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Related Concept Videos

Valence Bond Theory02:42

Valence Bond Theory

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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Structural Isomerism

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, SCN− can be...
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Metal-Ligand Bonds

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 Number and Geometry

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.
Coordination Compounds and Nomenclature02:54

Coordination Compounds and Nomenclature

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...
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Colors and Magnetism

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When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human eye.

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Three-coordinate and four-coordinate cobalt hydride complexes that react with dinitrogen.

Keying Ding1, William W Brennessel, Patrick L Holland

  • 1Department of Chemistry, University of Rochester, Rochester, New York 14618, USA.

Journal of the American Chemical Society
|July 23, 2009
PubMed
Summary

Researchers synthesized novel cobalt hydride complexes using bulky beta-diketiminate ligands. These complexes react with nitrogen gas (N(2)) to form new dinuclear nitrogen complexes, releasing hydrogen gas (H(2)).

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Area of Science:

  • Organometallic Chemistry
  • Coordination Chemistry
  • Inorganic Chemistry

Background:

  • Bulky beta-diketiminate ligands are crucial for stabilizing reactive metal centers.
  • Cobalt hydride complexes are of interest for their catalytic potential and unique reactivity.
  • Understanding the coordination environment of transition metals is key to designing new complexes.

Purpose of the Study:

  • To synthesize and characterize novel cobalt hydride complexes supported by bulky beta-diketiminate ligands.
  • To investigate the reactivity of these cobalt hydride complexes with nitrogen gas (N(2)).
  • To explore the formation of dinuclear nitrogen complexes and hydrogen release.

Main Methods:

  • Synthesis of cobalt hydride complexes via reaction of LCoCl with potassium triethylborohydride.
  • Crystallographic characterization of the resulting dinuclear cobalt hydride complexes.
  • Reaction of the cobalt hydride complexes with nitrogen gas at room temperature.

Main Results:

  • Formation of two novel cobalt hydride complexes, [LCo(mu-H)](2) (1) and K(2)[LCoH](2) (2), depending on reaction conditions.
  • Compound 2 represents the first crystallographically characterized three-coordinate transition metal hydride complex.
  • Both complexes react with N(2) to yield dinuclear N(2) complexes with the evolution of H(2).

Conclusions:

  • Bulky beta-diketiminate ligands effectively support the formation of unique cobalt hydride species.
  • The novel cobalt hydride complexes exhibit reactivity towards N(2), leading to the formation of dinuclear nitrogen complexes.
  • This work expands the understanding of transition metal hydride reactivity and nitrogen fixation chemistry.