Skip to main content

Thank you for visiting You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

Spectroscopic and computational investigation of actinium coordination chemistry


Actinium-225 is a promising isotope for targeted-α therapy. Unfortunately, progress in developing chelators for medicinal applications has been hindered by a limited understanding of actinium chemistry. This knowledge gap is primarily associated with handling actinium, as it is highly radioactive and in short supply. Hence, AcIII reactivity is often inferred from the lanthanides and minor actinides (that is, Am, Cm), with limited success. Here we overcome these challenges and characterize actinium in HCl solutions using X-ray absorption spectroscopy and molecular dynamics density functional theory. The Ac–Cl and Ac O H 2 O distances are measured to be 2.95(3) and 2.59(3) Å, respectively. The X-ray absorption spectroscopy comparisons between AcIII and AmIII in HCl solutions indicate AcIII coordinates more inner-sphere Cl1– ligands (3.2±1.1) than AmIII (0.8±0.3). These results imply diverse reactivity for the +3 actinides and highlight the unexpected and unique AcIII chemical behaviour.


Understanding of the chemistry of trivalent actinides has broad-potential impacts on society through diverse areas, including cancer therapy1,2,3, nuclear waste4,5,6, energy and global security7. However, with the exception of UIII (refs 6, 7, 8, 9), fundamental understanding of the early-to-mid-actinides in the trivalent oxidation state (An=AcIII, NpIII, PuIII, AmIII, CmIII, BkIII and CfIII) remains substantially less developed than that of the main group, transition metals and lanthanides. Significant experimental challenges associated with the highly radioactive samples, limited access to material of interest, and the redox instability of some AnIII ions have necessitated numerous heroic efforts to advance AnIII chemistry6,10,11,12,13,14,15.

The 2015 Long Range Plan for the DOE-NP Isotope Program16 highlighted the importance of advancing AcIII chemistry in comparison with the other AnIII ions. In this document, 225Ac was identified as a promising anticancer therapeutic agent. The report focused on global interest in exploiting the α-emissions from 225Ac and its radioactive daughters to selectively destroy the malignant cells17,18. To use these α-particles therapeutically, the 225Ac isotope must be attached to cancer-selective targeting vectors using a stable chelating agent. Unfortunately, the limited availability of 225Ac [t½=10.0(1) d; National Nuclear Data Center (NNDC)], or a useful surrogate, has impeded development of actinium chelators. For instance, the use of 227Ac, the longest-lived actinium isotope [t½=21.772(3) y; NNDC] provides the best possible alternative for improving ligand design. However, the worldwide inventory of 227Ac is currently insufficient for meeting this demand. Historically, these challenges were magnified by the electronic ground state of AcIII (5f0 6d0), which is essentially invisible to common spectroscopies (for example, ultraviolet–visible, fluorescence, electron paramagnetic resonance and so on). Hence, applying alternative characterization methods that account for (1) high radioactivity, (2) small samples sizes (1–30 μg) and (3) closed shell electronic configurations would facilitate innovative chelation designs for delivery of 225Ac through the biological milieu to the targeted tumour site.

Recent upgrades at the Stanford Synchrotron Radiation Lightsource (SSRL), such as the new 100-element solid-state Ge detector array on beamline 11-2, have provided new opportunities to overcome the aforementioned challenges. This capability has improved sensitivity for trace-level detection in environmental samples using X-ray absorption fine-structure (XAFS) spectroscopy19,20. While this instrumentation has been used primarily in environmental sciences, here we exploit the capability to conduct the first actinium XAFS study reported to date. Using this method, 227Ac in concentrated HCl solutions are characterized at the Ac L3-edge. Our interpretations of the spectra are guided by molecular dynamics density functional theory (MD-DFT) calculations21,22,23,24,25. To establish confidence in the spectroscopic and computational methods, the AcIII results are compared with analogous measurements on AmIII. This ion is selected because—among the redox stable trivalent actinides—its ionic radius is most similar to AcIII. Overall, this approach enables the Ac–Cl and Ac O H 2 O distances to be measured and allows the coordination chemistry of AcIII and AmIII to be directly compared. The experimental and computational data show more chloride ions in the inner coordination sphere for AcIII and the results are presented in comparison with previous actinide(III) XAFS studies. This study reveals an unexpected divergence in +3 f-element reactivity. Furthermore, the research highlights the need to better characterize AnIII chemistry in support of developing α-emitting therapeutic agents.


X-ray absorption near-edge structure spectroscopy

To evaluate AcIII and AmIII binding of Cl1– versus H2O, three solution-phase samples were prepared: actinium chloride (AcIII in HCl; 11 M); americium chloride (AmIII in HCl; 11 M); and the americium aquo ion (AmIII in HO3SCF3, 0.11 M), referred to hereafter as Ac-HCl, Am-HCl and Am-Aquo. To mitigate safety concerns associated with the 227Ac isotope, radioactive daughters (primarily 227Th and 223Ra) were removed before the measurements at the SSRL synchrotron, as previously described (see Methods)26,27. The samples were then returned to Los Alamos National Laboratory before a significant quantity of the daughters re-emerged (10 days). The Ac and Am L3-edge X-ray absorption near-edge structure (XANES) spectra from Ac-HCl, Am-HCl and Am-Aquo were background subtracted and normalized (Fig. 1). The spectra were similar as they contained a pronounced edge-peak superimposed on an absorption threshold. From the perspective of the free ion, the edge-feature could be crudely described as originating from electric-dipole allowed transitions from the actinide 2p-orbitals to unoccupied states that contain actinide 6d-character, that is, for AcIII 2p6…5f0 6d0→2p5…5f0 6d1 (refs 28, 29).

Figure 1: Solution phase AcIII and AmIII L3-edge XANES.
figure 1

(a) XANES spectra for Am-Aquo (0.11 M HO3SCF3) in blue trace. (b) XANES spectra for Am-HCl (11 M HCl) in orange trace. (c) XANES spectra for Ac-HCl (11 M HCl) in red trace. The actinium and americium spectra were calibrated in situ to RbCl pellet (15,203.81 eV) and Zr foil (17,998 eV) respectively.

