Principles of Molecular Orbital Theory

You can think of a molecular orbital as being formed from a combination of atomic orbitals. As atoms approach each other and their atomic orbitals overlap, molecular orbitals are formed. [Pg.400]

Liquid oxygen is poured between the poles of a strong magnet. Oxygen adheres to the poles, showing that it is paramagnetic. [Pg.400]

Formation of bonding and antibonding orbitals from Is orbitals of hydrogen atoms [Pg.401]

When the two Is orbitals overlap, they can either add to give a bonding molecular orbital or subtract to give an antibonding molecular orbital. [Pg.401]

Addition of orbitals builds up electron density in overlap region [Pg.401]

This chapter consists of the application of the symmetry concepts of Chapter 2 to the construction of molecular orbitals for a range of diatomic molecules. The principles of molecular orbital theory are developed in the discussion of the bonding of the simplest molecular species, the one-electron dihydrogen molecule-ion, H2+, and the simplest molecule, the two-electron dihydrogen molecule. Valence bond theory is introduced and compared with molecular orbital theory. The photo-electron spectrum of the dihydrogen molecule is described and interpreted. [Pg.34]

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