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Electron Configurations

Electron Configurations

Electron configurations and orbital diagrams can be determined by applying the Aufbau principle (each added electron occupies the subshell of lowest energy available), Pauli exclusion principle (no two electrons can have the same set of four quantum numbers), and Hund’s rule of maximum multiplicity (whenever possible, electrons retain unpaired spins in degenerate orbitals).
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p, 4s,...

The Aufbau Principle and Hund's Rule

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and continuing across the periods of the periodic table, we add one proton at a time to the nucleus and one electron to the proper subshell until we have described the electron configurations of all the elements. This procedure is called the aufbau principle, from the German word aufbau (“to build up”). Each added electron occupies the subshell of...

The Pauli Exclusion Principle

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that contains three pieces of information:

The Quantum-Mechanical Model of an Atom

The Quantum-Mechanical Model of an Atom

Shortly after de Broglie published his ideas that the electron in a hydrogen atom could be better thought of as being a circular standing wave instead of a particle moving in quantized circular orbits, Erwin Schrödinger extended de Broglie’s work by deriving what is now known as the Schrödinger equation. When Schrödinger applied his equation to hydrogen-like atoms, he was able to reproduce Bohr’s expression for the energy and, thus, the Rydberg formula governing hydrogen spectra. Schrödinger...

Electron Configuration of Multielectron Atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...

Electron Orbital Model

Electron Orbital Model

Orbitals are the areas outside of the atomic nucleus where electrons are most likely to reside. They are characterized by different energy levels, shapes, and three-dimensional orientations. The location of electrons is described most generally by a shell or principal energy level, then by a subshell within each shell, and finally, by individual orbitals found within the subshells.
The first shell is closest to the nucleus, and it has only one subshell with a single spherical orbital called the...

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Related Experiment Video

Updated: May 18, 2026

Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−

Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F⁻

Published on: July 27, 2018

Electron quantum optics: partitioning electrons one by one.

E Bocquillon¹, F D Parmentier, C Grenier

¹Laboratoire Pierre Aigrain, Ecole Normale Supérieure, CNRS (UMR 8551), Université P. et M. Curie, 24 rue Lhomond, 75231 Paris Cedex 05, France.

Physical Review Letters

|September 26, 2012

Summary

This summary is machine-generated.

Researchers performed a quantum optics experiment using single electrons. They demonstrated a method to directly count electron-hole pairs and probe energy distributions of emitted electronic excitations.

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Last Updated: May 18, 2026

Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−

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Published on: July 27, 2018

Excitonic Hamiltonians for Calculating Optical Absorption Spectra and Optoelectronic Properties of Molecular Aggregates and Solids

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Area of Science:

Quantum optics
Condensed matter physics
Quantum electronics

Background:

The Hanbury Brown-Twiss (HBT) experiment in quantum optics reveals particle statistics.
Implementing analogous experiments with electrons requires precise control over single charge carriers.
Understanding electron correlations is crucial for quantum information processing.

Purpose of the Study:

To realize a quantum optics-like HBT experiment using single electronic excitations.
To demonstrate a method for directly counting elementary excitations (electron-hole pairs) at the single-charge level.
To probe the energy distribution of emitted electronic wave packets.

Main Methods:

Partitioning single elementary electronic excitations on an electronic beam splitter.
Measuring output current correlations in an HBT geometry.
Utilizing antibunching of low-energy excitations to suppress thermal excitation contributions.

Main Results:

Successful realization of an electronic HBT experiment with an on-demand emitter.
Direct counting of single electron-hole pairs generated by the emitter.
Observation of antibunching suppressing partition noise from thermal excitations.
Demonstration of probing energy distribution of emitted wave packets.

Conclusions:

The electronic HBT experiment provides a powerful tool for single-charge detection.
The method allows for precise characterization of quantum emitters.
This technique opens new avenues for studying quantum transport phenomena.