The Ac L3-edge spectrum was of quintessential significance, as it represented the first actinium XANES measurement. The edge-peak line shape was quite broad and spanned over 30 eV, owing to the short core-hole lifetime. The peak maximum and inflection point (where first and second derivatives of the data equalled zero) were determined to be 15,877.3 and 15,873.9 eV, respectively. For the americium samples, the inflection point from Am-Aquo was found at 18,514.3 eV, which was consistent with americium in the +3 oxidation state30,31. Changing the solution matrix from HO3SCF3 (0.11 M) to HCl (11 M) shifted the edge-peak inflection point to lower energy by 0.7 eV. The Am L3-edge energy difference was attributed to an electronic change that accompanied Cl1– displacement of H2O in the AmIII inner coordination sphere (vide infra), that is, Am-Aquo versus Am-HCl. Given the relative ease with which the AcIII and AmIII L3-edge XANES measurements were obtained—and in light of the incompatibility of other spectroscopic techniques for probing dilute actinium samples—we anticipate that these results will provide a foundation for characterizing the coordination chemistry of actinium in other chemical environments in the future.

Extended X-ray absorption fine structure

Appreciable differences were observed in the solution-phase k3χ(k) extended X-ray absorption fine-structure (EXAFS) data (room temperature) from solutions containing Ac-HCl, Am-HCl and Am-Aquo (Fig. 2). For instance, a substantial phase shift and change in frequency in the EXAFS oscillations was observed in the spectrum from Ac-HCl in comparison with the americium spectra. The Ac-HCl spectrum was comprised of at least two substantial contributions; one characterized by a long frequency and the other by a short frequency. The presence of two frequencies was most likely associated with a significant number of both Cl1– and H2O molecules in the AcIII inner coordination sphere. In contrast, for Am-HCl, the frequency of EXAFS oscillations was dominated by one major sinusoidal component, such that the Am-HCl spectrum was almost superimposable on that from Am-Aquo. The similarity between Am-HCl and Am-Aquo suggested that H2O molecules dominated the inner coordination sphere in Am-HCl, with Cl1– content being slight. Overall, this comparison highlighted significant differences in AcIII versus AmIII solution speciation.

Figure 2: Solution phase AcIII and AmIII L3-edge EXAFS.
figure 2

(a) EXAFS k3χ(k) spectra for Am-Aquo (0.11 M HO3SCF3) in blue trace. (b) EXAFS k3χ(k) spectra for Am-HCl (11 M HCl) in orange trace. (b) EXAFS k3χ(k) spectra for Ac-HCl (11 M HCl) in red trace. Fits to the data have been provided as dashed black traces.

The EXAFS data were fit by allowing the coordination numbers (CN), the Debye–Waller factors (σ2), and the interatomic distances (R) to converge to reasonable values. Limitations associated with the solution-phase room-temperature EXAFS measurements constrained meaningful data to 10 k (9, 10.5 and 12 k for solutions containing Ac-HCl, Am-HCl and Am-Aquo, respectively). As a result, scattering pathways beyond the first coordination shell (including multiple scattering pathways, for example, Cl−M−H2O) were not considered. To most effectively describe how the EXAFS models were obtained, it was instructive to begin with Am-Aquo, then introduce the possibility of Cl1– ligation for Am-HCl, and conclude with the Ac-HCl.

Before modelling the EXAFS data from Am-Aquo, we initially calculated (FEFF8 (ref. 32)) an EXAFS spectrum using atomic coordinates obtained from the [Am(H2O)9][O3SCF3]3 single-crystal X-ray diffraction data, previously reported33. The calculated EXAFS spectrum was composed of two main scattering pathways. The first path originated from six oxygen atoms with an Am O H 2 O distance of 2.465 Å and the second path had three oxygen atoms at 2.578 Å. Although various EXAFS fitting parameters were considered based on these calculations, only one oxygen shell could be resolved in the experimental data, as our resolution between k of 2.6 and 12 was only 0.167 Å (π/2Δk). The final model of the EXAFS data with the lowest residual factor and reduced chi-squared value consisted of 9.5±0.9 oxygen atoms at 2.48(1) Å (Table 1 and Figs 2 and 3). These Am O H 2 O bond distances and CNs were consistent with the Am(H2O)93+ solid-state structure and EXAFS spectra previously obtained on AmIII aquo ions in different solvent matrices, for example, Stumpf et al.34 in 0.025 M HClO4 and Allen et al.35 in 0.25 M HCl (Table 1).

Table 1 Structural parameters determined using solution-phase EXAFS.
Figure 3: Fourier Transform of the AcIII and AmIII k3-EXAFS.
figure 3

(a) Fourier Transform of k3-EXAFS spectra from Am-Aquo (0.11 M HO3SCF3) in blue trace and its fit in dashed black trace. (b) Oxygen path contribution in the fitted data in dashed purple. (c) Fourier Transform of k3-EXAFS spectra from Am-HCl (11 M HCl) in red trace and its fit in dashed black trace. (d) Oxygen and chlorine paths contribution in the fitted data in dashed purple and green solid trace, respectively. (e) Fourier Transform of k3-EXAFS spectra from Ac-HCl (11 M HCl) in red trace and its fit in dashed black trace. (f) Oxygen and chlorine paths contribution in the fitted data in dashed purple and green solid trace, respectively.

The EXAFS fitting results can be interpreted using static or dynamic descriptions. A static interpretation suggested that the americium aquo ion had 9.5 H2O ligands held at a fixed 2.48(1) Å distance. In contrast, the dynamic interpretation described the EXAFS data as an averaged spectrum from a heterogeneous mixture over the lifetime of the experiment. In this scenario, the number of H2O molecules in the AmIII inner coordination sphere varied, as did the Am O H 2 O distances. To provide insight, MD-DFT calculations were carried out on a single AmIII ion inside a box (12.54 × 12.45 × 12.68 Å3) of explicit H2O (64 total) solvent molecules. Before the simulation, the components of the box were randomized (see Methods), and then the MD were modelled for 330 fs. The MD trajectory showed a time average of 8.1±0.3 H2O molecules within a 4 Å radius of the AmIII ion. The average Am O H 2 O distances were displayed by the red solid traces in Fig. 4. At the start of the calculations the variation in Am O H 2 O bond distances were large, ranging from 2.7 to 2.5 Å. However, after 50 fs, the magnitude of these oscillations became smaller and centred 2.5 Å. In general, these calculations were in excellent agreement with the EXAFS experiment. Both theory and experiment identified a CN around nine and the calculated average Am O H 2 O distances bracketed the experimental value (red dashed trace). The good agreement of the Am-Aquo experimental and computational EXAFS analyses with the single-crystal and solution-phase EXAFS studies provided confidence and credibility that our methods could be applied accurately to other actinide systems.

