Introduction

Arsenic, above a certain threshold level, is extremely toxic for human body1,2,3,4. Arsenic bearing minerals are abundant in the Earth’s crust which can gradually dissolve in groundwater from weathered rocks and soils1,5, thereby increasing contamination and toxicity in places with no history of arsenic related health problems6,7. Most disturbingly, human activities like mining and industrialization can further aggravate arsenic contamination locally. Therefore, the search for efficient method(s) of stable and long-serving arsenic remediation is essential.

The common arsenic species in circumneutral natural water are hydrated anions of As(V) (H2AsO4− and HA sO42−) and the hydrated As(III) - the neutral molecule H3AsO3. Existing arsenic removal techniques1,8,9,10,11,12 generally rely on surface adsorption of charged contaminant ions on adsorbent surfaces which fail to work for neutral H3AsO31,13,14,15,16,17. Therefore, there exists no single efficient method of direct As(III) removal. In contrary, As(III) is significantly more toxic than As(V)18 and more mobile in water17 which makes it one of the greatest dangers to humanity. For example, in the Gangetic basin of Indian peninsula, almost 100 million people are currently at a risk of As(III) contamination of varying degrees19,20,21. At present, As(III) remediation employs pre-oxidation of As(III) to As(V) and subsequent removal of As(V) by standard adsorption-based techniques1,8,9. Even then these efforts have serious limitations because adsorption-based technologies do not permanently remove As(V); which may simply be re-introduced into the natural cycle under reducing conditions22.

Interestingly, a few viable solutions to such contamination problems involving certain microorganisms (biomineralization) already exist in nature. For example, the oxidation of Fe(II) in acid mine drainage water containing both Fe(II) and As(III) results in trapping of As(III) by Acidithiobacillus ferrooxidans strains into Tooeleite mineral23,24,25,26 (general formula Fe6(AsO3)4SO4 (OH)4.4H2O). Such mineralization processes strongly limit the mobility of heavy metal ions such as arsenic and could offer an effective remediation strategy. However, natural crystalline Tooeleite forms in acidic medium, with SO42− ions and at prolonged timescales23,24,25,26,27. Therefore, natural Tooeleite formation process as such cannot be conceived as an As(III) removal method from natural water, unless there are means to implement it at neutral pH and without SO42− ions (usually absent in natural groundwater). Here, we show that it is possible to instigate nucleation of Tooeleite-like template even in natural contaminated water (pH~7) devoid of SO42− ions, bearing both As(III) and Fe(III) (Fe(III) is also a common natural contaminant) with the help of wurtzite ZnS nanorods. The underlying strategy here is to provide large number of insoluble nano-acidic-surfaces (will be abbreviated as INAS from now on) in the form of Zn-only polar planes of ZnS nanorods28,29,30 inside water, which initiates Tooeleite-like template formation within otherwise neutral aqueous media under moderate heating for 3 hours. This mechanism is unequivocally confirmed by our theoretical modelling and finally, we are being able to suggest a hitherto unknown efficient pathway of direct As(III) remediation of water.

Results and Discussion

The wurtzite structure possesses extremely polar all-cationic and all-anionic crystallographic planes and research shows28,29 that it tends to grow in a cylindrical rod-like morphology with nonpolar lateral surfaces and high surface energy polar bases consisting of all Zn2+ (0001) or all S2− (000ī) ions. A representative crystal structure of such a nanorod is shown in Fig. 1(a). We have previously demonstrated that polar planes, normal to the long axis of the nanorods, can trigger many unusual reactions/phase formations in water30. Here, we exploit this unique feature of ZnS nanorods for As(III) remediation, where Zn2+ (0001) polar planes have been supplied in water as INAS. High-resolution TEM images of the as-grown nanorods are shown in Fig. 1(b), indicating the presence of reasonably monodisperse nanorods 8–10 nm in length and 1–1.5 nm in diameter. The Zn-only ends of these nanorods are highly polar and of Lewis acidic nature (INAS), which floats around in neutral water offering a conducive atmosphere to the Fe(III) and As(III) ions to get mineralized in form of Tooeleite.

