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Logo of nihpaAbout Author manuscriptsSubmit a manuscriptHHS Public Access; Author Manuscript; Accepted for publication in peer reviewed journal;
 
Inorg Chem. Author manuscript; available in PMC 2010 December 7.
Published in final edited form as:
PMCID: PMC2873866
NIHMSID: NIHMS158999

Using the Antenna Effect as a Spectroscopic Tool; Photophysics and Solution Thermodynamics of the Model Luminescent Hydroxypyridonate Complex [EuIII(3,4,3-LI(1,2-HOPO))]-

Abstract

While widely used in bioassays, the spectrofluorimetric method described here uses the antenna effect as a tool to probe the thermodynamic parameters of ligands that sensitize lanthanide luminescence. The Eu3+ coordination chemistry, solution thermodynamic stability and photophysical properties of the spermine-based hydroxypyridonate octadentate chelator 3,4,3-LI(1,2-HOPO) are reported. The complex [EuIII(3,4,3-LI(1,2-HOPO))]- luminesces with a long lifetime (805 μs) and a quantum yield of 7.0% in aqueous solution, at pH 7.4. These remarkable optical properties were exploited to determine the high (and proton-independent) stability of the complex (log β110 = 20.2(2)) and to define the influence of the ligand scaffold on the stability and photophysical properties.

The high-affinity bidentate hydroxypyridonate (HOPO) metal-chelating groups are related to microbial siderophores: they combine the structural features of hydroxamic acids with the electronic properties of catechols. The 6-amide derivative of 1-hydroxy-pyridin-2-one (1,2-HOPO) has been linked to multiple polyamine scaffolds through amide coupling, to form multidentate ligand structures used for a variety of applications such as actinide (An) and iron chelation,1,2 MRI contrast enhancement3 and lanthanide (Ln) luminescence sensitization.4 The coordination chemistry properties of these ligands can be fine-tuned by systematic modifications of the denticity, geometry and acidity of the backbone. Octadentate ligands, each incorporating four 1,2-HOPO functionalities, are known to strongly bind Ln(III), An(III), and An(IV) and to act as antennae that sensitize the emission of Eu(III).1,5 The backbone geometry of the ligand must affect the thermodynamic stability and photophysical properties of the corresponding Ln- and An-complexes, but this has not been investigated in a systematic way. While the octadentate ligand 3,4,3-LI(1,2-HOPO) (1, Fig. 1) is composed of 1,2-HOPO units linked to a central linear spermine scaffold and has shown potential as a therapeutic Pu(IV) and Am(III) chelator,1 the branched tetrapodal ligand H(2,2)-1,2-HOPO (2, Fig. 1) has been studied for its ability to form a highly stable luminescent Eu(III) complex that contains a molecule of water in the inner coordination sphere at physiological pH.5 The work presented herein probes the coordination chemistry and photophysical properties of the Gd(III) and Eu(III) complexes of 1, showing that the geometry of the ligand scaffold strongly affects the inner coordination sphere of the metal ion and consequently its emissive properties. In addition, the Eu luminescence sensitization properties of the antenna ligand 1 are used as a spectroscopic tool to determine the solution thermodynamic stability of the corresponding metal-complex, which provides a new method for the accurate determination of these thermodynamic parameters.

Figure 1
Structures of the octadentate hydroxypyridonate ligands 3,4,3-LI(1,2-HOPO) (1, left) and H(2,2)-1,2-HOPO (2, right); the metal-coordinating oxygen atoms are indicated in red.

All photophysical properties were measured in buffered aqueous solutions at pH 7.4 and relevant parameters are summarized in Table 1. The electronic absorption spectrum of [EuIII(1)]- (Fig. 2) shows an absorption maximum due to ππ* transitions at λmax = 315 nm (ε = 17,700 M-1cm-1). This spectrum is blue-shifted and has a lower molar absorption coefficient than the spectrum of [EuIII(2)]0max = 343 nm, ε = 18,200 M-1cm-1,5 Fig. 2). The shift towards higher energies is attributed to the different ligand scaffolds: the four protonated amide nitrogen atoms in the molecular structure of 2 can form hydrogen bonds with the hydroxyl groups from the pyridinone rings, thereby stabilizing the first singlet excited state of the corresponding europium complex, whereas the backbone of 1 only contains two protonated amide nitrogen atoms yielding a complex with a singlet excited state slightly higher in energy, and a shoulder at lower energy on the main absorption peak.