Figure 4: MDDFT calculations.
figure 4

The calculated mean M-O H 2 O (solid red traces) and M–Cl (solid blue traces) distances for O and Cl atoms within 4 Å of the metal (Am or Ac) have been compared with the values obtained from the experimental EXAFS analyses ( M-O H 2 O dashed red and M–Cl dashed blue traces with their associated errors bars represented as shaded boxes). Experimental errors bars were 0.01 or 0.03 Å. See Table 1. (a) Data for Am-Aquo, (b) Data for Am-HCl and (c) Data for Ac-HCl.

To obtain atomic coordinates for modelling the Am-HCl data, we calculated EXAFS spectra using FEFF8 from two different sources. The first model employed atomic coordinates from previously reported [AmCl2(H2O)6]Cl single-crystal X-ray diffraction data36, which had two Cl1– and six H2O inner-sphere ligands. The second simulation utilized a DFT-optimized structure of AmCl2(H2O)41+. Refinement of the experimental EXAFS data using fitting parameters from either model converged to the same point (Table 1 and Figs 2 and 3), showing an approximate nine-coordinate AmIII ion with 0.8±0.3 Cl1– and 8.3±0.9 H2O molecules in the inner sphere. Although the contributions from Cl1– to the overall EXAFS spectrum seemed slight (Fig. 3), omitting the Cl1– shell provided a significantly worse model, by over 91% confidence as determined from the Hamilton statistical test37. The measured americium coordination environment seemed reasonable when compared with other solution-phase EXAFS studies. For instance, our Am-HCl CNs—collected in HCl solutions of 11 M—were bracketed by those determined from solutions with lower and higher Cl1– concentrations (Table 1). Allen et al.’s EXAFS experiments at lower HCl solutions (0.25 M) showed no inner-sphere Cl1– ligands, while those at higher Cl1– concentrations—a mixture of HCl (0.25 M) and LiCl (12.5 M)—showed 1.8 Cl1– ligands35. When experimental errors were considered, our data also agreed with measurements conducted at similar Cl1– concentrations, for example, Allen et al. identified 1.2 Cl1– ligands in solutions containing mixtures of HCl (0.25 M) and LiCl (10.0 M) (ref. 35). Our 2.75(3) Am–Cl and 2.48(1) Am O H 2 O distances also agreed with metrics from the solid-state single-crystal X-ray diffraction study, 2.799(2) and 2.462(9) Å, respectively36, and were consistent with Allen et al.’s solution-phase EXAFS results in LiCl (10.0 M, 12.5 M); which had Am–Cl distances between 2.80 and 2.81 Å and Am O H 2 O distances varying from 2.48 to 2.51 Å35.

These Am-HCl EXAFS results agreed with the MD-DFT calculations. The calculations were conducted similarly to those described above for Am-Aquo, with the exception that one Cl1– anion was included in the calculation. Over the course of 480 fs, we calculated an average of 1 Cl1– and 8.05±0.9 H2O molecules within a radius of 4 Å from the AmIII ion. The average Am–Cl and Am O H 2 O distances were quite similar to the experimental EXAFS values as shown in Fig. 4.

Given the paucity of actinium structural studies38,39, the DFT and MD-DFT calculations proved useful in guiding the interpretation of the EXAFS spectrum from Ac-HCl. Atomic coordinates for the EXAFS refinement were obtained from MD-DFT calculations on AcCl3(H2O)5. The resulting EXAFS analysis identified two unique scattering paths; one associated with the H2O ligands composed of 6.6±1.8 molecules at 2.59(3) Å and a second at 2.95(3) Å consisting of 3.2±1.1 Cl1– ligands (Debye–Waller factor=0.0074 Å2; Figs 2 and 3). These bond distances were in excellent agreement with the sum of the AcIII and Cl1- ionic radii, 1.12 Å+1.81 Å=2.93 Å (ref. 40). If the chlorine path was ignored and only the oxygen path used, the quality of the fit decreased (>93% confidence based on the Hamilton’s statistical test37), gave a high Debye–Waller factor value (0.018 Å2), and provided an unrealistic number of coordinated H2O molecules (14 total).

The Ac-HCl experimental data agreed well with MD-DFT calculations conducted on a box containing one AcIII, three Cl1– ligands and 64 H2O molecules for 1 ps. The MD-DFT revealed all three Cl1- and 6.14±0.34 H2O ligands within 4 Å of the AcIII ion for the duration of the calculation. The average Ac O H 2 O and Ac–Cl distances were calculated to be 2.76±0.08 and 3.04±0.13 Å, respectively. Although the magnitudes of these values were larger than that determined experimentally (by 0.17 Å for Ac O H 2 O and 0.09 Å for Ac–Cl), the calculated and experimental results agreed within 1σ for the Ac–Cl, and 2σ for the Ac O H 2 O . Such deviations between theory and experiment were not unusual and have been observed in calculations on other systems that employed the generalized gradient approximation functional. The calculated CNs also agreed with the experimental values, showing 3 Cl1– and 6 H2O inner-sphere ligands. We note that the agreement between experiment and theory was better in the two americium cases described above. It was possible that these subtle differences between theory and experiment resulted from the low signal-to-noise at high k in the experimental Ac L3-edge EXAFS spectrum, as the actinium concentrations were appreciably smaller than americium (μM versus mM). Alternatively, it was possible that the behaviour of AcIII was more difficult to model, as the fundamentals of actinium have been less well defined than those of americium. Regardless, both theory and experiment indicated substantial differences between the AcIII and AmIII coordination environments in HCl solutions, which represented an unexpected variation in actinide(III) reactivity. It is this observation that has inspired our future efforts to better understand the origin for diverging AcIII versus AmIII-binding preferences.


