Thermodynamic and Kinetic Studies of Zinc(II)–Triamine Complexes as Models of CA and AP

The formation constant (KZnL), enthalpy and entropy changes (ΔH and ΔS), and deprotonation constant (Ka) of coordinated water for hydrated zinc(II)–triamine (1 : 1) complexes (N3–Zn-(OH2)n (N3 = diethylenetriamine (dien), N-(2-aminoethyl)-1,3-propanediamine (epd), dipropylenetriamine (dpt), cis,cis-1,3,5-triaminocyclohexane (tach), and 1,5,9-triazacyclododecane ([12]aneN3)) were determined by potentiometry. The pKa linearly increased along with an increase in -ΔH, and was explained in terms of a ligand–ligand interaction through the N3–Zn-O bond on the bases of a thermodynamic analysis and strain-energy calculation (MM2). The zinc(II) complex-promoted hydrolysis of 2,4-dinitrophenyl diethyl phosphate was investigated in 1% (v/v) methanol–water; the rate constants linearly increased along with decreases of pKa and −ΔH. This fact indicates that the hydrolysis proceeds via a concerted direct nucleophilic attacking mechanism of the coordinated hydroxide ion, in which the phosphate ester coordinates to the zinc(II) ion. X-ray structure analyses for synthesized model complexes, [Zn(OAc)(dien)](ClO4), [{Zn(dpt)}3(CO3)](ClO4)4·NaClO4, and [Zn(OAc)(tach)](ClO4), are also reported.