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Electron configuration specifies how electrons are arranged in orbitals (or subshells) and is linked to the energy levels of an atom or molecule.
Electron configuration is the distribution of electrons of an atom (or molecule) among atomic or molecular orbitals. It is commonly written using subshell labels (s, p, d, f) and superscripts that indicate how many electrons occupy each subshell; for example, neon is written as 1s² 2s² 2p⁶. Each electron configuration corresponds to a set of energy levels, and transitions between configurations can occur when electrons absorb or emit energy (photons). The purpose of electron configuration is to provide a structured way to understand and predict chemical and physical behavior. Knowledge of electron configurations helps explain the organization of the periodic table, the nature of chemical bonding and molecular structure, and the properties of compounds. In addition, it supports interpretation of atomic spectra (often using term symbols) and, in bulk materials, helps explain behaviors relevant to lasers and semiconductors. Although simplified filling rules like the Aufbau principle are useful for ground states, the underlying quantum-mechanical reality is more complex because electron energies depend on interactions with other electrons.
Electron configuration specifies how electrons are arranged in orbitals (or subshells) and is linked to the energy levels of an atom or molecule.
Electron configurations are essential for explaining periodic trends, chemical bonding, molecular geometry, and the interpretation of atomic spectra.
Simplified rules (e.g., Aufbau/Madelung) approximate the order of orbital filling for ground states, but real multi-electron systems involve electron-electron interactions that make exact one-configuration energy assignments impossible.
The distribution of electrons of an atom or molecule among atomic or molecular orbitals.
A set of states within a shell defined by a common azimuthal quantum number l, labeled by s (l=0), p (l=1), d (l=2), and f (l=3).
The set of allowed electron states that share the same principal quantum number n.
The electron configuration corresponding to the lowest electronic energy of an atom.
Any electron configuration with higher energy than the ground state, reached by absorbing energy.
A rule stating that electrons fill orbitals in order of increasing energy, with a maximum of two electrons per orbital.
The filling order rule for subshells: subshells are filled by increasing n+l, and if tied, by increasing n.
An abbreviated electron configuration that replaces the core electrons with the symbol of the preceding noble gas, e.g., [Ne] 3s² 3p³.
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