Chem 334 - Fall 2001
Organic Chemistry I
Dr. Carl C. Wamser
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
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
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
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