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相关概念视频

Molecular Shapes01:18

Molecular Shapes

Molecules have characteristic shapes that are crucial for their function. The arrangement of various electron groups around the central atom dictates their molecular geometry. Electron pairs in the valence shell of a central atom will adopt an arrangement that minimizes repulsions between the electron pairs by maximizing the distance between them. The valence electrons form either bonding pairs, located primarily between bonded atoms, or lone pairs.Two regions of electron density in a diatomic...
Molecular Orbital Theory I02:35

Molecular Orbital Theory I

Overview of Molecular Orbital Theory
Molecular Orbital Theory II03:51

Molecular Orbital Theory II

Molecular Orbital Energy Diagrams
Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...
MO Theory and Covalent Bonding02:40

MO Theory and Covalent Bonding

The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...

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相关实验视频

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Ultrahigh Density Array of Vertically Aligned Small-molecular Organic Nanowires on Arbitrary Substrates
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Ultrahigh Density Array of Vertically Aligned Small-molecular Organic Nanowires on Arbitrary Substrates

Published on: June 18, 2013

在一维有机纳米结构中的分子相互作用.

Thuc-Quyen Nguyen1, Richard Martel, Phaedon Avouris

  • 1Department of Chemistry, Columbia University, New York, New York 10027 USA. tqn@chem.columbia.edu

Journal of the American Chemical Society
|April 22, 2004
PubMed
概括

六次替代的芳香分子通过pi-pi相互作用和键自组合成一维的分子纳米结构. 溶剂选择和分子替代剂允许调整这些纳米结构用于表面应用.

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:

  • 分子自我组装对于创建先进材料至关重要.
  • 六基替代芳香物为纳米结构形成提供可调节的特性.

研究的目的:

  • 为了研究六次替代芳香物的自我组装成一维 (1D) 的分子纳米结构.
  • 了解分子间相互作用 (pi-pi和键) 在驱动这种组件中的作用.
  • 探索控制纳米结构形成和表面沉积的方法.

主要方法:

  • 稳态和时间分辨率光谱学.
  • 扫描电子显微镜 (SEM) 和原子力显微镜 (AFM).
  • 基于溶液的自组装和溶液造技术.

主要成果:

  • 在溶液中形成了六基替代芳香物的有序的柱状堆.
  • 纳米结构的特性 (数量,大小,结构) 取决于所使用的溶剂.
  • 通过修改替代剂和溶剂选择,可以调整分子间相互作用.
  • 通过溶液造成功将1D堆转移到表面.

结论:

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  • 分子间相互作用,特别是pi-pi和结合,是从六次替代芳化合物中形成1D纳米结构的关键.
  • 溶剂和替代剂工程为纳米结构的形成和特性提供了有效的控制.
  • 开发的方法允许在各种表面上直接准备分子纳米结构.