Related Experiment Video
Updated: Apr 19, 2026
09:12
Facet-to-facet Linking of Shape-anisotropic Colloidal Cadmium Chalcogenide Nanostructures
Published on: August 10, 2017
8.1K
Crystal structure of the inter-metallic compound SrCdPt.
1Department of Chemical Education, Sriwijaya University, Inderalaya, Ogan Ilir 30662, South Sumatra, Indonesia.
Acta Crystallographica. Section E, Structure Reports Online
|January 2, 2015
Summary
The crystal structure of strontium cadmium platinum (SrCdPt) was determined, revealing a TiNiSi type. Platinum atoms form a 3D network, with strontium atoms located in channels within this structure.
Area of Science:
- Solid-state chemistry
- Crystallography
- Materials science
Background:
- Understanding intermetallic compound structures is crucial for materials development.
- The TiNiSi structure type is a common motif in intermetallic compounds.
Purpose of the Study:
- To determine and describe the crystal structure of strontium cadmium platinum (SrCdPt).
- To elucidate the atomic arrangement and bonding within the SrCdPt compound.
Main Methods:
- Single-crystal X-ray diffraction was used to determine the crystal structure.
- Analysis of atomic positions and coordination environments.
Main Results:
- SrCdPt crystallizes in the TiNiSi structure type.
- Strontium (Sr) atoms occupy the Ti sites, cadmium (Cd) atoms the Ni sites, and platinum (Pt) atoms the Si sites.
- Platinum atoms form a 3D network of cadmium-centered tetrahedra, with Sr atoms in the channels.
Conclusions:
- The crystal structure of SrCdPt is characterized by a 3D Pt-Cd tetrahedral network.
- Strontium atoms are located within channels formed by this network and exhibit six-membered ring arrangements.
- All atoms are positioned on a mirror plane, indicating specific symmetry properties.
Related Concept Videos
02:37Metallic Solids
21.6K
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...
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and...
21.6K
01:26Imperfections in Crystal Structure: Stoichiometric Point Defects
99
Schottky defects arise when some lattice points in a crystal, such as those in NaCl, remain unoccupied, creating lattice vacancies without disturbing the overall electrical neutrality of the crystal. This defect is common in ionic crystals where the positive and negative ions are similar in size, as seen in sodium chloride and cesium chloride. The presence of Schottky defects enables the crystal to conduct electricity to a small extent through an ionic mechanism. Electric fields cause nearby...
99
02:42Ionic Crystal Structures
21.7K
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...
21.7K
01:29Imperfections in Crystal Structure: Non-Stoichiometric Defects
99
Non-stoichiometric defects refer to a type of defect in the crystal structure of a compound where the ratio of its constituent elements deviates from the ideal stoichiometric ratio. There are two main types of non-stoichiometric defects: metal excess defects and metal deficiency defects.Metal excess defects occur when there is a slight surplus of metal ions than what is required by the stoichiometric ratio of the compound. For example, heating a sodium chloride crystal in sodium vapor results...
99
02:58Crystal Field Theory - Octahedral Complexes
32.2K
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...
32.2K
02:46Crystal Field Theory - Tetrahedral and Square Planar Complexes
50.1K
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...
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...
50.1K