Figure 1
figure 1

(a) Model of as synthesized ZnS nanorods, (b) TEM image of as-synthesized ZnS nanorods, (c) Percentage removal of arsenic and iron from natural water (from Kolkata, India (NW-Kolkata) and Sardinia, Italy (NW-Sardinia)) and artificial water (equivalent to the concentration of natural water of Kolkata (AF-Lab)) in the absence (Blank) and presence of ZnS nanorods (ZnS-NR). Inset shows the arsenic concentration (in ppb) in natural water collected during different time periods and locations in India before (orange dot) and after (blue dot) treatment with ZnSnanorods; World Health Organization (WHO) guideline of 10ppb (red line) is provided for comparison. (d) Shows TEM image of as-formed microcrystals from sample NW_Kolkata-ZnS_NR. Inset shows HRTEM of the same microcrystals, SAED diffraction of the microcrystal and the image of the actual product (light yellowish coloured) formed after ZnS treatment of NW-Kolkata.

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In this work, we experimented with three different samples of water, i.e., As(III) and Fe(III) contaminated ground water from West Bengal, India (NW-Kolkata: ‘NW’ denotes natural water), a laboratory-made aqueous solution of Fe3+ and As3+cations intended to mimic the concentrations of the previous sample (AF-Lab: ‘AF’ denotes As and Fe) and As-spiked natural water from Sardinia island, Italy (‘NW’-Sardinia: see Supplementary Table S1). The first two samples had ~0.4 mg/L of arsenic and the sample from Sardinia contained ~0.2 mg/L (Supplementary Table S1); the permissible amount of arsenic in potable water as defined by the World Health Organization is 0.01 mg/L31. Notably, the arsenic concentration in natural water sources vary quite significantly at different times of the year, especially before and after the rainy season (Supplementary Table S1)5. We thus collected water from the local area at different times of the year to confirm the efficiency and consistency of our method (see inset of Fig. 1(c)). However, in this paper, we only present detailed results from samples with the highest initial arsenic content. The simple treatment that we propose here is to add a given quantity of ODA-capped ZnS nanorods to a given volume of sample water and then heat the solution at 70 °C for a duration of 3 hours under continuous stirring. For analysis, the resultant solutions were filtered using Whatman 42 filter paper (~2.5 μm pore size) and the corresponding filtrates and residues (whenever available) were collected. In all cases, the solutions turned yellow with turbidity (right lower inset to Fig. 1(d)) after treatment. All samples (samples NW-Kolkata_ZnS-NR, AF-Lab_ZnS-NR and NW-Sardinia_ZnS-NR) before and after treatment were quantitatively analysed using ICP-OES/MS following standard protocol for determination of As and Fe concentrations. Water samples without ZnS nanorods were also treated identically, which are ‘Blank’ samples (NW-Kolkata_Blank, AF-Lab_Blank and NW-Sardinia_Blank) and analysed quantitatively before and after the heat treatment.

