Compounds

• Name any ionic or covalent compound:– NaClO4

– PCl5• Name simple organic compounds:– C3H8

– C3H7OH (this has two names)

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…

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??

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?

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?

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?

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?

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?

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

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)

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?

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