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Related Concept Videos

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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Complexation Equilibria: The Chelate Effect01:19

Complexation Equilibria: The Chelate Effect

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In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
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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...
27.6K
Structural Isomerism02:34

Structural Isomerism

22.3K
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...
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Coordination Number and Geometry02:57

Coordination Number and Geometry

19.4K
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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Related Experiment Video

Updated: Mar 8, 2026

Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex
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Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex

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Uranium rhodium bonding in heterometallic complexes.

J A Hlina1, J A L Wells, J R Pankhurst

  • 1EaStCHEM School of Chemistry, University of Edinburgh, Joseph Black Building, The King's Buildings, Edinburgh EH9 3FJ, UK. polly.arnold@ed.ac.uk.

Dalton Transactions (Cambridge, England : 2003)
|February 4, 2017
PubMed
Summary

New uranium-rhodium complexes exhibit exceptionally short metal-metal bonds, among the shortest reported for f-element and transition metal interactions. However, these strong solid-state interactions weaken significantly in solution.

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Area of Science:

  • Organometallic Chemistry
  • Inorganic Chemistry
  • Materials Science

Background:

  • Synthesis and characterization of heterometallic complexes containing f-elements and transition metals are crucial for understanding novel bonding and reactivity.
  • Uranium(IV) and Rhodium(I) complexes offer unique electronic properties for exploring metal-metal interactions.

Purpose of the Study:

  • To synthesize and characterize novel heterotetrameric and bimetallic uranium(IV)-rhodium(I) complexes.
  • To investigate the U-Rh intermetallic distances and bonding characteristics in both solid-state and solution.
  • To explore the influence of different rhodium(I) precursors on the resulting complex structures.

Main Methods:

  • Synthesis of uranium(IV)-rhodium(I) complexes using uranium(IV) iodide precursor and rhodium(I) iodide olefin complexes.
  • Characterization techniques including single crystal X-ray diffraction, NMR, UV-vis-NIR spectroscopy, and electrochemistry.
  • Analysis of metal-metal bond lengths and interactions in solid-state and solution.

Main Results:

  • Formation of heterotetrameric [UIVRhI]2 and bimetallic UIVRhI complexes.
  • Observed U-Rh intermetallic distances of 2.7601(5) Å and 2.7630(5) Å, among the shortest reported.
  • Significant weakening of metal-metal interactions in solution compared to solid-state observations.

Conclusions:

  • Successful synthesis of uranium(IV)-rhodium(I) complexes with record short U-Rh bond lengths.
  • Demonstration of distinct solid-state and solution-phase metal-metal interactions.
  • Highlights the importance of characterization in both phases for a complete understanding of metal-ligand systems.