Topics for Final Exam
CHEM 1412- General Chemistry II
Houston Community College System
About the Exam
1. Prepare for 35 multiple choice questions (two points each) and six (five points each) essay/show work problems.
Essay/show work problems will receive partial credit.
2. Bring a #2 lead pencil, and a Scantron answer sheet.
3. The final exam will be comprehensive and will include chapter 24
4. Review problems worked out in class as well as those assigned from each chapter.
5. A periodic table, values of constants, and relatively complex equations will be provided.
Values from appendices will be provided.
6. Remember that the final exam is system wide and is mandatory. The final exam grade will
not be
dropped.
CHAPTER 12
 Know the ways of expressing concentrations: w/w %, w/v %, M, m and X (mole fraction).
 Know how to calculate the quantity of solute given the volume and concentration of a solution.
 Know how various factors affect the solubility of a solute: nature of solvent and solute, pressure and temperature.
Know Henry’s Law.
 The colligative properties: lowering of vapor pressure (and Raoult’s Law), boiling point elevation, freezing point depression and
osmosis.
 Be able to rank the boiling point (or freezing point) of a set of solutions (Refer to Sample Exercise 13.8).
 Know the characteristics of true solution, colloidal dispersion and suspension. Be familiar with terms: hydrophilic, hydrophobic
and the Tyndall effect.
CHAPTER 13
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Know the factors that affect the rate of reactions: concentration, temperature, catalyst, surface area and the nature of reactants.
Know the terms and differences of: average rate, instantaneous rate, initial rate, rate law, and rate constant.
Know how to relate the rate of appearance or disappearance of one compound to another in a reaction.
Know the definition of reaction order, units of rate constants for 1st and 2nd order reactions.
Know how to use initial rates to determine rate laws.
Know how to apply the 1st and 2nd order reaction equations that relate concentration and time.
Know the definition of half-life, its relationship to rate constant and concentration and its unit.
Know the meaning of energy profiles (such as Fig. 14.15, 14.21), activation energy (Ea), and the Arrhenius equation.
Know the terms of: mechanism of a reaction, elementary step, molecularity, rate-determining step, homogeneous and
heterogeneous catalysis.
CHAPTER 14
 Given a reversible reaction, be able to write the expression for the equilibrium constant, Keq, in a homogeneous or a
heterogeneous reaction.
 Given the concentration of compounds in equilibrium, be able to calculate the value of the equilibrium constant, Keq.
 Know the relationship of Kc and Kp.
 Know how to use Q and Keq to predict the direction of a reaction. Use Keq to calculate the concentration of a compound in
equilibrium.
 Know how the Le Chatelier’s Principle works.
CHAPTER 15
 Know the definition of Kw, pH, Bronsted-Lowry acids and bases, Lewis acids and bases, conjugated acids and bases, strong and
weak acids and bases.
 Know formulas of typical strong acids and bases. The rest can be considered as weak acids and bases.
 Ka X Kb = Kw for conjugated acid and base pair.
 Know how to predict the acid-base properties of salt solutions.
 Know how to calculate the pH of a weak acid solution given the concentration and Ka for the acid.
CHAPTER 16
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Know the common-ion effect in a weak acid or a weak base.
Know the components making up a buffer solution and how to calculate the pH of the solution.
Know how to calculate the pH in the process of titration between a strong acid and a strong base.
Know how to calculate the pH in the process of titration between a strong base and a weak acid.
Know the definition of Ksp and its application in determining the solubility of the salt in pure water and in a solution which has
common ions.
 Know how to calculate Q and compare to Ksp to determine whether a precipitate will form.
Chapter 18
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Know the definition of entropy and the calculation of S.
Know the definition and calculation G and its sign in relation to spontaneity of a chemical process.
Know the second and the third law of thermodynamics.
Know how to calculate Keq from G.
Know the sign of H and S and its effects on G at high and low temperature and on spontaneity of a reaction.
Know the equations:
G = G + RT ln Q
G = H - T S
CHAPTER 19
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Know the definition of a redox reaction, oxidizing and reducing agents.
Know how to balance a redox reaction in an acidic or a basic solution using half reactions.
Know how to calculate Ecell from two half-cell voltages.
Know the sign of E and its relationship to the spontaneity of a redox reaction.
Know the Nernst equation: E = E - 0.0592/n log Q at 25oC
Know how to predict the cathode and anode products in an electrolytic cell.
Know how to calculate the quantity of neutral metal produced by running a current through the cell for a period of time.
CHAPTER 23
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Know the symbols of particles in a nuclear reaction: alpha, beta, gamma, position, neutron, proton etc.
Know the pattern of nuclear stability.
Know how to balance a nuclear reaction equation.
Know how to calculate the quantity of a radioactive species given its half-life and time.
Know how to calculate mass defect and nuclear binding energy using E=mc2
Know the definition and example of nuclear fission and nuclear fusion.
Know some of the units used in measuring radioactivity (e.g., the curie, rad, and rem)
CHAPTER 24
 Know the IUPAC rules of naming alkanes, cycloalkanes, alkenes alkynes, haloalkanes and benzene.
 Know the functional group of alcohol , ether, amine, aldehyde, ketone, caboxylic acid, ester and amide.