Abstract
The hydrogen bonded complexes between N-methylsuccinimide and phenols (pKa = 10.2 → 6) are investigated by infrared spectrometry. The thermodynamic parameters for the 1–1 complexes are determined in carbon tetrachloride-. The formation constants at 298 K range from 15 to 150 dm3 mol−1, the enthalpies of complex formation from - 20 to - 30 kJ mol−1, the changes of entropy from - 22 to - 40 J K−1 mol−1 and the frequency shifts of the v(OH) stretching vibration from 170 to 340 cm−1. The complexes are weaker than those involving the monocarbonyl bases. The decrease of the force constant of the bonded carbonyl group ranges from 0.48 to 0.65 N cm−1. The force constant of the free C=O group slightly increases upon complex formation, in agreement with the cooperatively theory.
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