Video Experimental Relacionado
Updated: Jun 26, 2026
10:52
Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex
Published on: July 27, 2022
Reducción de dos electrones de un complejo Rh-Mo-Rh ditionato para formar un estado fundamental triple asociado con
Satoshi Muratsugu1, Keitaro Sodeyama, Fusao Kitamura
1Department of Chemistry, School of Science, The University of Tokyo, 7-3-1, Hongo, Bunkyo-Ku, Tokyo, 113-0033, Japan.
Journal of the American Chemical Society
|January 14, 2009
Resumen
Los investigadores sintetizaron un nuevo complejo trinuclear heterométrico que exhibe reducción reversible de dos electrones. Este proceso redox implica cambios estructurales y de estado de espín, ofreciendo información sobre la química del metalladitioleno.
Área de la Ciencia:
- Química organometálica Química orgánica de los metales.
- Química Inorgánica La Química Inorgánica es la química inorgánica.
- Ciencia de los materiales Ciencia de los materiales.
Sus antecedentes:
- Los complejos metálicos multinucleares ofrecen propiedades electrónicas y estructurales únicas.
- Los complejos de metalla-diotioleno son de interés por su actividad redox.
Objetivo del estudio:
- Síntesis y caracterización de un nuevo complejo trinuclear heterométrico de ditiolatos y puentes.
- Para investigar el comportamiento redox y los cambios de estado estructural / espín asociados.
Principales métodos:
- Síntesis del complejo trinuclear heterométrico.
- Estudios electroquímicos para determinar los potenciales redox.
- Cálculos de la Teoría Funcional de Densidad (DFT) para el análisis estructural y electrónico.
Principales resultados:
- Se sintetizó un complejo trinuclear heterométrico con puente de ditiolato, [{(eta(5) -C(5) Me(5)) Rh(S(2) C(6) H(4)) }(2) Mo(CO) }(2) ] (1), fue sintetizado.
- El complejo 1 mostró reducción reversible de dos electrones en un solo paso con potencial de inversión.
- El proceso de redox implicó cambios reversibles en la coordinación de CO y el estado de espín (Rh{III}-Mo{0) -Rh{III} a Rh{II}-Mo{0) -Rh{II}).
Conclusiones:
- Este estudio presenta el primer ejemplo de un complejo de metalladitioleno multinuclear con un proceso redox multielectrónico reversible.
- Los cambios estructurales y de estado de espín inducidos por redox observados fueron confirmados por cálculos de DFT.
- Este trabajo proporciona una base para el diseño de complejos con propiedades electrónicas sintonizables.
Videos de Conceptos Relacionados
02:42Valence 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...
02:57Coordination 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.
03:02Colors and Magnetism
Color in Coordination Complexes
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.
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.
02:58Crystal Field Theory - Octahedral Complexes
Crystal Field Theory
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...
To explain the observed behavior of transition metal complexes (such as colors), a model involving electrostatic interactions between the electrons from the ligands and the electrons in the unhybridized d orbitals of the central metal atom has been developed. This electrostatic model is crystal field theory (CFT). It helps to understand, interpret, and predict the colors, magnetic behavior, and some structures of coordination compounds of transition metals.
CFT focuses on...
01:43Electron Transport Chain: Complex III and IV
During the electron transport chain, electrons from NADH and FADH2 are first transferred to complexes I and II, respectively. These two complexes then transfer the electrons to ubiquinol, which carries them further to complex III. Complex III passes the electrons across the intermembrane space to Cyt c, which carries them further to complex IV. Complex IV donates electrons to oxygen and reduces it to water. As electrons pass through complexes I, III, and IV, the energy released aids the pumping...
02:51Metal-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...
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...