#1 eprovesurveys.advanc-ed/surveys/#/action/2087/3110 #2

1. #1 http://eprovesurveys.advanc-ed.org/surveys/#/action/2087/3110 #2 http://eprovesurveys.advanc-ed.org/surveys/#/action/2088/31106

2. Bellringer Convert 925 ft/min2 = m/s2

3. Bellringer Solution

4. Ch. 13 - Liquids & Solids I. Physical Properties

5. A. Inter… and Intra… • Attractive forces between molecules. • Chemical bonds within molecules.

6. A. Inter… and Intra… • Intermolecular Forces • Intramolecular Forces

7. A. Types of Bonds COVALENT IONIC e- are transferred from metal to nonmetal e- are shared between two nonmetals Bond Formation Type of Structure true molecules crystal lattice Physical State liquid or gas solid Melting Point low high Solubility in Water yes usually not yes (solution or liquid) Electrical Conductivity no Other Properties Weak bonds Strong bonds

8. Types of IMF(InterMF)

9. LIQUIDS Stronger than in gases Yes high Somewhat slower than in gases SOLIDS Very strong No (?alloys) Very high No extremely slow B. Liquids vs. Solids IMF Strength Fluid Density Compressible Diffusion

10. B. Liquid Properties • Surface Tension attractive force between particles in a liquid that minimizes surface area

11. water mercury B. Liquid Properties • Capillary Action • attractive force between the surface of a liquid and the surface of a solid

12. B. Liquid Properties • Viscosity – resistance to motion between molecules of a liquid • Molasses and water – high viscosity because of strong IMF (hydrogen bonds) • Viscosity increases as temperature decreases

13. C. Properties of Water • Strong IMF (hydrogen bonds) • Most abundant substance on earth • High boiling point • Density of solid < density of liquid • High surface tension • High heat of vaporization

14. increasing melting point D. Types of Solids • Crystalline - repeating geometric pattern called a unit cell (ie. salt, sugar, snow, metals etc.) Amorphous - no geometric pattern (for example: glass) • covalent network • metallic • ionic • covalent molecular

15. D. Types of Solids Ionic (NaCl) Metallic

16. D. Types of Solids Covalent Molecular (H2O) Covalent Network (SiO2 - quartz) Amorphous (SiO2 - glass)

17. E. Phase Changes

18. E. Phase Changes • Evaporation • molecules gain enough energy to overcome IMF (without boiling) • Volatility (volatile) • measure of evaporation rate • ie. Gas, paint thinner, alcohol are very volatile (can smell the vapors)

19. E. Phase Changes • Equilibrium • trapped molecules reach a balance between evaporation & condensation

20. temp v.p. IMF E. Phase Changes p.482 • Vapor Pressure • pressure of vapor above a liquid at equilibrium v.p. temp

21. Patm b.p. IMF E. Phase Changes • Boiling Point- temp at which vapor pressure of liquid equals external atmospheric pressure ATMOSPHERIC PRESSURE VAPOR PRESSURE

22. IMF m.p. E. Phase Changes • Melting Point • equal to freezing point • Which has a higher m.p.? • polar or nonpolar? polar

23. E. Phase Changes • Sublimation • solid  gas ATMOSPHERIC PRESSURE VAPOR PRESSURE • EX: dry ice, mothballs, solid air fresheners • Opposite is deposition: H20 vapor snow

24. G. Phase Diagrams • Show the phases of a substance at different temps and pressures. See p.457 (For AP Chem p.489)

25. Gas - KE  Boiling - PE  Liquid - KE  Melting - PE  Solid - KE  F. Heating Curves

26. F. Heating Curves • Temperature Change • change in KE (molecular motion) • depends on heat capacity • Heat Capacity • energy required to raise the temp of 1 gram of a substance by 1°C • water has a very high heat capacity

27. F. Heating Curves • Phase Change • change in PE (molecular arrangement) • temp remains constant • Heat of Fusion (Hfus) • energy required to melt 1 gram of a substance at its m.p.

28. F. Heating Curves • Heat of Vaporization H20 (l) H20 (g) H=44 Kj • Heat of Fusion H20 (s) H20 (l) H=6 Kj

29. B. Heating Curves • Heat of Vaporization (Hvap) • energy required to boil 1 gram of a substance at its b.p. • usually larger than Hfus…why? • EX: sweating, steam burns