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Related Concept Videos

Metallic Solids02:37

Metallic Solids

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Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
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Ionic Crystal Structures02:42

Ionic Crystal Structures

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Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
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Valence Bond Theory02:42

Valence Bond Theory

9.9K
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...
9.9K
Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

Crystal Field Theory - Tetrahedral and Square Planar Complexes

45.4K
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,...
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Crystal Field Theory - Octahedral Complexes02:58

Crystal Field Theory - Octahedral Complexes

28.5K
Crystal Field Theory
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...
28.5K
Network Covalent Solids02:18

Network Covalent Solids

15.1K
Network covalent solids contain a three-dimensional network of covalently bonded atoms as found in the crystal structures of nonmetals like diamond, graphite, silicon, and some covalent compounds, such as silicon dioxide (sand) and silicon carbide (carborundum, the abrasive on sandpaper). Many minerals have networks of covalent bonds.
To break or to melt a covalent network solid, covalent bonds must be broken. Because covalent bonds are relatively strong, covalent network solids are typically...
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Visualizing Uniaxial-strain Manipulation of Antiferromagnetic Domains in Fe1+YTe Using a Spin-polarized Scanning Tunneling Microscope
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Atomic Stripe Formation in Infinite-Layer Cuprates.

Yoshiharu Krockenberger1, Ai Ikeda1, Hideki Yamamoto1

  • 1NTT Basic Research Laboratories, NTT Corporation, 3-1 Morinosato-Wakamiya, Atsugi, Kanagawa 243-0198, Japan.

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|September 9, 2021
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Summary
This summary is machine-generated.

High-temperature superconductivity in cuprates emerges when copper-oxygen bonds reach minimal energy. Atomic stripes form in CaCuO2 to maintain this state, unlike in SrCuO2, revealing insights into superconductivity mechanisms.

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Area of Science:

  • Materials Science
  • Condensed Matter Physics
  • Solid-State Chemistry

Background:

  • High-temperature superconductivity is observed in cuprate materials.
  • Superconductivity in cuprates is linked to the copper-oxygen (CuO2) planes.
  • The Jahn-Teller effect can disrupt the formation of these crucial CuO2 planes.

Purpose of the Study:

  • To investigate the atomic structure and stability of CuO2 planes in infinite-layer cuprates.
  • To understand the role of copper-oxygen bond length in maintaining minimal energy states.
  • To explore the formation of atomic stripes as a mechanism for stabilizing CuO2 planes.

Main Methods:

  • Synthesis of single-crystalline films of CaCuO2 and SrCuO2 using molecular beam epitaxy.
  • In-plane scanning transmission electron microscopy (STEM) mapping.
  • Analysis of atomic configurations and bond lengths within the CuO2 planes.

Main Results:

  • CaCuO2, with shorter Cu-O bonds, exhibits distinguished atomic stripes to maintain minimal energy.
  • SrCuO2, with longer Cu-O bonds, does not form atomic stripes.
  • Minimal energy states in CuO2 planes persist despite variations up to 10% in bond length.

Conclusions:

  • Atomic stripe formation is a key mechanism for stabilizing minimal energy CuO2 planes in certain cuprates.
  • The Cu-O bond length plays a critical role in the emergence of atomic stripes and superconductivity.
  • Charge reservoir layers are vital for maintaining infinite CuO2 planes and enabling superconductivity in cuprates.