相关实验视频
Updated: Jul 18, 2026

10:44
Preparation of Carbon Nanosheets at Room Temperature
Published on: March 8, 2016
基聚离子 (C6H6) 的气相离子流动性和结构n+,n = 2-6 基聚离子 (C6H6) n+,n = 2-6
Mark J Rusyniak1, Yehia M Ibrahim, Douglas L Wright
1Department of Chemistry, Virginia Commonwealth University, Richmond, Virginia 23284-2006, USA.
Journal of the American Chemical Society
|September 25, 2003
概括
使用离子流动性和理论计算确定了基聚酸 ((C(6) H(6)) (((n) (((+)) 结构. 饼剪切器堆核心是较小的集群的首选,而较大的集群采用具有三明治二元核心的二元体结构.
科学领域:
- 物理化学 物理化学
- 计算化学计算化学
- 纳米材料是一种纳米材料.
背景情况:
- 了解分子团的结构性质对于各种科学学科至关重要.
- 烯集群作为基本的芳香系统,为分子间相互作用和自我组装提供了洞察力.
- 之前的研究已经探讨了烯集群结构,但对阴离子结构的实验性确定仍然具有挑战性.
研究的目的:
- 为了确定团的三维结构 ((C(6) H(6)) ((n) ((+),n = 2-6).
- 研究分子间相互作用在团的形成和稳定性中的作用.
- 为了将实验性离子运动数据与结构阐明的理论计算相关联.
主要方法:
- 通过脉冲超音速光束扩张生成烯集群.
- 电子冲击的电离,其次是质量选择.
- 在缓冲气体中测量离子流动性.
- 密度函数理论 (DFT) 计算和蒙特卡洛最小能量搜索.
主要成果:
- 二聚离子 ((C(6) H(6)) (((2) ((+)) 呈现出稳定的三明治配置,通过实验横截断证实了这一点.
- 具有n = 3-6的烯集群显示至少有两个结构异构体,其中饼形堆核心被确定为最低能量的结构.
- 较大的集群 (n >= 14) 显示神奇的数字,暗示形成高度对称的二面体结构.
结论:
- 充电的芳香-芳香相互作用中的平行堆叠图案显著影响了多芳香系统的结构.
- 这些发现提供了对芳香集群中自我组装原理的更深入的理解.
- 这项研究为分子设计和涉及芳香系统的识别提供了宝贵的见解.
相关概念视频
Molecular Shape and Polarity
Dipole Moment of a Molecule
Intermolecular 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...
Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility
Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
Intermolecular 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...
Structure and Bonding of Alkenes
Olefins, which are unsaturated hydrocarbons containing one or more carbon–carbon double bonds, are broadly divided into alkenes and cycloalkenes. The general chemical formula of an alkene is CnH2n.
Doubly bonded carbons are sp2 hybridized and have a trigonal planar geometry. The double bond is composed of a σ bond formed by the overlap of hybrid orbitals and a π bond produced by the lateral overlap of unhybridized 2p orbitals on both the carbons. Each carbon atom is bonded to two hydrogen atoms...
Doubly bonded carbons are sp2 hybridized and have a trigonal planar geometry. The double bond is composed of a σ bond formed by the overlap of hybrid orbitals and a π bond produced by the lateral overlap of unhybridized 2p orbitals on both the carbons. Each carbon atom is bonded to two hydrogen atoms...
Structure of Benzene: Molecular Orbital Model
According to the molecular orbital (MO) model, benzene has a planar structure with a regular hexagon of six sp2 hybridized carbons. As shown in Figure 1, each carbon is bonded to three other atoms with C–C–C and H–C–C bond angles of 120°. The C–H bond length is 109 pm, and the C–C bond length is 139 pm which is midway between the single bond length of sp3 hybridized carbons (154 pm) and sp2 hybridized carbons (133 pm).

