FILLING OF ATOMIC ORBITALS- AUFBAU PRINCIPLE

Modern Periodic Table|Electronic Configuration Of First 30 Elements|Concept Of Quantum Numbers|Types Of Quantum Numbers|Electrons Filling In Orbitals Of An Atom|n+l Rule|Aufbau Principle|Hund's Rule Of Maximum Multiplicity|Question|OMR|Summary

Rules OF Filling OF Electrons || Aufbau's Principle || (n+l) rule || Hund's Rule OF Maximum Multiplicity || Pauli's Exclusion Principle || Reason OF Stability OF Half filled and Fully filled Orbitals || Electronic Configuration OF First 30 elements

Comprehension # 1 Read the following rules and answer the questions at the end of it. Electrons in various suborbits of an filled in increasing order to their energies. Pairing of electrons in various orbitals of a suborbit takes places only after each orbital is half-filled. No two electrons in an atom can have the same set of quantum number. While writing the following electronic configuration of Fe some rules have been violated : I : Aufbau's rule, II : Hund's rule III : Pauli's exclusion principle

Concept OF Degenerate Orbitals || Spin Quantum Number || Rules For writing Electronic Configuration || Aufbau Principle((n +l) Rule) || Energy Order OF all Elements OF Periodic Table

Modern Periodic Table|Quick Recap To Filling Of Electrons In Orbitals Of Shells|Aufbau Principle|General Electronic Configuration Of S Block|General Electronic Configuration Of P Block|General Electronic Configuration Of D Block|General Electronic Configuration Of F Block|OMR|Summary

The above electronic configuration deviates from (I) Hund's rule (II) Aufbau principle (III) Pauli's rule

Magnetic quantum number,spin quantum number,AUFBAU''''s rule,pauli''''s exclusion principle