Crystallographic searches for weak interactions – the limitations of data mining

Schneider, Hans Jorg

doi:10.1107/s2052520618007783

Cited by 3 publications

(2 citation statements)

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“…The answer to the second question is "yes". The obvious reason for this is that van der Waals complexes usually have a weak binding energy of less than -1.0 kcal mol −1 [92][93][94][95][96][97][98]. The importance of such weakly bound interactions have been much appreciated in many fields including polymer science, biology, and crystal engineering [92][93][94][95][96][97][98].…”

Section: Figurementioning

confidence: 99%

“…The obvious reason for this is that van der Waals complexes usually have a weak binding energy of less than -1.0 kcal mol −1 [92][93][94][95][96][97][98]. The importance of such weakly bound interactions have been much appreciated in many fields including polymer science, biology, and crystal engineering [92][93][94][95][96][97][98]. For instance, van der Waals interactions are always weaker than any other chemical interaction and are the determinant of structure of proteins or even the overall shape of polymer structures [92,95,96,98] and the significance of such weakly bound interactions cannot be overlooked thus assuming that only strong interactions are significant for materials design and weak interactions do not play an important role in the field of noncovalent interactions.…”

Section: Figurementioning

confidence: 99%

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Does Chlorine in CH3Cl Behave as a Genuine Halogen Bond Donor?

Varadwaj

Marques

2020

Crystals

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The CH3Cl molecule has been used in several studies as an example purportedly to demonstrate that while Cl is weakly negative, a positive potential can be induced on its axial surface by the electric field of a reasonably strong Lewis base (such as O=CH2). The induced positive potential then has the ability to attract the negative site of the Lewis base, thus explaining the importance of polarization leading to the formation of the H3C–Cl···O=CH2 complex. By examining the nature of the chlorine’s surface in CH3Cl using the molecular electrostatic surface potential (MESP) approach, with MP2/aug-cc-pVTZ, we show that this view is not correct. The results of our calculations demonstrate that the local potential associated with the axial surface of the Cl atom is inherently positive. Therefore, it should be able to inherently act as a halogen bond donor. This is shown to be the case by examining several halogen-bonded complexes of CH3Cl with a series of negative sites. In addition, it is also shown that the lateral portions of Cl in CH3Cl features a belt of negative electrostatic potential that can participate in forming halogen-, chalcogen-, and hydrogen-bonded interactions. The results of the theoretical models used, viz. the quantum theory of atoms in molecules; the reduced density gradient noncovalent index; the natural bond orbital analysis; and the symmetry adapted perturbation theory show that Cl-centered intermolecular bonding interactions revealed in a series of 18 binary complexes do not involve a polarization-induced potential on the Cl atom.

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