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Semester 2 Review

Semester 2 Review. Chapters 13 - 20. Chapter 13. Intermolecular Forces, Liquids and Solids. Packing 1 atom 2 atoms 4 atoms. Cohesive Forces. Viscosity Surface Tension Adhesive forces Hydrogen Bonding in Water. Clausius-Claperon Equation. Phase Diagrams -- Water. Chapter 14.

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Semester 2 Review

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  1. Semester 2 Review Chapters 13 - 20

  2. Chapter 13 Intermolecular Forces, Liquids and Solids

  3. Packing1 atom 2 atoms 4 atoms

  4. Cohesive Forces • Viscosity • Surface Tension • Adhesive forces • Hydrogen Bonding in Water

  5. Clausius-Claperon Equation

  6. Phase Diagrams -- Water

  7. Chapter 14 Solutions and Their Behaviors

  8. Concentration Units • Molarity of solution, M • Molality of solute, m • Mole Fraction A, A • Weight % A

  9. Solubility Factors • Like Dissolves Like • Solubility of Solid in Liquid as a Function of Temperature • Solubility of a Gas in a Liquid as a Function of Temperature

  10. Henry’s Law • Sg = kHPg • Solublity of a gas is equal to the product of the partial pressure of the gaseous solute above the solution times a constant.

  11. Raoult’s Law • PS = S P0S • The equilibrium vapor pressure of a solvent over a solution at a given temperature is the product of the mole fraction of that solvent and the vapor pressure of the pure solvent.

  12. Colligative Properties • Freezing Point Depression • Tfp = i Kfpmsolute (i = van’t Hoff factor) • Boiling Point Elevation • Tbp = i Kbpmsolute (i = van’t Hoff factor) • Osmotic Pressure •  = i MRT (Used to Determine Molar Mass)

  13. Chapter 15 Chemical Kinetics

  14. Rate Laws are Determined by Experimental Data! • Use ratio method to solve for m and n • R0 = k[A0]m[B0]n

  15. Zero Order

  16. 1st Order (Nuclear Decay)

  17. 2nd Order

  18. Arrhenius Equation

  19. Chapter 16 Chemical Equilibria

  20. aA + bB  cC + dD • Not at Equilibria • At Equilibria

  21. ICE Table

  22. aA + bB  cC + dD • No pure solids or liquids in an equilibrium expression • Their concentrations can not change! • Keq > 1 Products are Favored • Keq < 1 Reactants are Favored

  23. Chapter 17 Acids and Bases

  24. Theory • Arrhenius • Bronstead-Lowry • Lewis • Conjugate Acid-Base Pairs

  25. Other Applications • pH • pOH • Kw • Selecting an Indicator • Ka • Kb • Strong and Weak

  26. Chapter 18 Aqueous Equilibria

  27. Review • Common Ion Effect • Buffer Solutions • Titration Curves • Hydrolysis of Salts

  28. Review • Ksp • Qsp > Ksp a precipitate will form • Complex Ion Formation • Qualatative Analysis

  29. Henderson-Hasselbalch Equation

  30. Chapter 19 Entropy and Free Energy

  31. Heat • q = mCpT • Hrxn = nHf0(prod) -nHf0(prod)

  32. Free Energy • G0rxn = nGf0(prod) -nGf0(prod) • G0sys =H0sys - T S0sys • Negative Spontaneous

  33. Free Energy and Equilibrium or Not ∆Gorxn= - RT ln k ∆G = ∆G˚ + RT ln Q

  34. Chapter 20 Electron Transfer Reactions

  35. Cell Potential • Sketch Simple Cells and Be Able to Predict E0 • Balance Redox Equations

  36. Non-Standard Electrochemical Cells • The Nernst Equation

  37. Free Energy • G0 = - nFE0 • 1V = 1J/coul • Amps = Coul/sec

  38. And Finally……. Equations!

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