The experimentally obtained removal percentages of As and Fe are summarized in Fig. 1(c). Figure 1(c) reveals that treatment with ZnS nanorods works efficiently and removes more than 90% of the contaminant As(III) ions, whereas the ‘Blank’ treatment results in ≤10% removal. The NW-Kolkata sample is expected to contain some As(V) along with large amounts of As(III), as is known from arsenic speciation studies of the region32,33,34,35,36, which is likely the reason for ~30% arsenic removal, even without ZnS nanorods (see NW-Kolkata_Blank in Fig. 1(c)). However, the AF-Lab and NW-Sardinia samples consisted of only As(III) by design and so it can be concluded that this single-step treatment removes 90±5% of total As(III). The inset to Fig. 1(c) shows the consistency of our method, where samples collected year-round in Kolkata were treated with ZnS nanorods and it is observed that arsenic is reduced to <10 ppb in most of the cases. Even for samples, which have a relatively small initial As-content (~50 ppb), the contaminant is reduced convincingly below 10 ppb, which is otherwise known to be a daunting task1. One important point to note here that our method is able to remove nearly 7g As/g of ODA-coated ZnS, which in an average is three orders of magnitude more efficient than other known methods9,15,37,38,39 of As(III) removal. Moreover, nearly comparable removal efficiency observed with natural water samples (NW-Kolkata and NW-Sardinia) as well as laboratory water (AF-Lab) confirms that other ions do not adversely affect the reaction to any noticeable extent. Fig. 1(d) provides a representative TEM image of the residual solid of NW-Kolkata_ZnS-NR sample and in each case, spindle-like microparticles (~1 μm in length) are found, which readily precipitates and is removed by standard pore-filtration. High Resolution TEM (right upper inset of Fig. 1(d)) shows definite lattice patterns and in selected area electron diffraction (SAED) (left inset of Fig. 1(d)) spots are clearly visible which indicates the residue is crystalline in nature.

The residual microparticles were characterized in details to identify the As-containing phase(s) and to understand the chemical mechanism of the phase formation. Figure 2(b,d,f) provides 2D-XRD images from AF-Lab_ZnS-NR, NW-Kolkata_ZnS-NR and NW-Sardinia_ZnS-NR residues and the extracted θ–2θ patterns are shown in Fig. 2(a,c,e). It was observed that XRD pattern of the AF-Lab_ZnS-NR residue is similar to that of Tooeleite23,24,25,26,40,41 (Fe6(AsO3)4SO4(OH)4.4H2O)), with certain differences, as SO42− is absent in AF-Lab_ZnS-NR residue. Moreover, the pH of the solution was maintained neutral throughout the reaction, unlike acidic medium required for natural Tooeleite23,24,25,26,27. The situation is more complex for natural water samples with multiple ions and microorganisms, where various crystalline phases are formed. The difficulty in analyzing the natural water residues is clear from Fig. 2(d,f), where with weak Tooeleite-like diffraction rings, intense spots of Ca2+ bearing Calcite phase and broader rings of Aragonite phase can be identified. However, the high statistics/resolution patterns obtained from SR-XRD allowed for a multiphase full-profile Rietveld refinement analysis and reliable recognition of the Tooeleite pattern (Fig. 2(c)). The phase identification was more difficult for NW-Sardinia_ZnS-NR residue (Fig. 2(e,f)), where Tooeleite-like peaks were hidden even in the extracted pattern. Nevertheless, it was still possible to identify the presence of a Tooeleite-like structure (see enlarged version of Fig. 2(e)) as the As-bearing entity. Rietveld refinements of these data (except for the NW-Sardinia_ZnS-NR residue) were performed and structural parameters were extracted (Supplementary Table S2). These results were further confirmed by As K-edge Extended X-ray Absorption Fine Structure (EXAFS) spectra (shown in Fig. 2(g)) from which all the local atomic distances were obtained and compared with existing Tooeleite data26 (see Table 1). As the formation of Tooeleite-like structure is confirmed in every case, one also understands the reason for the development of yellow color in the resultant solution every time, which is indeed precipitation of the yellow colored mineral Tooeleite during reaction.

