四坐标铁 (I) 复合体的电子结构由一个 bis () 乙烯 () 胺连接体支
Yumiko Nakajima1, Yoshihide Nakao, Shigeyoshi Sakaki
1Institute for Chemical Research, Kyoto University, Uji, Kyoto 611-0011, Japan.
Journal of the American Chemical Society
|July 3, 2010
概括
一个新的15电子铁 (I) 复合体[FeBr (BPEP) ]被合成和特征化. 它独特的三角形单结构源于铁-子pi相互作用,揭示了高旋转的Fe (I) 中心.
科学领域:
- 无机化学 无机化学
- 有机金属化学 有机金属化学
- 协调化学 协调化学
背景情况:
- 铁复合物在催化和材料科学中至关重要.
- 了解不同寻常的协调几何和电子结构是设计新功能分子的关键.
- 低价值铁复合物的合成和表征提供了对新型反应性和结合性的见解.
研究的目的:
- 为了合成和表征一个15电子铁复合体与一个正式的Fe (I) 中心.
- 为了阐明由此产生的复合物的结构和电子特性,[FeBr(BPEP) ].
- 为了研究金属-联结体相互作用在确定复合物的几何学中的作用.
主要方法:
- 双化物前体的单电子还原产生铁 (I) 复合体.
- 单晶X射线衍射用于结构确定.
- 用SQUID磁力测量和莫斯尔光谱学进行电子表征.
- 密度函数理论 (DFT) 计算用于电子结构分析.
主要成果:
- 成功合成了15电子铁 (I) 复合体[FeBr (BPEP) ] .
- X射线衍射揭示了铁中心周围扭曲的三角形单形几何.
- 磁力测量证实了高旋转的S = 3/2基本状态,与Fe ((I)) 一致.
- 莫斯巴乌尔光谱学和DFT计算支持高旋转Fe (I) 电子配置,并突出突出分离的分子轨道.
结论:
- 合成的铁(I) 复合体表现出一种不常见的三角形单形协调几何.
- 这种扭曲的结构归因于铁d(z(2)) 轨道和BPEP联体的pi*轨道之间的有效pi-pi相互作用.
- 这项研究为低价值铁复合物的结合和电子结构提供了宝贵的见解.
相关概念视频
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...
Metal-Ligand Bonds
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
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,...
Coordination 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.
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.


