Related Experiment Video
Updated: Jun 5, 2026

Hyperspectral Imaging as a Tool to Study Optical Anisotropy in Lanthanide-Based Molecular Single Crystals
Published on: April 14, 2020
Magnetic Anisotropy in the Homoleptic [CoX4]2- (X = Cl, Br, I) Series: Spectroscopic Determination and Ligand Field
Adiat A Fakolujo1, Michael J Jenkins1, J Krzystek2
1Department of Chemistry, University of Tennessee, Knoxville, Tennessee 37996, United States.
Abstract:
Four-coordinate transition metal complexes with unpaired electrons (S ≥ 1) typically exhibit structures deviated from perfect Td geometry, leading to magnetic anisotropy. (NEt4)2[CoX4] (X = Cl, Co-Cl; Br, Co-Br; I, Co-I) with pseudotetrahedral structures are an ideal series to explore how deviation from perfect Td geometry is reflected in magnetic anisotropy. This work presents comprehensive studies of Co-X, including single-crystal X-ray diffraction of Co-Cl and Co-I, measurements of DC and AC magnetic susceptibilities, inelastic neutron scattering (INS), far-infrared magneto-spectroscopy (FIRMS), and high-frequency and -field electron paramagnetic resonance (HFEPR). Both [CoCl4]2- and [CoBr4]2- ions have crystallographically imposed D2d symmetry, while the [CoI4]2- ion adopts slightly distorted tetrahedral geometry approximating D2d symmetry. Magnetic anisotropy increases from Co-Cl to Co-I. Also, only Co-Cl and Co-Br show field-induced SMM behaviors. FIRMS of Co-I reveals spin-phonon couplings, suggesting that these couplings may lead to fast magnetic relaxation and the lack of SMM behavior. Ligand field theory calculations indicate that an increase in spin-orbit couplings (SOC) from Co-Cl to Co-Br and to Co-I leads to increased magnetic anisotropy. These compounds provide insight into how crystal fields, crystallographic symmetries, and SOC affect magnetic anisotropy and spin relaxation in a well-defined series of homoleptic complexes.
Related Concept Videos
Crystal Field Theory - Octahedral Complexes
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...
Valence Bond Theory
Colors and Magnetism
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.
Stereoisomerism
Isomers are different chemical species that have the same chemical formula.
Transition metal complexes often exist as geometric isomers, in which the same atoms are connected through the same types of bonds but with differences in their orientation in space. Coordination complexes with two different ligands in the cis and trans positions from a ligand of interest form isomers. For example, the octahedral [Co(NH3)4Cl2]+ ion has two isomers (Figure 1) In the cis...
Structural Isomerism
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 be...
Crystal Field Theory - Tetrahedral and Square Planar 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,...

