突出的BaAl4结构类型的s-p结合代表:关于极性金属间网络结构的结构稳定性的案例研究
Ulrich Häussermann1, Shahrad Amerioun, Lars Eriksson
1Department of Inorganic Chemistry, Stockholm University, S-10691 Stockholm, Sweden.
Journal of the American Chemical Society
|April 19, 2002
概括
这项研究研究了具有BaAl4结构的s-p结合化合物,发现了稳定性的14电子规则. 然而,电子缺乏是常见的,而离子大小影响了这些极性金属间的结构变化.
科学领域:
- 固态化学 固态化学
- 材料科学 材料科学 材料科学
- 计算材料科学科学 计算材料科学
背景情况:
- 研究极性金属间结构的形成和原子排列是复杂的.
- BaAl4结构类型 (空间组I4/mmm) 是s-p结合化合物的关键框架.
研究的目的:
- 对具有BaAl4结构类型的s-p结合化合物的结构稳定性进行综合实验和理论研究.
- 探索极地金属间结构的结构形成和原子排列.
主要方法:
- 使用伪电位和平面波基设置的ab initio计算来确定结构参数,结合能和电子结构.
- 使用X射线单晶和粉末衍射的实验合成和结构特征.
主要成果:
- 每个公式单位14个电子的费米级状态密度的伪差距表明BaAl4型化合物的最佳稳定性.
- 实验结果显示,合成的BaAl4型极性金属间金属中经常存在电子缺陷.
- "X"元素的位置偏好受到"色彩能量"和电阳性Ae元件的大小的影响.
- 阴离子大小显著影响近邻距离和聚离子网络 (X4(2-)) 的灵活性.
结论:
- 虽然14电子计数有利于稳定性,但导致电子缺乏的偏差在BaAl4型极性金属间金属中很常见.
- 结构变化,包括单临床扭曲和EuIn4类型的形成,发生的原因是与聚离子子的大小不匹配.
- 这项研究提供了关于极性金属间结构性质关系的见解.
更多相关视频
相关概念视频
Hybridization of Atomic Orbitals I
The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
Ionic 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...
Metallic 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...
Valence 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...
Complexation Equilibria: Factors Influencing Stability of Complexes
In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
Imperfections in Crystal Structure: Non-Stoichiometric Defects
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...


