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Comprehensive Review of Chemistry Concepts: Semester 2

Explore key topics in chemistry including intermolecular forces, solutions, chemical kinetics, equilibria, acids and bases, entropy, and electron transfer reactions. Dive into important equations and principles essential for understanding the material.

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Comprehensive Review of Chemistry Concepts: Semester 2

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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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