Table 1 Coordination numbers and bond lengths obtained from EXAFS analysis of samples.
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Figure 2
figure 2

Deconvoluted powder XRD pattern obtained from 2D-XRD of samples (a) AF-Lab_ZnS-NR, (c) NW-Kolkata_ZnS-NR and (e) NW-Sardinia_ZnS-NR. Actual 2D-XRD images of samples (b) AF-Lab_ZnS-NR, (d) NW-Kolkata_ZnS-NR (along with other phases from calcium containing minerals, such as calcite and aragonite) and (f) NW-Sardinia_ZnS-NR (contains multiple new phases). (g) As K-edge (experimental and best fit (red line)) obtained for AF-Lab_ZnS-NR (green) and NW-Kolkata_ZnS-NR (purple). (h) Crystal structure obtained by Rietveld refinement of deconvoluted XRD pattern from AF-Lab_ZnS-NR, (i) As K-edge XANES spectra and (j) Photoemission spectra of S 2p for different samples.

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The diffraction data from sample AF-Lab_ZnS-NR allowed for ab-initio structure determinations using the charge-flipping algorithm approach and the model confirmed the presence of the Fe-As-O layers closely resembling Tooeleite, as shown in Fig. 2(h). The central template is nearly identical to that of Tooeleite; made by corner linked Fe octahedra stapled by As in a bridging configuration. These templates are separated by non-bonded anionic entities, which are shown as orange spheres in the image. Furthermore, to probe whether As in the residue were in +3 or +5 oxidation state(s), core level X-ray photoelectron spectroscopy (XPS) and X-ray absorption near edge spectroscopy (XANES; As and Fe K-edge) measurements on all samples were carried out. Whereas the Fe 2p XPS and K-edge XANES spectra (see Supplementary Fig. S2(a,b)) proved +3 oxidation state, the As 3d XPS spectra (Supplementary Fig. S2(c) available online) and As K-edge XANES spectra (Fig. 2(i)) confirmed the presence of As in +3 states in all residual solids. These results establish that indeed synthesized structures mimic the central template of the Tooeleite mineral, chemically and structurally. There could still be arguments regarding the presence and form of sulphur in the residues as externally added ZnS may act as a source of sulphur (although only 20% of the total sulphur needed to form the ideal Tooeleite composition for the amount of residue obtained is provided by the added ZnS) and may even provide SO42− anions. To further confirm this point, sulphur 2p core-level XPS experiments were carried out (see Fig. 2(j)), to identify different sulphur anions42. It is known that S 2p core levels for S2− and SO42− anions appear at two different binding energies42,43,44,45,46, (161.5 eV, as in ZnS and 169.0 eV, as in Tooeleite respectively) and in our experiments, the major sulphur component is S2−, though there is also an accompanying SO42− signal in some cases. Moreover, in AF-Lab_ZnS-NR where the only source of sulphur could be from the added ZnS nanorods, only the S2− signal is observed (see Fig. 2(j)). Therefore, it is established from all the chemical and structural characterizations that our procedure of ‘artificial mineralization’ allows As(III) removal and incorporation on a mineral phase within a structure closely resembling Tooeleite, made up of As-Fe-O layers, separated by non-bonded molecules (e.g. water).

Next, quantum chemical methods were employed to understand the formation of the Tooeleite-like central template in water bearing Fe(III) and As(III) in presence of ZnS nanorods. Generally, Fe(III) ions in water exists as Fe(H2O)6 (A, Fig. 3(a)), which may spontaneously dimerise to form an oxyhydroxide (Fe2(H2O)6(OH)42+: B), with two -OH bridging two Fe-centres (Fig. 3(b))47. Aqua linkages too are possible, but hydroxy linkages are more stable. The enthalpy of formation of A and B are,

Figure 3
figure 3

Optimized structures of various species involved are shown in ball and stick models.

The colour code is brown: Fe(III), red: O, green: As(III), grey: Zn2+, yellow: S2− and small bluish-white spheres are hydrogens.

