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
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% 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
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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
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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 -TS
– An endothermic reaction could be spontaneous at
what temperature range?
– Equilibrium: G° = -RTlnK, G = G° + RTlnQ
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