相关实验视频
Updated: May 27, 2026

08:28
Single-molecule Manipulation of G-quadruplexes by Magnetic Tweezers
Published on: September 19, 2017
一个由四个交换偏差的单分子磁铁组成的超分子聚合物
Tu N Nguyen1, Wolfgang Wernsdorfer, Khalil A Abboud
1Department of Chemistry, University of Florida, Gainesville, Florida 32611-7200, USA.
Journal of the American Chemical Society
|December 6, 2011
概括
这项研究详细介绍了基于的新型高分子四聚合物的合成. 这个复合体表现出单分子磁铁行为,显示磁化的量子道化.
科学领域:
- 超分子化学 超分子化学
- 无机化学 无机化学 有机化学
- 磁电化学 磁电化学 磁电化学
背景情况:
- -氧气集群因其磁性特性而引起人们的兴趣.
- 单分子磁铁 (SMM) 是表现出磁性歇斯底里的分子单位.
研究的目的:
- 为了合成和描述一种新型的高分子复合物.
- 为了研究合成复合物的磁性和SMM行为.
主要方法:
- 3--1,5-bis(pyridin-2-yl) -1,5-二氧化物 (pdpdH(2)) 与三角形[Mn(III) ((3) O((2) CMe) (((py) ((3))) ((ClO ((4)) 的前体发生反应.
- 固态 dc 和 ac 磁感应度测量. 固态 dc 和 ac 磁感应度测量.
- 磁化与直流电场在单晶上进行扫描.
主要成果:
- 一个矩形的超分子四聚合物, [Mn(12) O(4) ((O(2) CMe) ((12) ((pdpd) ((6)) ] ((ClO(4)) ((4) (3) 被合成.
- 复合体3由四个[Mn(3) O](7+) 三角形单元组成,由二氧化物联体连接在一起.
- 四个单分子磁体 (SMM) 的单分子磁体 (Mn3) 与一个S = 6基态被确定在四重体内.
- 低于1K的歇斯底里循环证实了磁化的交换偏差量子道化.
结论:
- 合成的复合物是四个弱交换合的SMM单元的超分子聚合物.
- 该研究表明,通过较小的SMM单元的共价链接,复杂的SMM组件的形成.
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...
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.
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.
Ferromagnetism
Materials like iron, nickel, and cobalt consist of magnetic domains, within which the magnetic dipoles are arranged parallel to each other. The magnetic dipoles are rigidly aligned in the same direction within a domain by quantum mechanical coupling among the atoms. This coupling is so strong that even thermal agitation at room temperature cannot break it. The result is that each domain has a net dipole moment. However, some materials have weaker coupling, and are ferromagnetic at lower...
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,...
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...

