一金属离子选择性规则:Zn (II),Cd (II) 和Co (II) 与不同蛋白质协调球的相互作用,以确定可变热稳定性和折叠场景
Martina Dragone1, Gaetano Caputo1, Gianluca D'Abrosca2
1Department of Environmental, Biological and Pharmaceutical Science and Technology, University of Campania "Luigi Vanvitelli", Via Vivaldi 43, Caserta, 81100, Italy, unina2.it.
Bioinorganic chemistry and applications
|March 2, 2026
概括
这项研究调查了蛋白质金属离子相互作用,揭示了Ros87中的协调球氨基酸变化如何影响金属结合和蛋白质折叠途径. 这种CysAspHis2突变体显示了Zn (II),Co (II) 和Cd (II) 的双态折叠机制.
科学领域:
- 生物化学 生物化学
- 结构生物学 结构生物学
- 生物有机化学 生物有机化学
背景情况:
- 蛋白质 - 金属离子相互作用对于生物过程和金属离子选择性至关重要.
- 罗斯/MucR指家族为研究具有不同协调球体的结构结合提供了一个模型.
- 野生类型的Ros87蛋白质表现出Cys2His2协调,而同类蛋白通常具有CysAspHis2球体.
研究的目的:
- 为了研究Ros87-C27D突变体 (CysAspHis2) 与Zn,Co和Cd的金属结合特性.
- 为了比较突变的解离常数,结构效应和折叠机制与野生型Ros87.
- 阐明金属离子类型和协调性氨基酸如何影响蛋白质折叠路径.
主要方法:
- 紫外线对紫外线的光谱学.
- 循环二元化 (CD) 光谱学 循环二元化 (CD) 光谱学
- 核磁共振 (NMR) 谱学是指核磁共振的光谱学.
主要成果:
- 在CysAspHis2协调球中,所有测试的金属 (Zn(II),Co(II),Cd(II)) 产生了双态折叠机制.
- 野生型的Cys2His2协调球,当与Zn (II) 或Co (II) 复合时,形成了一个稳定的金属结合折叠中间体.
- 根据金属离子和协调性氨基酸集,观察到金属结合亲和度 (Kd) 和折叠路径的差异.
结论:
- 金属离子和协调性氨基酸之间的特定相互作用决定了蛋白质折叠机制和金属结合亲和力.
- 在协调球体中用阿斯巴酸替代囊素显著改变了蛋白质的折叠行为.
- 这项研究提供了对金属离子选择性和蛋白质结构动态的分子基础的见解.
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
9.9K
14:44Structure and Coordination Determination of Peptide-metal Complexes Using 1D and 2D 1H NMR
Published on: December 16, 2013
10.1K
相关概念视频
01:09Complexation Equilibria: Factors Influencing Stability of Complexes
892
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...
892
02:51Metal-Ligand Bonds
24.9K
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...
24.9K
02:42Valence Bond Theory
11.4K
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...
11.4K
02:57Coordination Number and Geometry
19.3K
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.
19.3K
03:02Colors and Magnetism
14.3K
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...
14.3K
02:58Crystal Field Theory - Octahedral Complexes
31.3K
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...
31.3K