Abstract
The recent IUPAC recommendation on the definition of hydrogen bonding points out that directionality is a defining characteristic of a hydrogen bond and the angle ∠X-H-Y is generally linear or 180∘. It also suggests that the X-H⋯Y angle be greater than 110∘ for an interaction to be characterized as a hydrogen bond but does not provide any rationale for the same. This article reports a rationale for limiting the angle, based on the electron density topology using the quantum theory of atoms in molecules. Electron density topology for common hydrogen bond donors HF, HCl, HBr, HNC, HCN and HCCH are reported in this work. These calculations lead to an interesting observation that the atomic basins of H atom in all these donor molecules are limited justifying the restriction of hydrogen bond angle. Moreover, similar analysis on some hydrogen bonded complexes confirms that beyond this angle the acceptor atom Y starts interacting with the atomic basin on X. However, conclusions based on bond lengths and angles have to be treated with care and as the IUPAC recommendation points out that independent ‘evidence for bond formation’ in every case is important.
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Acknowledgments
Authors would like to thank the Super Computer Research Center and Inorganic and Physical Chemistry department at the Indian Institute of Science for providing good computational facilities and the Indo-French Centre for Promotion of Advanced Scientific Research for financial support. AS would like to thank Council of Scientific and Industrial Research (CSIR) for the fellowship. AS also thanks Sharon Priya Gnanasekar and Kabir Kumbhar for their help in calculations.
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AS is presently at the Institute of Chemistry, The Hebrew University of Jerusalem, Israel. 91904.
Special Issue on CHEMICAL BONDING
Celebrating 100 years of Lewis Chemical Bond
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SHAHI, A., ARUNAN, E. Why are Hydrogen Bonds Directional?. J Chem Sci 128, 1571–1577 (2016). https://doi.org/10.1007/s12039-016-1156-3
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DOI: https://doi.org/10.1007/s12039-016-1156-3