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相关概念视频

Molecular Orbital Theory I02:35

Molecular Orbital Theory I

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Overview of Molecular Orbital Theory
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Molecular Orbital Theory II03:51

Molecular Orbital Theory II

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Molecular Orbital Energy Diagrams
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Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation04:01

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

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Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and molecular formula problems to determining the density and molar mass of a gas. However, the behavior of a gas is often non-ideal, meaning that the observed relationships between its pressure, volume, and temperature are not accurately described by the gas laws.
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Van der Waals Equation01:10

Van der Waals Equation

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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...
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Valence Bond Theory and Hybridized Orbitals02:38

Valence Bond Theory and Hybridized Orbitals

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According to valence bond theory, a covalent bond results when: (1) an orbital on one atom overlaps an orbital on a second atom, and (2) the single electrons in each orbital combine to form an electron pair. The strength of a covalent bond depends on the extent of overlap of the orbitals involved. Maximum overlap is possible when the orbitals overlap on a direct line between the two nuclei.
A σ bond (single bond in a Lewis structure) is a covalent bond in which the electron density is...
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The Quantum-Mechanical Model of an Atom02:45

The Quantum-Mechanical Model of an Atom

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Shortly after de Broglie published his ideas that the electron in a hydrogen atom could be better thought of as being a circular standing wave instead of a particle moving in quantized circular orbits, Erwin Schrödinger extended de Broglie’s work by deriving what is now known as the Schrödinger equation. When Schrödinger applied his equation to hydrogen-like atoms, he was able to reproduce Bohr’s expression for the energy and, thus, the Rydberg formula governing hydrogen spectra.
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Computation of Atmospheric Concentrations of Molecular Clusters from ab initio Thermochemistry
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真实空间哈伯德纠正密度的功能理论.

Sayan Bhowmik1, Andrew J Medford1, Phanish Suryanarayana1,2

  • 1College of Engineering, Georgia Institute of Technology, Atlanta, Georgia 30332, USA.

The Journal of chemical physics
|December 17, 2025
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概括
此摘要是机器生成的。

我们开发了一个快速,准确的真实空间框架,用于哈伯德纠正密度函数理论 (DFT) 的计算. 这种计算方法显著优于大型系统的现有方法,使新材料的发现.

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Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics
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科学领域:

  • 计算材料科学 计算材料科学
  • 量子化学是一种量子化学.
  • 固态物理 固态物理

背景情况:

  • 密度函数理论 (DFT) 是一种强大的量子力学建模方法.
  • 准确的DFT计算往往需要大量的计算资源,特别是对于高度相关的材料.
  • 实时空间方法提供了传统的互换空间 (平面波) 方法的替代方案.

研究的目的:

  • 开发一个准确和有效的真实空间框架,用于哈伯德纠正的DFT.
  • 实施和并行化大型计算的框架.
  • 调查交换相关性不一致性的影响,并优化哈伯德参数.

主要方法:

  • 能量,原子力和应力张量为实空间有限差异离散的公式.
  • 制定框架的大规模并行实施方案.
  • 根据已建立的平面波方法进行验证,并应用于TiO2多态.

主要成果:

  • 哈伯德校正的现实空间DFT框架提供了与平面波方法相比较准确的结果.
  • 该实现表现出高效率和可扩展性,在解决时间上超过一个数量级的平面波代码.
  • 性能优势随着系统大小和处理器数量的增加而增加.
  • 该框架用于研究交换相关性不一致性,并优化Hubbard对TiO2.2的参数.

结论:

  • 开发的真实空间Hubbard纠正的DFT框架是准确的,高效的,并且具有高度可扩展性.
  • 这种计算工具可显著加快材料模拟,特别是对于大型和复杂的系统.
  • 这种方法促进了对电子结构和材料性能的先进研究,有助于发现新材料.