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Upon completion of the course, the student should be able to:
1. compare Arrhenius, Bronsted-Lowery and Lewis acids and bases.
2. predict relative acid and base strengths.
3. assign oxidation numbers.
4. balance oxidation-reduction reactions by the half-reaction method
and the oxidation number method.
5. solve acid-base and oxidation-reduction stoichiometric problems.
6. determine the rate of a reaction.
7. explain the dependence of reaction rate on concentration and
temperature.
8. describe and explain collision theory and transition-state theory.
9. solve problems based on the Arrhenius equation.
10. determine the order of a chemical reaction.
11. describe the influence of a catalyst on reaction rate.
12. determine the rate law for a reaction based on the reaction mechanism.
13. determine the extent of molecular reactions through the study of
chemical equilibria.
14. apply Le Chatelier's principle to chemical equilibria.
15. describe the self-ionization of water.
16. compute the pH of a solution of a strong acid or strong base.
17. solve problems based on the ionization of a weak acid or weak base.
18. predict the acid-base properties of salt solutions.
19. describe the preparation of a buffer.
20. perform buffer calculations.
21. calculate points on a titration curve.
22. predict the appearance of a titration curve.
23. determine the solubility product expressions for sparingly soluble
ionic solids.
24. perform calculations based on solubility product expressions.
25. apply equilibrium concepts to complex-ions.
26. use qualitative analysis schemes to determine the identities of the
substances present in a mixture.
27. explain the first, second and third laws of thermodynamics.
28. solve problems based on the laws of thermodynamics.
29. determine the spontaneity of a reaction.
30. relate the free energy of a reaction to the reaction's equilibrium
constant.
31. describe the construction of voltaic cells.
32. use standard reduction potentials to compute a cell's potential.
33. compute the equilibrium constant for a voltaic cell form the cell's
emf.
34. describe some commercial voltaic cells.
35. compare electrolytic cells with voltaic cells.
36. solve stoichiometric calculations based on electrolysis.
37. define radioactivity and describe the different types of radiation.
38. balance nuclear reaction equations.
39. solve problems based on the rate of the radioactive decay of an
isotope.
40. describe the detection and biological effects of radiation.
41. describe the applications of radioactive isotopes.
42. solve mass-energy calculations for nuclear reactions.
43. describe nuclear fusion and nuclear fission.
44. describe the basic steps involved in metallurgy.
45. describe the different models of metallic bonding.
46. describe the chemistry of the alkali metals, the alkaline earth
metals, and the metals of groups IIIA and IVA.
47. describe the chemistry of the nonmetals of groups IVA-VIIIA.
48. describe and explain the periodic trends in the transition elements.
49. describe the formation and structure of complex-ions and coordination
compounds.
50. name coordination compounds.
51. describe the valence bond theory and the crystal field theory of
complexes.
52. describe the structures of alkanes, cycloaalkanes, alkenes, alynes,
aromatic hydrocarbons, alcohols, ethers, aldehydes, ketones,
carboxylic acids, amines and amides.
53. use standard nomenclature of alkanes, cyloalkanes, alkenes, alkynes,
aromatic hydrocarbons, alcohols, ethers, aldehydes,ketones, carbo-
xylic acids, esters, amines and amides.
54. predict reactions of hydrocarbons.
55. predict reactions of oxygen-containing organic compounds.
56. predict reactions of nitrogen-containing organic compounds.
57. describe the structures of organic polymers.
