Chemistry > Structure of Atom > 14.0 Electronic Configuration of Elements
Structure of Atom
1.0 Introduction
2.0 Cathode Ray Discharge Tube
3.0 Thomson Model of Atom
4.0 Rutherford Model of Atom
5.0 Atomic Number and Mass Number and It's Relation
6.0 Planck's Quantum Theory
7.0 Bohr’s Atomic Model
8.0 Dual Behaviour of Matter
9.0 Heisenberg Uncertainity Principle
10.0 Photoelectric Effect
11.0 Atomic Spectra
12.0 Quantum Mechanical Model of Atom
13.0 Quantum Number
14.0 Electronic Configuration of Elements
14.1 Aufbau (or building up) Principle
14.2 Pauli’s Exclusion Principle
14.3 Hund’s Rule
14.4 Stability of Completely Filled and Half Filled Subshells
14.2 Pauli’s Exclusion Principle
14.2 Pauli’s Exclusion Principle
14.3 Hund’s Rule
14.4 Stability of Completely Filled and Half Filled Subshells
- This principle concerns the spin of electrons present in an orbital. According to the Pauli’s principle, no two electrons can have all the four quantum numbers to be same. For example, if a given electron in an atom has the set of four quantum numbers as n =2, l=1, ${m_l}$=1 and ${m_s}$= + ½ then no other electron in the atom can have the same set of quantum numbers.
- Pauli exclusion principle can also be stated as : “Only two electrons may exist in the same orbital and these electrons must have opposite spin.”
- The maximum number of electrons in the shell with principal quantum number n is equal to $2{n^2}$.
