单核铜的结构和光谱表征 (I) 酸复合物:NO与铜的端对侧协调 (I)
Kiyoshi Fujisawa1, Akira Tateda, Yoshitaro Miyashita
1Graduate School of Pure and Applied Sciences, University of Tsukuba, Tsukuba 305-8571, Japan. kiyoshif@chem.tsukuba.ac.jp
Journal of the American Chemical Society
|January 9, 2008
概括
本研究介绍了铜(I) - 尼托复合物的晶体结构和光谱分析. 结果揭示了对铜-酸盐结合和电子结构的洞察力,有助于理解酶中间体.
科学领域:
- 无机化学 无机化学
- 协调化学 协调化学
- 频谱学是一种光谱学.
背景情况:
- 铜-基复合物是各种生物和催化过程中的关键中间体.
- 了解铜-酸盐 (Cu-NO) 部分的电子结构和结合对于阐明反应机制至关重要.
- 之前的研究已经探讨了铜-尼托西尔相互作用,但详细的结构和光谱表征仍然很重要.
研究的目的:
- 合成和表征两种新型单核铜 (I) - 尼托西尔复合体,具有不同的结合体.
- 通过使用全面的光谱技术,研究Cu-NO单元的电子结构和粘合模式.
- 将光谱数据与理论计算相关联,以确定Cu-NO相互作用的结合模式和稳定性.
主要方法:
- 进行X射线晶体学以确定铜(I) - 尼托西尔复合物的精确晶体结构.
- 振动光谱 (IR) 分析N-O和Cu-NO拉伸频率和力常数.
- 电子偏磁共振 (EPR) 和磁圆二元化 (MCD) 光谱,支持密度函数理论 (DFT) 计算,探测电子结构和结合.
主要成果:
- 确定了 [Cu(L3) ((NO)) 和 [Cu(L3') ((NO) ] ((ClO4) 的晶体结构.
- 光谱分析显示,与复合体2相比,复合体1中的Cu-NO键和不稳定性较弱,归因于第二协调球效应.
- EPR和DFT的计算证实了Cu (I) -NO (radical) 电子结构,并且确定了EPR参数与Cu-N-O角之间的相关性.
结论:
- 这项研究提供了详细的光谱证据,证明合成复合物中的 NO 与铜 (I) 结合的末端NO.
- 这些发现使得能够确定Cu-NO中间体在像铜酸还原酶这样的酶中的结合方式.
- 研究表明,一个强烈曲的 (约. 135度),但不是在溶液中的Cu-NO中间体的侧向结合模式.
更多相关视频
11:04Ion Mobility-Mass Spectrometry Techniques for Determining the Structure and Mechanisms of Metal Ion Recognition and Redox Activity of Metal Binding Oligopeptides
Published on: September 7, 2019
06:31Preparation of SNS Cobalt(II) Pincer Model Complexes of Liver Alcohol Dehydrogenase
Published on: March 19, 2020
相关概念视频
Structural Isomerism
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 be...
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 be...
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.
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...
Coordination Compounds and Nomenclature
In most main group element compounds, the valence electrons of the isolated atoms combine to form chemical bonds that satisfy the octet rule. For instance, the four valence electrons of carbon overlap with electrons from four hydrogen atoms to form CH4. The one valence electron leaves sodium and adds to the seven valence electrons of chlorine to form the ionic formula unit NaCl (Figure 1a). Transition metals do not normally bond in this fashion. They primarily form coordinate covalent bonds, a...
Stereoisomerism
Isomerism in Complexes
Isomers are different chemical species that have the same chemical formula.
Transition metal complexes often exist as geometric isomers, in which the same atoms are connected through the same types of bonds but with differences in their orientation in space. Coordination complexes with two different ligands in the cis and trans positions from a ligand of interest form isomers. For example, the octahedral [Co(NH3)4Cl2]+ ion has two isomers (Figure 1) In the cis...
Isomers are different chemical species that have the same chemical formula.
Transition metal complexes often exist as geometric isomers, in which the same atoms are connected through the same types of bonds but with differences in their orientation in space. Coordination complexes with two different ligands in the cis and trans positions from a ligand of interest form isomers. For example, the octahedral [Co(NH3)4Cl2]+ ion has two isomers (Figure 1) In the cis...
