rules in filling up orbitals

Rules for Filling Molecular Orbitals - The following rules are followed for filling up molecular orbitals with electrons in order to write molecular configurations: 1. The molecular orbital having the lowest energy is filled..

Each molecular orbital can accommodate maximum of two electrons having opposite spins. This is in accordance with Pauli's exclusion principl..

Electron pairing will not take place in orbitals of same energy (same sub-shell) until each orbital is first singly filled with parallel spi..

Hund's Rule of Maximum Multiplicity - According to this rule, electron pairing will not take place in orbitals of same energy (same sub-shell) until each orbital is first singly filled with parallel spin. In other words in a set of orbitals..

Molecular orbital theory was proposed by F. Hund and R.S. Mulliken in 1932. The basic idea of molecular orbital theory is that atomic orbitals of individual atoms combine to form molecular orbitals. The electrons in molecules are present in the molecula..

Molecular Orbital Theory - Molecular orbital theory was proposed by F. Hund and R.S. Mulliken in 1932. The basic idea of molecular orbital theory is that atomic orbitals of individual atoms combine to form molecular orbitals. The electrons in molecu..

The configurations in which all the orbitals of the same subshell are half-filled or completely filled involves symmetrical distribution of electrons. Symmetry of electronic distribution leads to extra stability. Example: ..

Covalent bonds are formed by the overlap of atomic orbitals. As orbitals have different shapes, it is difficult to represent the actual shape of the orbitals on the paper. Hence a pictorial notation is adopted with the following rules: An orbital..

Two half filled 'p' orbitals overlap along the line joining the two nuclei. This is also called as head on, end on or end to end linear overlap. p-p sideways overlap Two half filled 'p' orbitals overlap along the line perpendicular to the nuclear axis. T..

The principle states that the electron in an atom are so arranged that they occupy orbitals in the order of their increasing energy. Since the energy of a 'n' orbital in the absence of any magnetic field depends on the 'n' and 'l' quantum number values, the order of fillin..