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Related Concept Videos

Bonding in Metals02:32

Bonding in Metals

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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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The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
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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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Overview of Valence Bond Theory
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Organometallic compounds are compounds that contain a carbon–metal bond. Carbon belongs to an organyl group like alkyl, aryl, allyl, or benzyl groups. The metal can be from Group I or Group II of the periodic table, a transition metal, or a semimetal.
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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Related Experiment Video

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Synthesis and Characterization of Fe-doped Aluminosilicate Nanotubes with Enhanced Electron Conductive Properties
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Multiple Bonding Between Group 3 Metals and Fe(CO)3.

Jia-Qi Wang1, Chaoxian Chi2, Han-Shi Hu1

  • 1Department of Chemistry & Key Laboratory of Organic Optoelectronics and Molecular Engineering of Ministry of Education, Tsinghua University, Beijing, 100084, China.

Angewandte Chemie (International Ed. in English)
|November 27, 2019
PubMed
Summary

New Group 3 metal/iron carbonyl anion complexes exhibit unique metal-metal bonding. Quantum-chemical calculations and spectroscopy reveal complex bonding interactions, including covalent and dative bonds.

Keywords:
group-3 metalsinfrared photodissociation spectroscopyironmetal-metal bondsquantum-chemical studies

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Area of Science:

  • Inorganic Chemistry
  • Organometallic Chemistry
  • Quantum Chemistry

Background:

  • Heteronuclear metal carbonyl anions are crucial in understanding chemical bonding.
  • Group 3 metals (Sc, Y, La) and iron carbonyls offer a unique system for exploring novel bonding motifs.

Purpose of the Study:

  • To synthesize and characterize novel Group 3 metal/iron carbonyl anion complexes.
  • To elucidate the bonding interactions and electronic structure of these complexes using experimental and computational methods.

Main Methods:

  • Gas-phase preparation of ScFe(CO)3-, YFe(CO)3-, and LaFe(CO)3- anion complexes.
  • Mass-selective infrared (IR) photodissociation spectroscopy.
  • Quantum-chemical calculations.

Main Results:

  • All three complexes adopt a C3v equilibrium geometry with metal-metal bonding.
  • A closed-shell singlet electronic ground state was determined for all complexes.
  • Detailed bonding analyses revealed multiple interactions, including a covalent sigma bond, two dative pi bonds from Fe to the Group 3 metal, and multicenter covalent bonding.

Conclusions:

  • The studied complexes display intricate bonding between Group 3 metals and the Fe(CO)3- fragment.
  • The findings contribute to a deeper understanding of bonding in heteronuclear metal carbonyls.