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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,...
Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

Crystal Field Theory - Tetrahedral and Square Planar Complexes

Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
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...
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...
Valence Bond Theory02:42

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
Exceptions to the Octet Rule02:55

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:

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Electronic structure of EuFe2As2.

Ganesh Adhikary1, Nishaina Sahadev, Deepnarayan Biswas

  • 1Department of Condensed Matter Physics and Materials Science, Tata Institute of Fundamental Research, Homi Bhabha Road, Colaba, Mumbai-400 005, India.

Journal of Physics. Condensed Matter : an Institute of Physics Journal
|May 10, 2013
PubMed
Summary
This summary is machine-generated.

Antiferromagnetism in EuFe2As2 survives superconductivity, influencing electronic structure and conduction electrons below 20 K. This study reveals spin density wave transitions and peak-dip features in this unique pnictide material.

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Area of Science:

  • Condensed Matter Physics
  • Materials Science
  • Solid State Chemistry

Background:

  • EuFe2As2 is a unique pnictide material exhibiting both antiferromagnetism and superconductivity.
  • The interplay between magnetic order and superconductivity is crucial for understanding exotic electronic phases.

Purpose of the Study:

  • To investigate the temperature evolution of the electronic structure of EuFe2As2.
  • To understand how antiferromagnetism influences the superconducting phase in this material.

Main Methods:

  • High-resolution photoemission spectroscopy was employed to study the electronic structure.
  • Analysis focused on temperature-dependent changes and spectral features.

Main Results:

  • Peak-dip features with significant p orbital character were observed.
  • Spin density wave transition induced band folding was identified in the electronic structure.
  • Significant spectral weight redistribution below 20 K indicated the influence of antiferromagnetic order on conduction electrons.

Conclusions:

  • Antiferromagnetism in the Eu layer persists within the superconducting phase of EuFe2As2.
  • The electronic structure is significantly affected by magnetic ordering, particularly below 20 K.