Related Experiment Video
Updated: Jul 12, 2026
13:58
Probing C84-embedded Si Substrate Using Scanning Probe Microscopy and Molecular Dynamics
Published on: September 28, 2016
Scandium clusters in fullerene cages.
Science (New York, N.Y.)
|May 22, 1992
Summary
This study characterizes fullerene-encapsulated scandium clusters using electron paramagnetic resonance (EPR) spectroscopy. Findings reveal the structure of Sc(3)C(82) and ScC(82), suggesting potential for novel nanostructured materials.
Area of Science:
- Materials Science
- Nanotechnology
- Spectroscopy
Background:
- Fullerene-encapsulated metal-atom clusters are novel materials with potential applications.
- Electron paramagnetic resonance (EPR) spectroscopy is a key technique for characterizing paramagnetic species.
Purpose of the Study:
- To produce and spectroscopically characterize fullerene-encapsulated scandium-atom clusters.
- To elucidate the electronic structure and atomic arrangement within these metallofullerenes.
Main Methods:
- Solution and solid-state electron paramagnetic resonance (EPR) spectroscopy.
- Mass spectrometry to identify metallofullerene species.
Main Results:
- EPR spectra were obtained for Sc(3)C(82) and ScC(82).
- Sc(3)C(82) results suggest a triangular arrangement of scandium atoms.
- ScC(82) exhibits characteristics of a Sc+3 cation within a C82-3 radical anion, similar to LaC(82) and YC(82).
- EPR-silent Sc2Cn species were observed despite EPR-active Sc(2).
Conclusions:
- The study provides structural insights into scandium-based metallofullerenes.
- The findings suggest potential for creating new nanostructured materials with isolated metal-atom clusters within fullerene hosts.
Related Concept Videos
03:26Electron Configuration of Multielectron Atoms
The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...
02:37Metallic Solids
Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
02:58Crystal 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...
02:42Ionic Crystal Structures
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
03:35Hybridization of Atomic Orbitals II
sp3d and sp3d 2 Hybridization
02:42Valence 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...