Figure 2
Electronic absorption (solid, left) and normalized steady-state emission spectra (solid, right, λexc = 325 nm) of [EuIII(1)]-, and electronic absorption spectrum (dash) of [EuIII(2)]0, in 0.1 M TRIS buffer (pH 7.4).
Table 1
Summary of Photophysical Parameters for [EuIII(1)]- a

The Gd(III) complex of 1 was prepared in situ, to determine the ligand centered triplet excited state energy. Because the Gd3+ ion exhibits a size and atomic weight similar to Eu3+ but lacks an appropriately positioned electronic acceptor level, the phosphorescence of the ligand can be observed by luminescence measurements in a solid matrix (1:3 (v/v) MeOH:EtOH) at 77 K. Upon cooling to 77 K, the spectrum of [GdIII(1)] reveals an intense unstructured emission band from 400 to 570 nm (Fig. S1), assigned to phosphorescence from the ligand T1 excited state. The lowest T1 state energy was estimated by spectral deconvolution of the 77 K luminescence signal into several overlapping Gaussian functions.6 The resulting T1 energy was calculated at 24,390 cm-1, which is higher than the values found for other 1,2-HOPO derivatives (T1 ~ 19,500-21,500 cm-1),4 and the energy gap between T1 and the 5D1 accepting state was determined at 5,360 cm-1, a value larger than that found for 2, implying that the energy transfer efficiency of [EuIII(1)]- should be less efficient. This increase of the triplet excited state energy is in line with the increase of the singlet excited state energy determined by UV-Visible absorption spectroscopy and can also be attributed to the absence of two protonated amide nitrogen (destabilizing the triplet excited state as compared to that of [EuIII(2)]0).

The luminescence spectrum of [EuIII(1)]- displays the characteristic features of EuIII(1,2-HOPO) complexes; the very intense 5D07F2 hypersensitive transition results in almost pure red luminescence (λem = 612 nm, Fig. 2). The luminescence quantum yield of [EuIII(1)]- in aqueous solution (pH = 7.4), Φtot = 7.0%, is two-fold higher than that of [EuIII(2)]0 (3.6%),5 thus [EuIII(1)]- is much brighter than [EuIII(2)]0 (the brightness is defined as the product of molar absorption coefficient and luminescence quantum yield). The optical properties of the 3,4,3-LI backbone are superior to those of the H(2,2) backbone at high energy, up to 337 nm, and are slightly inferior at lower energies (Fig. S2).

Corresponding time resolved analysis of [EuIII(1)]- luminescence, measured at 612 nm in H2O and D2O, revealed monoexponential decays with decay times of ca. 805 μs and ca. 1120 μs, respectively, which are slightly longer than the typical lifetimes determined for bis-tetradentate EuIII(1,2-HOPO) complexes.6,7 Using the improved Horrocks equation,8 the number of inner sphere water molecules on the [EuIII(1)]- complex was determined as q = 0.1 ± 0.1, essentially zero. In contrast to complexes formed with H(2,2) ligand derivatives,5 the 3,4,3-LI linear backbone promotes the formation of a Eu(III) complex with no inner sphere water molecule.

In order to investigate in detail further particularities of the sensitization process by the linear ligand 1, the kinetic parameters were determined.9,10 The sensitization efficiency, ηsens, defined as the product of the efficiency of the energy transfer, ηET, and the quantum yield of the antenna, Φantenna, was determined using the equation: Φtot = Φantenna× ηET × ΦEu. The radiative decay rate, krad, of [EuIII(1)]- is higher than that of [EuIII(2)]0 (538 s-1 vs. 333 s-1), and the non-radiative decay rate, knonrad, is much lower for the linear complex than for the branched complex with values of 705 s-1 and 1750 s-1, respectively. This result reflects the absence of water molecule in the inner sphere of [EuIII(1)]-, inducing a decrease of the quenching by OH vibrations. Consequently, the metal centered luminescence efficiency (ηEu), is higher for [EuIII(1)]- than for [EuIII(2)]0 (43.2% vs. 16.0%), while the sensitization efficiency, ηsens, is lower (16.2% vs. ca. 22.5%). The intersystem crossing and the energy transfer are therefore affected when using the 3,4,3-LI backbone, which limits the corresponding luminescence quantum yield to 7.0%. These values emphasize the important trade off existing between the sensitization and metal efficiency of the EuIII complexes.

