金 (I),银 (I) 和铜 (I) 的复合物与五[60]富勒化物
Merissa Halim1, Robert D Kennedy, Mitsuharu Suzuki
1Department of Chemistry and Biochemistry, University of California, Los Angeles, California 90095-1569, USA.
Journal of the American Chemical Society
|April 12, 2011
概括
合成了新的黄金,银和铜氨酸复合物,其中含有五甲基富勒化物. 这些金属复合体表现出多样化的协调模式,银复合体表现出意想不到的相互作用和由于富勒化绝缘屏蔽的增强稳定性.
科学领域:
- 有机金属化学 有机金属化学
- 富勒烯的化学结构
- 协调化学 协调化学
背景情况:
- 富勒烯衍生物是材料科学中的多功能构建模块.
- 金属斯复合体提供可调节的电子和硬质性质.
- 了解金属富勒烯相互作用对于开发新的功能性材料至关重要.
研究的目的:
- 为了合成和表征新型的黄金,银和铜,五[60]富勒的素复合物.
- 为了研究富勒的环丁烯环和金属中心之间的协调模式.
- 探索这些独特的金属富勒烯化合物的结构和电子特性.
主要方法:
- 金 ((I),银 ((I) 和铜 ((I) 氨酸复合物的合成.
- 频谱学表征 (NMR,IR,质谱学).
- 单晶X射线衍射分析.
- 密度函数理论 (DFT) 的计算.
主要成果:
- 成功合成和表征了七种金属富勒化物复合物.
- 观察到不同的协调模式:金的 η(1) 到 η(3),银的 η(2)/η(3) 和铜的 η(5).
- 结晶学数据显示出意想不到的Ag ((I) 协调到富勒里德环环.
- 用富勒里德1a和1b进行绝缘屏蔽,使得稀有Ag ((I) 环二烯的稳定和表征成为可能.
- DFT计算提供了对几何和电子结构的洞察.
结论:
- 这项研究提出了具有多样化协调化学的新型金属富勒化物复合物.
- 富勒的绝缘质量是稳定不寻常的银复合物的关键.
- 这些发现有助于理解金属富勒烯相互作用,并为新材料设计打开了道路.
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...
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.
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...
Formation of Complex Ions
A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
Complexation Equilibria: The Chelate Effect
In complexation reactions, metal atoms or cations interact with ligands to form donor-acceptor adducts called metal complexes. Ligands that bind through one donor site are monodentate, ligands with two donor sites are bidentate, and those with more than two donor sites are polydentate ligands. For example, ethylene diamine is a bidentate ligand that binds through two nitrogen donor atoms, forming a five-membered ring. EDTA is a polydentate ligand that binds through four oxygen and two nitrogen...
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.

