Chemical Bonding Theory and Electronic Structure Analysis

Chemical bonding theory offers a framework for understanding how atoms associate to form molecules and materials through the sharing, donation or redistribution of electrons. From the early valence‐bond and Lewis concepts to modern molecular orbital and density functional approaches, advances in theory have progressively refined our view of bond formation, bond order and reactivity. Electronic structure analysis complements this by providing quantitative insights into the distribution of electron density, the energy levels of molecular orbitals and the interplay of electrostatic, exchange and correlation forces. Together, these disciplines underpin rational design in fields as diverse as catalysis, materials science and drug discovery. Contemporary developments have emphasised unified descriptions of so-called covalent and noncovalent phenomena, the role of multicentre and electron‐deficient bonds in phase‐change materials, and the use of natural bond orbital and resonance analyses to connect intuitive bonding pictures with high‐level computational results. Such work has global significance in guiding the synthesis of novel functional materials, understanding biochemical interactions and optimising energy conversion processes.

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Chemical Bonding Theory and Electronic Structure Analysis publication trend

The graph below shows the total number of articles in chemical bonding theory and electronic structure analysis across all publications each year (not limited to Nature Index journals).

Technical terms

Valence‐bond theory: A model describing bonding as the overlap of atomic orbitals and paired electron spins between atoms.

Molecular orbital theory: A framework in which electrons occupy delocalised orbitals that extend over an entire molecule, forming bonding and antibonding combinations.

Density functional theory (DFT): A quantum mechanical method for computing electronic structure by expressing total energy as a functional of electron density.

Hypervalency: A bonding situation in which an atom appears to have more than eight electrons in its valence shell, often arising from multicentre or delocalised interactions.

σ-hole bond: A directional noncovalent interaction arising from an area of positive electrostatic potential opposite to a covalent bond, commonly observed in halogen, chalcogen or pnicogen chemistry.

Natural bond orbital (NBO) analysis: A computational tool that decomposes electronic structure into localized bonding descriptors closely aligned with Lewis resonance concepts.

References

1. “Noncovalent Interaction”: A Chemical Misnomer That Inhibits Proper Understanding of Hydrogen Bonding, Rotation Barriers, and Other Topics. Molecules (2023).
2. What Is the Nature of Supramolecular Bonding? Comprehensive NBO/NRT Picture of Halogen and Pnicogen Bonding in RPH2···IF/FI Complexes (R = CH3, OH, CF3, CN, NO2). Molecules (2019).
3. σ-Hole Bonds and the VSEPR Model—From the Tetrahedral Structure to the Trigonal Bipyramid. Sci (2022).
4. Electron-Deficient Multicenter Bonding in Phase Change Materials: A Chance for Reconciliation. Materials (2024).