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Valence Bond Theory

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...

Coordination Number and Geometry

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.

Metal-Ligand Bonds

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...

Coordination Compounds and Nomenclature

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...

Colors and Magnetism

Colors 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.

Complexation Equilibria: Factors Influencing Stability of Complexes

Complexation Equilibria: Factors Influencing Stability of Complexes

In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...

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Preparation of 6-aminocyclohepta-2,4-dien-1-one Derivatives via Tricarbonyl(tropone)iron

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Stable eight-coordinate iron(III/II) complexes.

Ashis K Patra¹, Koustubh S Dube, Georgia C Papaefthymiou

¹Department of Chemistry, The University of Georgia, Athens, Georgia 30602, USA.

Inorganic Chemistry

|January 30, 2010

Summary

This summary is machine-generated.

Researchers developed a stable method for creating eight-coordinate (8C) iron complexes. These unique high-spin iron(II) and iron(III) compounds are stable in solution and characterized structurally and spectroscopically.

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Area of Science:

Coordination Chemistry
Organometallic Chemistry
Bioinorganic Chemistry

Background:

Unusual coordination numbers in transition-metal complexes are significant in biological systems and catalysis.
Eight-coordinate (8C) metal complexes are relatively rare and challenging to synthesize and stabilize.

Purpose of the Study:

To establish a systematic and predictable approach for isolating stable eight-coordinate (8C) iron(III/II) systems.
To synthesize and characterize novel 8C iron complexes with unusual coordination environments.

Main Methods:

Synthesis of the high-spin (HS) eight-coordinate iron(II) complex [Fe(L(N4))(2)](BF(4))(2) (1).
Structural characterization of complex 1, revealing a distorted square-antiprism geometry.
Electrochemical analysis to confirm the Fe(II) oxidation state and chemical oxidation to synthesize the Fe(III) analogue.

Main Results:

Successful isolation and characterization of a stable, high-spin eight-coordinate iron(II) complex.
Demonstration of remarkable solution stability for the 8C iron complex under various conditions.
Synthesis of the corresponding high-spin (HS) eight-coordinate iron(III) complex via chemical oxidation.

Conclusions:

A reliable method for accessing stable eight-coordinate iron complexes has been developed.
The synthesized 8C iron complexes exhibit unique structural, spectroscopic, and electrochemical properties.
These findings contribute to the understanding of unusual coordination numbers in iron chemistry.