Ketten, Leitern und Schichten durch Halogen‐Halogen‐ und Halogen‐Wasserstoff‐Wechselwirkungen

Abstract

Intermolekulare Wechselwirkungen werden traditionell nach der Art der zugrundeliegenden energetischen Beziehung klassifiziert: Wasserstoffbriickenbindungen, van-der-Waals-Wechselwirkungen, Charge-Transfer-Krafte etc. [

Orthogonal Multipolar Interactions in Structural Chemistry and Biology

“…On the one hand, the array of simultaneous halogen···halogen and hydrogen···halogen interactions formed by aromatic compounds carrying a halogen substituent ortho to an unsubstituted position, has been shown to build up molecular chains, ladders, and twodimensional sheets in the crystal state. [48] On the other hand, a triangular interaction motif, in which three halogen atoms are located in short contact distance with respect to each other forming an equilateral triangle has been repeatedly reported as a useful synthon for the engineering of crystals or the assembly of host-guest complexes. [49]…”

Substitution Effect on Crystal Packings of Iodobenzonitriles and Iodophenols

“…The hydrogen atom is the most common electron acceptor site, and hydrogen bonding is by far the most frequently occurring noncovalent interaction in recognition processes. But a number of weaker and softer interactions, such as X···X synthons with X = halogen, nitro, or cyano, also have been shown to play a role in structure stabilization. − The nature of halogen−halogen interactions in crystals has long been a matter of interest and debate. Intermolecular interactions associated with distances shorter than the sum of the van der Waals radii of contacting atoms have been variously referred to earlier as “donor−acceptor” interactions and, more recently, as interactions between the highest occupied molecular orbitals (HOMO−LUMO). − …”

Axial Chirality and Supramolecular Interactions: The Case of [(κ2-P,P-{PPh2NMe}2CO)CuICl]2

“…The two copper atoms are 315.3 pm apart and thus too far to consider a bonding interaction. The Cl−Cl distance at 349.5 pm is equally too long. , The copper atoms have the usual tetrahedral coordination, with the two phosphorus atoms of the ligand occupying the remaining two coordination sites. Thus, each ligand forms a six-membered ring with the respective copper atom.…”