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Core Concepts of Electronic Configuration

Shells and Subshells: Electrons occupy principal energy levels (shells 1, 2, 3...) which are further divided into subshells labeled s, p, d, and f.

Orbital Capacity: Each subshell contains a specific number of orbitals, with each orbital holding a maximum of two electrons.

s subshell: 1 orbital (2 electrons max).

p subshell: 3 orbitals (6 electrons max).

d subshell: 5 orbitals (10 electrons max).

f subshell: 7 orbitals (14 electrons max).

Governing Principles:

Aufbau Principle: Electrons fill lower-energy orbitals first (e.g., 1s before 2s).

Pauli Exclusion Principle: No two electrons in an atom can have the same set of four quantum numbers.

Hund’s Rule: Electrons will occupy empty orbitals of the same subshell individually before pairing up. 

Notation Methods 

Standard Notation: Lists every occupied subshell with a superscript indicating the number of electrons (e.g., Oxygen:



1s22s22p41 s squared 2 s squared 2 p to the fourth power


).

Noble Gas (Condensed) Notation: Uses the symbol of the previous noble gas in brackets to represent the "core" electrons, followed by the remaining valence electrons (e.g., Calcium: [Ar]



4s24 s squared

4𝑠2

).