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Related Concept Videos

Bonding in Metals02:32

Bonding in Metals

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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Covalent Bonds

When two atoms share electrons to complete their valence shells they create a covalent bond. An atom’s electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.A Covalent...
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Overview
When two atoms share electrons to complete their valence shells, they create a covalent bond. An atom's electronegativity—the force with which shared electrons are pulled towards an atom—determines how the electrons are shared. Molecules formed with covalent bonds can be either polar or nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds; the electrons are shared equally. Atoms with different electronegativities share electrons unequally, creating polar bonds.
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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.
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Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual attraction of atoms for a “shared” pair of electrons.

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Making a robust carbon-cobalt(III) bond.

Erik Larsen1, Anders Østergaard Madsen, Pauli Kofod

  • 1IGV, Faculty of Life Sciences, University of Copenhagen, Thorvaldsensvej 40, DK-1871 Frederiksberg, Denmark. Erik@Life.ku.dk

Inorganic Chemistry
|July 3, 2009
PubMed
Summary
This summary is machine-generated.

This study details the synthesis and characterization of a novel cobalt(III) complex with a carbon-cobalt bond, revealing its unique stability and reactivity. The research explores the electronic structure and bonding in cobalt complexes, offering insights into ligand transformations.

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Area of Science:

  • Coordination Chemistry
  • Organometallic Chemistry
  • Inorganic Chemistry

Background:

  • The study focuses on cobalt(III) complexes, specifically those featuring a carbon-cobalt bond.
  • The ligand (1,4,7-triazacyclononane)(1,6-diamino-3-thia-4-hexanido)cobalt(III) dication, denoted as [Co(tacn)(C-aeaps)](2+), is a key component.
  • Understanding the nature and reactivity of the carbon-cobalt bond is crucial in coordination chemistry.

Purpose of the Study:

  • To synthesize and characterize the S-methyl thionium derivative of the [Co(tacn)(C-aeaps)](2+) complex.
  • To elucidate the structural properties, including the carbon-cobalt bond length and trans-elongating effect, of the new derivative.
  • To investigate the reactivity and stability of the cobalt(III) complex in acidic conditions and with iodide.

Main Methods:

  • Reaction of [Co(tacn)(C-aeaps)](2+) with iodomethane to form the S-methyl thionium derivative.
  • X-ray diffraction techniques at 122 K to determine the crystal structure of [Co(tacn)(C-aeaps-SCH(3))]Br(3) x 3 H(2)O.
  • Comparison of experimentally obtained cobalt(III) distances with Density Functional Theory (DFT) computations.

Main Results:

  • The crystal structure of the S-methyl thionium derivative was determined, confirming its formation.
  • The carbon-cobalt bond length in the derivative (2.001(4) Å) is shorter than in the precursor (2.026(3) Å), with a less pronounced trans-elongating effect.
  • The [Co(tacn)(C-aeaps-SCH(3))]3+ ion exhibits remarkable robustness in strongly acidic aqueous solutions, though the methyl group can be removed by excess iodide.

Conclusions:

  • The study provides detailed structural and reactivity data for a novel S-methylated cobalt(III) complex.
  • DFT calculations show varying agreement with experimental data depending on the chosen functionals, highlighting the complexity of modeling these systems.
  • The participation of a sulfur 3p orbital in bonding to cobalt(III) is significant for understanding the interconversion between carbon- and sulfur-bound aeaps ligands.