| Syllabus / Schedule | 
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| Chem 109, Dr. Paselk |
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Summer 2002 |
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Review: Problem sets and appropriate lab calculations.
Nomenclature: Know the elements, ions, and common names on the Nomenclature Supplements on the web. Be able to name compounds using "Stock" (systematic) nomenclature as in your text and lab manual appendix. Be able to write formulae for compounds named systematically and using the -ous -ic system for common metal ions (iron, copper, tin, mercury, lead).
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), including liters to m3 etc., know prefixes in metric system we discussed (mega-, kilo-, deci-, centi-, milli-, micro-, nano-, pico-, femto-.), make approximate conversions between American and metric systems (one inch = 2.54 cm exactly; a yard is about a meter; a quart is about a liter); solve density problems.
Atoms: Be able to describe/discuss the basic premises of the Dalton atom model. Be able to describe/discuss the basic premises of the Thompson and Rutherford atom models, and know what key problem/experiment led to the rejection of each. What is the make-up of an atom according to the modern picture? Be able to fill out tables as we did in class for isotopes (for example: given A & Z find numbers of protons, symbol, etc.). What is an isotope? How do isotopes differ from each other? Are there significant chemical differences between isotopes of the same element? Be able to determine the % composition of elements in terms of their isotopes. Be able to determine the atomic weight of an element given its isotopic % composition.
Moles and formulae: What is a mole? (One mole = number of atoms in exactly 12 grams of 12C = 6.022 x 1023 particles). What is a formula unit? What is the mass of one atom in grams? What is the mass of one amu? Be able to solve mole problems such as in your lab book. (How many moles of _ in _ ? How many atoms of _ in _ ? How many molecules of _ in _ ? How many grams of _ in _ ? etc.). Be able to find formula weights of compounds. Be able to find % composition of compounds given formulae. Be able to find formulae of compounds given % composition. Be able to find molecular formulae given % composition and MW. Be able to determine molarity. Be able to find number of moles given molar concentration. Be able to do dilution problems.
Chemical Equations: Be able to balance simple equations by inspection such as we have done in class.
Solutions: Define/describe: solution, salt, solvent, solute, saturated solution, unsaturated solution, super saturated solution, mass %, molarity, neutralization, equivalent (in chemical reactions, e.g. titrations). 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: 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 problems in problem set.
Solution Reactions: 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 definition. What are the meanings of "strong" and "weak" for acids and bases by these definitions? What are precipitation and complexation reactions? You should always write net ionic equations when appropriate, so be prepared to do so! Be familiar with classification scheme for reactions in text. Be familiar with solubility rules and strengths of electrolytes.
Oxidation-Reduction:What is oxidation? What is reduction? Redox. Be able to recognize oxidizers/reducers, oxidants/reductants in chemical reactions. Know rules for determining oxidation numbers. Be able to assign oxidation numbers to atoms in compounds and compound ions (e.g. sulfate or acetate ion). Be able to write half-reactions. Be able to balance ionic redox reactions by the half-reaction method.
Stoichiometry: What is stoichiometry? Be able to solve problems involving stoichiometric relationships in chemical reactions. Be able to do both problems involving reactant excess and problems with a limiting reagent. (Lecture examples, and don't forget problems in lab book and text.)
Gases: Define/describe: pressure, barometer, manometer, Boyle's Law, Charles Law, Standard Atmosphere, Avogadro's Principle, Ideal Gas, Perfect Gas, STP, Dalton's Law of Partial Pressures, Kinetic Energy (=1/2 mv2), Ideal Gas Law (PV=nRT), Graham's Laws of effusion and diffusion (remember diffusion law is off). What does absolute zero represent? What is the rationale behind this concept? (can't have negative volume). Be able to solve Ideal Gas Law and gas problems such as we have seen in class and on the homework and problem sets. Remember: all temperatures must be in K (absolute temperature!), and if you are using R, pressures must be in atmospheres, volumes in liters and quantity in moles for our value of R! What is the volume of one mole of an ideal gas at STP? Be able to do gas stoichiometry problems. 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?
Memorize: The gas constant, R= 0.082 1 L*atm*mol-1*K-1. Avogadro's number = 6.02 x 1023. Mass of one amu in grams (one gram divided by Avogadro's number), equations needed to solve gas problems.
| Syllabus / Schedule |
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© R A Paselk
Last modified 21 May 2002