The experimental and computational results described here represented an exciting leap forward from previous actinium coordination chemistry studies. To most effectively communicate to the reader the significance of these results, we found it instructive to summarize the previous AcIII coordination chemistry. The majority of actinium chemistry has been inferred from methodical radio-analytical and extraction studies conducted on trace-level quantities of actinium39,41,42,43. Although these previous efforts revealed differences between AcIII and the other trivalent actinide and lanthanide elements, in general, they have been interpreted as suggesting that AcIII is a hard oxophilic tri-cation, in direct analogy to other actinide(III) cations. In addition, there have been a few studies that used macroscopic quantities of AcIII for analysis by ultraviolet–visible spectroscopy43,44. However, these spectra were essentially featureless—owing to the actinium 5f0 6d0 ground-state electronic configuration—and did not provide an insight into the actinium coordination environment. The majority of actinium structural data was obtained during the Manhattan project and through the years shortly after World War II. For example, Fried et al.38 and Zachariasen45,46,47 deduced structures and cell parameters using X-ray diffraction patterns from crystalline powders of nine actinium compounds assumed to be AcF3, AcCl3, AcBr3, Ac2O3, Ac2S3, AcOF, AcOCl, AcOBr and AcPO4·H2O. Subsequently, Farr et al. used X-ray diffraction to characterize microgram quantities of a mixture of actinium metal and actinium hydride48. Years later, an attempt to prepare some inorganic compounds with 10 mg of 227Ac occurred. Unfortunately, radiation damage to samples and the diffraction films limited this effort to generate a single powder pattern of actinium oxalate, Ac2(C2O4)3·10H2O (ref. 49).

Reported here, we overcame some of the challenges associated with spectroscopic analyses of bulk actinium samples using new XAFS capabilities, which have been typically employed in trace-level environmental science studies. Briefly, we characterized the chemistry of AcIII and AmIII in concentrated HCl (11 M) solutions and compared the results with solution-phase measurements from the americium aquo ion in dilute HO3SCF3 (0.11 M). Calculations involving MD-DFT, previously reported single-crystal X-ray diffraction, and previous solution-phase EXAFS results (when possible) were employed to guide our spectral interpretations. These efforts enabled the Ac–Cl and Ac O H 2 O distances to be directly measured for the first time. Moreover, the studies revealed a substantial difference between AcIII and AmIII solution speciation. In concentrated HCl solutions, we observed that AcIII and AmIII were coordinated by approximately nine ligands; however, AcIII preferred approximately six H2O molecules and three Cl1– ions, while AmIII was coordinated by approximately eight H2O and one Cl1– ligands. It is well known that evaluating CN using EXAFS typically provides values with high uncertainty, 20%. In spite of the large errors associated with the AcIII (CNCl=3.2±1.1) and AmIII (CNCl=0.8±0.3) chloride CNs, these values clearly indicated that AcIII had more Cl1- ligands in the inner coordination sphere than AmIII. These results were indeed unexpected, for example, stability constants for Ac–Cl and Am–Cl were reported to be nearly identical6.

Perhaps differences in steric crowding accounted for the varied H2O and Cl1– CNs for the large AcIII versus smaller AmIII ions (Fig. 5). However, AcIII electronic structure contributions may also contribute to difference in H2O versus Cl1– binding. While the generality and origin of these results have yet to be established, they tempt us to revisit the traditional descriptions of AcIII. For example, consider the possibility that AcIII is substantially less polarizing than the rest of the f-elements, which are well established as hard and oxophilic ions. In this sense, one might crudely compare the changes in chemical hardness from AcIII to AmIII to that of iodine to fluorine. It is conceivable that a reclassification could provide insight into previous reports where actinium behaved substantially different than trivalent actinides and lanthanides41,42. Given that many AcIII chelators are based on the coordination chemistry of lanthanides and minor actinides, better characterization of the long Ac–ligand bond distances, binding preferences, and speciation has the potential to improve design parameters for actinium chelators. In this context, the results here serve as motivation for future work focused on using XAFS spectroscopy and MD-DFT calculations to advance understanding of actinium reactivity with ligands that are more relevant to α-therapy development.

Figure 5: Ionic radii of the early to mid-actinides.
figure 5

Scheme showing the ionic radii (Å) of trivalent actinides from actinium to californium drawn to scale for six-coordinate ions40.


General consideration

Caution! The 243Am and 227Ac isotopes α-, β- and γ-emitting radionuclides have high specific activity and decay to α-, β- and γ-emitting isotopes. Hence, this research was conducted in a radiological facility with appropriate analyses of these hazards and implementation of controls for the safe handling and manipulation of these toxic and radioactive materials. All direct handling of these radionuclides was conducted within certified fume hoods and monitored with appropriate α-, β- and γ-particle detecting instruments. The 227Ac and 243Am isotopes were supplied by the United States Department of Energy Office of Science Isotope Program in the Office of Nuclear Physics. Hydrochloric acid and trifluoromethanesulfonic acid were obtained commercially (Fisher Scientific). Water was purified to 18.2 MΩ/cm resistivity using Thermo-Scientific Barnstead Nanopure or Millipore Nanopure water purification systems. Resins used for separations—DOWEX AG1-X8 (BioRad; 100–200; Cl form) and branched DGA (Eichrom)– were suspended in water, and the fines decanted before use. Separations were characterized using γ-spectroscopy using an EG&G Ortec Model GMX-35200-S HPGe detector system in combination with a Canberra Model 35-Plus multichannel analyser associated with Gamma Vision software. Characterization was also performed using α-spectroscopy with and Ortec Octete+ α-spectrometer associated with Ortec Alpha Vision analytical software to control the spectrometer, to acquire and analyse the data.

Sample preparation

The coordination chemistry studies described herein made use of 227Ac (2 mCi; 28 μg) and 243Am (0.5 mg per sample). Safety concerns regarding the radiation dose from the 227Ac sample were mitigated by removing the 227Ac daughters (primarily 227Th and 223Ra) the day before shipping to the SSRL synchrotron facility and by completing the measurements before significant quantities of the 227Ac daughters re-emerged, 10 days from separation.

Given the scarcity of 227Ac and 243Am, these actinide isotopes were recycled after the XAFS data collections. In the case of actinium, the sample matrix was converted from HCl to HNO3 (8 M) and the actinium was recovered and purified using the chromatographic procedures described below26,27. For americium, samples were recovered and purified using cation exchange chromatography50. In general, the samples were dissolved in dilute acid (five drops HCl in 5 mL H2O) and loaded onto a Biorad column (10 ml) charged with AG50x8 resin (2 ml) that had been conditioned with HCl (1 M; 5 × 10 ml). The column was washed with HCl (0.1 M; 6 × 10 ml), and americium was eluted from the column using concentrated HCl (12 M; 5 × 5 ml). The recovered actinium and americium samples were analysed by γ-spectroscopy to confirm isotopic purities and the americium samples by ICP-AES to confirm chemical purities.

