Related Experiment Video
Updated: Sep 29, 2025

Combining Solid-state and Solution-based Techniques: Synthesis and Reactivity of ChalcogenidoplumbatesII or IV
Published on: December 29, 2016
Structural Diversity of Rare-Earth Oxychalcogenides
Melissa Orr1, Glen R Hebberd2, Emma E McCabe2
1Department of Chemistry and Biochemistry, University of Texas at Arlington, Arlington, Texas 76019, United States.
Solid-state chemists are exploring mixed-anion compounds, like rare-earth oxychalcogenides, for advanced applications. This review covers their structural diversity and synthetic methods, from 2D layers to 3D networks.
Area of Science:
- Solid-state chemistry
- Materials science
- Inorganic chemistry
Background:
- Mixed-anion systems offer unique properties for energy conversion, electronics, and catalysis.
- Rare-earth containing materials are crucial for modern technologies.
- Oxychalcogenides represent a promising class of mixed-anion compounds.
Purpose of the Study:
- To review recent advances in rare-earth oxychalcogenides.
- To discuss the structural diversity of ternary and quaternary rare-earth oxychalcogenides.
- To highlight the progression towards 3D networks and novel synthetic approaches.
Main Methods:
- Review of existing literature on rare-earth oxychalcogenides.
- Analysis of structural characteristics of ternary and quaternary compounds.
- Discussion of synthetic strategies for layered and network structures.
Main Results:
- Ternary rare-earth oxychalcogenides exhibit layered structures showcasing oxide and chalcogenide anion behavior.
- Quaternary compounds demonstrate combined anionic and cationic design, leading to structural diversity.
- Advancements include the transition from 2D layered materials to 3D networks.
Conclusions:
- Rare-earth oxychalcogenides are a key area of mixed-anion materials research.
- Structural complexity and synthetic methods are advancing the field.
- These materials hold significant potential for future technological applications.
Related Concept Videos
Ionic Crystal Structures
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...
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...
Properties of Transition Metals
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...
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...
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,...

