The Hydrogen Bond in the Solid State

Angewandte Chemie International EditionVolume 41, Issue 1 p. 48-76 Review The Hydrogen Bond in the Solid State Thomas Steiner Dr., Thomas Steiner Dr. steiner@chemie.fu-berlin.de Institut für Chemie—Kristallographie Freie Universität Berlin Takustrasse 6, 14195 Berlin, Germany, Fax: (+49) 30-838-56702Search for more papers by this author Thomas Steiner Dr., Thomas Steiner Dr. steiner@chemie.fu-berlin.de Institut für Chemie—Kristallographie Freie Universität Berlin Takustrasse 6, 14195 Berlin, Germany, Fax: (+49) 30-838-56702Search for more papers by this author First published: 02 January 2002 https://doi.org/10.1002/1521-3773(20020104)41:1<48::AID-ANIE48>3.0.CO;2-UCitations: 4,653Read the full textAboutPDF ToolsRequest permissionExport citationAdd to favoritesTrack citation ShareShare Give accessShare full text accessShare full-text accessPlease review our Terms and Conditions of Use and check box below to share full-text version of article.I have read and accept the Wiley Online Library Terms and Conditions of UseShareable LinkUse the link below to share a full-text version of this article with your friends and colleagues. Learn more.Copy URL Share a linkShare onFacebookTwitterLinked InRedditWechat Abstract A difficult dividing line: The hydrogen bond is the most important of all the directional intermolecular interactions (see picture). It is understood from modern bonding concepts as a very broad phenomenon with open borders to other interactions, such as covalent bonding, ionic, cation–π, and van der Waals interactions. There are dozens of different types of X−H⋅⋅⋅A hydrogen bonds (A=acceptor) with dissociation energies that span more than two orders of magnitude. This review brings together the research of the last ten years on hydrogen bonds, particularly in the solid state. Abstract The hydrogen bond is the most important of all directional intermolecular interactions. It is operative in determining molecular conformation, molecular aggregation, and the function of a vast number of chemical systems ranging from inorganic to biological. Research into hydrogen bonds experienced a stagnant period in the 1980s, but re-opened around 1990, and has been in rapid development since then. In terms of modern concepts, the hydrogen bond is understood as a very broad phenomenon, and it is accepted that there are open borders to other effects. There are dozens of different types of X−H⋅⋅⋅A hydrogen bonds that occur commonly in the condensed phases, and in addition there are innumerable less common ones. Dissociation energies span more than two orders of magnitude (about 0.2–40 kcal mol−1). Within this range, the nature of the interaction is not constant, but its electrostatic, covalent, and dispersion contributions vary in their relative weights. The hydrogen bond has broad transition regions that merge continuously with the covalent bond, the van der Waals interaction, the ionic interaction, and also the cation–π interaction. All hydrogen bonds can be considered as incipient proton transfer reactions, and for strong hydrogen bonds, this reaction can be in a very advanced state. In this review, a coherent survey is given on all these matters. Citing Literature Volume41, Issue1January 4, 2002Pages 48-76 RelatedInformation