Chapter 14 Study Guide

Chapter 14 Study Guide - Chapter 14 Study Guide...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapter 14 Study Guide Hybridization: a mixing of the native orbitals on a given atom to form special atomic orbitals for bonding Hybridization is a modification of the LE model to account for the observation that atoms often seem to use special atomic orbitals in forming molecules. sp 3 hybridization: 1(s orbital) + 3(p orbitals) 4 sp 3 orbitals sp 3 hybridization gives a tetrahedral set of orbitals. Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, this model assumes that the atom forms a set of sp 3 orbitals. Hybrid orbitals: a set of atomic orbitals adopted by an atom in a molecule different from those of the atom in the free state sp 2 hybridization: 1(s orbital) + 2(p orbitals) 3 sp 2 orbitals The assumption that a double bond acts as one effective electron pair, equivalent to a single bonding pair, works well to give the approximate molecular structure. sp 2 hybridization gives a trigonal planar arrangement of atomic orbitals. sigma (σ) bond: a covalent bond in which the electron pair is shared in an area centered on a line running between the atoms pi (Π) bond: a covalent bond in which parallel p orbitals share an electron pair
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 09/19/2011 for the course CHEM 43L taught by Professor Therien during the Fall '09 term at Duke.

Page1 / 3

Chapter 14 Study Guide - Chapter 14 Study Guide...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online