The protonation constants of 1 were determined by potentiometric titrations, and four protonation equilibria (Table 2) were assigned to sequential removal of one proton from each of the four 1,2-HOPO units. The overall basicity of 1 (quantified from the sum of the log Ka values associated to only those protonation steps that result in the neutral ligand species,11 Σ log Ka = 21.2) is increased when compared to the branched ligand 2 (Σ log Ka = 18.9).5 Initial attempts were made to determine the Eu(III) affinity of 1 by direct spectrophotometric titration (Fig. S3). However, few changes occur in the UV-Visible absorption of the complex over the pH range 3.0-8.0, limiting accurate spectral deconvolution and data refinement. The Eu3+ complexation of 1 was thus studied by spectrofluorimetric titration: a solution containing an equimolar ratio of Eu and 1 was divided into separate aliquots, and base was added to each sample to give a pH range from 2.2 to 9.5. After a 24 h equilibration time, each emission spectrum (λexc = 325 nm) and pH was recorded and analyzed to ascertain the proton-independent stability constant (Kf = β110 = 1020.2(2)) and protonation constant (Ka = 104.6(1)) of the corresponding europium complex (Table 2). In contrast to previous studies,12 the present method relies on the sensitization of the Eu luminescence by the excited ligand rather than on the emission resulting from direct excitation of the metal ion. Upon acidification, the luminescence of the solution decreases (Fig. 3), corresponding to the disappearance of the emissive species [EuIII(1)]- and the formation of the protonated complex [EuIII(1H)]0. In addition, only a single mono-exponential decay lifetime (805 μs +/- 10%), corresponding to the parent complex [EuIII(1)]-, was detected through time-resolved measurements of the titration samples.

Figure 3
Spectrofluorimetric titration of [EuIII(1)]- ([Eu3+] = [1] = 0.01 mM, 0.1 M KCl, 0.2 mM Hepes, 0.2 mM Mes, 25.0 °C, λexc = 325 nm). Insert: Normalized integration of the emission spectra (data points) and calculated speciation diagram ...
Table 2
Protonation and Eu Complex Formation Constants for Ligand 1a

The conditional stability constant pEuIII could then be calculated as a function of pH for a standard set of conditions (Fig. S4, initial concentrations: [Eu] = 10-6 M, [L] = 10-5 M), to allow comparisons between 1 and other ligands of varying denticity and/or acidity. Both 1 (pEuIII7.4) = 21.1(1)) and 2 (pEuIII7.4 = 21.2) exhibit similar affinities for Eu(III), not only at pH = 7.4, but over the pH range 2.0–10, despite the differences in ligand acidity and water coordination of the corresponding complexes. To validate the use of this spectrofluorimetric method, the affinity of 1 for Eu(III) was verified via direct competition against diethylenetriaminepentaacetic acid (DTPA) at pH = 7.4, following a previously described method (Fig. S5-S6, Table 2).5

While the linear spermine-based 1,2-HOPO ligand 1 and the tetrapodal ligand 2 both exhibit similar affinities for Eu(III), the photophysical properties of the resulting complexes differ significantly. In contrast to [EuIII(2)]0, the high quantum yield of the bright complex [EuIII(1)]- comes mainly from its high metal-centered luminescence efficiency and from the lack of an inner-sphere water molecule. The remarkable luminescence properties of [EuIII(1)]- were used to design a direct method of stability constant determination. This method will be applied to other ligand systems that sensitize lanthanide and actinide luminescence.

figure nihms158999f4

Supplementary Material

1_si_001

Acknowledgments

This work was supported by the National Institutes of Health (Grant AI074065-01), and the Director, Office of Science, Office of Basic Energy Sciences, and the Division of Chemical Sciences, Geosciences, and Biosciences of the U.S. Department of Energy at LBNL under Contract No. DE-AC02-05CH11231. The authors thank Dr. Jide Xu for providing the ligands and Prof. Gilles Muller (San Jose State University) for the use of a low temperature time-resolved luminescence spectrometer. This technology is licensed to Lumiphore, Inc. in which some of the authors have a financial interest.

Footnotes

Supporting Information Available: Detailed experimental procedures and spectral data. This material is available free of charge via the Internet at http://pubs.acs.org.

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