<P> In chemistry, a molecular orbital (MO) is a mathematical function describing the wave - like behavior of an electron in a molecule . This function can be used to calculate chemical and physical properties such as the probability of finding an electron in any specific region . The term orbital was introduced by Robert S. Mulliken in 1932 as an abbreviation for one - electron orbital wave function . At an elementary level, it is used to describe the region of space in which the function has a significant amplitude . Molecular orbitals are usually constructed by combining atomic orbitals or hybrid orbitals from each atom of the molecule, or other molecular orbitals from groups of atoms . They can be quantitatively calculated using the Hartree--Fock or self - consistent field (SCF) methods . </P> <P> A molecular orbital (MO) can be used to represent the regions in a molecule where an electron occupying that orbital is likely to be found . Molecular orbitals are obtained from the combination of atomic orbitals, which predict the location of an electron in an atom . A molecular orbital can specify the electron configuration of a molecule: the spatial distribution and energy of one (or one pair of) electron (s). Most commonly a MO is represented as a linear combination of atomic orbitals (the LCAO - MO method), especially in qualitative or very approximate usage . They are invaluable in providing a simple model of bonding in molecules, understood through molecular orbital theory . Most present - day methods in computational chemistry begin by calculating the MOs of the system . A molecular orbital describes the behavior of one electron in the electric field generated by the nuclei and some average distribution of the other electrons . In the case of two electrons occupying the same orbital, the Pauli principle demands that they have opposite spin . Necessarily this is an approximation, and highly accurate descriptions of the molecular electronic wave function do not have orbitals (see configuration interaction). </P> <P> Molecular orbitals arise from allowed interactions between atomic orbitals, which are allowed if the symmetries (determined from group theory) of the atomic orbitals are compatible with each other . Efficiency of atomic orbital interactions is determined from the overlap (a measure of how well two orbitals constructively interact with one another) between two atomic orbitals, which is significant if the atomic orbitals are close in energy . Finally, the number of molecular orbitals formed must be equal to the number of atomic orbitals in the atoms being combined to form the molecule . </P>

Where are the electrons most likely located in a molecular bonding orbital
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