1 Lecture 2 Simple Molecular Orbitals - Sigma and …

1 Lecture 2 Simple Molecular Orbitals - Sigma and Pi Bonds in molecules bond order = (number of bonding electrons) - (numberof antibonding e lectrons) 2= amount of bonding 1sahydrogen molecule = H2 LUMOHOMO = 1sa + 1sb = bonding MO =potential energy higher,less stable lower,more stableLUMO = lowest unoccupied Molecular orbitalHOMO = highest occupied Molecular orbitalSimilar phase of electron density (no node) adds together of isolated atomsbond order (H2 molecule) =(2) - (0) 2= 1 bond1sbHHHHHH = 1sa - 1sb = antibonding MO =LCAO = linear combination of atomic orbitalsnode = zero electron density because of opposite phases E = bond energyThere is a big energy advantage for a hydrogen molecule over two hydrogen atoms.

1 Lecture 2 Simple Molecular Orbitals - Sigma and Pi Bonds in Molecules bond order = (number of bonding electrons) - (number of antibonding elect rons)

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