Terminology to recall from your general chemistry class:
(Note that your Study Guide has a glossary with definitions)
atomic orbitals: s, p, d
molecular orbitals: sigma and pi bonds
hybrid orbitals: sp, sp2, sp3
types of bonds: ionic, covalent, polar covalent
valence: normal bonding patterns for C, H, N, O, halogens
electronegativity: higher to the right and up the Periodic Table
Bronsted-Lowry definition of acids and bases: H+ donors and acceptors
Lewis definition of acids and bases: electron pair acceptors and donors
acidity constant (Ka) and pKa: indicators of acid strength
The Periodic Table: periodic trends in valence, electronegativity,
etc.
Lewis structures: all electrons shown
Kekule structures: lines represent bonds
line structures: omit Cs and Hs
condensed structures: abbreviations for standard structural units
hybridization: hybrid orbitals allow optimum bonding
acid/base reactions: identify acids and bases
conjugate acid/base pairs: stronger acids have weaker conjugate bases
create appropriate Lewis structures, including formal charges
recognize different resonance forms for a given molecule
interpret Kekule, line, and condensed structures
identify polar bonds and direction of polarity
predict major form of conjugate acid or base, knowing pH and pKa
predict the preferred direction of acid-base equilibria
identify the hybridization of a given C based on the number of atoms
it is bonded to
using the hybridization of each C, write good 3D structures for molecules