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Force can be calculated from the expression for potential energy, which is a function of position. The component of a conservative force, in a particular direction, equals the negative of the derivative of the corresponding potential energy with respect to the displacement in that direction. For regions where potential energy changes rapidly with displacement, the work done and force is maximum. Also, when force is applied along the positive coordinate axis, the potential energy decreases with...
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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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The molecular orbital theory describes the distribution of electrons in molecules in a manner similar to the distribution of electrons in atomic orbitals. The region of space in which a valence electron in a molecule is likely to be found is called a molecular orbital. Mathematically, the linear combination of atomic orbitals (LCAO) generates molecular orbitals. Combinations of in-phase atomic orbital wave functions result in regions with a high probability of electron density, while...
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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...
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A general transformation to canonical form for potentials in pairwise interatomic interactions.

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This study introduces a new method to understand chemical and intermolecular bonds using a canonical potential. It reveals a unified perspective on bonding, suggesting no fundamental difference between various bond types.

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Area of Science:

  • Physical Chemistry
  • Computational Chemistry
  • Chemical Physics

Background:

  • Understanding interatomic and intermolecular forces is crucial in chemistry.
  • Existing models often treat different bond types (covalent, van der Waals, hydrogen) distinctly.

Purpose of the Study:

  • To introduce a generalized force-based transformation formulation.
  • To investigate the concept of a canonical potential for chemical and intermolecular bonding.
  • To provide a unified perspective on the nature of interatomic interactions.

Main Methods:

  • Developed a generalized formulation of explicit force-based transformations.
  • Applied transformations to reference various ground electronic state pairwise interatomic interactions.
  • Analyzed accurately determined potentials of diatomic molecules (H2, H2(+), HF, LiH) and model systems (Ar dimer, Ar-HBr, OC-HF, OC-Cl2).

Main Results:

  • Demonstrated the application of canonical potential transformations to diverse bonding scenarios.
  • Accurately evaluated equilibrium dissociation energies for the studied systems.
  • Illustrated a unified perspective on intermolecular interactions, challenging traditional classifications.

Conclusions:

  • The canonical potential approach offers a unified framework for understanding diverse chemical bonds.
  • This formulation highlights the lack of fundamental distinction between covalent, van der Waals, hydrogen, and halogen bonds.
  • The method provides advantages for accurate energy calculations and a new conceptualization of bonding.