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In case of complex B there are two OH bridges between the two central Fe atoms and Fe-Fe distance is 2.89 Å and Fe-O(bridge) distance is 1.86 Å, whereas other Fe-O (O from bound water moelcules) distances range from 2.01–2.04 Å (Fig. 3(b)). Therefore, it can be assumed that in experimental conditions, complexes such as A, B along with neutral H3AsO3 are present in the water medium to which ZnS nanorods are added. It is observed that hydrated Fe(H2O)63+, As(OH)3 and Fe-dimer B may form stable inorganic complex BFe4As1(Fig. 3(c)), as

In the complex BFe4As1, the distance between two Fe centers is 2.98 Å and the Fe-O distances are 1.90 Å, while the Fe-As distance is 2.99 Å, As-O distances are 1.76–1.86 Å and Fe-O distances range from 1.85–1.95 Å. Since the enthalpy of formation is positive, the reaction is not spontaneous. Once BFe4As1is formed, the reaction with more molecules of As(OH)3 are favorable and formation of BFe4As4(Tooeleite, Fig. 3(d))is feasible,

To explore the role of ZnS nanorods in forming the tooeleite template and to understand the experimental observations, we theoretically try to model the formation of BFe4As1 in presence of ZnS nanostructures. As a model nanorod we have used a small cluster of Zn14S14, which mimicks the wurtzite nature of the ZnS nanorod. The uniqueness of this nanorod structure is its polar ends, i.e it has one pure Zn end and one pure S end which are highly reactive. In the studies involving model Zn14S14 cluster a partial optimization of atomic positons were carried out, where the positions of only first layer Zn atoms directly interacting with As(OH)3 are allowed to change and the rest three layers were kept fixed30. In any such adsorption reaction the surface atoms are most reactive, thus optimising only the first layer is not very unrealistic. After optimization of the Zn14S14 cluster when the positions of the top Zn atoms were relaxed, the surface Zn-Zn bond-distances decrease, as shown in Fig. 3(e). To study the formation of BFe4As1 from its reactants in the presence of Zn14S14, we probed the simultaneous formation and subsequent binding of BFe4As1 to Zn14S14 cluster (Fig. 3(f), where the oxygen atoms connected to As are bound to the Zn layer) from the reaction:

We find a large binding energy (~1299 kcal/mol), indicating the spontaneous formation of BFe4As1 complex bound to Zn14S14 cluster. The high binding energy stems from strong binding of As(OH)3 on the free Zn surface of the ZnS nanorod. It is seen that, for the chemisorption reaction Zn14S14+ As(OH)3→ (Zn14S14)-As(OH)3 (chemisorbed product), the binding energy is:

Close inspection shows, upon adsorption of As(OH)3 on Zn surface, As-OH distances increase from 1.8 Å as in As(OH)3, only one OH group is retained solely by As and two OH groups interact less with As forming bridge bonds to free surface Zn atoms. Thus, it could be concluded that the reactive free Zn end of the ZnS nanorods does act as INAS and bind to the -OH groups of As(OH)3 virtually causing an elongation of As-OH bonds which makes the As(III) ions more available for attachment to the Fe-complex and the Zn14S14-BFe4As1moiety is easily formed (Fig. 3(f)).

Overall, we show that treatment of contaminated water bearing As(III) and Fe(III) ions with ZnS nanorods at 70 °C for 3 hours permanently removes the contaminants. Our process has two significant improvements over the natural one; it works at neutral pH without SO42− ions and the reaction time is shorter (3 hours). This is achieved by supplying INAS in water in the form of Zn-only ends of the ZnS nanorods instead of a bulk acidic environment as is needed for natural growth of Tooeleite. Moreover, ZnS nanorods break completely after treatment, so no secondary nanoparticle based pollutant is produced. We believe that our results present an archetype to entrap As(III) in artificial minerals and many permanent remedies of environmental contamination issues can be addressed through such artificial mineralization processes and current research should be focused along these directions.

