Related Experiment Video
Updated: Aug 14, 2026

09:43
Synthesis of Immunotargeted Magneto-plasmonic Nanoclusters
Published on: August 22, 2014
Gold Clusters With Open-Shell Ligands: Superatom Mediated Magnetic Interaction
Katsuya Mutoh1, Kosei Hayashi1, Yoichi Kobayashi2
1Department of Chemistry, Graduate School of Science, Osaka Metropolitan University, Osaka, Japan.
Angewandte Chemie (International Ed. in English)
|August 12, 2026
Summary
Researchers synthesized Ir-doped gold clusters functionalized with organic radicals. They observed electronic interactions and magnetic communication, paving the way for new magnetic nanomaterials.
Area of Science:
- Nanomaterials Science
- Supramolecular Chemistry
- Magnetism
Background:
- Superatomic orbitals in gold clusters are key for nanoscale magnetic materials.
- Functionalizing metal clusters with organic radicals offers new avenues for magnetic properties.
Purpose of the Study:
- To synthesize and characterize Ir-doped Au12 clusters with verdazyl radicals.
- To investigate the electronic, magnetic, and photophysical properties of these hybrid materials.
Main Methods:
- Synthesis of Ir-doped Au12 clusters functionalized with verdazyl radicals.
- Ultrafast time-resolved absorption spectroscopy.
- Electron Paramagnetic Resonance (EPR) spectroscopy at variable temperatures.
Main Results:
- Photoluminescence quenching upon radical functionalization.
- Evidence of electron transfer from the Ir@Au12 core to verdazyl ligands.
- Spin density delocalization and weak magnetic communication between radicals mediated by the cluster core.
Conclusions:
- Demonstrated electronic interaction between organic radicals and the Ir@Au12 superatomic core.
- Established superatom-organic radical hybrids as a new class of multi-spin systems.
- Provided a design strategy for photofunctional and magnetic nanomaterials.
Related Concept Videos
Colors and Magnetism
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 eye.
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.
Valence Bond Theory
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...
Crystal Field Theory - Octahedral Complexes
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...
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...
Metal-Ligand Bonds
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...
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...
Complexation Equilibria: The Chelate Effect
In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
Complexation Equilibria: Factors Influencing Stability of Complexes
In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
