The IR spectra (4000-400 cm-1) of COF2/BF3 mixtures, dissolved in liquefied argon (LAr), krypton
(LKr), and nitrogen (LN2), have been examined. In all spectra evidence was found for the formation of a 1:1
van der Waals complex. Using spectra recorded at several temperatures between 81 and 172 K the complexation
enthalpies ΔH° in LAr, LKr, and LN2 were determined to be −11.8(3), −10.6(3), and −7.8(3) kJ mol-1,
respectively. A theoretical study, using both density functional theory at the B3LYP/6-311++G(d,p) level
and ab initio at the MP2/aug-cc-pVTZ level, indicates that the complexation can occur either via the oxygen
or via a fluorine atom of COF2. From a comparison of the experimental and calculated frequencies it was
concluded that the observed complex bands are due to a species in which the boron atom coordinates with the
oxygen lone pairs. The complexation energy Δc
E is obtained from the ΔH° by correcting for solvent influences,
and thermal contributions equals −15.0(6) kJ mol-1. This value agrees well with the MP2/aug-cc-pVTZ
level result, −12.4 kJ mol-1. The complexation entropy ΔS° has been found to be influenced by the solvent
and is correlated with ΔH°. This correlation reflects the existence of the compensation effect for the
thermodynamics of van der Waals complexes.