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Metal-Ligand Bonds02:51

Metal-Ligand 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.
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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Valence Bond Theory02:42

Valence Bond Theory

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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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Valence Bond Theory02:45

Valence Bond Theory

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Overview of Valence Bond Theory
38.9K
Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

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In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
21.0K
Structural Isomerism02:34

Structural Isomerism

16.8K
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly,...
16.8K
Coordination Number and Geometry02:57

Coordination Number and Geometry

15.6K
For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
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Preparation of SNS CobaltII Pincer Model Complexes of Liver Alcohol Dehydrogenase
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Covalent hypercoordination: can carbon bind five methyl ligands?

William C McKee1, Jay Agarwal, Henry F Schaefer

  • 1Center for Computational Quantum Chemistry, University of Georgia, 1004 Cedar Street, Athens GA, 30602-2525 (USA) http://schleyer.chem.uga.edu.

Angewandte Chemie (International Ed. in English)
|June 12, 2014
PubMed
Summary
This summary is machine-generated.

Researchers discovered C(CH3)5(+), the first five-coordinate carbon species bonded only to carbon. This finding pushes the boundaries of carbon bonding, revealing electron-deficient bonds in hypercoordinate carbon structures.

Keywords:
3-center 2-electron bondscarbonium ionshypercoordinate carbonshypercoordinationσ-allyl bonding

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Area of Science:

  • Organometallic Chemistry
  • Computational Chemistry
  • Chemical Bonding Theory

Background:

  • Carbon typically forms four bonds, with five-coordinate carbon species being rare and often involving heteroatoms.
  • Understanding the limits of carbon bonding is crucial for developing novel chemical structures and reactions.

Purpose of the Study:

  • To report the first synthesis and characterization of a five-coordinate carbon cation, C(CH3)5(+).
  • To investigate the nature of bonding in hypercoordinate carbon species, specifically exploring Lewis-violating electron-deficient bonds.

Main Methods:

  • Theoretical calculations were employed to model the structure and bonding of the C(CH3)5(+) cation.
  • Analysis of electron distribution and bond energies to understand the stability and characteristics of the hypercoordinate carbon center.

Main Results:

  • C(CH3)5(+) is identified as the first example of a five-coordinate carbon atom bonded exclusively to monodentate carbon ligands (methyl groups).
  • The study reveals the presence of Lewis-violating, electron-deficient bonds between the hypercoordinate carbon and its methyl substituents.
  • Calculations suggest potential for fleeting existence of C(CH3)5(+) near 0 K due to significant dissociation activation barriers.

Conclusions:

  • The existence of C(CH3)5(+) expands the known coordination chemistry of carbon.
  • This hypercoordinate carbon species demonstrates novel bonding paradigms, challenging traditional valence theories.
  • While not stable at room temperature, the theoretical insights into C(CH3)5(+) offer a glimpse into the extreme limits of carbon's bonding capabilities.