CH 101 Chapter Notes - Chapter 9: Bond Length, Formal Charge, Chemical Polarity
Document Summary
In lewis theory, named after g. n. lewis, valence electrons are represented as dots. We can draw lewis electron-dot structures (or simply lewis structures) to depict molecules. Simplest model for making quick, everyday predictions about most molecules. Chemical bonds form because they lower the potential energy between the charged particles that compose atoms. Ionic bond- when a metal bonds with a nonmetal, transferring one or more electrons to the nonmetal. The metal atom becomes a cation and the nonmetal atom becomes an anion. The oppositely charged ions then attract one another, lowering their overall potential energy. Covalent bond- when a nonmetal bonds with another nonmetal; neither atom transfers electrons to the other. Shared electrons interact with the nuclei of both of the bonding atoms, lowering their potential energy. Metallic bonding- electrons are pooled and delocalized over the entire metal. Positively charged metal atoms are then attracted to the sea of electrons, holding the metal together.