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The resulting electron configuration can be described in terms of bond type, parity and occupancy for example dihydrogen 1σ g 2. Alternatively it can be written as a molecular term symbol e.g. 1 Σ g + for dihydrogen. Sometimes, the letter n is used to designate a non-bonding orbital. For a stable bond, the bond order defined as
In chemistry, molecular orbital theory (MO theory or MOT) is a method for describing the electronic structure of molecules using quantum mechanics. It was proposed early in the 20th century. The MOT explains the paramagnetic nature of O 2, which valence bond theory cannot explain.
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.
In atomic, molecular, and optical physics, a magneto-optical trap (MOT) is an apparatus which uses laser cooling and a spatially varying magnetic field to create a trap which can produce samples of cold neutral atoms.
A linear combination of atomic orbitals or LCAO is a quantum superposition of atomic orbitals and a technique for calculating molecular orbitals in quantum chemistry. [1] In quantum mechanics, electron configurations of atoms are described as wavefunctions.
Diagram of the HOMO and LUMO of a molecule. Each circle represents an electron in an orbital; when light of a high enough frequency is absorbed by an electron in the HOMO, it jumps to the LUMO. 3D model of the highest occupied molecular orbital in CO 2 3D model of the lowest unoccupied molecular orbital in CO 2
For example, the hexaaquo complexes M(H 2 O) 6 are all octahedral for M = V 3+, Mn 3+, Co 3+, Ni 2+ and Zn 2+, despite the fact that the electronic configurations of the central metal ion are d 2, d 4, d 6, d 8 and d 10 respectively.
For example, manganese (Mn) has configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5; this is abbreviated to [Ar] 4s 2 3d 5, where [Ar] denotes a core configuration identical to that of the noble gas argon. In this atom, a 3d electron has energy similar to that of a 4s electron, and much higher than that of a 3s or 3p electron.