Copper(II) 12-metallacrown-4 complexes of alpha-, beta- and gamma-aminohydroxamic acids: a comparative thermodynamic study in aqueous solution.
A complete thermodynamic study of the protonation and Cu(II) complex formation equilibria of a series of alpha- and beta-aminohydroxamic acids in aqueous solution was performed. The thermodynamic parameters obtained for the protonation of glycine-, (S)-alpha-alanine-, (R,S)-valine-, (S)-leucine-, beta-alanine- and (R)-aspartic-beta-hydroxamic acids were compared with those previously reported for gamma-amino- and (S)-glutamic-gamma-hydroxamic acids. The enthalpy/entropy parameters calculated for the protonation microequilibria of these three types of ligands are in very good agreement with the literature values for simple amines and hydroxamic acids. The pentanuclear complexes [Cu5L4H(-4)]2+ contain the ligands acting as (NH2,N-)-(O,O-) bridging bis-chelating and correspond to 12-metallacrown-4 (12-MC-4) which are formed by self-assembly between pH 4 and 6 with alpha-aminohydroxamates (HL), while those with beta- and gamma-derivatives exist in a wider pH range (4-11). The stability order of these metallomacrocycles is beta- >> alpha- > gamma-aminohydroxamates. The formation of 12-MC-4 with alpha-aminohydroxamates is entropy-driven, and that with beta-derivatives is enthalpy-driven, while with gamma-GABAhydroxamate both effects occur. These results are interpreted on the basis of specific enthalpies or entropy contributions related to chelate ring dimensions, charge neutralization and solvation-desolvation effects. The enthalpy/entropy parameters of 12-MC-4 with alpha-aminohydroxamic acids considered are also dependent on the optical purity of the ligands. Actually, that with (R,S)-valinehydroxamic acid presents an higher entropy and a lower enthalpy value than those of enantiopure ligands, although the corresponding stabilities are almost equivalent. Moreover, DFT calculations are in agreement with a more exothermic enthalpy found for metallacrowns with enantiomerically pure ligands.
Tegoni
Matteo
M
Dipartimento di Chimica Generale ed Inorganica, Chimica Analitica, Chimica Fisica, Università di Parma, Viale G.P. Usberti, 17A, 43100 Parma, Italy. matteo.tegoni@unipr.it
Remelli
Maurizio
M
Bacco
Dimitri
D
Marchiò
Luciano
L
Dallavalle
Francesco
F
D000409:Alanine / Q000031:analogs & derivatives; D000588:Amines / Q000737:chemistry*; D001224:Aspartic Acid / Q000031:analogs & derivatives; D003124:Colorimetry; D003300:Copper / Q000737:chemistry*; D006877:Hydroxamic Acids / Q000737:chemistry*; D007930:Leucine / Q000031:analogs & derivatives; D009942:Organometallic Compounds / Q000737:chemistry*; D011199:Potentiometry; D011522:Protons; D012996:Solutions / Q000737:chemistry; D013816:Thermodynamics; D014633:Valine / Q000031:analogs & derivatives; D014867:Water / Q000737:chemistry*
D000588:Amines; D006877:Hydroxamic Acids; D009942:Organometallic Compounds; D011522:Protons; D012996:Solutions; D014867:Water; D001224:Aspartic Acid; D003300:Copper; D007930:Leucine; D014633:Valine; D000409:Alanine