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Related Concept Videos

Coordination Number and Geometry02:57

Coordination Number and Geometry

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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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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...
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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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Colors and Magnetism03:02

Colors and Magnetism

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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...
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Crystal Field Theory - Octahedral Complexes02:58

Crystal Field Theory - Octahedral Complexes

32.2K
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...
32.2K
Valence Bond Theory02:42

Valence Bond Theory

11.9K
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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Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
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Metal ion oxidation state assignment based on coordinating ligand hyperfine interaction.

Paul H Oyala1, Troy A Stich, R David Britt

  • 1Department of Chemistry, University of California-Davis, One Shields Avenue, Davis, CA, 95616, USA.

Photosynthesis Research
|February 10, 2015
PubMed
Summary
This summary is machine-generated.

The effective ligand hyperfine interaction (HFI) in spin systems helps determine metal ion oxidation states and coordination geometry. This method was recently used to identify manganese oxidation states in photosystem II.

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Area of Science:

  • * Biophysical Chemistry
  • * Inorganic Chemistry
  • * Quantum Chemistry

Background:

  • * Exchange-coupled mixed-valence spin systems exhibit ligand hyperfine interactions (HFI).
  • * The magnitude and sign of HFI are influenced by the projection factor (Clebsch-Gordon coefficient).
  • * This factor relates local paramagnetic center spin to the total spin of the system.

Purpose of the Study:

  • * To describe the origin and evolution of using ligand HFI.
  • * To demonstrate the utility of HFI in determining metal ion oxidation states.
  • * To provide insights into coordination geometry in spin systems.

Main Methods:

  • * Analysis of effective ligand hyperfine interaction (HFI).
  • * Application of projection factors (Clebsch-Gordon coefficients).
  • * Examination of exchange-coupled mixed-valence spin systems.

Main Results:

  • * Ligand HFI magnitude and sign correlate with metal ion oxidation state.
  • * HFI provides information on coordination geometry.
  • * Successful application in identifying Mn oxidation states in photosystem II.

Conclusions:

  • * Effective ligand HFI is a valuable tool for characterizing spin systems.
  • * The study highlights the importance of HFI in understanding metalloenzymes like photosystem II.
  • * This approach offers a pathway to probe electronic structure and oxidation states.