Actinium-227 samples

Using previously established methods26,27, radiochemical purification of 227Ac was accomplished by exploiting oxidation state differences between the AcIII parent and the tetravalent (ThIV) and divalent (RaII) daughters (Fig. 6). The 227Ac isotope, and its daughters, were dissolved in HNO3 (1 ml; 8 M). The solution was loaded using HNO3 (4 × 1 ml; 8 M) onto a Biorad column charged with an anionic exchange resin (1 ml, AG1-X8, BioRad). The resin had been conditioned with H2O (5 × 3 ml), HNO3 (5 × 3 ml 8 M), H2O (1 × 2 ml) and HNO3 (3 × 3 ml 8 M). Under these conditions, 227Ac, 223Ra, 211Pb and 211Bi, eluted from the column during the load and with subsequent washes with HNO3 (10 ml; 8 M). Meanwhile 227Th was retained on the resin. The eluted 227Ac fractions were combined and diluted with water by a factor of two, such that the resulting solution contained HNO3 (4 M). The solution was loaded onto a Biorad column charged with branched DGA resin (1 ml). The resin has been conditioned with HNO3 (3 × 2 ml; 0.05 M) followed by HNO3 (3 ml; 4 M). Under these conditions, 223Ra eluted while 227Ac remained bound to the resin. The resin was washed with HNO3 (3 × 2 ml; 4 M). Subsequently, 227Ac was eluted using with HNO3 (4 × 2 ml; 0.05 M). The 227Ac concentration was determined by γ-spectroscopy to be highest in the first two fractions. The 227Ac fractions were combined and the solution evaporated in a conic shape glass vial on a hot plate under a slow stream of air to a soft dryness. The solid residue was converted from NO31− to Cl1− to generate a solution of actinium in concentrated HCl by repeated evaporation and dissolution in HCl (11 M; 2 × 2 ml). The solid residue was then dissolved in HCl (0.455 ml; 11 M) and transferred to the XAFS holder.

Figure 6: Cartoon describing 227Ac radiochemical purification.
figure 6

Scheme showing the procedure followed to separate 227Ac from its daughters 229Th and 223Ra using anion exchange resin and DGA resin, respectively.

Americium-243 samples

Americium samples in either HCl (11 M) or HO3SCF3 (0.11 M) acidic solutions were prepared from a stock of AmO2 dissolved in HCl (6 M). Solutions of americium in HCl (11 M) were generated in direct analogy to the method described above for actinium. Briefly, an aliquot from an 243Am stock solution containing AmIII (0.6875, mg) in HCl (0.250 ml; 6 M) was heated to dryness in a glass vial in a sand bath on a hot plate. The solid was then dissolved in concentrated HCl (0.5 ml; 11 M) and this evaporation/dissolution process was repeated two more times. The resulting solid residue was dissolved (peach colour) in HCl (0.455 ml; 11 M) and transferred to the XAFS holder.

The solution containing americium aquo ion was prepared from an aliquot of an 243Am stock solution containing AmIII (0.6875, mg) dissolved in HCl (0.250 ml; 6 M). The solvent was removed by heating the solution in a glass vial in a sand bath on a hot plate. The solid residue was then dissolved in Millipore H2O and transferred to an Eppendorf tube (2 ml volume). Quickly, NaOH (0.050 ml; 2 M) was added, the solution shaken, and centrifuged for 3 min (6,000 r.p.m.). The supernate was decanted from the resulting pink precipitate and discarded. The solid was washed with NaOH (2 × 0.06 ml; 10 mM) and with Millipore H2O. The solid precipitate was then dissolved in trifluoromethanesulfonic acid (0.455 ml; 0.11 M) and transferred to the XAFS holder.

XAFS Sample preparation

All XAFS samples were loaded into XAFS cells that were triply contained, which protected against release of radiological material during samples shipment and XAFS experiments. The XAFS holder consisted of a plastic holder body with a 2 mm well equipped with a set of Teflon and a Kapton windows (1 mil). Solutions were introduced into the holder through an injection hole sealed with a gasket that was held in place by an aluminium plate. The sample cell holder was then transferred into the secondary and the tertiary container, which were best described as a set of nested aluminium holders equipped with Kapton windows (2 mil).

XAFS measurements

The XANES and EXAFS were measured at SSRL under dedicated operating conditions (3.0 GeV, 5%, 500 mA) on end station 11-2. This beamline was equipped with a 26-pole, 2 Tesla wiggler, utilized a liquid nitrogen-cooled double-crystal Si[220] monochromator and employed a collimating and focusing mirrors. A single energy was selected from the white beam with a liquid-N2-cooled double-crystal monochromator utilizing Si[220] (ϕ=0) crystals. The crystals were run de-tuned by 35%, 500 eV above the absorption edge to eliminate higher harmonics from the monochromatic light. The samples were attached to the beamline 11-2 XAFS rail. The rail was equipped with three ionization chambers through which nitrogen gas was continually flowed. One chamber was positioned before the sample holder, to monitor the incident radiation (I0, 10 cm). The second chamber was positioned after the sample holder, such that sample transmission (I1, 30 cm) could be evaluated against I0, while a third chamber (I2, 30 cm) positioned downstream from I1, so that the XANES of a calibration foil could be measured in situ during the XAFS experiments against I1. Conditions for the americium aqua ion sample was also optimized for transmission data collection. Actinium and americium solution samples in concentrated HCl were measured in fluorescence mode using solid-state 100-Ge element detector against the incident radiation (I0). Low-energy contributions to the fluorescence signal were removed using a bromine filter (three path lengths) for actinium and yttrium (three path lengths) for americium. Before measurements, dead-time correction measurements were performed at 400 eV above the element edge of the filter. The dead time correction curve corresponds to the plot of the windowed counts of the emission line of interest versus the total of incoming counts in the solid-state detector. This procedure was performed by putting filters (Se for Ac and Sr for Am) in front of the fluorescence detector.

