Final Exam Review Chem 123N Page 1 of 6 CHEM 123N Principles of Chemistry II FINAL EXAM REVIEW SHEET Liquids, Solids, and Intermolecular Forces I. Intermolecular Forces (IMF)—dispersion forces, dipole-dipole, hydrogen bonding, ion-dipole a. be able to ID all IMF available in a compound b. make sure you understand how IMF affects boiling point and vapor pressure c. drawing shapes (bent, linear, trigonal planar, etc.) is essential in knowing which IMF are present II. Phase diagrams a. ID regions (solid, liquid, gases) and name of phase changes (sublimation, condensation, vaporization, etc.) b. Understand how the water’s phase diagram is different from most compounds (slope of the line between solid and liquid III. Vaporization and Fusion a. Know why ΔHvap > ΔHfus b. Know when to use them in the heating/cooling reactions c. Understand dynamics of equilibrium in vaporization d. Understand how volume in a closed container affects vaporization IV. Heating/Cooling Curve a. Know how to draw (Temp vs. Heat added) b. Phase changes there is no temperature change (why??) c. Calculate q for all of the regions heating solid, fusion, heating liquid, vaporization, heating gas(q = mCsΔT or q = nΔH) d. This is not the same thing as a phase diagram V. Vapor Pressure a. Factors affecting vapor pressure b. Relationship of vapor pressure to boiling and melting points VI. Clausius Clapyeron a. Linear relationship between vapor pressure (Pvap) and heat of vaporization (ΔHvap), understand formula and what is plotted to give a linear graph b. There are two equations (1 point and 2 point) VII. Crystalline Solids a. Know how to figure out the empirical formula from a crystal picture i. Atoms on edge, corner, face, or inside all occupy a different amount of the unit cell b. Understand ionic, atomic, and molecular solidsSolutions I. Entropy and Mixing of Solutions a. Types of solutions b. How entropy affects mixing, how IMF affects mixing II. Energetics of Solution formation a. ΔH solution formula, heats of hydration III. Factors that affect solubility and solubility calculations a. Like dissolves like b. Temp, pressure IV. Solution Concentration a. Molarity, molality, parts by mass, parts by volume (%, ppm, ppb), mole fraction V. Colligative Properties a. Vapor pressure lowering (Raoult’s Law – equation not given) b. Boling point elevation, freezing point depression, osmotic pressure c. “i”: moles of particles in solution/moles of units dissolved, Van’t Hoff Factor Chemical Kinetics I. Rate of chemical reaction a. Rate = change in concentration/change in time (make sure you remember sign for formation ordepletion of a product and stochiometry) II. Rate Laws a. Rate constant b. Order of reaction (method of initial rates) c. Integrated rate laws (zero, first, second order reactions) d. What makes a linear plot for each zero, 1st, 2nd order reactions e. ½ Life equation first order = 0.693/k III. Temperature and Rate—Arrhenius a. Activation energy b. Collision frequency – increases with Increased temp, density, and molecules. c. Arrhenius Plots (1 and 2 point) IV. Reaction mechanisms—elementary steps a. What defines rate? Slow step! V. Catalysts—definitions, be able to identify in mechanism Final Exam Review Chem 123N Page 3 of 6Chemical Equilibrium I. Equilibrium Constant (K) a. Be able to write out in terms of products/reactants; don’t forget about stochiometry b. Manipulations of equations and effect on K (inverse equation, 1/K, etc.) c. Kp and Kc relationship d. Solids and pure liquids, leave out of K expression e. ICE Tables—given initial conditions, find eqb concentrations (given K) f. Knowing when to use assumption and when to use quadratic equation II. Reaction Quotient (Q) a. Comparison of Q and K, predict direction of reaction – is the rule that if Q is greater than K, the reaction will shift to the products? III. Le Chatelier’s Principle a. Concentration b. Temperature (endo and exothermic reactions) **this is the only manipulation that changes the value of K c. Volume and pressure changes—look to the moles of gas Acids and Bases I. Definitions of Acids and Bases a. Lewis b. Arrhenius definition: acids always have H ions, and bases are always OH- c. Bronsted-Lowry—ID conjugate acid/base pairs II. Acid Ionization constant (Ka) a. Ka definition b. Find Ka given pH and concentrations (ICE table) c. Understand % ionization and Ka calculations a/b, or 10^-(pH)/ [M]III. Autoionzation of Water a. Kw, [H3O+], [HO-] IV. pH and pOH scales V. Finding pH of a. Strong acid solutions pH= -log[H+]; 100% ionization b. Weak acid solutions, ICE table using Ka; know when to use x is small approximation VI. Base Ionization constant (Kb) a. Strong base solutions pOH= -log[OH-]; 100% ionizationb. Weak base solutions, ICE table using Kb; know when to use x is small approximation VII. pH of a Salt Solution- acidic, basic, neutral, WHY!! VIII. Predicting Acid strength Aqueous Ionic Equilibrium I. Buffers a. What makes a solution a buffer? b. Calculating pH of a buffer c. Calculate pH of a buffer after addition of a strong acid or base d. Henderson Hasselbach equation e. Buffer range and capacity II. Titration and pH Curves a. Calculate pH along all 4 regions of a weak acid titrated with a strong base titration curve b. pH = pKa when [base] = [acid] c. Identify titration curves for both monoprotic and polyprotic III. Relationship between pKa and the identity of the species present in solution at a certain pH IV. Solubility Equilibria, Ksp a. Molar Solubility versus Ksp b. ICE tables to calculate S or Ksp c. Effect of a common ion on solubility (calculations as well as qualitative effects) Free Energy and Thermodynamics I. Entropy and 2nd Law a. ΔSuniv, ΔSsystem, ΔSsurroundings b. ID factors that affect entropy and which species has lowest/highest entropy c. Predict sign of ΔS d. Spontaneity and entropy and enthalpy e. Affect of temperature on entropy of system and surroundings (temperature and spontaneity) II. Free Energy a. Definition b. Predicting spontaneity based on enthalpy, entropy, and temperature c. ΔS°rxn, ΔH°rxn, ΔG°rxn: calculations d. Free energy calculations at non-standard conditions e. K and ΔGo, Q and ΔGf. Understanding thermodynamically favored but kinetically disfavored (exothermic, slow—largeEa) III. Reversible and irreversible reactions Electrochemistry I. Balancing Redox reactions a. Acid or base b. ID which species is oxidized and which is reduced