Molecular orbital theory is a model used in chemistry to explain the bonding and properties of molecules. It describes the behavior of electrons in a molecule by considering the overlapping of atomic orbitals to form molecular orbitals.
Molecular orbital theory explains bonding by considering the constructive and destructive interference of atomic orbitals. When two atomic orbitals overlap in phase, a bonding molecular orbital is formed, while when they overlap out of phase, an antibonding molecular orbital is formed.
Mixing in molecular orbital theory refers to the combination of atomic orbitals to form molecular orbitals. This process involves the overlapping of atomic orbitals and the redistribution of electrons to form new molecular orbitals with different properties.
There is mixing in molecular orbital theory because it allows for a more accurate description of the electronic structure and properties of molecules. By considering the overlapping of atomic orbitals, molecular orbital theory can explain the observed bond lengths, bond energies, and other properties of molecules that cannot be explained by simple Lewis structures.
Molecular orbital theory predicts the properties of molecules by considering the distribution of electrons in molecular orbitals. The number of electrons in bonding and antibonding molecular orbitals can determine the stability and reactivity of a molecule, as well as its overall shape and properties such as bond angles and dipole moments.