| Syllabus / Schedule | 
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| Chem 109, Dr. Paselk |
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Summer 2002 |
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The Final Exam will be Comprehensive!
Approximately 1/3-1/2 will focus on recent material and those things you need to know to understand latest material, while the remainder will be on materials from previous exam Study Guides.
Review: Problem sets since Exam I. Review nomenclature so that you can read questions and understand them. Review concepts from exam I that we have used in looking at additional systems etc.
Be able to: convert numbers to scientific notation and
use numbers expressed in scientific notation; do all calculations
with proper significant figures; make all conversions within the
metric system (SI)
Solutions: Define/describe: solution, salt, solvent, solute, saturated solution, unsaturated solution, super saturated solution, mass %, ppm, ppb, molarity (M), molality (m), mole fraction (X), neutralization, equivalent (in chemical reactions). Why do some substances dissolve in each other? Why do others not? ("Like Dissolves Like"). Be able to solve problems involving concentrations as we have seen in class and in the lab: find mass %, molarity, molality, mole fraction of solutions given their components. Be able to find concentrations of solutions after dilution or mixing with other components. Be able to do problems in problem set.
Heat of solution. How does solubility vary with temperature? Why? How does the solubility of gases vary with pressure? Explain this variation. What is Henry's law? Raoult's law? Ideal solution. What does each relate to? How are they different? What are colligative properties? What do they depend on? Be able to solve problems involving the colligative properties we have discussed (vapor pressure lowering [Raoult's law], boiling-point elevation, freezing point depression, osmotic pressure).
Kinetics: What does chemical kinetics refer to? What kinds of information can we get with kinetics studies? Define: rate, d[A]/dt, mechanism, kinetics, reaction order. How are rates dependent on concentration? What are 1st, 2nd, and 3rd order reactions? 0 order. How are these different orders distinguished graphically? Be able to determine the order of a reaction given appropriate kinetics data. Collision Theory: What are the factors, on the microscopic level, which influence the rate of a reaction? (Frequency of collision, Z; activation energy, Ea; and orientation effect/steric factor, p). How does the rate of a reaction vary with concentration? Explain why this is true on a microscopic level (increased number of collisions). Temperature, KE distributions, and Activation Energy: Why are rates affected by temperature (plot)-how is the distribution of KE's of molecules affected by T? Know how to use the Arrhenius equation: ln k = (-Ea/R) (1/T) + ln A or ln k1/k2 = -Ea/R (1/T1 - 1/T2). What does this equation say about rates and temperature? What kind of a plot do we get for this relationship (what are axis)? Arrhenius plot-describe it. Be able to use Arrhenius equation in problem solving. Be able to find Ea from Arrhenius plot. Diffusion controlled-reactions. Transition State Theory and the Activated Complex: What is a transition state? activated complex? What is transition state theory? Be able to draw and completely label potential energy-reaction coordinate diagrams for various reactions and mechanisms. Be able to interpret such diagrams. Be able to draw the same type of diagram for a catalyzed reaction. What is a catalyst? What, mechanistically, does it do?
Chemical Equilibria: Le Chatelier's Principle-be able to use it to guess outcomes with equilibria. Precisely define it as well. What do we mean when we say that chemical equilibria are dynamic? Define the equilibrium state briefly and precisely. Think about how systems, starting from different initial conditions approach equilibria. What is the mass action expression"? Define Q. How is Q different from K, the equilibrium constant? When are they equal? Is an equilibrium constant "constant" at different concentrations? at different temperatures? What is the equilibrium condition? How is Kp related to Kc in the case of gases. gases. Do K's have units? What is a homogeneous equilibrium? Heterogeneous equilibrium? Be able to solve problems involving both. What is the relationship between values of Keq for forward and reverse reactions? Be able to solve equilibrium problems like the examples we have seen in class. When are approximations legitimate? What assumptions are involved? Be sure you note assumptions. Be able to use quadratic equation if necessary.
Acid-base Equilibria: Electrolytes. Dissociation. What
is meant by "strong" and "weak" in reference
to electrolytes, acids and bases? Degree of dissociation. Aqueous
Solution Reactions: Be able to define acids and bases by the
Arrhenius, Brönsted-Lowry, and Lewis definitions. What do
we mean by conjugate acid and/or conjugate base in the "Brönsted"
definition. What are the meanings of "strong" and "weak"
for acids and bases by these definitions? What are precipitation
and complexation reactions? Be able to write net ionic equations!
Be able to write net ionic equations! Be familiar with classification
scheme for reactions, solubility rules and strengths of electrolytes.
What is Kdiss? Ka? Kb? Ki?
Be able to write K's for acid/base reactions in both the Arrhenius
and Brönsted-Lowry formulations. Be able to solve all manner
of acid/base equilibrium problems. % dissociation problems. Polyprotic
acids. What is an ion product? Know the ion product (Kw)
for water. What is pH? Define it. be able to solve pH problems.
what is the relation of pH to pOH? What is the pH of a neutral
solution? salt solutions? What does this depend on? Hydrolysis
problems-what is going on here? What is Kh? What is
its relationship to Ka and/or Kb? Correlate
the Kh expression with chemical equation. Why are the
various terms where they are? Titrations: Be able to draw
and interpret titration curves as we have seen in class and lab.
Be able to find the equivalence point, buffer range, Ka
or Kb and to identify the acid and base species in
solution at any point along the curve. What is an indicator? How
does it work? Buffers: What is a buffer? Define precisely.
Be able to do buffer problems. How can you make a buffer?
| Syllabus / Schedule |
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© R A Paselk
Last modified 24 July 2002
