Abstract
The complexation reaction of Hg2+, Pb2+, Zn2+, and Cd2+ cations with four newly synthesized triazene ligands was studied spectrophotometrically in nonaqueous solvents (MeOH, EtOH, DMF, and DMSO) at various temperatures. Stability constants (K1 and K2) and stoichiometries of formed adducts (1:1 and 1:2 ligand to metal ion) were calculated by computer refinement of experimental spectral mole ratio data by SQUAD program. The results indicated that the donor number, dielectric constant, the acceptor number of the solvents play an important role in the complex stability. Besides, the shape and size of the solvent molecules were significant factors in the studied reactions. Between log β1 and log β2, a linear relationship was illustrated for most of the complexes under different conditions. The Van't Hoff equation was used to calculate ΔG°, ΔS°, and ΔH° from the dependence of formation constants on temperature. After calculating thermodynamic data at different temperatures, a good linear correlation was obtained from the TΔS° − ΔH° plot resulting in the entropy-enthalpy compensation for complexation reactions.
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