How to fill the orbital with electron
This article would enable you to know that what are the different processes of filling Electrons in the Orbitals. I think it will help those people who generally take Interests in Inorganic Chemistry.
Rules which govern the filling of Electrons in Different Orbitals
1) The first principal is Pauli's Exclusion Principle which was proposed by Wolfgang Pauli in year 1925.This principal explains that two electrons in an atom can never have identical sets of four quantum numbers. This implies that each electron possesses an unique set of four quantum numbers.
This is possible only when atleast one quantum number is different for any two electrons. Two electrons can have atleast three quantum numbers but the fourth one is always different.
2) Second rule is known as Aufbau's Principle. According to this rule, in the ground state of an atom, the electron enter into the available orbitals in the increasing order of energies and fill up the orbitals of lower energy first.
The increasing order of energies of various orbitals is:-
1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s
Aufbau Principle indicates that 1s orbital is filled first of all because it is the orbital of lowest energy. After filling 1s orbital, electrons go in succession to 2s, 2p, 3s, 3p orbitals.
3) This is last rule of filling electrons in the orbitals called Hund's Rule of Maximum multiplicity.
Its tells that while filling different orbitals of a subshell, the electrons prefer to remain unpaired as far as possible and possess the same direction of spin. Pairing of electrons takes place only when all the orbitals of a subshell are singly occupied.
Dear Vikas
you should also remember half/full filled orbital is more stable than partial filled.
K.Choudhary