CHEM 120A Lecture Notes - Lecture 7: Linear Combination, Diamagnetism, Antibonding Molecular Orbital
15 Oct 2016
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Document Summary
Lewis structures and vsepr shapes imply that electrons are simple dots that belong to atoms; they do not represent electrons as particles with quantum behavior. In this theory, it is proposed that the different valence electrons within an atom move along their different orbitals. The number of standard atomic orbtals added together always equals the number of hybrid orbitals formed. The number of standard atomic orbitals determine the shapes and energies of the hybrid orbitals formed: the hybridized orbital is the one that yields the lowest overall energy for the molecule. Sigma-bond: orbitals that overlap each other: most common type of hybrid bond, occurs within single bonds. Pi-bond: orbital that occurs when p-orbitals are parallel to each other: only occurs within double and triple bonds. Example: if an atom within a molecule has a triple bond to one atom and a single bond to another, it is said to have 2 sigma-bonds and 2 pi- bonds.
