金属化物形成强键和键:测量溶液中的相互作用和
Stefano Libri1, Naseralla A Jasim, Robin N Perutz
1Department of Chemistry, University of Sheffield, Sheffield S3 7HF UK.
Journal of the American Chemical Society
|May 30, 2008
概括
这项研究表明,一种特定的化合物作为溶液中和素键的强受体. 这些发现量化了素键的强度,表明它在超分子化学应用中与键相竞争.
科学领域:
- 有机金属化学 有机金属化学
- 超分子化学 超分子化学
- 化学物理 化学物理
背景情况:
- 有机金属化合物可以参与非共价相互作用.
- 关于素键的能量学的实验数据很少.
- 了解分子间力量对于分子设计至关重要.
研究的目的:
- 为了研究和烯酸二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二二
- 用模型和素键捐赠者实验确定NiF的结合常数,和.
- 用实验数据比较素键与键的强度.
主要方法:
- 合成和表征有机金属化合物NiF的合成和表征.
- 多核核核磁共振光谱测试以确认相互作用类型.
- 19F在不同的溶剂 (托卢-d8,) 中进行NMR定位实验,以量化结合亲和度和热力学参数.
主要成果:
- NiF作为一个强大的键接受器与内醇,形成1:1和2:1复合体具有显著的结合和.
- 尼作为一种素键受体与酸,形成1:1和2:1复合体,其热力学参数取决于溶剂.
- 发现与NiF的键相互作用与键相互作用具有竞争力.
结论:
- NiF中的化物联体是溶液中和素键的有效受体位点.
- 提供了素键的实验热力学数据,作为理论研究的基准.
- 这些发现突显了NiF在超分子化学和晶体工程中的潜力,因为它具有强大的分子间相互作用能力.
更多相关视频
09:32A New Straightforward Method for Lipophilicity (logP) Measurement using 19F NMR Spectroscopy
Published on: January 30, 2019
12:05Preparation of Hydrophobic Metal-Organic Frameworks via Plasma Enhanced Chemical Vapor Deposition of Perfluoroalkanes for the Removal of Ammonia
Published on: October 10, 2013
相关概念视频
03:13Intermolecular Forces
Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
03:13Intermolecular Forces
Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
03:37Molecular Shape and Polarity
Dipole Moment of a Molecule
03:01Halogens
Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. Astatine is a highly unstable radioactive element, so currently, most of its properties are unknown due to its short half-life. Tennessine is a synthetic element also predicted to be in this group.
01:04Hydrogen Bonds
A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
00:26Hydrogen Bonds
Hydrogen BondsHydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.Hydrogen Bonds Control the World!Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are...