随机相近似方法的一般性扰动单项校正:对封闭和开放二分体的非共价相互作用能量的影响
Pulkit Joshi1, Vamsee K Voora1
1Department of Chemical Sciences, Tata Institute of Fundamental Research, Homi Bhabha Road, Colaba, Mumbai 400005, India.
The Journal of chemical physics
|January 23, 2024
概括
我们开发了一种新的方法来改进对弱键分子的相互作用能量计算. 这种RPA单项 (RPAS) 校正显著提高了开系统的准确性,在非共价相互作用中实现了化学准确性.
科学领域:
- 计算化学是一种计算化学.
- 量子化学是一种量子化学.
- 理论化学是一种理论化学.
背景情况:
- 后科恩-沙姆 (KS) 随机相近似 (RPA) 由于近似KS函数的密度错误,与弱结合分子的相互作用能量作斗争.
- 准确计算非共价相互作用对于理解分子行为和化学反应至关重要.
研究的目的:
- 为RPA方法的扰动单项 (pS) 校正开发一个通用的形式主义.
- 改进对弱键分子,特别是开系统的相互作用能量的描述.
主要方法:
- 开发了一种通用形式主义,使用轨道旋转作为扰动参数进行扰动单元 (pS) 校正.
- 提出了一个特定的ps方案,RPA单元 (RPAS) [哈特里-福克 (HF) ],利用RPA轨道旋转梯度和时间依赖的哈特里-福克 (HF) 赫西安.
- 将RPAS (HF) 校正应用于封闭和开放的二次体,以评估非共价相互作用能量.
主要成果:
- RPAS (HF) 校正显著降低了非对应相互作用能量的错误,无论是封闭的还是开放的二次体.
- 对于开二元体,RPAS (HF) 与标准RPA方法相比,在各种相互作用类型 (结合,金属溶剂,碳溶剂,分散) 中,始终可以将误差降低50%或更多.
- 发现扰乱性单个校正对于减少错误比RPA方法的更高阶交换校正更为关键.
结论:
- 经RPAS (HF) 校正的RPA方法在开系统中实现非共价相互作用的化学精度.
- 这种超RPA校正比其他扰动方案和分散校正密度函数近似更可靠,使其成为准确计算化学的宝贵工具.
- 开发的形式主义提供了一个强大的方法来提高基于RPA的方法的准确性,用于研究分子相互作用.
更多相关视频
05:51Isotopic Effect in Double Proton Transfer Process of Porphycene Investigated by Enhanced QM/MM Method
Published on: July 19, 2019
6.2K
08:04Excitonic Hamiltonians for Calculating Optical Absorption Spectra and Optoelectronic Properties of Molecular Aggregates and Solids
Published on: May 27, 2020
8.4K
相关概念视频
Molecular Geometry and Dipole Moments
13.0K
The VSEPR theory can be used to determine the electron pair geometries and molecular structures as follows:
13.0K
VSEPR Theory and the Effect of Lone Pairs
42.3K
Effect of Lone Pairs of Electrons on Molecule Geometry
42.3K
Free Energy Changes for Nonstandard States
11.4K
The free energy change for a process taking place with reactants and products present under nonstandard conditions (pressures other than 1 bar; concentrations other than 1 M) is related to the standard free energy change according to this equation:
where R is the gas constant (8.314 J/K·mol), T is the absolute temperature in kelvin, and Q is the reaction quotient. This equation may be used to predict the spontaneity of a process under any given set of conditions.
Reaction Quotient...
where R is the gas constant (8.314 J/K·mol), T is the absolute temperature in kelvin, and Q is the reaction quotient. This equation may be used to predict the spontaneity of a process under any given set of conditions.
Reaction Quotient...
11.4K
Van der Waals Interactions
64.0K
Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions between particles with permanent, partial, or temporary charges. The intermolecular forces between neutral atoms and molecules are ion–dipole, dipole–dipole, and dispersion forces, collectively known as van der Waals forces.
64.0K
Molecular Orbital Theory II
19.2K
Molecular Orbital Energy Diagrams
19.2K
Van der Waals Equation
4.1K
The ideal gas law is an approximation that works well at high temperatures and low pressures. The van der Waals equation of state (named after the Dutch physicist Johannes van der Waals, 1837−1923) improves it by considering two factors.
First, the attractive forces between molecules, which are stronger at higher densities and reduce the pressure, are considered by adding to the pressure a term equal to the square of the molar density multiplied by a positive coefficient a. Second, the volume...
First, the attractive forces between molecules, which are stronger at higher densities and reduce the pressure, are considered by adding to the pressure a term equal to the square of the molar density multiplied by a positive coefficient a. Second, the volume...
4.1K
