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Related Concept Videos

Electron Configurations02:46

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,...
Electron Configuration of Multielectron Atoms03:26

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...
The Aufbau Principle and Hund's Rule03:02

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...
Electronic Structure of Atoms02:28

Electronic Structure of Atoms


An atom comprises protons and neutrons, which are contained inside the dense, central core called the nucleus, with electrons present around the nucleus. Taking into account the wave–particle duality of electrons and the uncertainty in position around the nucleus, quantum mechanics provides a more accurate model for the atomic structure. It describes atomic orbitals as the regions around the nucleus where electrons of discrete energy exist, characterized by four quantum numbers:  n, l, ml, and...
The Pauli Exclusion Principle03:06

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:
Electron Orbital Model01:18

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

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Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−
06:53

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Published on: July 27, 2018

Cu 4s → 4p atomic like excitations in the Ne matrix.

Yasuyo Hatano1, Hiroshi Tatewaki, Shigeyoshi Yamamoto

  • 1School of Information Sciences and Technology, Chukyo University, Toyota 470-0393, Japan.

Physical Chemistry Chemical Physics : PCCP
|April 26, 2013
PubMed
Summary

Copper atom excited states in neon matrices are clarified. A large vacancy with residual neon atoms is crucial for explaining observed spectra, revealing complex electronic structures and interactions.

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Area of Science:

  • Atomic physics
  • Solid-state chemistry
  • Quantum mechanics

Background:

  • Experimental studies of copper (Cu) atom excited states in neon (Ne) matrices suggest a 4p(1) electronic configuration.
  • The origins of triplet and quartet states remain unclear, with trapping site variations proposed to explain spectral complexity.

Purpose of the Study:

  • To clarify the electronic structures of ground and excited states of Cu atoms in Ne matrices.
  • To elucidate the role of matrix environment and interactions in observed spectral features.

Main Methods:

  • Ab initio molecular orbital calculations using a cluster model.
  • Simulations focused on a face-centered cubic (fcc)-like Ne cluster (66 atoms) with a central Cu atom.

Main Results:

  • A large vacancy with residual Ne atoms in the first coordination shell is essential for reproducing experimental spectra.
  • The presence of residual Ne atoms explains the observation of more than three excited states.
  • Both electron-electron (including crystal field) and spin-orbit interactions are significant.

Conclusions:

  • The study clarifies the electronic structure of Cu in Ne matrices, identifying a specific vacancy model.
  • The findings reconcile theoretical calculations with experimental spectral data, highlighting the importance of matrix interactions.