In the laboratory upon completion of the course, the student should be
able to:
1. observe all of the fundamental safety procedures elucidated at the
beginning of the course and repeated throughout the semester;
2. properly dispose of waste chemicals;
3. manipulate standard laboratory apparatus including chemical dispensers,
4. perform gravimetric analysis;
5. perform titrimetic analysis;
6. collect and analyze scientific data using graphical and statistical
methods;
7. summarize laboratory results in both formal and informal report
formats;
8. use a Macintosh personal computer (or equivalent) to perform word-
processing, spreadsheet computations, graphing and statistical
calculations for laboratory reports;
9. use microcell plates and micropipettes
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Lecture Material
1. Chemical Reactions: Acid-base and Oxidation-Reduction Concepts
a) Arrhenius concept
b) Bronsted-Lowery concept
c) Lewis concept
d) Relative strengths of acids and bases
e) Oxidation numbers
f) Describing oxidation-reduction reactions
g) Acid-base and oxidation reduction stoichiometry
2. Rates of Reactions
a) Reaction rates
b) Collision and transition-state theories
c) Arrhenius equation
d) Reaction mechanisms
3. Chemical equilibrium; Gaseous Reactions
a) The equilibrium constant
b) Qualitative and quantitative aspects of the equilibrium constant
c) Le Chatelier's principle
4. Acid-base Equilibria
a) Self-ionization of water
b) Strong and weak acids and bases
c) Solution pH
d) Acid and base ionization equilibria
e) Polyprotic acids
f) Hydrolysis
g) Buffers
h) Acid-base titration curves
5. Solubility and Complex-Ion Equilibria
a) Solubility product constant
b) Precipitation calculations
c) Complex-ion formation
d) Qualitative analysis
6. Thermodynamics and Equilibria
a) Enthalpy and entropy
b) First, second and third laws of thermodynamics
c) Free-energy
7. Electrochemistry
a) Construction and notation of voltaic cells
b) Electromotive force
c) Cell potential
d) Free-energy and equilibrium constants from emf's
e) Electrolytic cells
f) Stoichiometry of electrolysis
8. Nuclear Chemistry
a) Radioactivity and its detection
b) Nuclear reactions and equations
c) Rate of radioactive decay
d) Mass-energy calculations
e) Nuclear fission and nuclear fusion
f) Applications of radioactive isotopes
9. Metallurgy and Chemistry of the Main-Group Elements
a) Metallurgy
b) Bonding in metals
c) The alkali metals
d) The alkaline earth metals
e) The metals of groups IIIA and IVA
10.Chemistry of the Nonmetals
a) The carbon family
b) The nitrogen family
c) The oxygen family
d) The halogens
e) The noble gases
11.The Transition Elements
a) Properties of the transition elements
b) Complex-ions and coordination compounds
c) Naming coordination compounds
d) Structure
e) Valence bond theory and crystal theory
12.Organic Chemistry
a) Hydrocarbons
b) Derivatives of hydrocarbons
c) Organic polymers
Laboratory Material
1. Volumetric analysis
2. Titrimetric analysis
3. Chemical kinetics
4. Acid-base chemistry
5. Oxidation-reduction chemistry
6. Electrochemistry
7. Chemical equilibria
8. Synthesis
9. Instrumental analysis
10.Spectroscopy
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LECTURE TEXTS:
GENERAL CHEMISTRY by Darrell Ebbing, Houghton Mifflin, 1996.
CHEMISTRY: by Steven Zumdahl, D.C. Heath, 1997
CHEMISTRY: SCIENCE OF CHANGE by Oxtoby, Nachtrieb & Freeman, Saunders,1994
CHEMISTRY: THE STUDY OF MATTER AND ITS CHANGES by Brady & Holum,Wiley,1993
LABORATORY MANUALS:
CHEMISTRY IN THE LABORATORY by Roberts, Hollenberg, Postma, Freeman, 1997.
CHEMISTRY IN THE LABORATORY by Jo Beran, Wiley, 1993
EXPERIMENTS IN GENERAL CHEMISTRY by R. Wentworth, Houghton Mifflin, 1993
EXPERIMENTAL CHEMISTRY by James F. Hall, D.C. Heath, 1993
SPECIAL STUDENT MATERIALS:
Laboratory apron
Scientific calculator
Laboratory data notebook
Safety goggles
