Abstract
Thermodynamic data have been obtained calorimetrically for the reaction of a range of Group VI transition metal carbonyl derivatives with mercury(II) halides in 1,2-dichloroethane solution. The results show that the enthalpies of adduct formation are more negative when the transition metal atom has a lower electronegativity, due to large size or coordination of arenes or phosphines. Enthalpies of adduct formation are slightly more negative than those of adducts of mercury(II) halides with conventional Lewis bases, suggesting that the mercurymetal bonds formed are at least as strong as equivalent HgN or HgP bonds. The influence of entropy effects on adduct stabilities is shown by the high stabilities of chromium compounds, despite generally less negative enthalpies of formation.
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