Polar Molecules - Valence Bond (VB) Theory Molecular Shapes...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Polar Molecules: The Influence of shape Polar Molecules must meet two requirements: One polar bond or one lone pair of electrons on central atom. Neither bonds nor lone pairs can be symmetrically arranged that their polarities cancel. Valence Bond (VB) Theory Covalent bonds are formed by the overlap of atomic orbitals. Atomic orbitals on the central atom can mix and exchange their character with other atoms in a molecule. Process is called hybridization . Hybrids are common: Pink flowers Mules Hybrid Orbitals have the same shapes as predicted by VSEPR.
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Valence Bond (VB) Theory Molecular Shapes and Bonding In the next sections we will use the following terminology: A = central atom B = bonding pairs around central atom U = lone pairs around central atom For example: AB 3 U designates that there are 3 bonding pairs and 1 lone pair around the central atom. Linear Electronic Arrangement:AB 2 Species (No Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: – BeCl 2 , BeBr 2 , BeI 2 , HgCl 2 , CdCl 2 All of these examples are linear, nonpolar molecules....
View Full Document

This note was uploaded on 11/25/2011 for the course CHEM 1211 taught by Professor Atwood during the Fall '07 term at University of Georgia Athens.

Ask a homework question - tutors are online