Knowledge - Level 1

Terminology to recall from your general chemistry class:
(Note that your textbook 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

functional groups: alcohols, ethers, carbonyls (aldehydes, ketones), carboxylic acids

isomers: different compounds having the same molecular formula

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

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Concepts - Level 2

The Periodic Table: periodic trends in valence, electronegativity, etc.

Lewis structures: all electrons shown, dashes represent bonding electron pairs

line structures: omit Cs and Hs

condensed structures: abbreviations for standard structural units

VSEPR: method of identifying preferred 3D structures

hybridization: hybrid orbitals allow optimum bonding

functional groups: carbon and oxygen bonding patterns, isomerism

acid/base reactions: identify acids and bases

conjugate acid/base pairs: stronger acids have weaker conjugate bases

understand structural effects on acid strength

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Applications - Level 3

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, knowing Ka data

predict relative acid strengths, based on structures

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Analytical Skills - Level 4

identify the hybridization of a given atom or a given bond

using hybridization or VSEPR, write good 3D structures for molecules

identify constitutional isomers for a given molecular formula