Chapter 1 Skills

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