Chemistry 101A Study Guide 2

CHEMISTRY 101A

Study Guide for Exam 2

1. As a general rule, study (in order of decreasing priority):: a. Your class notes - these will tell you what the instructor thinks is important,; b. The problem sets and suggested practice problems - problems on the exams will be similar to these, (In each case rework the problems from scratch, don't just look over solved problems.); c. The text - to fill in the details,; d. Old exams - this will help you relax by showing you what to expect.
2. You should know from memory:: The names, formulas, and charges of the ions in Table 4.4 (p 91).; The general trends in electronegativity (referred to the periodic table).; Boyle's law, Gay-Lussac's law, Charles' law, the combined gas law, the ideal gas law, Dalton's law, Avogadro's law, and; Graham's law of diffusion.; The difference between solute and solvent.; Examples of the main types of solutions.; The principal characteristics of a solution.; The solubility "rules" in the notes and on p 151.; What is meant by solubility, saturated, unsaturated, supersaturated.
3. You should know how to:: Determine the chemical formulas of simple covalent compounds.; Write Lewis dot structures of atoms and simple molecules and ions (including molecules with single-, double-, and triple- bonds).; Tell the difference between å bonding, ã bonding, and nonbonding electron pairs.; Draw Lewis dot structures of molecules that contain coordinate covalent bonds.; Determine the shapes and bond angles of a molecule or ion using VSEPR.; Use electronegativities to determine if a compound is ionic or covalent.; Determine if a molecule is polar or nonpolar.; Name binary compounds and compounds of metals and polyatomic ions.; Determine the formula weight of a compound.; Calculate the number of moles and the number of molecules in a given weight of a compound.; Balance a chemical reaction equation.; Work stoichiometry problems, including finding percent yield and limiting reagents.; Write reactions between ionic compounds in water solution and eliminate spectator ions.; Recognize a redox reaction.; Find the oxidation number of an element in a compound or ion and tell which elements are oxidized or reduced in a chemical reaction.; Recognize typical combustion, respiration, and corrosion reactions.; Convert back and forth between various pressure units.; Do gas law problems using Boyle's law, Gay-Lussac's law, Charles' law, the combined gas law, or the ideal gas law.; Find the formula weight of a compound from gas data.; Determine relative diffusion rates of pairs of gases.; Tell which intermolecular forces a particular compound will have.; Predict relative vapor pressures and boiling points of pairs of compounds.; Predict solubilities of compounds in liquids.
4. You should understand:: What is meant by covalent bond and electron sharing.; The difference between single, double, and triple bonds.; The octet rule and its exceptions.; The difference between exothermic and endothermic chemical reactions.; The qualitative differences between gases, liquids, and solids.; The origin of gas pressure.; How mercury barometers and manometers work.; What is meant by the vapor pressure of a liquid.; What is meant by systolic and diastolic blood pressures.; The difference between London dispersion forces, dipole-dipole forces, and hydrogen bonding forces.; The relationship between kinetic energy and intermolecular forces in condensation and freezing.; What is meant by super cooling, and sublimation.; The effect of temperature on the solubility of solids and gases in liquids.; The effect of pressure on the solubility of solids and gases in liquids.; The origin of "the bends."

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Last updated 19 Aug 97