Test 2 Topics PDF

**Monday** **Wednesday** **Friday** *Aug. 12* *Aug. 14* Syllabus Review, Intro, Scientific Method *Aug. 16* Units of measurement, sci notation, accuracy & precision, Sig. Figs. *Aug. 19* Group Activity on states of matter/chem, phys changes *Aug. 21* Dimensional Analysis (unit conversions, te...

**Monday** **Wednesday** **Friday** *Aug. 12* *Aug. 14* Syllabus Review, Intro, Scientific Method *Aug. 16* Units of measurement, sci notation, accuracy & precision, Sig. Figs. *Aug. 19* Group Activity on states of matter/chem, phys changes *Aug. 21* Dimensional Analysis (unit conversions, temp, density) *Aug. 23* History (mention), periodic table, elements, subatomic particles *Aug. 26* Group Activity on Nuclear reactions *Aug. 28* Atomic Mass, Isotopes Naming *Aug. 30* Naming *Sep. 2* *Labor Day* *Sep. 4* Group activity on Naming *Sep. 6* Concept of mole, molar mass of compounds, % composition *Sep. 9* Empirical and molecular formulas *Sep. 11* Start Stoichiometry *Sep. 13* No Class, Tests available for viewing in office only *Sep. 16* Stoichiometry/ LR/ % yield *Sep. 18* Group Activity on Stoichiometry *Sep. 20* Solutions- Molarity, soln. stoichiometry, dilution *Sep. 23* Solubility, electrolytes, non-electrolytes, acids and bases *Sep. 25* Precipitation reactions *Sep. 27* Gas Evolution rxns, Titration, Redox *Sep. 30* Finish Redox *Oct. 2* Electromagnetic Radiation *Oct. 4* Quantum Numbers, Atomic Spectra *Oct. 7* Group activity on Reactions *Oct. 9* No Class, Tests available for viewing in office only *Oct. 11* Fall Pause *Oct. 14* Electron Configurations *Oct. 16* Finish electron configurations, periodic trends *Oct. 18* Periodic Trends *Oct. 21* Lewis structures, formal charge *Oct. 23* Lewis structures *Oct. 25* Bond Polarity, Resonance *Oct. 28* VSEPR *Oct. 30* VSEPR, Molecule Polarity *Nov. 1* Hybridization *Nov. 4* Group Activity on Structures/ Polarity *Nov. 6* Types of energy; system vs surroundings, ΔE = q+w *Nov. 8* No Class, Tests available for viewing in office only *Nov. 11* Specific heat, q=msΔT, PV work *Nov. 13* ΔH; potential energy diagrams; calorimetry, ΔH~rxn~ stoichiometry *Nov. 15* Hess's Law; heats of formations, bond enthalpy *Nov. 18* Group Activity on Thermochemistry *Nov. 20* Gases; Kinetic Molecular Theory, Simple Gas Laws -- Boyles, Charles, Avogadro *Nov. 22* Ideal gas law, MM of gases, density, and partial pressures *Nov. 25* Effusion/Diffusion, Graham's and Henry's law *Nov. 27 - Thanksgiving Holiday* *Nov. 29 Thanksgiving Holiday* ***Final Exam Dec. 9, 5-7 pm*** **Content outcomes** (You could read each of these as "The student will \...") **Chemical Formulas and Equations (Stoichiometry)** 44\. Define the concept of the mole and Avogadro's number and relationship between the two\ 45. Determine molar masses of compounds given the chemical formulas\ 46. Relate the mass of substances to the numbers of atoms, molecules, or ions contained in the\ substances using chemical formulas\ 47. Calculate percentage elemental composition by mass from chemical formulas\ 48. Define empirical formula and molecular formulas\ 49. Distinguish between empirical and molecular formulas\ 50. Determine the empirical formula given either masses of element in a compound or percentages of\ element in a compound\ 51. Determine molecular formulas from empirical formulas given the molar mass of the compound\ 52. Employ data from combustion analysis to the determine the empirical formula of compounds\ containing mainly carbon and hydrogen\ 53. Interpret chemical reactions/equations by identifying products, reactants, phases, and conditions\ (i.e., Δ = heat, catalysts, solvents, hν = light)\ 54. Balance chemical equations\ 55. Relate masses, particle (atoms, ions, molecules) and/or moles of different substances in a chemical\ reaction\ 56. Define: limiting reactant, excess reactant, theoretical yield, maximum yield, actual yield and percent\ yield\ 57. Identify the limiting reactant (or excess reactant) from graphical mass data and masses (or moles) of\ reactants\ 58. Determine the theoretical (maximum) yield from the amount of limiting reactant\ 59. Determine the percent yield from reaction data\ 60. Determine actual yield from percent yield and reaction data **Reactions in Aqueous solution** 61\. Memorize solubility rules (from "List of things to Memorize")\ 62. Apply solubility rules to determine whether or not an ionic substance is substantially soluble in water\ 63. Write dissociation reactions for soluble ionic compounds\ 64. Identify whether substances dissolved in water exist as ions, molecules, or a mixture of the two\ (identify or express with pictorial representation)\ 65. Define electrolyte, strong electrolyte, weak electrolyte and nonelectrolyte\ 66. Classify substances as strong electrolyte, weak electrolyte or nonelectrolyte (from formulas)\ 67. Identify double replacement (metathesis) reactions\ 68. Predict the products of a double replacement reaction\ 69. Identify the precipitate in a reaction\ 70. Write balanced molecular, complete ionic, and net ionic equations\ 71. Identify spectator ions in a reaction\ 81. Define: molarity, dilute, concentrated, dilution\ 82. Determine the molarity of a solution given mass of solute and volume of solution\ 83. Determine mass of solute needed to prepare a given volume at a specific molarity\ 84. Calculate an unknown quantity for a dilution process (using MiVi = MfVf)\ 86. Solve stoichiometry problems for reactions in solution (using molarity as conversion factor)