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12 Σεπ 2022 · Unlike valence bond theory, which uses hybrid orbitals that are assigned to one specific atom, MO theory uses the combination of atomic orbitals to yield molecular orbitals that are delocalized over the entire molecule rather than being localized on its constituent atoms.
14 Αυγ 2020 · Oxygen (atomic number 8) has a pair of electrons in any one of the 2 p orbitals (the electrons have opposite spins) and a single electron in each of the other two. Fluorine (atomic number 9) has only one 2 p orbital containing an unpaired electron.
Figure \(\PageIndex{3}\): Electron configuration of nitrogen and oxygen atoms. The way electrons move from one orbital to the next is very similar to walking up a flight of stairs. When walking up stairs, you place one foot on the first stair and then another foot on the second stair.
Outline the basic quantum-mechanical approach to deriving molecular orbitals from atomic orbitals. Describe traits of bonding and anti-bonding molecular orbitals. Calculate bond orders based on molecular electron configurations. Write molecular electron configurations for first- and second-row diatomic molecules.
Shells, subshells, and orbitals. Introduction to electron configurations. The Aufbau principle. Valence electrons. Electron configurations of ions. Electron configurations of the 3d transition metals. Atomic structure and electron configuration.
Molecular orbital theory (MO theory) provides an explanation of chemical bonding that accounts for the paramagnetism of the oxygen molecule.
The most natural basis functions are the atomic orbitals of the individual Hydrogen atoms. If the bond length is very large, the system will approach the limit of two non-interacting Hydrogen atoms, in which case the electronic wavefunction can be well approximated by a product of an orbital on atom “A” and an orbital on atom “B” and
