为什么有些针复合体是平面的,而另一些是金字塔的?
Tyler J Hannah1, Tamina Z Kirsch1, Saurabh S Chitnis1
1Chemistry Department, Dalhousie University, 6243 Alumni Crescent, B3H4R2, Halifax, Nova Scotia, Canada.
Chemistry (Weinheim an der Bergstrasse, Germany)
|July 30, 2024
概括
一个新的模型通过平衡对立的sigma和pi结合效应来解释pnictogen的复杂几何形状. 这个框架预测并帮助设计具有特定构造和反应性的复合体.
科学领域:
- 有机金属化学 有机金属化学
- 计算化学计算化学
- 材料科学 材料科学 材料科学
背景情况:
- 菌素具复合体表现出各种不同的几何形状,这对于它们的反应性至关重要.
- 现有的模型缺乏对观察到的形状变化的统一解释.
研究的目的:
- 开发一个统一的计算模型,解释菌器复合体的构造多样性.
- 预测和指导这些复杂的合理设计.
主要方法:
- 在64个综合体中对1300多个结构进行计算分析.
- 审查债券稳定性 (债券长度,维伯格债券指数) 和费用转移 (NPA,希尔什菲尔德费用).
主要成果:
- 提出了一个基于基于竞争的基基的s-结合 (有利于金字塔化) 和基于联体的π-结合 (有利于平面性) 的模型.
- 这些相反的力量之间的平衡调和了结构变化.
结论:
- 提出的σ/π-结合模型成功地解释了观察到的几何形状,并预测了未来的结果.
- 这种框架可以帮助合理设计具有量身定制性质的pnictogen具复合体.
相关概念视频
Valence Bond Theory
8.5K
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...
8.5K
Structural Isomerism
19.2K
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can...
Isomers are different chemical species that have the same chemical formula. Structural isomerism of coordination compounds can be divided into two subcategories, the linkage isomers and coordination-sphere isomers.
Linkage isomers occur when the coordination compound contains a ligand that can bind to the transition metal center through two different atoms. For example, the CN− ligand can bind through the carbon atom or through the nitrogen atom. Similarly, SCN− can...
19.2K
Coordination Number and Geometry
15.6K
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.
15.6K
Colors and Magnetism
11.6K
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...
11.6K
Crystal Field Theory - Tetrahedral and Square Planar Complexes
41.9K
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,...
41.9K


