Related Experiment Video
Updated: May 19, 2026

Methods of Ex Situ and In Situ Investigations of Structural Transformations: The Case of Crystallization of Metallic Glasses
Published on: June 7, 2018
Modeling hyperfine parameters observed from the charge-ordered to valence-mixed state of NdBaFe2O5
Abstract:
Orbital populations of the minority-spin Fe(2+) electron in NdBaFe(2)O(5) are extracted from electric and magnetic hyperfine parameters of (57)Fe Mössbauer spectra across the temperature interval where charge ordering of the valence state 2.5 + of iron occurs. The previously used approach that assigns the minority-spin population to a single lowest-energy d orbital is expanded to three orbitals by setting up a system of equations in terms of the Fe(2+)/Fe(3+) balance from isomer shift, a point-charge model for the valence and ligand contributions to the electric-field gradient, a point-dipole model for the dipolar contribution and an iterative scheme for small orbital contributions to the internal magnetic field. This allows us to model the hyperfine fields (electric and magnetic) in the intermediate temperature range of partial charge ordering between T(V ) ≈ 210 K and T(p) ≈ 285 K, for which the one-orbital model was insufficient.
Related Concept Videos
Valence Bond Theory
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...
Electron Configurations
The relative energies of the subshells determine the order in which atomic orbitals are filled (1s, 2s, 2p, 3s, 3p, 4s,...
Electron Configuration of Multielectron Atoms
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.
Ferromagnetism

