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Unformatted text preview: To see how we use these concepts in Molecular Orbital Theory, let's start with H 2 , the simplest of all molecules. The 1s orbitals of the H-atom are standing waves of the electron wavefunction. In Molecular Orbital Theory we view the bonding of the two H-atoms as partial constructive interference between standing wavefunctions of the 1s orbitals. We can also have partial destructive interference. The energy of the H 2 molecule with the two electrons in the bonding orbital is lower by 435 kJ/mole than the combined energy of the two seperate H-atoms. On the other hand, the energy of the H 2 molecule with two electrons in the antibonding orbital is higher than two separate H-atoms. To show the relative energies we use diagrams like this: In the H 2 molecule, the bonding and anti-bonding orbitals are called sigma orbitals ( )....
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