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Compounds

Compounds . Name any ionic or covalent compound: NaClO 4 PCl 5 Name simple organic compounds: C 3 H 8 C 3 H 7 OH (this has two names). Equations. Combination, decomposition, combustion, acid/base, precipitation, single replacement, redox: iron and oxygen react…

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Compounds

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  1. Compounds • Name any ionic or covalent compound: • NaClO4 • PCl5 • Name simple organic compounds: • C3H8 • C3H7OH (this has two names)

  2. Equations • Combination, decomposition, combustion, acid/base, precipitation, single replacement, redox: • iron and oxygen react… • hydrogen peroxide decomposes… • propane combusts… • nitric acid reacts with magnesium hydroxide… • sodium sulfate reacts with lead nitrate… • magnesium and lead nitrate… • magnesium and sulfuric acid…

  3. Empirical formula /% mass / combustion analysis • Find the formula: • 73.9% Hg and 26.1% Cl by mass • 12.64g of S is present in a sample of sulfuric acid. How many grams of O & H are present? • A hydrocarbon sample weighing 0.5992g contains 0.5040g C and 0.09515g H. The molecular mass is 114g. What is the formula of the hydrocarbon??

  4. Stoichiometry • Identify limiting reactants/Theoretical yield: • 40L of hydrogen reacts with 40g of oxygen – how many grams of water should be produced (& what volume)? • What is the actual yield if 22g of water are produced?

  5. Solutions • Concentration: 571.6g H2SO4 per liter of solution. Density = 1.329g/cm3 • % mass? • Mole fraction? • Molality? • Molarity? • Factors that affect dissolving: pressure, temperature, solvent/solute interactions • Colligative properties: 1M NaF, 1M MgCl2, 1M C2H5OH • Lowest electrical conductivity? • Lowest freezing point? • Highest pH?

  6. Kinetics • Rate law/order of reaction • Formula for calculating 1st order rate? 2nd order? • Reaction mechanism • Order of reaction with respect to Cl-?, MnO4-? • It is 3rd order for H+ - write the rate law • Is this likely to be an elementary reaction?

  7. Equilibrium • Expression for Kc & Kp • Predict reaction using Q • Le Chatelier’s principle • C + CO2 2CO • Equilibrium pressure is 8.37atm. PCO2 = 1.63atm. Calculate Kp • 10g of C is placed in a container with CO2 & CO, each with a partial pressure of 2.0atm. Will the partial pressure of CO2 increase/decrease/stay the same as the system approaches equilibrium?

  8. Acids & Bases • Kw, Ka, Kb, pH, strong & weak acids & bases • Kb for C2H3O2-? pH of 1.0M NaC2H3O2? • Strong or weak? – Ca(OH)2, CaO, Fe(OH)2 • Carboxylic acid: R-C-OOH • Lewis acid • Buffer: Ka = [H+][A-]/[HA], [H+] = Ka[HA]/[A-] • Titration: • pH of 20ml of 0.2M HF? • pH after it is titrated with 10ml 0.2M NaOH • pH at equivalence point?

  9. Thermochemistry/Thermodynamics • Enthalpy: Hess’ Law, H°f • Entropy: S, molecular motion & Boltzmann • Greater entropy – NO or NO2? explain • Gibbs: G =  H -TS • An endothermic reaction could be spontaneous at what temperature range? • Equilibrium: G° = -RTlnK, G = G°+ RTlnQ

  10. Electrochemistry • Voltaic cell set-up: • Mg/Mg2+ and Cu/Cu2+. Cathode? Anode? ½ reactions? Cell potential? • G° = -nFE ° =-RTlnK. • Explain why E is intensive but G is extensive. • Non-standard conditions: E= E° + (RT/nF)lnQ, E = E° - (0.0592/n)logQ • Explain how a concentration cell works • Electrolysis: 1 mole e- = 96500C = 1F (1C = 1amp x sec) • G = work = nFE (work: 1W = 1J/s, 1kWhr = 3.6x106J)

  11. Gases • Ideal gas law: • density of 2 moles He at 35°C, 2atm? • Dalton’s law: • Pressure of 20ml He collected over water at 25°C when atmospheric pressure measures 755Torr? • Kinetic molecular theory • Effusion/diffusion: • He and Ne at 25°C. highest energy? Fastest? • Real gases: conditions?

  12. Intermolecular/atomic • 3 types of forces • H2O BP = 100°C, H2S BP = -180°C explain • Vapor pressure & Phase diagrams • Lewis diagrams: formal charge, resonance, octet exceptions • LDD for O3 • VSEPR: electron domain geometry & molecular shapes • Shape: BrO2-, XeF2 • Hybridization: BrO2-, XeF2

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