```Hund’s Rule of Maximum Multiplicity:
This rule deals with the filling of electrons in the equal energy (degenerate) orbitals of the same sub shell (p, d and f). According to this rule, “Electron pairing in p, d and f orbitals cannot occur until each orbital of a given sub shell contains one electron each or is singly occupied”.
This is due to the fact that electrons being identical in charge, repel each other when present in the same orbital. This repulsion can, however, be minimized if two electrons move as far apart as possible by occupying different degenerate orbitals. All the electrons in a degenerate set of orbitals will have same spin.
Electronic Configuration of Elements: Electronic configuration is the distribution of electrons into different shells, subshells and orbitals of an atom. Keeping in view the above mentioned rules, electronic configuration of any orbital can be simply represented by the notation]

Alternatively:
Orbital can be represented by a box and an electron with its direction of spin by arrow. To write the electronic configuration, just we need to know (i) the atomic number (ii) the order in which orbitals are to be filled (iii) maximum number of electrons in a shell, sub–shell or orbital.

Each orbital can accommodate two electrons

The number of electrons to be accommodated in a subshell is 2 x numbers of degenerate orbitals.

Subshell

Maximum number of electrons

s

2

p

6

d

10

f

14

The maximum number of electrons in each shell (K, L, M, N…) is given by 2n2where n is the principal quantum number.

The maximum number of orbitals in a shell is given by n2 where n is the principal quantum number.

Importance of Knowing the Electronic Configuration:
The chemical properties of an element are dependent on the relative arrangement of its electrons.```
Related Resources
Problems with Solutions

Problems with Solutions True and False Problem:...

Calculation of velocity of Electron

Calculation of Velocity: We know that mvr =...

Quantum Numbers

QUANTUM NUMBERS An atom contains large number of...

Atomic Models

ATOMIC MODELS We know the fundamental particles of...

Photoelectric Effect

PHOTOELECTRIC EFFECT Sir J.J. Thomson, observed...

Quantum Mechanical Model of Atom

QUANTUM MECHANICAL MODEL OF ATOM The atomic model...

Discovery of Electron

DISCOVERY OF ELECTRON: CATHODE RAYS During the...

Discovery of Neutron

DISCOVERY OF NEUTRON After the discovery of...

Fundamental Particles

Shapes and Size of Orbitals

Pauli’s Exclusion Principle: According to...

Relation-Kinetic Energy and Wavelength

Relation between Kinetic Energy and Wavelength:...

Atomic Spectrum

ATOMIC SPECTRUM If the atom gains energy the...

Discovery of Proton

DISCOVERY OF PROTON: POSITIVE RAYS OR CANAL RAYS...

Atomic Structure Terms

ATOMIC TERM Nuclide: Various species of atoms in...

Solved Questions of Atomic Structure Part I

Solved Questions of Atomic Structure Part I...

Limitations of Bohrs Theory

Merits of Bohr’s Theory: * The experimental...

Radius and Energy Levels of Hydrogen Atom

Radius and Energy Levels of Hydrogen Atom:...

Dual Character

Dual Character DUAL CHARACTER (PARTICLE AND WAVE...

Characteristics of Wave

Characteristics of Wave SOME IMPORTANT...

A-Scattering Experiment

A-Scattering Experiment Conclusions of...

Heisenbergs Uncertainty Principle

HEISENBERG’S UNCERTAINTY PRINCIPLE All...

Bohrs Atomic Model

BOHR’S ATOMIC MODEL Bohr developed a model...

Calculation of Energy of Electron

Calculation of Energy of an Electron: The total...

Hydrogen Atom

HYDROGEN ATOM If an electric discharge is passed...

Objective Questions of Atomic Structure

Objective Questions of Atomic Structure Problem:...

Derivation of Angular Momentum from de Broglie Equation

Derivation of Angular Momentum from de Broglie...

Plancks Quantum Theory

PLANCK’S QUANTUM THEORY When a black body is...

Rules for Filling of Electrons in Various Orbitals

RULES FOR FILLING OF ELECTRONS IN VARIOUS ORBITALS...