Related Experiment Video
Updated: Dec 11, 2025

11:17
Spark Plasma Sintering Apparatus Used for the Formation of Strontium Titanate Bicrystals
Published on: February 9, 2017
10.1K
Crystal structure solution for the A6B2O17 (A = Zr, Hf; B = Nb, Ta) superstructure
Scott J McCormack1, Waltraud M Kriven1
1Department of Material Science and Engineering, University of Illinois at Urbana-Champaign, Urbana, Illinois, 61801, USA.
Summary
New crystal structures for Zr6Ta2O17, Hf6Nb2O17, and Hf6Ta2O17 were solved. These compounds form an orthorhombic family, A6B2O17, with potential for cation ordering.
Area of Science:
- Solid-state chemistry
- Crystallography
- Materials science
Background:
- The A6B2O17 orthorhombic compound family exhibits complex crystal structures.
- Understanding cation ordering and structural variations is crucial for materials design.
Purpose of the Study:
- To solve and characterize the crystal structures of Zr6Ta2O17, Hf6Nb2O17, and Hf6Ta2O17.
- To classify these compounds within the A6B2O17 family and investigate structural mechanisms.
- To explore cation order-disorder phenomena and compositional variations.
Main Methods:
- Synchrotron X-ray powder diffraction
- Neutron powder diffraction
- Simulated annealing
- Charge flipping
- Rietveld refinement
- Bond valence method
Main Results:
- Crystal structure solutions were obtained for Zr6Ta2O17, Hf6Nb2O17, and Hf6Ta2O17.
- These structures are isomorphous with Zr6Nb2O17, confirming the A6B2O17 orthorhombic family (Ima2 symmetry).
- The structures comprise specific arrangements of six-, seven-, and eight-coordinated polyhedra, with mechanisms for compositional variation identified.
Conclusions:
- The A6B2O17 (A = Zr, Hf; B = Nb, Ta) orthorhombic compound family is established with Ima2 symmetry.
- Cation order/disorder potentials were analyzed using diffraction and bond valence methods.
- Compositional variations are linked to the addition/removal of specific polyhedral units and oxygen tilts.
Related Concept Videos
Ionic Crystal Structures
16.5K
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...
16.5K
Metallic Solids
20.2K
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....
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
20.2K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
47.2K
Tetrahedral 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,...
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,...
47.2K
Crystal Field Theory - Octahedral Complexes
29.9K
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...
29.9K
Structures of Solids
17.1K
Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds typically form ordered, crystalline solids. A crystalline solid has a precise melting temperature because each atom or molecule of the same type is held in place with the same forces or energy. Amorphous solids or non-crystalline solids (or, sometimes, glasses) which lack an ordered internal structure and are randomly arranged. Substances that...
17.1K
Coordination Number and Geometry
18.4K
For transition metal complexes, the coordination number determines the geometry around the central metal ion. Table 1 compares coordination numbers to molecular geometry. The most common structures of the complexes in coordination compounds are octahedral, tetrahedral, and square planar.
18.4K

