在它们的组装过程中,具有不同中心金属原子的结构相同的棒状宏离子在组装过程中自我识别
Panchao Yin1, Jin Zhang, Tao Li
1Department of Chemistry, Lehigh University, Bethlehem, Pennsylvania 18015, USA.
Journal of the American Chemical Society
|March 1, 2013
概括
两种相似的宏子自组装成不同的结构,即使混合. 这种由微妙的电荷差异驱动的自我识别,突出了选择性分子组合.
科学领域:
- 超分子化学 超分子化学
- 材料科学是一种材料科学.
- 纳米技术 纳米技术
背景情况:
- 宏离子是带电的大分子,在自组装中具有潜在的应用.
- 了解自组装机制对于设计先进材料至关重要.
- 生物系统表现出了显著的自我识别和自我组装现象.
研究的目的:
- 为了研究两个具有不同中心金属原子的类似宏子的自我组装行为.
- 探索密切相关的宏观体之间的自我识别现象.
- 阐明选择性自组装背后的驱动力和机制.
主要方法:
- 合成和表征两个棒状的宏子: ((C4H9) 4N) 7[Mo6O18NC(OCH2) 3XMo6O18(OCH2) 3CNMo6O18 (X = Mn(III) (1),Fe(III) (2)).它们的合成和表征.
- 在稀释溶液中观察自我组装成"黑"类型的超分子结构.
- 在混合溶液中使用动态光散射 (DLS),静态光散射 (SLS) 和带有能量散射X射线光谱 (TEM/EDS) 的传输电子显微镜进行自我组装的分析.
- 使用密度函数理论 (DFT) 和解离实验进行理论计算,以了解电荷分布差异.
主要成果:
- 这两种宏单独自我组装成同质的"黑"类型的超分子结构.
- 值得注意的是,这两种巨表现出自我分类,并在混合溶液中形成单独的同质组件,证明了自我识别.
- 这种自我识别被归因于由中心的Mn (III) 和Fe (III) 原子引起的电荷分布的轻微差异,加上组装的高激活能量.
- 电静电吸引被确定为驱动力,对微妙的宏观离子差异敏感.
结论:
- 远距离的对电离子介导的静电吸引使相似的宏离子之间能够进行选择性自我组装.
- 观察到的自我识别现象为理解生物系统中类似行为提供了一个模型.
- 这项工作表明,基于微小的结构变化,在超分子组合中存在微妙选择性的潜力.
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...
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...
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...
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...
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...
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.


