Related Experiment Video
Updated: Jul 5, 2025

06:15
Interactive Molecular Model Assembly with 3D Printing
Published on: August 13, 2020
10.0K
Reliable Dimerization Energies for Modeling of Supramolecular Junctions
1Institute of Macromolecular Chemistry, Czech Academy of Sciences, Heyrovsky Square 2, 16200 Prague, Czech Republic.
International Journal of Molecular Sciences
|January 11, 2024
Summary
Accurate intermolecular interaction energy (ΔE) calculations are vital for organic electronics. A new "silver standard" method and a cost-effective DFT approach offer reliable predictions for noncovalent complexes.
Area of Science:
- Computational chemistry
- Materials science
- Quantum chemistry
Background:
- Accurate estimation of intermolecular interaction energy (ΔE) is essential for modeling organic electronic materials.
- Benchmark data for ΔE are needed to evaluate computational methods.
Purpose of the Study:
- To compile benchmark ΔE data for a diverse set of 50 dimers (Set50-50).
- To assess the performance of various density-functional theory (DFT) and localized coupled cluster methods against benchmark data.
- To identify cost-effective and reliable methods for calculating ΔE.
Main Methods:
- Focal-point strategy using coupled cluster theory with singles, doubles, and perturbative triples [CCSD(T)] with large basis sets.
- Extrapolation of energy components to the complete basis set (CBS) limit.
- Evaluation of DFT-based approaches and a localized CCSD(T) method on the Set50-50 dataset.
Main Results:
- A proposed "silver standard" approach (localized CCSD(T) with CBS extrapolations) achieves accuracy better than 2 kJ/mol for absolute ΔE values.
- The computationally inexpensive "ωB97X-3c/vDZP" DFT method demonstrated remarkable performance.
- Established benchmark data for 50 diverse dimers, including models of single-stacking junctions.
Conclusions:
- The "silver standard" method provides highly accurate ΔE values for noncovalent complexes.
- The ωB97X-3c/vDZP method offers a computationally efficient and reliable alternative for ΔE calculations.
- Findings facilitate cost-effective searches of potential energy surfaces for noncovalent interactions.
More Related Videos
Related Concept Videos
Bond Energies and Bond Lengths
25.3K
Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
25.3K
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
Bond Dissociation Energy and Activation Energy
8.9K
Bond energy is the energy required to break a bond homolytically. These values are usually expressed in units of kcal/mol or kJ/mol and are referred to as bond dissociation energies when given for specific bonds or average bond energies when indicated for a given type of bond over many compounds. Firstly, the bond dissociation energy for a single bond is weaker than that of a double bond, which in turn is weaker than that of a triple bond. Secondly, hydrogen forms relatively strong bonds with...
8.9K
Molecular Orbital Theory II
19.2K
Molecular Orbital Energy Diagrams
19.2K
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
Noncovalent Attractions in Biomolecules
50.8K
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,...
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,...
50.8K

