quantity of electrons in the valence shell
filling the orbitals with lower energy first
the filling of degenerated orbitals
quantum numbers of electrons
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Pauli Exclusion Principle: This principle states that no two electrons in an atom can have the same set of quantum numbers. In simpler terms, within an atom, no two electrons can have identical values for all their quantum numbers, including their spin. This principle underlies the structure of the periodic table and the electronic configuration of atoms.
Aufbau Principle: This principle states that electrons fill atomic orbitals of the lowest available energy levels first before occupying higher energy levels. In other words, electrons are added to an atom's electron cloud in a specific order based on their increasing energy levels. This principle helps in understanding the order in which electrons fill the shells and subshells of atoms.
Hund's Rule: Hund's Rule states that within a subshell, electrons occupy orbitals singly with parallel spins before pairing up. This means that electrons prefer to occupy empty orbitals of the same energy level (degenerate orbitals) and with the same spin before pairing up with opposite spins. This principle helps to explain the electronic configuration of atoms and the distribution of electrons within subshells.