Methods

Materials

ODA (Sigma, >99%), potassium ethyl xanthogenate (Sigma, >96%), zinc acetate dihydrate (Sigma, 98%) were used as received. The ODA was stored in argon all the time prior to use. Ethanol absolute (VWR International, Normapur) and Chloroform (Emparta ACS) were used for synthesis. KOH (Chem Labs, 85%), As2O3 (Nice Laboratories ~99.5%) and Suprapur HNO3 (Merck, Germany, 65%) was used to make AF-Lab water. Deionized water (resistivity 18.2 MΩ cm) used for making artificial arsenic contaminated water, was obtained from a Millipore filter system.

Nanoparticle Synthesis

The synthesis of ZnS nanorods with an average of 8–10 nm in length and 1–2 nm in diameter has been reported previously48,49, which we followed with some modifications. To briefly describe, the precursor Zinc-ethylxanthate (Zn(SSCOC2H5)2) was prepared by dissolving 3.00 g of potassium ethyl xanthogenate and separately 2.05 g of zinc acetate dihydrate in water. The solutions were mixed together and zinc-ethylxanthate salt precipitated out. The salt was washed with water, filtered and dried in vacuum. ODA-coated ZnS nanoparticles were prepared using 0.08 g of as prepared zinc-ethylxanthate, which was dissolved in 1.53 g of molten ODA. ODA was initially exposed to CO2 for 30 mins to form OAOC, zinc-ethylxanthate was added to molten OAOC, under Ar at 100 °C. The nanorod synthesis was carried out in two-steps, first at 105 °C for 5 min and then an additional 10 min at 130 °C. The ODA-coated ZnS nanoparticles were collected by flocculating the sample with ethanol, separated by centrifugation, redispersed in chloroform and drying in vacuum.

Water Treatment

The polar surfaces of the nanorods are relatively more reactive than the mixed Zn-S surface and can trigger formation of new phases as well as precipitation of heavy cations present in an aqueous system30. An identical treatment protocol for ZnS nanorods30 in aqueous solutions containing Fe(III) and As(III) was followed here with an idea of using the Zn-only ends as INAS facilitating Tooeleite nucleation within the overall neutral aqueous media. Three different water samples were targeted here: 1) As(III) contaminated ground water from Baruipur area of West Bengal, India (NW-Kolkata: NW denotes Natural Water); 2) a laboratory-made aqueous solution of As(III) and Fe(III) cations in concentrations matching the concentrations of sample 1 (AF-Lab: ‘AF’ denotes As and Fe); and 3) natural water similar to Baccu Locci mine area of Sardinia, Italy. Sample 3 was prepared using natural water from Iglesias, Sardinia, Italy, which had an identical aquatic composition as in Baccu Locci but without any arsenic, which was later spiked by As(III) in the laboratory with an amount equivalent to the concentration in Baccu Locci water (NW-Sardinia). All these details of the samples are tabulated in Supplementary Table S1 available online. For laboratory experiments, each 10 ml water sample was treated with 0.97 mg of solid containing ODA capped-ZnS nanorods; however, several scaled-up experiments showed that as little as 5 mg of the ZnS-ODA solid is sufficient for the decontamination of 1 litre of water. All treatments (10 ml or 1 L) were carried out at 70 °C for 3 hours, the resultant solutions were filtered using Whatman 42 filter paper (~2.5 μm pore size). In all cases, the corresponding filtrates and residues (whenever available) were collected for quantitative analysis. All of the results presented on the Iglesius water artificially spiked by As(III), are from scaled-up treatments. To ensure the recovery of residue mass, sufficient for different experimental analysis, the natural contaminated water was pre-concentrated significantly by prolonged water evaporation under continuous Argon gas flow (to nullify oxidation of As(III) to As(V)) e.g., the natural water sample from Baruipur, Kolkata was concentrated by 1000–2000 times.

