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.


Comments

Author: Dr. Kapileshwar Choudhary09 Apr 2011 Member Level: Gold   Points : 1

Dear Vikas

you should also remember half/full filled orbital is more stable than partial filled.
K.Choudhary

Author: Nilesh29 Jul 2017 Member Level: Gold   Points : 3

One other thing to remember is that not all the atoms follow Aufbau rule. There are many exceptions. Ex:- The valence shell configuration of copper according to Aufbau rule should have been 4s-2, 3d-4 but actually it is 4s-1, 3d-5. This is because half shell configuration of 3d-5 provides extra stability to the atom. Similarly there are many other atoms which don't follow this rule. Almost all the f block elements show deviation from this rule.



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