XAFS data analysis

Data manipulation and analysis was conducted as previously described51. First the data were dead-time corrected and calibrated to the energy of the first inflection point of the calibration foil measured in situ. The measurements were calibrated as follows. For actinium, a RbCl pellet was prepared by sandwiching RbCl diluted with BN to a one absorption length thickness. The energy for the first inflection point was determined in comparison with the Bi LII-edge (15,711 eV) to be 15,203.81 eV. Americium samples were calibrated to a zirconium foil at 17,998 eV. Data from the analytes were analysed by fitting a line to the pre-edge region, which remove the background from experimental data in the spectra. Then a second- to third-order polynomial fitting was chosen for the post-edge region. The difference between pre- and post-edge lines is set to unity at the first inflection point, normalizing the absorption jump to 1.0. Each of the samples were measured for several hours resulting in the collection of 25 scans for Ac and five scans for Am. Fittings using ATHENA and ARTEMIS52 were performed using crystallographic data from americium triflate33, americium trichloride hexahydrate36 and FEFF8 calculations32. The spectra were fitted using only single-scattering paths obtained from FEFF8. The adjustments of spectra were performed in different k and R ranges for each samples, where R is the distance to the neighbouring atom; americium triflate was adjusted in 2.6<k<12 Å–1 and 1.25<R<3 Å, americium in concentrated HCl in 2.6<k<10.5 Å–1 and 1.1<R<3.5 Å and actinium in concentrated HCl in 2.6<k<9 Å–1 and 1.2<R<3.45 Å. For the fitting procedure, the CN, the distance (R) and the Debye–Waller factor (σ2) were allowed to vary but for the last factor a single value was chosen for both paths used for the first shell. A single value of energy shift (ΔE0) was used for all scattering paths. The amplitude reduction factor (S02) was set at 0.9 based on initial fits.

MD-DFT calculations

The Born–Oppenheimer MD simulations in the Helmholtz ensemble (NVT) were performed using the computer code VASP (Vienna Ab-initio Simulations Package)53 version 5.35. In this code, the forces on the ions are calculated from the electronic structure of the whole system computed using DFT at the generalized gradient approximation level using the functional by Purdue–Burke–Enzerhof54. A simulation box of (12.54 × 12.45 × 12.68 Å3) was used, including the metal ion (M3+), three Cl1− counter-ions maintained the simulation box neutral, and for solvent medium we used 64 water molecules. However, for the simulations of the single aquo ion no counter-ions were added to the system and a uniform background charge of −3 was added to keep the neutrality of the simulation box. The basis set consists in an expansion into plane-wave functions. Because of the large size of the simulation box, the k-space representation included only the Γ point. The energy cutoff for the plane-wave expansion was set at 500 eV and scalar relativistic effects were included using the PAW-PBE potentials55. Initially the metal ion and the closest neighbouring molecules and counter ions were kept frozen and the solvent plus remaining counter-ion atoms were heated up to 498 K to be thermalized for 1 ps. After that a 1 ps run was done at 298 K with all the degrees of freedom released to thermalize the complex with the solvent. Finally a 1 ps data collection run was performed where we monitored the solvent and ion dynamics.

Data availability

The data that support the findings of this study are available within the article or from the corresponding authors on request.

Additional information

How to cite this article: Ferrier, M. et al. Spectroscopic and computational investigation of actinium coordination chemistry. Nat. Commun. 7:12312 doi: 10.1038/ncomms12312 (2016).


  1. McDevitt, M. R. et al. Radioimmunotherapy with alpha-emitting nuclides. Eur. J. Nucl. Med. 25, 1341–1351 (1998).

    CAS  Article  Google Scholar 

  2. Steinbach, O. C. The latest developments in therapeutic delivery. Ther. Deliv 5, 113–118 (2014).

    CAS  Article  Google Scholar 

  3. Parker, S. et al. Alpha emitter radium-223 and survival in metastatic prostate cancer. N. Engl. J. Med. 369, 213–223 (2013).

    CAS  Article  Google Scholar 

  4. Mathur, J. N., Murali, M. S. & Nash, K. L. Actinide partitioning—a review. Solvent Extr. Ion Exc. 19, 357–390 (2001).

    CAS  Article  Google Scholar 

  5. Poinssot, C., Rostaing, C., Baron, P., Warin, D. & Boullis, B. Main results of the French program on partitioning of minor actinides, a significant improvement towards nuclear waste reduction. Proc. Chem.y 7, 358–366 (2012).

    CAS  Article  Google Scholar 

  6. Morss, L. R., Edelstein, N. M. & Fuger, J. The Chemistry of the Actinide and Transactinide Elements Springer (2006).

  7. Paviet-Hartmann, P., Cerefice, G., Stacey, M. R. & Bakhtiar, S. in Proceedings of ICONE19, 19th International Conference on Nuclear Engineering (Chiba, Japan, 2011).

  8. Evans, W. J. & Kozimor, S. A. Expanding the chemistry of U3+ reducing agents. Coord. Chem. Rev. 250, 911–935 (2006).

    CAS  Article  Google Scholar 

  9. Drozdzynski, J. Tervalent uranium compounds. Coord. Chem. Rev. 249, 2351–2373 (2005).

    CAS  Article  Google Scholar 

  10. Knope, K. E. & Soderholm, L. Solution and solid-state structural chemistry of actinide hydrates and their hydrolysis and condensation products. Chem. Rev. 113, 944–994 (2013).

    CAS  Article  Google Scholar 

  11. Antonio, M. R., Williams, C. W. & Soderholm, L. Berkelium redox speciation. Radiochim. Acta 90, 851–856 (2002).

    CAS  Article  Google Scholar 

  12. Skanthakumar, S., Antonio, M. R., Wilson, R. E. & Soderholm, L. The curium aqua ion. Inorg. Chem. 46, 3485–3491 (2007).

    CAS  Article  Google Scholar 

  13. Polinski, M. J., Alekseev, E. V., Depmeier, W. & Albrecht-Schmitt, T. E. Recent advances in trivalent f-element borate chemistry. Z. Kristallogr. 228, 489–498 (2013).

    CAS  Google Scholar 

  14. Cary, S. K. et al. Emergence of californium as the second transitional element in the actinide series. Nat. Commun. 6, 1–8 (2015).

    ADS  Article  Google Scholar 

  15. Cross, J. N. et al. Syntheses, structures, and spectroscopic properties of plutonium and americium phosphites and the redetermination of the ionic radii of Pu(III) and Am(III). Inorg. Chem. 51, 8419–8424 (2012).

    CAS  Article  Google Scholar 

  16. NSAC Isotopes Subcommittee, Meeting Isotope Needs and Capturing Opportunities for the Future: The 2015 Long Range Plan for the DOE-NP Isotope Program. (July 2015).

  17. Miederer, M., Scheinberg, D. A. & McDevitt, M. R. Realizing the potential of the actinium-225 radionuclide generator in targeted alpha particle therapy applications. Adv. Drug Deliv. Rev. 60, 1371–1382 (2008).

