高旋转d4复合物的电子和分子结构:对图顿盐中的[Cr(D2O) 6+2离子进行实验和理论研究
Christopher Dobe1, Christopher Noble, Graham Carver
1Department of Chemistry and Biochemistry, University of Bern, Freiestrasse 3, CH-3000, Bern 9, Switzerland.
Journal of the American Chemical Society
|December 17, 2004
概括
可变温度研究揭示了的动态变化
科学领域:
- 无机化学 无机化学 有机化学
- 固态物理 固态物理
- 量子化学 是一个量子化学.
背景情况:
- (II) 图顿盐 (MI) 2Cr (X2O) 6 (SO4) 2被研究以了解高旋转的d4复合体.
- 之前的研究对此类系统缺乏详细的可变温度电子结构数据.
研究的目的:
- 严格定义的基态电子结构 (II) 图顿盐在广泛的温度范围内.
- 研究这些复合体中的温度依赖的立体化学和电子变化.
- 开发一种新的理论方法来计算可变温度EPR光谱.
主要方法:
- 可变温度不弹性中子散射 (INS) 和多频电子磁共振 (EPR) 光谱.
- 结晶学研究.结晶学研究.
- 使用旋转汉密尔顿式和Jahn-Teller汉密尔顿式进行建模.
主要成果:
- 轴向和形零场分裂参数与温度的剧烈变化.
- 在[Cr(D2O) 6+复合体中,温度依赖的立体化学变化,Cr-O键长度合并在150K以上.
- 使用温度依赖的异构菌株模型和新的EPR光谱计算方法的成功解释.
结论:
- 的电子结构和立体化学 (II) 图顿盐具有显著的温度依赖性.
- 一种温度依赖的异构菌株对于解释观察到的现象至关重要.
- 开发的理论方法为INS和EPR技术的不同时间尺度提供了洞察力.
相关概念视频
Lewis Structures of Molecular Compounds and Polyatomic Ions
To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:
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...
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...
Crystal Field Theory - Octahedral Complexes
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...
Crystal 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,...
Colors and Magnetism
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 eye.
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 eye.


