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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...
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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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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.
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Ladder diagrams are useful for evaluating equilibria involving metal-ligand complexes. The vertical scale of the ladder diagram represents the concentration of unreacted or free ligand, pL. The horizontal lines on the scale depict the log of stepwise formation constants for metal-ligand complexes and indicate the dominant species in all the regions.
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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.
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Conformational dynamicity in a copper(II) coordination complex.

Paul J Griffin1, Matthew J Dake1, Alesandro D Remolina1

  • 1Department of Chemistry, Center for Biophysics and Quantitative Biology, and Materials Research Laboratory, University of Illinois at Urbana-Champaign, Urbana, Illinois, 61801, USA. lolshans@illinois.edu.

Dalton Transactions (Cambridge, England : 2003)
|June 2, 2023
PubMed
Summary

Copper complexes show dynamic structural changes upon oxidation. This study reveals [CuCl(dpaSMe)]+/0 shifts between geometries, impacting electron transfer. Understanding these dynamics is key.

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Area of Science:

  • Coordination Chemistry
  • Inorganic Chemistry
  • Materials Science

Background:

  • Copper coordination complex geometry influences electron transfer.
  • The role of dynamics in these electron transfer processes remains unclear.
  • Previous work showed CuI fluxionality and CuII rigidity in CuCl(dpaOMe).

Purpose of the Study:

  • To synthesize and characterize [CuCl(dpaSMe)]+/0.
  • To investigate the structural dynamics of this copper complex in its CuI and CuII states.
  • To correlate observed dynamics with electron transfer capabilities.

Main Methods:

  • X-ray diffraction for solid-state structure.
  • Cyclic voltammetry for electrochemical properties.
  • Electron Paramagnetic Resonance (EPR) spectroscopy for solution-state dynamics.

Main Results:

  • [CuCl(dpaSMe)]+/0 exhibits rigidity in the CuI state and dynamics in the CuII state.
  • Temperature-dependent interconversion between trigonal bipyramidal and square pyramidal geometries was observed for the CuII complex.
  • Solid and solution-state data were combined to assign coordination geometries.

Conclusions:

  • The synthesized copper complex displays distinct dynamic behavior upon oxidation.
  • Observed structural dynamics are linked to coordination geometry changes.
  • These findings provide insights into factors affecting electron transfer in copper complexes.