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Compounds Name any ionic or covalent compound:

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Presentation on theme: "Compounds Name any ionic or covalent compound:"— Presentation transcript:


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

3 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…

4 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 g contains g C and g H. The molecular mass is 114g. What is the formula of the hydrocarbon??

5 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?

6 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?

7 Kinetics Rate law/order of reaction Reaction mechanism
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?

8 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?

9 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?

10 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

11 Electrochemistry Voltaic cell set-up: G° = -nFE ° = -RTlnK.
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)

12 Gases Ideal gas law: Dalton’s law: Kinetic molecular theory
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?

13 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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