Thermodynamic characteristics of XeF2 stepwise defluorination reaction have been studied using sophisticated methods of quantum chemistry. The set of standard enthalpies of formation for the XeF2-related intermediates (radicals, ions) was obtained using approximation of coupled clusters level of theory [CCSD(T)/complete basis set extrapolation] with Peterson’s effective core potential correlation consistent basis sets for Xe. The standard enthalpy of formation for xenon monofluoride radical was determined to be ΔfH°(XeF) = 15.4 kcal mol−1 (298 K). The radical is formed in the first step of XeF2 homolytic decomposition which requires 59.7 kcal mol−1. The second step (XeF dissociation) is characterized by an extremely low binding energy (BDE(XeF) = 3.1 kcal mol−1) explaining the high fluorinating potential of the xenon difluoride. An interpretation of low XeF stability was given in terms of MO – AO correlation diagrams. It was shown that the electronic structure of XeF radical may be described as combination of two main configurations, the first of them has a canonical set of MOs with single-occupied HOMO of antibonding character, whereas the second configuration is characterized by low-lying SOMO with main contributions from 5S AO of Xe and 2pz AO of fluorine.
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