed position. Most solids are more dense than liquids. Ice is not more dense than water.

17. Crystalline solids are solids with atoms, ions, or molecules arranged in an orderly, geometric shape. Crystalline solids

18. Amorphous solids are solids in which the particles are not arranged in a regular, repeating pattern. Amorphous solids Amorphous solids form when molten material cools quickly, like in a candle.

19. Section 12.4 Phase Changes Phase Changes That Require Energy Melting occurs when heat flows into a solid object. Heat is the transfer of energy from an object at a higher temperature to an object at a lower temperature.

20. Vaporization is the process by which a liquid changes to a gas or vapor. Vaporization Evaporation is vaporization only at the surface of a liquid. Evaporation

21. The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure.boiling point

22. Sublimation is the process by which a solid changes into a gas without becoming a liquid. Dry ice, frozen CO 2, will sublime.

23. Phase Changes That Release Energy As heat flows from water to the surroundings, the particles lose energy. The freezing point is the temperature at which a liquid is converted into a crystalline solid.freezing point

24. The process by which a gas or vapor becomes a liquid is called condensation.condensation Deposition is the process by which a gas or vapor changes directly to a solid, and is the reverse of sublimation. Deposition

25. The Normal Freezing Point and Normal Boiling Point both occur at 1.00 atm.

26. A = Triple Point B = Critical Point Triple Point – the temperature and pressure at which all three states of matter can coexist. All 6 phase changes can occur at this time. Critical Point – the distinction between liquid and gas is lost and is often called a supercritical fluid