    CAS  Article  Google Scholar 

  18. Kim, Y.-S. & Brechbiel, M. W. An overview of targeted alpha therapy. Tumor Biol. 33, 573–590 (2012).

    CAS  Article  Google Scholar 

  19. Duckworth, O. W., Bargar, J. R. & Sposito, G. Sorption of ferric iron from ferrioxamine B to synthetic and biogenic layer type manganese oxides. Geochim. Cosmochim. Acta 72, 3371–3380 (2008).

    CAS  ADS  Article  Google Scholar 

  20. Lukens, W. W., Shuh, D. K., Schroeder, N. C. & Ashley, K. R. Identification of the non-pertechnetate species in Hanford waste tanks, Tc(I)-carbonyl complexes. Environ. Sci. Technol. 38, 229–233 (2004).

    CAS  ADS  Article  Google Scholar 

  21. Jensen, M. P., Neuefeind, J., Beitz, J. V., Skanthakumar, S. & Soderholm, L. Mechanisms of metal ion transfer into room-temperature ionic liquids: the role of anion exchange. J. Am. Chem. Soc. 125, 15466–15473 (2003).

    CAS  Article  Google Scholar 

  22. Spezia, R., Beuchat, C., Vuilleumier, R., D'Angelo, P. & Gagliardi, L. Unravelling the hydration structure of ThX4 (X=Br, Cl) water solutions by molecular dynamics simulations and X-ray absorption spectroscopy. J. Phys. Chem. B. 116, 6465–6475 (2012).

    CAS  Article  Google Scholar 

  23. Atta-Fynn, R. et al. Structure and hydrolysis of the U(IV), U(V), and U(VI) aqua ions from ab initio molecular simulations. Inorg. Chem. 51, 3016–3024 (2012).

    CAS  Article  Google Scholar 

  24. Bera, M. K. et al. Aggregation of heteropolyanions in aqueous solutions exhibiting short-range attractions and long-range repulsions. J. Phys. Chem. C 120, 1317–1327 (2016).

    CAS  Article  Google Scholar 

  25. Priest, C., Tian, Z. & Jiang, D. First-principles molecular dynamics simulation of the Ca2UO2(CO3)3 complex in water. Dalton Trans. 45, 9812–9989 (2016).

    CAS  Article  Google Scholar 

  26. Zielinska, B., Apostolidis, C., Bruchertseifer, F. & Morgenstern, A. An improved method for the production of Ac-225/Bi-213 from Th-229 for targeted alpha therapy. Solvent Extr. Ion Exc. 25, 339–349 (2007).

    CAS  Article  Google Scholar 

  27. Apostolidis, C., Molinet, R., Rasmussen, G. & Morgenstern, A. Production of Ac-225 from Th-229 for targeted α therapy. Anal. Chem. 77, 6288–6291 (2005).

    CAS  Article  Google Scholar 

  28. Teo, B. K. EXAFS: Basic Principles and Data Analysis Springer (1986).

  29. Stohr, J. NEXAFS Spectroscopy 25 (Springer-Verlag Berlin Heidelberg, (1992).

  30. Soderholm, L., Williams, C., Skanthakumar, S., Antonio, M. R. & Conradson, S. The synthesis and characterization of the superconductor-related compound Pb2Sr2AmCu3O8 . Z. Phys. B 101, 539–545 (1996).

    CAS  ADS  Article  Google Scholar 

  31. Runde, W. H. & Mincher, B. J. Higher oxidation states of americium: preparation, characterization and use for separations. Chem. Rev. 111, 5723–5741 (2011).

    CAS  Article  Google Scholar 

  32. Ankudinov, A. L., Ravel, B., Rehr, J. J. & Conradson, S. D. Real space multiple-scattering calculation and interpretation of X-ray absorption near-edge structure. Phys. Rev. B 58, 7565–7576 (1998).

    CAS  ADS  Article  Google Scholar 

  33. Lindqvist-Reis, P. et al. The structures and optical spectra of hydrated transplutonium ions in the solid state and in solution. Angew. Chem. Int. Ed. Engl. 46, 919–922 (2007).

    CAS  Article  Google Scholar 

  34. Stumpf, T., Hennig, C., Bauer, A., Denecke, M. A. & Fanghanel, T. An EXAFS and TRFLS study of the sorption of trivalent actinides onto smectite and kaolinite. Radiochim. Acta 92, 133–138 (2004).

    CAS  Article  Google Scholar 

  35. Allen, P. G., Bucher, J. J., Shuh, D. K., Edelstein, N. M. & Craig, I. Coordination chemistry of trivalent lanthanide and actinide ions in dilute and concentrated chloride solutions. Inorg. Chem. 39, 595–601 (2000).

    CAS  Article  Google Scholar 

  36. Burns, J. H. & Peterson, J. R. The crystal structures of americium trichloride hexahydrate and berkelium trichloride hexahydrate. Inorg. Chem. 10, 147–151 (1971).

    CAS  Article  Google Scholar 

  37. Downward, L., Booth, C. H., Lukens, W. W. & Bridges, F. A variation of the F-test for determining statistical relevance of particular parameters in EXAFS fits. AIP Conf. Proc. 882, 129–131 (2006).

    ADS  Article  Google Scholar 

  38. Fried, S., Hagemann, F. & Zachariasen, W. H. The preparation and identification of some pure actinium compounds. J. Am. Chem. Soc. 72, 771–775 (1950).

    CAS  Article  Google Scholar 

  39. Kirby, H. W. & Morss, L. R. The Chemistry of the Actinide and Transactinide Elements Ch. 2 (Springer, Dordrecht (2006).

  40. Shannon, R. D. Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides. Acta Crystallogr. A32, 751–767 (1976).

    CAS  ADS  Article  Google Scholar 

  41. Radchenko, V. et al. Application of ion exchange and extraction chromatography to the separation of actinium from proton-irradiated thorium metal for analytical purposes. J. Chromatogr. A 1380, 55–63 (2015).

    CAS  Article  Google Scholar 

  42. Horwitz, E. P., McAlister, D. R., Bond, A. H. & Barrans, R. E. Jr Novel extraction of chromatographic resins based on tetraalkyldiglycolamides: characterization and potential applications. Solvent Extr. Ion Exc. 23, 319–344 (2005).

    CAS  Article  Google Scholar 

  43. Hagemann, F. T. in National Nuclear Energy Series, Manhattan Project Technical Section, Division 4: Plutonium Project, Vol. 14A (eds Joseph J. K. and Seaborg G. T.), 14–44 (McGraw-Hill, 1954).

