Related Experiment Video
Updated: Aug 13, 2026
08:15
Synthesis of Nine-atom Deltahedral Zintl Ions of Germanium and their Functionalization with Organic Groups
Published on: February 11, 2012
New tetragonal structure type for A2Ca10S(9 (A = Li, Mg). Electronic variability around a Zintl phase
Ashok K Ganguli1, Shalabh Gupta, John D Corbett
1Department of Chemistry and Ames Laboratory, Iowa State University, Ames, 50010, USA. ashok@chemistry.iitd.ernet.in
Inorganic Chemistry
|January 5, 2006
Summary
New Zintl phases LiMgCa(10)Sb(9), Mg(2)Ca(10)Sb(9), and Li(1.38(2))Ca(10.62)Sb(9) were synthesized and characterized. These compounds exhibit unique electronic properties, with one being electron-precise and another electron-rich.
Area of Science:
- Solid-state chemistry
- Materials science
- Crystallography
Background:
- Exploration of Zintl phases provides insights into structure-property relationships.
- Understanding complex alkali and alkaline earth metal antimonides is crucial for novel material discovery.
Purpose of the Study:
- To synthesize and characterize novel Zintl phases with the formula A(x)B(y)Sb(z).
- To investigate the crystallographic and electronic properties of these new compounds.
Main Methods:
- High-temperature solid-state synthesis.
- Single-crystal X-ray diffraction for structural determination.
- Property measurements including magnetic susceptibility and conductivity.
Main Results:
- Three new phases, LiMgCa(10)Sb(9), Mg(2)Ca(10)Sb(9), and Li(1.38(2))Ca(10.62)Sb(9), were successfully synthesized.
- Crystal structures were determined in space group P4(2)/mnm, revealing a Ca-Sb network with specific anion arrangements.
- Electronic properties varied, with LiMgCa(10)Sb(9) identified as an electron-precise Zintl phase, diamagnetic and semiconducting.
Conclusions:
- The synthesized compounds represent new additions to the Zintl phase family.
- Structural and electronic diversity within these phases offers potential for tailored material properties.
- Further research can explore applications based on their semiconducting and magnetic characteristics.
More Related Videos
Related Concept Videos
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...
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...
02:46Crystal Field Theory - Tetrahedral and Square Planar Complexes
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,...
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...
02:48Ionic Bonding and Electron Transfer
Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions.
02:57Coordination Number and Geometry
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.