CHEM 1101 Lecture Notes - Lecture 10: Valence Bond Theory, Sigma Bond, Yorkshire Carnegie

• School: Carleton University
• Department: Chemistry
• Course: CHEM 1101
• Professor: Pam Wolff

Document Summary

This can be shown with a lower case greek delta" and the sign of the partial charge. It can also be shown as a vector (drawn on the line(s) of the bond, pointing in the direction that the electron density has shifted, toward the more electronegative). The definition of this is the overall shift in electron density on the entire molecule. It is the vector sum of the bond dipoles -- and is also shown with an arrow or with partial charge symbols[ Note: lone pairs do not contribute to dipole moments by themselves. Non-zero formal charges do (in the direction of a negative f. c. and away from a positive f. c. ) Two atomic orbitals overlap so that the electrons are attracted to both nuclei. Bond orders (lewis diagrams are based on valence bond theory) Molecular shapes (vsepr diagrams are also based on valence bond theory) see below for sigma bonds.