Quizzes (all quiz keys are posted on Moodle) and problem sets since Exam I. Review nomenclature so that you can read questions and understand them.
Be able to write formulas from names and names from formulas for ionic compounds. Be able to recognize and name acids and bases, and to write formulas of acids and bases given names. Predict the charges of the ions of the representative elements. Note why they have these charges (stable octets, attain "electronic structure" of "nearest" Inert gas, etc.). Practice problems are available in the Nomenclature Supplemental Study Module.
Be able to draw correct Lewis Structures for molecules with multiple bonds and for molecules with resonace structures. [Predict whether a bond between two atoms is covalent or ionic. Predict the charges of ions of the representative elements. Explain why they have these charges (stable octets). Octet Rule. Valence electrons. Lewis Dot Structures. What does the kernel of a Lewis Structure represent? Be able to write Lewis Structures for atoms, ions and compounds of the representative elements (PS in lab manual, pg 49 ff). How do you guess whether a compound is likely to be ionic or covalent? (hi, lo, intermediate rules for electronegativity). Don't forget charges for ions and brackets for negative ions! ] Practice problems are available in the Lewis Structures Supplemental Study Module.
VSEPR Theory. Steric number. Electronic shapes (linear, trigonal planar, tetrahedral) vs. molecular shapes (linear, bent, trigonal planar, trigonal pyramidal, tetrahedral). When and why do the various electronic shapes give rise to the different molecular shapes (electronic shape determined by connecting electron pairs and/or bonding electron clouds, molecular shape determined by connecting nuclei of attached atoms). Be able to predict the shapes of simple molecules using VSEPR Theory. Dipole. Dipole moment. Be able to predict the polarity of a covalent bond and the direction of its dipole moment. Practice problems are available in the VSEPR Theory and Molecular Geometry Supplemental Study Module.
What is a weak bond? What are the different types? (van der Waal's and Hydrogen bonds). What are van der Waal's bonds? How do they work? (generally contact only). When are they important?
Be able to balance simple equations by inspection such as we have done in class. Be able to identify redox reactions. Be able to identify oxidant and reductant, oxidizer and reducer, oxidized and reduced substances in chemical reactions. Be able to balance redox equations using the half-reaction method, as in the lecture example & Redox Balancing Supplemental Study Module.
What is a mole? (One mole = number of atoms in exactly 12 grams of 12C = 6.02 x 1023 particles). What is a formula unit? What is the mass of one atom in grams? (Atomic mass in g/Avogadro's number) What is the mass of one amu? What is stoichiometry? Be able to solve mole problems such as we have seen in class; How many moles in _ ? How many atoms of _ in _ ? How many molecules of _ in _ ? How many grams of _ in _ ? etc.) Practice problems are available in the Stoichiometry-Moles Supplemental Study Module. Be able to solve concentration and dilution problems. 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 solve problems involving stoichiometric relationships in chemical reactions. Be able to do simple problems involving reactant excess and problems with a limiting reagent. Practice problems are available in the Reaction Stoichiometry Supplemental Study Module.
Define/describe: pressure, barometer, manometer, Boyle's Law, Charles' Law, Standard Atmosphere, Avogadro's Principle, Ideal Gas, Perfect Gas, Dalton's Law of Partial Pressures, Kinetic Energy (=1/2 mv2), Ideal Gas Law (PV=nRT). What does absolute zero represent? What is the rationale behind this concept? (Can't have negative volume.) Be able to solve gas law problems such as we have seen in class. 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! What is the volume of one mole of an ideal gas at STP? Practice problems are available in the Gas Law Problem Supplemental Study Module (1-5 only for this exam).
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© R Paselk
Last modified 6 November 2006