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Bonding in Metals02:32

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Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. 
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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...
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Chemical bonding theories were pioneered by American chemist Gilbert N. Lewis. He developed a model called the Lewis model to explain the type and formation of different bonds. Chemical bonding is central to chemistry; it explains how atoms or ions bond together to form molecules. It explains why some bonds are strong and others are weak, or why one carbon bonds with two oxygens and not three; why water is H2O and not H4O. 
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Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
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The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
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Understanding metal bonding.

Volker Heine1, Siyu Chen1

  • 1TCM Group, Cavendish Laboratory, JJ Thomson Ave, Cambridge CB3 0HE, United Kingdom.

Journal of Physics. Condensed Matter : an Institute of Physics Journal
|May 24, 2024
PubMed
Summary
This summary is machine-generated.

This study introduces a simple formula based on the Moment Method to explain various metallic bonding effects. The formula, dependent on coordination number, helps understand properties like malleability and surface catalysis in solids.

Keywords:
electronic structuremalleablemetallic bondingmetals

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Area of Science:

  • Solid-state physics
  • Materials science
  • Theoretical chemistry

Background:

  • Metallic bonding governs many material properties.
  • Understanding local electronic structure is key to predicting material behavior.
  • Previous models often lack a unified approach to diverse metallic phenomena.

Purpose of the Study:

  • To present a simple theoretical formula for metallic bonding.
  • To demonstrate the formula's applicability to a wide range of material properties.
  • To provide a foundational understanding of local electronic structure in solids.

Main Methods:

  • Utilizing the initial steps of the Moment Method for electronic structure calculations.
  • Developing a formula based on the square root of the total coordination number (C).
  • Analyzing the 'saturation' curvature of the square root function.

Main Results:

  • The formula successfully explains diverse metallic properties including malleability, crystal structure, phase transitions, and vacancy formation energy.
  • Applications extend to surface catalysis, surface reconstruction, and graphite stability.
  • The model offers insights into the benzene molecule as a metallic ring.

Conclusions:

  • A single, simple formula derived from the Moment Method can elucidate numerous metallic bonding effects.
  • The coordination number and the square root function's curvature are critical factors.
  • This approach offers a unified perspective on the behavior of solids and atomic metallic rings.