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Compounds
• Name any ionic or covalent compound:– NaClO4
– PCl5• Name simple organic compounds:– C3H8
– C3H7OH (this has two names)
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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…
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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??
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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?
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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?
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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?
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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?
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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?
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Thermochemistry/Thermodynamics
• Enthalpy: Hess’ Law, H°f
• Entropy: S, molecular motion & Boltzmann– Greater entropy – NO or NO2? explain
• Gibbs: G = H -TS– An endothermic reaction could be spontaneous at
what temperature range?– Equilibrium: G° = -RTlnK, G = G° + RTlnQ
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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)
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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?
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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