Characterization

The chemical analysis of the water samples, both before and after treatment and of the residue were carried out by ICP-OES (Perkin-Elmer Optima 2100 DV), ICP-OES (Shimadzu ICPE-9000) and ICP-MS instruments (ICP-MS, Elan DRC-e, Perkin-Elmer). The bulk structure of the residues were analyzed using powder X-ray diffraction (PXRD) experiments, which were carried out in the BL-18B Indian beamline of Photon Factory, Japan and by 2-dimentional X-ray diffraction (2D-XRD) in ID09 beamline at the ESRF, France. The integrated 2D-XRD patterns were interpreted with a search-match algorithm through the ICSD database and the presence of Tooeleite was revealed. A Le Bail fit using the monoclinic cell of Tooeleite allowed for lattice parameter extraction for the different samples. The quality of the AF-Lab_ZnS-NR pattern allowed for a structural determination, by the charge-flipping algorithm approach and Rietveld refinement, using the JANA2006 and superflip software50,51. First, a background profile fitting and then lattice parameters were refined using the Le Bail method. A reliable fit was obtained using anisotropic broadening modelling, which resulted in the significant broadening of the (001) peak and its harmonics. The extracted intensity was used for the ab-initio structure solution, which provided the positions of As and Fe and confirmed the C2/m symmetry. The oxygen coordinating these cations were located by a Fourier difference calculation. The interlayer molecules were not located because Fourier maps indicated a significant disorder, as was also confirmed by the (00l) peak broadening. The atomic coordinates of the refined atoms and a plot of the observed, calculated and difference profile curves are shown in Supplementary Table S3 and Fig. S1 available online.

The local structure of the solid was probed by X-ray absorption spectroscopy (XAS) at the Fe and As K-edges in the XAFS beamline of Elettra Synchroton Center, Italy. XAS data analysis was performed by looking at the near-edge (XANES) region (see Supplementary Fig. S2(b) for Fe K-edge XANES, available online) and compared with spectra of reference material and fitting of the extended (EXAFS) signal was carried out within a multi-shell model using a local atomic cluster based on the Tooeleite crystallographic structure (ICSD code number 156179), as shown in Supplementary Fig. S2(d). The structural parameters of all of the samples obtained from XAS experiments (Table 1) matches well with the As and Fe local environment of the Tooeleite structure. X-ray photoelectron spectroscopy (XPS) experiments were carried out in the Materials Science beamline of Elettra Synchroton Center, Italy and in an Omicron photoemission spectrometer equipped with EA-125 analyser and Mg Kα x-ray source. Supplementary Fig. S2(a,c) show the Fe 2p and As 3d core level spectra, respectively, from three solid residue samples and confirm the presence of Fe3+ and As3+ ions in them. The morphology, composition and structure of nanorods and the solid residue were probed in a JEOL-JEM 2100F electron microscope using a 200 kV electron source ultrahigh-resolution transmission electron microscope (UHR FEG-TEM).

The electronic structure studies for all molecules and related species were performed using density functional theory (DFT), as implemented in the Gaussian 09 suite of programs52. Studies were performed using the B3LYP53,54,55 hybrid functional with the 6–31G** basis set for all atoms. For any reaction Reactants → Products, the enthalpy of formation is calculated as:

The stable structures of all isolated molecules and complexes were determined by full geometry optimization in the gas-phase and consequent harmonic frequency calculations were performed to ascertain the stationary points. To obtain the stable structures, a double-check was carried out using the PBE56 functional along with a double zeta polarized (DZP) basis set employing the Quantumwise software57,58,59. The Fe complexes studied here are all low-spin, as there are even numbers of Fe-ions (experimentally also no net moment was found in residues). However, high-spin cases have also been looked into, theoretically. Though the absolute values of energies change for high spin complexes, all important results remain unaltered. The growth of the As(III)-Fe(III) template as in Tooeleite in all directions, predicted by our calculation, is schematically presented in Supplementary Fig. S3 available online.

Additional Information

How to cite this article: Malakar, A. et al. Efficient artificial mineralization route to decontaminate Arsenic(III) polluted water - the Tooeleite Way. Sci. Rep. 6, 26031; doi: 10.1038/srep26031 (2016).