title: Binding of nitrate to a CuII-cyclen complex bearing a ferrocenyl pendant: synthesis, solid-state X-ray structure, and solution-phase electrochemical and spectrophotometric studies.
abstract: The reaction of Cu(NO3)2.3H2O with the ligand 1-(ferrocenemethyl)-1,4,7,10-tetraazacyclododecane (L) in acetonitrile leads to the formation of a blue complex, [Cu(L)(NO3)][NO3] (C1). The X-ray structure determination shows an unexpected binding of a nitrate anion in that the CuII center is surrounded by four N atoms of the 1,4,7,10-tetraazacyclododecane (cyclen) macrocycle and two O atoms from a chelating nitrate anion, both Cu-O distances being below the sums of the van de Waals radii. Hydrogen-bonding interactions in the crystal lattice and a weak interaction between a second nitrate O and the CuII center in C1 give rise to a highly distorted CuII geometry relative to that found in the known structure of [Cu(cyclen)(NO3)][NO3] (C5). Electrochemical studies in acetonitrile containing 0.1 M [Bu4N][NO3] as the supporting electrolyte showed that oxidation of C1 in this medium exhibits a single reversible one-electron step with a formal potential E degrees f of +85 mV vs Fc0/+ (Fc = ferrocene). This process is associated with oxidation of the ferrocenyl pendant group. Additionally, a reversible one-electron reduction reaction with an E degrees f value of -932 mV vs Fc0/+, attributed to the CuII/I redox couple, is detected. Gradual change of the supporting electrolyte from 0.1 M [Bu4N][NO3] to the poorly coordinating [Bu4N][PF6] electrolyte, at constant ionic strength, led to a positive potential shift in E degrees f values by +107 and +39 mV for the CuII/I(C1) and Fc0/+(C1) redox couples, respectively. Analysis of these electrochemical data and UV-vis spectra is consistent with the probable presence of the complexes C1, [Cu(L)(CH3CN)2]2+ (C2), [Cu(L)(CH3CN)(NO3)]+ (C3), and [Cu(L)(NO3)2] (C4) as the major species in nitrate-containing acetonitrile solutions. In weakly solvating nitromethane, the extent of nitrate complexation remains significant even at low nitrate concentrations, due to the lack of solvent competition.
authors: School of Chemistry, Monash University, Clayton, Victoria 3800, Australia.
authors: Gilles
authors: G
authors: Gasser
authors: Matthew J
authors: MJ
authors: Belousoff
authors: Alan M
authors: AM
authors: Bond
authors: Leone
authors: L
authors: Spiccia
mesh_terms: D002614:Chelating Agents / Q000737:chemistry*; D003300:Copper / Q000737:chemistry*; D018360:Crystallography, X-Ray; D000080027:Cyclams; D004563:Electrochemistry; D005296:Ferrous Compounds / Q000737:chemistry*; D006571:Heterocyclic Compounds / Q000737:chemistry*; D006860:Hydrogen Bonding; D007202:Indicators and Reagents; D009682:Magnetic Resonance Spectroscopy; D008958:Models, Molecular; D009566:Nitrates / Q000737:chemistry*; D013056:Spectrophotometry, Ultraviolet
chemical_list: D002614:Chelating Agents; D000080027:Cyclams; D005296:Ferrous Compounds; D006571:Heterocyclic Compounds; D007202:Indicators and Reagents; D009566:Nitrates; D003300:Copper; C038072:cyclen