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-
- 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
- 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."
From here you can go back to the Chemistry 101A home page.
Last updated 19 Aug 97