Theoretical Study Of Non-Covalent Interactions In Benzene And Substituted Benzene

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The role of non-covalent interaction in various physical, chemical, and biochemical processes are well known and, hence, have attracted many researchers towards their nature [1-5]. This has become one of the recent and major interests for computational chemistry to understand and characterize varieties of non-covalent interaction.

Among these noncovalent interactions, the hydrogen bond is mostly analyzed due to its critical role in stabilizing various supramolecular framework, in proton transfer reactions, crystal engineering, and others [6-9].  However, recently halogen-substituted (mostly fluorine) molecules have been found to increase the role of other types of interaction and are becoming an expanding area of both experimental and theoretical research [10-13].

While the interaction of benzene with water takes place via the hydrogen atom of water and the π cloud of benzene, the interaction of water with fluorinated benzene takes place via the lone pair of the oxygen atom of water and π cloud of benzene of benzene (Scheme 1).  This lone pair-π interaction has recently been verified both theoretically and experimentally [12]. The first experimental proof of the lone pair pair-π interaction was provided by Reedijk and co-workers in 2004 in the complex between Cl and pyridine [14]. Meyer and co-workers [15] in the same year reported experimental evidence for the stabilizing interaction between Cl- and triazine igniting further theoretical and experimental investigations in this area. Recently, rotational spectroscopy coupled with theoretical calculations have provided an unambiguous evidence of the lone pair-π hole interaction between the oxygen atom of water and the π cloud of fluorinated benzene (Scheme 1b) [12,16].

Scheme 1. Interactions between (a) benzene-water system and (b) hexafluoro benzene-water system.

The formation of this lone pair-π interaction is facilitated by the inductive effect of fluorine atoms, which withdraws electron density from the benzene ring and creates a “hole” in the region perpendicular to the molecular framework. This region of this hole can attract lone pairs of oxygen atoms and leads to the formation of this lone pair-π interaction. Thus, it seems that this lone pair-π interaction is also competitive with the traditional hydrogen bonds in stabilizing many supramolecular framework. Inspired by this finding, we have undertaken a detailed theoretical study on the structure, energy, and topology of electron density of some selected molecules, as shown in Scheme 2. The molecules considered in this study are benzene (B), hexafluorobenzene (HFB), hexacyanobenzene (HCB), and 1,3,5-trinitrobenzene (TNB), and we considered their interaction with the lone pair as well as hydrogen bond donors such as H2O, NH3, HF and HCl.

Scheme 2. Selected molecules for the present study having π…X interaction.

The interaction of these molecules with benzene takes place via the H atoms of H2O, NH3, HF, HCl and the π cloud of benzene implying that the π cloud of benzene is acting like a heap of electron density which attracts the electropositive H atom of these molecules. On the other hand, the introduction of electron withdrawing substituents such as F, CN, NO2 etc. to benzene makes the aromatic surface electron deficient which then attracts the lone pair region of H2O, NH3, HF, HCl molecules. Thus, the aromatic surface of these substituted benzenes is acting like a heap. Both electrostatic, as well as dispersion, are the dominating contributors to the attractive interaction. The dominance of dispersion interactions points towards the free rotation of H2O, NH3, HF, and HCl molecules, which are also in accordance with the recent experimental observation [12].

These findings are described in the article entitled Non-covalent interaction in benzene and substituted benzene: A theoretical study, recently published in the journal Computational and Theoretical ChemistryThis work was conducted by Chayanika Kashyap, Sabnam S. Ullah, Lakhya J. Mazumder, and Ankur Kanti Guha from Cotton University.


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