在a-site-ordered perovskites中的平方坐标mn的各种价值状态
Youwen Long1, Takashi Saito, Masaichiro Mizumaki
1Institute for Chemical Research, Kyoto University, Uji, Kyoto 611-0011, Japan. ywlong@msk.kuicr.kyoto-u.ac.jp
Journal of the American Chemical Society
|October 17, 2009
概括
研究人员合成了A位点排序的矿LaMn3Cr4O12和LaMn3Ti4O12. 他们发现,在A位点的价值可以有所变化,挑战了长期以来认为它仅仅是Mn3+的信念.
科学领域:
- 材料科学 材料科学 材料科学
- 固态化学 固态化学
- 晶体学 晶体学是指结晶学.
背景情况:
- A-site-ordered矿是一种具有独特结构和电子特性的材料类.
- 在这些矿中,正方形坐标的A位点传统上与Jahn-Teller活性Mn3+) 离子有关.
- 了解矿中离子的价值状态对于预测和调整它们的性质至关重要.
研究的目的:
- 为了合成和描述新的A位点排序的矿,特别是LaMn3Cr4O12和LaMn3Ti4O12.
- 为了研究这些合成化合物的离子在A位点的价值状态.
- 重新评估对Jahn-Teller活动和Mn价值在A位点在A位点排序的矿石的既定理解.
主要方法:
- 使用高压和高温合成技术来获得目标矿结构.
- 为了阐明离子配置,进行了化学公式的确定和电荷状态分析.
- 频谱或衍射方法 (隐含的,没有明确说明) 可能用于结构和价值状态分析.
主要成果:
- 合成和表征了LaMn3Cr4O12,揭示了LaMn(3+) ((3) Cr ((3+) ((4) O ((12) 的电荷公式与Mn ((3+) 在A位点.
- 还合成了LaMn3Ti4O12,在A位点表现出低于+2的价值,其拟议的电荷组合是LaMn{1.67+) {3) Ti{4+) {4) O{12).
- 这些发现表明,在A位点的价值可以从+3到大约+1.67不等,这与之前的假设相反.
结论:
- 在研究中,在苛刻的条件下,成功合成了新型A位点排序的矿.
- 这些结果挑战了长期以来的假设,即这些材料中的A位点Mn仅为Mn3+).
- 观察到的可变价值突出了通过组成控制调整A位点排序矿的性能的潜力.
相关概念视频
Valence Bond Theory
10.2K
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...
10.2K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
46.3K
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,...
46.3K
Ionic Crystal Structures
16.2K
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...
16.2K
Coordination Number and Geometry
17.7K
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.
17.7K
VSEPR Theory and the Effect of Lone Pairs
50.2K
Effect of Lone Pairs of Electrons on Molecule Geometry
50.2K
Colors and Magnetism
12.9K
Color in Coordination Complexes
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
When atoms or molecules absorb light at the proper frequency, their electrons are excited to higher-energy orbitals. For many main group atoms and molecules, the absorbed photons are in the ultraviolet range of the electromagnetic spectrum, which cannot be detected by the human eye. For coordination compounds, the energy difference between the d orbitals often allows photons in the visible range to be absorbed and emitted, which is seen as colors by the human...
12.9K


