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Related Concept Videos

Van der Waals Equation01:10

Van der Waals Equation

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...
The Van der Waals Equation01:26

The Van der Waals Equation

The ideal gas law is based on two simplifying assumptions: first, that there are no intermolecular attractions between gas molecules, and second, that the volume occupied by the molecules themselves is negligible compared with the volume of the container. However, these assumptions don't hold up under all conditions - specifically, at high pressures and low temperatures, as gas tends to deviate from ideal gas behavior.The van der Waals equation is an enhanced version of the ideal gas law,...
Energy Associated With a Charge Distribution01:21

Energy Associated With a Charge Distribution

The work done to bring a charge through a distance r is given by the potential difference between the initial and the final position. To assemble a collection of point charges, the total work done can be expressed in terms of the product of each pair of charges divided by their separation distance, defined with respect to a suitable origin. Solving this expression gives the energy stored in a point charge distribution.
Van der Waals Interactions01:24

Van der Waals Interactions

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.Polar molecules have a partial positive charge on one end and a partial negative charge on the other end of the molecule,...
The Energies of Atomic Orbitals03:21

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
Thermodynamic Potentials01:26

Thermodynamic Potentials

Thermodynamic potentials are state functions that are extremely useful in analyzing a thermodynamic system. They have dimensions of energy. The four important thermodynamic potentials are internal energy, enthalpy, Helmholtz free energy, and Gibbs free energy. These thermodynamic potentials can be expressed using two of the following variables: pressure, volume, temperature, and entropy. These two variables are expressed as the rate of change of the thermodynamic potential with respect to other...

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Computation of Atmospheric Concentrations of Molecular Clusters from ab initio Thermochemistry
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Toward improved density functionals for the correlation energy.

Ajit J Thakkar1, Shane P McCarthy

  • 1Department of Chemistry, University of New Brunswick, Fredericton, New Brunswick E3B 5A3, Canada. ajit@unb.ca

The Journal of Chemical Physics
|October 10, 2009
PubMed
Summary
This summary is machine-generated.

This study tested density functionals for predicting electron correlation energies in atoms. New functionals show improved accuracy for heavier atoms, addressing limitations of existing methods.

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Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Materials Science

Background:

  • Accurate prediction of electron correlation energies is crucial for understanding atomic and molecular properties.
  • Existing density functionals often struggle with heavier elements and closed-shell systems.
  • Developing improved functionals is essential for advancing computational chemistry.

Purpose of the Study:

  • To evaluate the performance of eleven widely used density functionals for predicting nonrelativistic electron correlation energies.
  • To develop novel, few-parameter density functionals for improved accuracy, especially for heavier atoms.
  • To assess the impact of reparametrization on the performance of existing functionals.

Main Methods:

  • Testing eleven established density functionals on atoms (He-Ar), cations (Li+-K+), and (1)S state atoms (Ca-Rn).
  • Heuristically developing several new, few-parameter density functionals.
  • Reparametrizing existing functionals to assess performance improvements.

Main Results:

  • Existing density functionals exhibit poor performance for heavier atoms.
  • Reparametrization enhances accuracy for light atoms but not for heavier, closed-shell atoms.
  • Four newly developed functionals demonstrate qualitatively improved predictions for heavier atoms without sacrificing accuracy for lighter ones.

Conclusions:

  • Novel density functionals offer a promising approach to accurately predict electron correlation energies for a wider range of atoms.
  • Further advancements require reliable electron correlation energy data for more atoms, particularly heavy ones.
  • The developed functionals represent a step forward in computational chemistry for electronic structure calculations.