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AP Chemistry Final Exam Review

AP Chemistry Final Exam Review. Chapter 1. Matter and Measurements. Important Terms. Atom Element Law Of Definite Proportions. Mixture Solution Physical Properties Chemical Properties. Intensive Property Extensive Property SI units. Precision Accuracy Significant figures

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AP Chemistry Final Exam Review

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  1. AP Chemistry Final Exam Review

  2. Chapter 1 Matter and Measurements

  3. Important Terms • Atom • Element • Law Of Definite Proportions

  4. Mixture • Solution • Physical Properties • Chemical Properties

  5. Intensive Property • Extensive Property • SI units

  6. Precision • Accuracy • Significant figures • Dimensional Analysis

  7. Equations • Density = m/v • K = oC + 273

  8. Things You Should Be Able To Do • Solve simple problems using dimensional analysis. • Convert between Celsius and Kelvin

  9. Chapter 2 Atoms, Molecules, and Ions

  10. Important Terms • Nucleus • Proton, Neutron, Electron • Atomic Mass Unit

  11. Isotope • Group • Period • Metal, nonmetal, metalloid

  12. Molecule • Compound • Empirical Formula • Molecular Formula

  13. Ion • Ionic Compound • Polyatomic Ion

  14. Equations • None

  15. Things You Should Be Able To Do • Calculate number of subatomic particles in an atom based on basic information about AMU’s and the type of element the atom is. • Work with empirical and molecular formulas. • Name ionic compounds. • Determine the formula of an ionic compound when given the name.

  16. Example Problems • 20, 22, 47, 53, 69

  17. Chapters 3 and 4 Stoichiometry

  18. Important Words • Chemical Equation • Reactants • Products

  19. Formula Weight • Mole • Molar Mass • Limiting Reactant

  20. Theoretical Yield • Percent Yield • Aqueous solution • Sovlent

  21. Solute • Electrolyte • nonelectrolyte • Strong and weak electrolyte

  22. Precipitation Reaction • Molecular Equation • Complete Ionic Equation • Net Ionic Equation

  23. Acid • Base • Neutralization Reaction • Oxidation • Oxidation state

  24. Reduction • Concentration • Titration • Equivalence Point

  25. Equations • Molarity = moles/L • M1V1 = M2V2

  26. Things You Should Be Able To Do • Balance Equations • Calculate Molar Masses • Convert between moles and mass • Convert between Mass, moles, and number of particles. • Determine percent composition • Determine empirical and molecular formulas from percent composition data. • Calculate percent yeild

  27. Example Problems • 1, 8, 9, 19, 21, 25, 41, 44, 63, 68, 74

  28. Chapter 5 and 19 Thermodynamics and Thermochemistry

  29. Important Terms • Thermodynamics • Thermochemistry • Kinetic Energy

  30. Potential Energy • Joule • Calorie • System

  31. Surroundings • Heat • First Law Of Thermodynamics • Endothermic

  32. Exothermic • Enthalpy • Calorimetry • Heat Capacity

  33. Molar Heat Capacity • Specific Heat • Hess’s Law • Enthalpy Of Formation

  34. Standard Enthalpy of Reaction • Standard Enthalpy of Formation • Spontaneous • Isothermal

  35. Second Law Of Thermodynamics • Third Law Of Thermodynamics • Gibbs Free Energy • Standard Free Energy of Formation

  36. Equations • q = C xmx ΔT • ΔHorxn = sum(nΔHof products) – sum(ΔHof reactants) • Δso = sum(nΔS products) – sum(nΔS reactants) • ΔG = ΔH - TΔS • ΔGorxn = sum(nΔGof products) – sum(ΔGof reactants) • ΔG = ΔGo + RT lnQ • ΔGo =- RT lnk

  37. Things You Should Be Able To Do • Understand the mathematical signs associated with thermodynamics. • Use Hess’s law to determine the heat energy transfer during a chemical reaction. • Calculate the heat transferred in a process using calorimetry. • Use standard enthalpies of formation to determine the standard enthalpy of a reaction. • Qualitatively describe entropy and entropy changes.

  38. Calculate the standard entropy change for a process using standard molar entropies. • Calculate gibbs free energy from the enthalpy and entropy changes at a given temperature. • Predict the effect of temperature on spontaneity given ΔH and ΔS. • Calculate ΔG under nonstandard conditions. • Relate Δgo and equilibrium constants.

  39. Example Problems • 29, 37, 46, 52,

  40. Chapter 6 Electronic Structure Of Matter

  41. Important Terms • Electron Configuration • Ground State • Excited State • Pauli exclusion principle

  42. Hunds Rule • Valance Electrons

  43. Equations • None

  44. Things You Should Be Able To Do • Be able to interpret electron energy level diagrams. • Be able to write electron configurations.

  45. Example Problems • 23

  46. Chapter 7 Periodic Properties Of The Elements

  47. Important Terms • Effective Nuclear Charge • Atomic Radius • Isoelectronic

  48. Ionization Energy • Electron Affinity • Metallic Character

  49. Equations • None

  50. What You Should Be Able To Do • Understand how effective nuclear charge affects first ionization energy. • Use the periodic table to predict atomic radii, ionic radii, ionization energy, and electron affinity. • Understand how the ionization energy changes as we remove successive electrons.

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