The Final Exam will be Comprehensive! Approximately 1/2 will focus on recent material and those things you need to know to understand the latest material, while about 1/2 will be on problems/materials similar to what has been seen on previous exams.
Approximately 1/4 of the exam will be multiple choice, the remainder will be similar to previous exams and the example on the web.
Review: Study Guides I & II; Quizzes and problem sets since Exam I & II. Review nomenclature so that you can read questions and understand them.
Be able to do gas stoichiometry problems (Gas Law Module, #6 & 7) . What is the Kinetic Molecular Theory for gases? What are its postulates? What is the meaning of temperature (what is it a measure of)? What relationship is there between temperature and pressure (in microscopic terms-what are the particles doing)? temperature and volume?
Define/describe: weak forces, Hydrogen bonds, vapor pressure, phase change, boiling, solid, boiling point (bp), heat of vaporization/condensation, melting point (mp), heat of fusion/crystallization.
Be able to draw/interpret heating/cooling curves. (Remember that the cooling curve is just like the heating curve, but backwards - that is you start at the gas phase and remove heat.) Remember that the vapor pressure of a pure substance is dependent only on the nature of the substance and the temperature. Why is water's boiling point so high (vapor pressure so low)? How does it compare to other molecules? What are the other special properties of water and how do we explain them? Are there any molecules with similarly high boiling points? Why do liquids boil? When? Why are boiling points lower in the mountains?
What are the basic premises of Collision Theory? Why are three body termolecular and higher reactions rare? What three factors did we discuss as affecting the rates of reactions (collision frequency, activation energy {Eact}, and orientation). How are these factors related to measurable macroscopic properties (concentration and temperature). Be able to draw and interpret Reaction Progress (or Reaction Coordinate) Diagrams. Note how these diagrams indicate/reflect changes in rate (kinetics) and completion of reaction(equilibrium).
Define/describe: Equilibrium, Le Chatelier's Principle, Mass Action Expression (Q), Equilibrium Expression (Keq or K), acid and base dissociation equilibria (Ka & Kb). Be able to do equilibrium problems as we have seen in class and on homework. Be able to write balanced chemical equations, equilibrium expression (Keq = ([P][Q[)/([A][B]), for A + B Æ P + Q), and solve for unknown quantities. Remember special expressions for ion product of water (Kw = [H+][OH-]) & solubility product (Ksp = [A+][B-] for AB(s) Æ A+ + B-). How would pressure affect gaseous equilibria? How does temperature affect equilibria? Chemical Equilibria Module , Dissociation Equilibria Module
Define/describe: Arrhenius acid model, Brønsted-Lowry acid theory (acid = proton donor, base = proton acceptor, conjugate acid/base pair), hydronium ion, salt, electrolyte, non electrolyte, strong acid/base (100% dissociated when < 1M), strong electrolyte, weak acid/base (less than 100% dissociated when < 1M), weak electrolyte, neutralization, titration, Kw.
pH, pKa, pOH, buffer. Be able to calculate [H+] & [OH-] given pH & pOH, and vice versa. Note that acid/base dissociation reactions and buffers are equilibrium systems. Be able to find [H+], [OH-], pH, & pOH for weak acid or weak base solutions. Be able to use the Henderson-Hasselbalch equation and/or the equilibrium expression to determine the pH of a buffer and/or the ratios of acid:salt in a buffer of a given pH. pH Module
Define/describe: solution, salt, solvent, solute, saturated solution, unsaturated solution, super saturated solution, mass %, ppm, ppb, molarity (M, moles/liter solution), molality (m, moles/kilogram solvent), neutralization, equivalent (in chemical reactions), electrolyte, water of hydration, suspension, colloid, emulsion.
Why do some substances dissolve in each other? Why do others not? ("Like Dissolves Like"). How does temperature effect solubility of gases? Solids or liquids? What factors effect the rate of dissolution? Be able to solve problems involving concentrations as we have seen in class and on the quizzes: find mass %, molarity of solutions given their components. Be able to find concentrations of solutions after dilution or mixing with other components. Be able to do neutralization problems, especially for acids and bases. Colligative properties (properties which depend only on the number or concentration, not on the type, of particles). Be able to solve problems for freezing point depression (T = - k'm, where m = molality and k = the freezing point constant).
FYI - NOT required for F2008 Mole fraction (X, moles/total moles); Be able to solve problems for: boiling point elevation (T = km), freezing point depression (T = - k'm), osmotic pressure ( |
The gas constant, R= 0.0821. Avogadro's number = 6.02 x 1023, volume of a gas at STP (what is STP?). Mass of one amu in grams (one gram divided by Avogadro's number). Values for: h (Plank's constant) & c (speed of light). The electronegativities of the Period 2 elements. Conversions within the Metric System. Temperature at absolute zero in °C and K. Freeezing and boiling points of water in °C and K. One atm = 760 mmHg.
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© R Paselk
Last modified 11 December 2008
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