Chemistry 122 Fall Quarter 2013 - Review

1. Chemistry 122Fall Quarter 2013 - Review 1) Sapling HW 1411:50 pm Wednesday, 12/4/2013 2) Final Exam:(~ 2/3 Quantitative & ~ 1/3 Qualitative) Wednesday, 12/11/2013, 8:00-10:00 am SL 120

2. Chapter 5- The Gaseous State Pressure: Lb/in2, Atm, mm Hg, Torr, Pa Pressure conversions for atmospheric pressure Barometers, Manometers Gas Laws: Boyle’s, Charles’s, Avogadro’s, Dalton’s, Combined, Ideal, Graham’s, Van der Waal’s Using Gas Laws for calculations STP (0oC & 1 atm) (1 mole gas = 22.4 L @ STP) Limitation to Ideal gas law - Van der Waal’s work Kinetic-Molecular Theory – Basics behind gas laws Significant Figures ~ 13 % (Point %)

3. Chapter 6 - Thermochemistry Uses of thermochemistry Units for Energy: joules & calories Types of Energy – PE, KE (formula: KE = 1/2mV2) Heat Energy – SIGNS, units, names, symbols State Function Simple & Bomb Calorimeters Heat Capacity (C), Specific Heat Capacity (s) Heat Equations: q=CxΔT q=sxgxΔT ΔHr = ∑HBBroke-∑HBformΔHr = ∑ Hof prod – ∑Hof react Hess’s Law (add & subtract reactions to get new ΔHr) ∆Hof : Definition and use Above 5 ways to calculate heats of reaction- From: 1) C, 2) s, 3) Hess’s Law, 4) Bond energies, 5) Heats of formation Standard State (o) = 1 atm & 25oC Drawing Lewis Structures ~ 15 %

4. Chapter 11 – Liquid & Solid States Phase Changes & Names Vapor Pressure Heating Curves & Calculations: q= g x s x ΔT; q= ΔHv,fx n MP, BP, TP, CT – Definitions & Uses Phase Changes & Energies Involved: ΔHvap & ΔHfusion Phase Diagrams - Draw and Interpret Polarity of both Bonds & Molecules Intermolecular Forces – Names, types, ~ strength Solids – ionic, molec, metal, cov; amorp, cryst Unit Cells – cubic types & simple calculations X-Ray Diffraction Lewis Structures ~ 11 %

5. Chapter 12 - Solutions Solubility Rules Definitions Solution Types Lattice & Solvation Energies Le Chatelier’s Principle Henry’s Law for gas solubility: (s2/s1 = p2/p1) Concentration Terms: Xa, W/W%, pp_, M, m Colligative Properties: BP, FP, VP, Osmosis Van Hoft’s Factor, i Equations: Henry’s, BP, MP, Osmosis Use equations for calculations of: ΔT, i, MW, K’s, x, n, m Colloids; Tyndal effect Dilution Problems: C1V1 = C2V2 ~ 15 %

6. Chapter 13 – Rates of Reactions Rate definition Factors that influence rates of reactions How measure rates Rate Law / Rate Expressions Rates, Orders, Rate Constant - what they are & calculations How to get complete Rate Law (orders) - Two ways Integrated Rate Laws & Plots (integrated rate eqns; given) Uses of Integrated Rate Equations Half-Life (t1/2) for 1st Order Rxn Mechanisms – Definition, terms & Uses Catalysts & Intermediates Arrhenius Equation & Energy of Activation (Ea) Progress of Reaction Plot - ∆H & Ea Enzymes as Catalysts ~ 22 %

7. Chapter 14 – Chemical Equilibrium Definition of Chemical Equilibrium Equilibrium Reaction & Expression Equilibrium Constant, K or Ka, Kb, Ksp, Kf Equilibrium Expression: Write from reaction Calculations: “IE Table”; K; initial & equilibrium concentrations (amount of H+ for a weak acid & solubility of a slightly soluble compound); simplification of math with ([ ]/K > 100); use of Q Le Chatelier’s Principle Kw = 1.00x10-14 (for water) Beer’s Law: A = εbc Water & Solids Dropping from Equil. Expression ~ 22 %

8. Study for the Final – Even if you are content with your present grade. Without study you will end up like these miserable felines. “Lion Cut” Cat in Minnesota