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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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Electron Paramagnetic Resonance (EPR) Spectroscopy: Organic Radicals01:17

Electron Paramagnetic Resonance (EPR) Spectroscopy: Organic Radicals

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Ideally, an unpaired electron shows a single peak in the EPR spectrum due to the transition between the two spin energy states. However, coupling interactions can occur between the spins of the unpaired electron and any neighboring spin-active nuclei. This hyperfine coupling results in hyperfine splitting, where the EPR signal is split into multiplets. The signals split into 2nI + 1 peaks, where n is the number of equivalent nuclei and I is the nuclear spin. These splitting patterns provide...
3.6K
Crystal Field Theory - Octahedral Complexes02:58

Crystal Field Theory - Octahedral Complexes

31.2K
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...
31.2K
Crystal Field Theory - Tetrahedral and Square Planar Complexes02:46

Crystal Field Theory - Tetrahedral and Square Planar Complexes

49.0K
Tetrahedral Complexes
Crystal field theory (CFT) is applicable to molecules in geometries other than octahedral. In octahedral complexes, the lobes of the dx2−y2 and dz2 orbitals point directly at the ligands. For tetrahedral complexes, the d orbitals remain in place, but with only four ligands located between the axes. None of the orbitals points directly at the tetrahedral ligands. However, the dx2−y2 and dz2 orbitals (along the Cartesian axes) overlap with the ligands less than the dxy,...
49.0K
Valence Bond Theory02:42

Valence Bond Theory

11.4K
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...
11.4K
Structural Isomerism02:34

Structural Isomerism

21.8K
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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Related Experiment Video

Updated: Feb 25, 2026

Author Spotlight: Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks
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Author Spotlight: Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks

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Correlating EPR Parameters With Structural Anisotropy in Cu(II) Complexes.

Sriparna Roy1, Anirban Misra1, Satadal Paul2

  • 1Department of Chemistry, University of North Bengal, Darjeeling, India.

Journal of Computational Chemistry
|February 23, 2026
PubMed
Summary
This summary is machine-generated.

Quantum chemical calculations link molecular geometry to Electron Paramagnetic Resonance (EPR) parameters in Cu(II) complexes. Metal-ligand bonds influence spin orbit coupling and g-value shifts, revealing spin distribution patterns.

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Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Spectroscopy

Background:

  • Electron Paramagnetic Resonance (EPR) parameters provide insights into the electronic structure and geometry of open-shell molecules.
  • Interpreting EPR parameters like g-tensor and hyperfine coupling constants requires robust theoretical frameworks.
  • Understanding the relationship between molecular geometry and spectroscopic features is crucial for characterizing transition metal complexes.

Purpose of the Study:

  • To elucidate the electronic structure origins of spectroscopic behavior in pseudo-octahedral Cu(II) systems.
  • To correlate molecular geometry with EPR parameters, specifically the g-tensor and hyperfine coupling constants.
  • To determine the orientation of the g-tensor relative to the molecular coordinate frame using advanced computational methods.

Main Methods:

  • Employed Density Functional Theory (DFT) and wave function-based theories to compute spin Hamiltonian parameters.
  • Utilized multireference configuration interaction (MRCI) calculations to determine spin orbit coupling (SOC) and g-tensor orientation.
  • Analyzed the shift in the free electron g-value (Δg) as a fingerprint of geometry and electronic structure.

Main Results:

  • Established a correlation between metal-ligand bond characteristics, orbital degeneracy, SOC, and Δg values.
  • Demonstrated that the isotropic (Aiso) and parallel (A∥) hyperfine coupling constants reflect spin distribution, with higher values indicating greater spin density on the ligand atom due to covalency.
  • Successfully mapped EPR parameters to molecular geometry using electronic structure information.

Conclusions:

  • Quantum chemical calculations provide a reliable interpretation of EPR parameters, linking molecular geometry and electronic structure in Cu(II) complexes.
  • The study highlights the sensitivity of EPR parameters to subtle changes in metal-ligand bonding and molecular symmetry.
  • This work offers a computational approach to orienting the g-tensor and understanding spin distribution in transition metal systems.