  44. Karalova, Z. K., Myasoedov, B. F. & Rodionova, L. M. Spectrophotometric determination of actinium. J. Anal. Chem. 28, 942–945 (1973).

    CAS  Google Scholar 

  45. Zachariasen, W. H. Crystal chemical studies of the 5f-series of elements. I. New structure types. Acta Crystallogr. 1, 265–268 (1948).

    CAS  Article  Google Scholar 

  46. Zachariasen, W. H. Crystal chemical studies of the 5f-series of elements. VI. The Ce2S3-Ce3S4 type of structure. Acta Crystallogr. 2, 57–60 (1949).

    CAS  Article  Google Scholar 

  47. Zachariasen, W. H. Crystal chemical studies of the 5f-series of elements. XII. New compounds representing known structure types. Acta Crystallogr. 2, 388–390 (1949).

    CAS  Article  Google Scholar 

  48. Farr, J. D., Giorgi, A. L., Bowman, M. G. & Money, R. K. The crystal structure of actinium metal and actinium hydride. J. Inorg. Nucl. Chem. 18, 42–47 (1961).

    CAS  Article  Google Scholar 

  49. Weigel, F. & Hauske, H. The lattice constants of actinium(III) oxalate decahydrate. J. Less Common Metals 55, 243–247 (1977).

    CAS  Article  Google Scholar 

  50. Stevenson, P. C. & Nervik, W. E. The Radiochemistry of the Rare Earths, Scandium, Yttrium, and Actinium. (National Academy of Sciences National Research Council (US). Subcommittee on Radiochemistry (1961).

  51. Calvin, S. XAFS for Everyone CRC Press (2013).

  52. Ravel, B. & Newville, M. ATHENA, ARTEMIS, HEPHAESTUS: data analysis for X-ray absorption spectroscopy using IFEFFIT. J. Synchrotron Radiat. 12, 537–541 (2005).

    CAS  Article  Google Scholar 

  53. Kresse, G. & Hafner, J. Ab initio molecular dynamics for liquid metals. J. Phys. Rev. B 47, 558–561 (1993).

    CAS  ADS  Article  Google Scholar 

  54. Perdew, J. P., Burke, K. & Ernzerhof, M. Generalized gradient approximation made simple. Phys. Rev. Lett. 77, 3865–3868 (1996).

    CAS  ADS  Article  Google Scholar 

  55. Kresse, G. & Joubert, J. From ultrasoft pseudopotentials to the projector augmented-wave method. Phys. Rev. B 59, 1758–1775 (1999).

    CAS  ADS  Article  Google Scholar 

  56. Brendebach, B. et al. X-ray absorption spectroscopic study of trivalent and tetravalent actinides in solution at varying pH values. Radiochim. Acta 97, 701–708 (2009).

    CAS  Article  Google Scholar 

  57. Kirsh, R. et al. Oxidation state and local structure of plutonium reacted with magnetite, mackinawite and chukanovite. Environ. Sci. Technol. 45, 7267–7274 (2011).

    ADS  Article  Google Scholar 

  58. Marques Fernandes, M., Scheinost, A. C. & Baeyens, B. Sorption of trivalent lanthanides and actinides onto montmorillonite: macroscopic, thermodynamic and structural evidence for ternary hydroxo and carbonato surface complexes on multiple sorption sites. Water Res. 99, 74–82 (2016).

    Article  Google Scholar 

  59. Galbis, E. et al. Solving the hydratation structure of the heaviest actinide aqua ion known: the californium(III) case. Angew. Chem. Int. Ed. Engl. 122, 3899–3903 (2010).

    Article  Google Scholar 

  60. Revel, R. et al. First investigation on the L edges of the 249Cf aquo ion by X-ray absorption spectroscopy. Inorg. Chem. 38, 4139–4141 (1999).

    CAS  Article  Google Scholar 

Download references


The work was supported under the LANL LDRD program (JMB, ERV and JWE) and work under the Heavy Element Chemistry Program by the Division of Chemical Sciences, Geosciences and Biosciences, Office of Basic Energy Sciences, the US Department of Energy and the US Department of Energy (ERB and SAK). Portions of this work were supported by postdoctoral and graduate Fellowships from the Glenn T. Seaborg Institute (MGF, BWS, SCES and JJW), and the Director’s Postdoctoral Fellowship (HSLP and JNC). Los Alamos National Laboratory is operated by Los Alamos National Security, LLC, for the National Nuclear Security Administration of the US Department of Energy (contract DE-AC52-06NA25396). We are grateful to the United States Department of Energy, Office of Science, Isotope Development and Production for Research and Application subprogram within Office of Nuclear Physics for support and for supplying the 227Ac and 243Am isotopes. Use of the Stanford Synchrotron Radiation Lightsource, SLAC National Accelerator Laboratory, was supported by the US Department of Energy, Office of Science, Office of Basic Energy Sciences under Contract No. DE-AC02-76SF00515. The SSRL Structural Molecular Biology Program is supported by the DOE Office of Biological and Environmental Research, and by the National Institutes of Health, National Institute of General Medical Sciences (including P41GM103393). The contents of this publication are solely our responsibility and do not necessarily represent the official views of NIGMS or NIH.

Author information

Authors and Affiliations



E.R.B, J.W.E., S.A.K., J.M.B., J.J.W. and M.G.F. conceived and designed the experiments. M.G.F., S.A.K., J.N.C. and S.C.E.S. prepared the analysed samples. M.G.F., H.S.L.P., S.A.K., J.L.P. and B.W.S. did the XAFS measurements on samples. M.G.F. and J.L.P did the XAFS data analysis. E.R.B. performed the DFT calculations. All the authors discussed the results and wrote the paper.

Corresponding authors

Correspondence to Enrique R. Batista or Stosh A. Kozimor.

Ethics declarations

Competing interests

The authors declare no competing financial interests.

Rights and permissions

This work is licensed under a Creative Commons Attribution 4.0 International License. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in the credit line; if the material is not included under the Creative Commons license, users will need to obtain permission from the license holder to reproduce the material. To view a copy of this license, visit

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Ferrier, M., Batista, E., Berg, J. et al. Spectroscopic and computational investigation of actinium coordination chemistry. Nat Commun 7, 12312 (2016).

Download citation

  • Received:

  • Accepted:

  • Published:

  • DOI:

Further reading


By submitting a comment you agree to abide by our Terms and Community Guidelines. If you find something abusive or that does not comply with our terms or guidelines please flag it as inappropriate.


Quick links

Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing