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.

Light absorption engineering of a hybrid (Sn3S72−)n based semiconductor – from violet to red light absorption


The crystalline two-dimensional thiostannate Sn3S7(trenH)2 [tren = tris(2-aminoethyl)amine] consists of negatively charged (Sn3S72−)n polymeric sheets with trenH+ molecular species embedded in-between. The semiconducting compound is a violet light absorber with a band gap of 3.0 eV. In this study the compound was synthesized and functionalized by introducing the cationic dyes Methylene Blue (MB) or Safranin T (ST) into the crystal structure by ion exchange. Dye capacities up to approximately 45 mg/g were obtained, leading to major changes of the light absorption properties of the dye stained material. Light absorption was observed in the entire visible light region from red to violet, the red light absorption becoming more substantial with increasing dye content. The ion exchange reaction was followed in detail by variation of solvent, temperature and dye concentration. Time-resolved studies show that the ion exchange follows pseudo-second order kinetics and a Langmuir adsorption mechanism. The pristine and dye stained compounds were characterized by powder X-ray diffraction and scanning electron microscopy revealing that the honeycomb hexagonal pore structure of the host material was maintained by performing the ion exchange in the polar organic solvent acetonitrile, while reactions in water caused a break-down of the long-range ordered structure.


Metal oxides and -chalcogenides have been studied extensively due to their semiconducting and photocatalytic properties. With an ever increasing global demand for energy, photocatalysis has the potential to provide a sustainable solution by converting two inexhaustible resources, namely sunlight and water, into chemical fuel in the form of hydrogen1,2,3. Another application of photocatalysis is the degradation of organic pollutants including halogenated benzene and phenol derivatives4,5 as well as organic dyes6. Materials such as TiO2, ZnO and SnS2 have been employed in the photogenerated production of hydrogen7,8 and for degradation of pollutants9,10. However, the efficiencies of single phase semiconductors are often limited by charge recombination11,12, and in some cases by large band gaps. While UV-light corresponds to less than 5% of the solar spectrum13, materials may be functionalized to red-shift their solar light response.

Layered metal chalcogenides is a promising group of semiconducting materials with structural features that may be tuned towards desired properties such as heavy metal uptake14,15, catalysis16,17,18 and photocatalysis19,20. A family of violet light absorbing semiconducting two-dimensional thiostannates was denoted R-SnS-1 by Bedard and co-workers21. These compounds have the composition R2Sn3S7 (R is a monovalent cation) and consist of polymeric anionic (Sn3S72−)n sheets separated by charge stabilizing species such as alkali- or alkyl-ammonium based cations. The R-SnS-1 compounds are often prepared by templated hydrothermal or solvothermal synthesis, and the template acts as a structure directing agent in addition to being incorporated into the structure as the cation R. Templates of various nature have been used including Cs+22, Rb+23, tetramethylammonium (TMA)24, protonated quinuclidine (QUINH)25, and protonated 1,4-diazabicyclo[2.2.2]octane (DABCOH)26, and even metal-organic complexes such as Fe[(1,10-phenanthroline)3]2+ have been incorporated in the selenium analogues R-SnSe-127.

The (Sn3S72−)n thiostannate layers are composed of Sn3S4 broken-cube clusters held together by double bridge Sn-(μ-S)2-Sn covalent bonds. This creates a honeycomb-like structure with 24-atom hexagonal pores with a size of approximately 1 nm. Despite consisting of the same structural motifs, the pores can be either regular or distorted hexagonal depending on the synthesis template. As the (Sn3S72−)n layers and the cationic species are only held together by electrostatic interactions, the interlayer distance is flexible and depends on the cation size. This enables post-synthetic exchange of the intercalated cations. Functionalization by ion exchange has been widely applied for layered materials including layered double hydroxides (LDHs)28 and three-dimensional compounds such as metal-organic frameworks (MOFs)29. Comparatively little has still been done in this area for R-SnS-1 type compounds, where the main focus has been on ion exchange by alkali-, alkali earth- or transition metal ions24,30,31,32. Furthermore, it has been proven that the organic cation tert-butyl ammonium (TBA) can be replaced by tetramethylammonium (TMA) while keeping the framework intact25.

In this paper, we report the solvothermal synthesis of lamellar Sn3S7(trenH)2 (tren = tris(2-aminoethyl)amine) and its subsequent functionalization by cationic organic dyes. The aim is to modify the light absorption properties of the pristine violet light absorbing material by post-synthetic modification. The intercalation of Methylene Blue (MB) and Safranin T (ST) into the thiostannate host was carried out by ion exchange in solution and studied in detail. The solvent, temperature, nature of the dye, and dye concentration were varied, and the kinetics of the reactions were investigated. The structural features of the Sn3S7(trenH)2-dye nanocomposites were examined by powder X-ray diffraction (PXRD) and scanning electron microscopy (SEM), while the optical properties were investigated by diffuse reflectance spectroscopy (DRS). Solid state NMR spectroscopy was used to investigate the nature of the cationic species of the parent compound Sn3S7(trenH)2.

Results and Discussion

Structural characterization of pristine Sn3S7(trenH)2

R-SnS-1 type compounds are stacked materials consisting of polymeric anionic (Sn3S72−)n thiostannate layers with charge stabilizing molecular cations located in-between (Fig. 1). The thiostannate layers in Sn3S7(trenH)2 may be described in the hexagonal space group P63/mmc with unit cell dimensions of a = 13.3 Å and c = 19.1 Å33. The thiostannate layers stack in an ABAB sequence along the c-axis. The diameter of the hexagonal pores is 11 Å, while the interlayer distance is 9.6 Å, corresponding to half of the c-axis.

Figure 1: The structure of Sn3S7(trenH)2 consists of honeycomb (Sn3S72−)n layers with cationic species embedded in-between.
figure 1

Sulfur and tin atoms are displayed in orange and grey, respectively. Tris(2-aminoethyl) amine (tren) was used as the synthesis template, and trenH+ ions were intercalated in the structure of the as-synthesized material. The organic dyes Methylene Blue (MB) or Safranin T (ST) were introduced into the structure by ion exchange.

The molecular cations are statically disordered in the crystal structure of Sn3S7(trenH)233, and the nature of the embedded cationic species has not been verified in previous studies. It is proposed by Pienack et al. that the molecular cations are present as protonated tren (trenH+) in agreement with elemental analysis33. In the synthesis of other R-SnS-1 type materials, however, it was reported that the synthesis template may undergo intramolecular structural changes during the solvothermal reaction34. In order to investigate the nature of the templating cation, a solid-state 13C{1H} CP/MAS NMR spectrum was acquired for a sample of as-synthesized Sn3S7(trenH)2 (Fig. 2). The spectrum shows sharp peaks of low relative intensity at 15 and 27 ppm whereas a broad peak of overlapping resonances at approximately 41, 45, 53 and 57 ppm dominates the spectrum. If trenH+ ions were present in an isotropic environment with a proton at the tertiary amine, the three alkyl chains would be equivalent, and only two 13C chemical shifts would be expected as confirmed by the theoretical chemical shifts for trenH+ of 38 and 44 ppm. For comparison the 13C chemical shifts for tren in the liquid state are 40 and 58 ppm (Fig. S1). However, the fact that the cation is disordered in the crystal structure points to small variations in the local chemical environment due to different cation-anion interactions. This results in chemical shift dispersion and thereby broad peaks. The chemical shifts of the broad peak (41–57 ppm) can be assigned to aliphatic C-N carbon atoms. The shifts at 15 and 27 ppm could represent methyl- or methylene groups, respectively. As no other solvents or carbon containing precursors than tren and acetonitrile were used for the synthesis, the peaks at low chemical shifts point to partial breakdown of tren. Due to the low intensity of these peaks in comparison with those at 41–57 ppm, we can conclude that tren is most likely present as trenH+ in the structure.

Figure 2
figure 2

13C CP{1H}/MAS NMR spectrum (9.4 T, 4.0 kHz spinning speed) of pristine Sn3S7(trenH)2.

Structural characterization of dye modified Sn3S7(trenH)2

The disorder of the molecular cations points to weak cation-anion interactions in Sn3S7(trenH)2 enabling ion exchange of colorless trenH+ by optically active cationic species. Aiming to modify the optical properties of the material, Sn3S7(trenH)2 was functionalized by the cationic dyes Methylene Blue (MB) and Safranin T (ST). Samples of pristine Sn3S7(trenH)2 were treated with commercial chloride salts of the cationic dyes. Figure 1 shows a schematic representation of the ion exchange procedure. Initial inspection of the dye stained compounds by optical microscopy (Fig. S2) suggests the dye diffuses into the crystals from the side (i.e. parallel to the [001] crystal faces), as illustrated in Fig. 1. Alternatively, it could have diffused through the hexagonal pores.

Powder X-ray diffraction (PXRD) data were collected on pristine and dye-modified Sn3S7(trenH)2 (Fig. 3). The pattern for the pristine phase matches the phase reported in the literature33. In addition, an impurity of the SnO2 precursor is present; the concentration of SnO2 in a representative Sn3S7(trenH)2 sample was estimated to be 8 wt% by Rietveld refinement (Fig. S4 and Table S1). A later optimization of the synthesis has proven that phase pure Sn3S7(trenH)2 can be obtained by using an excess of sulfur in the solvothermal reaction (Methods Section and Fig. S5). It is expected that SnO2 does not affect the dye adsorption due to its chemically inert and non-porous nature (see Supplementary Information). The crystal structure of Sn3S7(trenH)2 treated with dye in acetonitrile (MeCN) is well preserved. In contrast, treatment of the powder with an aqueous dye solution breaks down the crystalline nature of the material leaving a blue amorphous powder in which only the SnO2 trace is left crystalline. This reveals a loss of long-range crystalline order of the R-SnS-1 compound.

Figure 3: Powder X-ray diffraction data collected on a pristine and two MB stained samples in water and acetonitrile revealing that the crystal structure is maintained by performing the ion exchange in acetonitrile.
figure 3

Reference diagrams for SnO2 (ICSD 160667) and Sn3S7(trenH)233 are shown revealing presence of a SnO2 impurity. Characteristic Sn3S7(trenH)2 peaks have been indexed.

In order to investigate the effect on the unit cell of the ion exchange, powder diffraction data were modelled by Le Bail fitting using the unit cell of pristine Sn3S7(trenH)2 as starting model33. The unit cell c-axis decreases with the dye content, revealing that the distance between the thiostannate layers decreases upon dye exchange (Table 1 and Fig. S3). Due to the planar nature of the MB molecule it seems plausible that the average distance between thiostannate sheets decreases when bulky species such as trenH+ are being exchanged. While the orientation of MB cations between the layers is unknown, they will arrange to have strong cation-anion interactions. This will be achieved by minimizing the cation-anion distance i.e. if the cation is parallel to the thiostannate layers. The width (Hw) of the (004) reflection increases by introducing MB (Table 1 and Fig. S3). This is either an indication of: (1) Particle size decrease along the c-axis, (2) increased strain in the structure or (3) presence of a distribution of interplanar distances in the sample. The two latter are very like to be the case, as MB only partly replaces trenH+ in the as-synthesized sample (see the quantification in the following section). For comparison, the a-axis only changes slightly as does the width of the (200) reflection. This shows that the thiostannate layers maintain their geometry during ion exchange. Overall, the changes of the (00 l) peak width and of the unit cell c-axis reveal ion exchange inside the crystal and not only at the crystal surfaces in agreement with optical microscopy (Fig. S2).

Table 1 Unit cell data determined by Le Bail fitting of PXRD data reveal that the a-axis largely remains unchanged by ion exchange, while introduction of MB decreases the c-axis length representing the interlayer distance.

The structural observations are in excellent agreement with the SEM images of pristine and dye-stained Sn3S7(trenH)2 treated in acetonitrile and aqueous solution (Fig. 4 and Figs S6–9). Images of the pristine compound exhibit plate-like structures, owing to the microporous (Sn3S72−)n sheets spanning the unit cell ab-plane. SEM images of Sn3S7(trenH)2-dye composites treated in acetonitrile reveal the same plate morphology as the unmodified phase, which suggests that the dispersion of Sn3S7(trenH)2 in acetonitrile does not affect the crystal structure of the parent phase as proven by PXRD. However, treatment of the parent thiostannate with an aqueous dye solution results in needle-like domains, which were proven to be amorphous by diffraction (Fig. 3). Treatment of the pristine powder in water without a dye caused a similar loss in crystallinity, which is therefore neither related to the cation nature nor the dye concentration. Possible explanations for the structural breakdown could be either: (1) Water reacts with trenH+ in acid-base reactions, or (2) water acts as a nucleophile and cleaves the Sn-S bonds. The first suggestion is most likely, when taking into account that other R-SnS-1 type compounds templated by tetraalkyl ammonium ions (R4N+) may be synthesized in water21. The R4N+ ion will not undergo acid-base reactions with water. In contrast, modification of the charge of trenH+ following acid-base reactions could lead to a structural collapse due to changed cation-anion interactions between the cations and the thiostannate host. This could possibly lead to cleavage of the layers perpendicular to the stacking direction. Such cleavage would most likely result in thin disc shaped particles. Therefore, it is surprising that needle shaped domains form; however, it cannot be ruled out that the particles are plates seen from the side rather than needles. Regardless, the well-defined needles lack crystalline order. Furthermore, the argument on the acid-base reaction also conflicts the findings by C. Bowes et al.25 who demonstrated aqueous ion exchange of tert-butylammonium (TBA) by tetramethylammonium (TMA). They observed the framework stayed intact even though TBA may react in acid-base reactions similarly to trenH+. This suggests that a complex mechanism causes the breakdown of the lamellar crystal structure, and it is beyond the scope of this study to investigate this reaction in larger detail.

Figure 4
figure 4

SEM images of pristine Sn3S7(trenH)2 and MB stained Sn3S7(trenH)2 functionalized in water and acetonitrile.

Time resolved ion exchange: Effect of dye and solvent

The dye uptake is plotted as a function of reaction time in Fig. 5, as determined by UV-VIS spectroscopy (see the Methods section and the Supplementary Information). The amount of MB that is adsorbed by Sn3S7(trenH)2 at room temperature is substantially larger when the ion exchange is performed in water in comparison with acetonitrile (Fig. 5a) despite the structural change of the parent structure. After 3 hours at room temperature and an initial dye concentration of approx. 230 mg L−1, the uptake of MB reaches 38.8 mg g−1 from water and 4.0 mg g−1 from acetonitrile. This corresponds to a molar substitution of 6.0% and 0.6%, respectively, of trenH+ in Sn3S7(trenH)2, assuming that all cations have a charge of +I. Performing the adsorption in a highly polar solvent such as water most likely facilitates the ion exchange process, thereby increasing the adsorption capacity and enhancing the kinetics. Moreover, the suspected partial exfoliation of the structure in water may cause easier access to more adsorption sites. Despite the superior uptake of dye from aqueous solutions, the majority of adsorption experiments in this study are performed in acetonitrile, as to preserve the crystalline structure of the parent Sn3S7(trenH)2 compound.

Figure 5
figure 5

Adsorbed dye amounts qt (in mg dye ions removed from the solution per g of adsorbent material) in Sn3S7(trenH)2 at different conditions using an initial dye concentration of approx. 230 mg L−1: (a) Solvent effect: Adsorbed MB at room temperature in water and acetonitrile, (b) Dye effect: Adsorbed MB and ST in acetonitrile at 333 K, (c) Temperature effect: Adsorbed MB in acetonitrile at variable temperatures. (d) Kinetics: Pseudo-second order kinetics model fitted to data based on (c).

Under similar experimental conditions, the adsorption of MB vastly exceeds that of ST (Fig. 5b). After 3 hours at 333 K in acetonitrile, the adsorption capacity just reaches 1.9 mg g−1 of ST (molar substitution of 0.1%) in comparison with 33.3 mg g−1 of MB (molar substitution of 5.1%) after 2.5 hours. This might be attributed to the pore size and interlayer distance Sn3S7(trenH)2, which were reported to be 10.9 × 10.9 Å and 6.04 Å, respectively, by N. Pienack et al.33 Li et al. have stated that adsorption can occur in micropores 1.3–1.8 times larger than the kinetic diameter of an adsorbate35. By using this approach, the diffusion along the hexagonal pores in Sn3S7(trenH)2 would allow the transport of molecules with sizes of 6.1–8.4 Å. Given the molecular dimensions of MB (14.3 × 6.1 × 4 Å3)36, it would be possible for the molecules to diffuse lengthwise through the pore channels. Similarly, the diffusion of MB molecules between the (Sn3S72−)n layers should be possible without causing changes in the interlayer distances. Despite the chemical resemblance between MB and ST (Fig. 1) the adsorption of dye onto Sn3S7(trenH)2 was observed to be very selective towards MB. Selectivity often arises due to either electrostatic interaction between adsorbate and adsorbent or due to structurally hindered diffusion37,38. In this case, differences in electrostatic interactions can be ruled out, as both MB and ST have charges of +I. The main structural difference between the two dyes is the additional phenyl-substituent in ST, which increases the bulkiness of ST compared to MB, especially if the phenyl ring is oriented perpendicular to the tricyclic aromatic system. The size of the dye might sterically hinder its diffusion through the pores and in-between the (Sn3S72−)n layers, thus limiting the adsorption capacity of ST in Sn3S7(trenH)2.

Temperature is also shown to play a significant role on the ion exchange ratio. The adsorption capacity of MB in Sn3S7(trenH)2 from acetonitrile at various temperatures is shown in Fig. 5c. At low temperatures, i.e. 293 K and 303 K, equilibrium was reached within the first 60 min., but the maximum adsorption capacities are relatively low: 4.0 mg g−1 at 293 K and 7.3 mg g−1 at 303 K. For comparison, the adsorption capacity reached 19.2 mg g−1 at 318 K, and 33.3 mg g−1 at 333 K, indicating a maximum adsorption capacity that is heavily dependent on temperature. It is not surprising that the diffusion kinetics increase with the temperature. At 333 K the ion exchange capacity is nearly as high as the room temperature ion exchange in water (Fig. 5a).

The ion exchange capacity of MB reaches an equilibrium value of 33.3 mg g−1 at 333 K in acetonitrile. This value is similar to adsorption of MB in e.g. the unfunctionalized clay mineral kaolinite (56.5 mg g−1 at 333 K)39. However, this value is low in comparison with the adsorption capacities of for example commercial activated carbon where values up to 980 mg g−1 have been reported40. However, it should be stressed that the main purpose of this study is functionalization of a smart semiconductor rather than removal of organic substances from e.g. waste. A member of the R-SnS-1 family templated by Me2NH2+ and Me3NH+ has shown Cs+ and Sr2+ exchange capacities of 409 mg g−1 and 65 mg g−1, respectively, at 338 K41. The latter is similar to what we observed for MB, even though the molar exchange ratio is higher for Sr2+ when the molar mass difference between MB and Sr2+ is taken into account. The higher molar exchange ratio for Cs+ and Sr2+ may be explained by the smaller size and possibly a higher diffusivity of the monoatomic cations in comparison with the cationic dyes. Importantly, the ion exchange capacity is also highly dependent on the initial dye concentration as discussed below.

Ion exchange kinetics

The pseudo first order (PFO), pseudo second order (PSO), and intraparticle diffusion (IPD) kinetic models (see Methods section and Fig. S22) were fitted to the time resolved adsorption data for experiments carried out in acetonitrile at variable temperatures (Fig. 5c). All kinetic parameters were extracted and have been summarized in Table 2 alongside the linear correlation coefficients (R2).

Table 2 Kinetic parameters from pseudo first order (PFO), pseudo second order (PSO) and intraparticle diffusion (IPD) kinetics.

Amongst the examined models, the PSO model describes the experimental data best, i.e. R2 > 0.97 at all temperatures, and reasonable agreement between calculated and experimental qe values is observed (Fig. 5d and Table 2). Hence, this study suggests that the adsorption of MB onto Sn3S7(trenH)2 is best represented by the PSO model. A ~20% overestimation on the calculated adsorption capacity (qe, calc) is found for all datasets, which might imply that the equilibrium is not established within three hours. It is worth noting that at 318 K and 333 K, the IPD model also fit the data quite well, suggesting that the adsorption involves intraparticle diffusion. However, the linear regression does not pass through the origin (Table 2), meaning that intraparticle diffusion is not the rate-determining step. Several studies on the kinetics of dye adsorption onto various adsorbents ranging from clay to almond shells have been performed as reviewed by e.g. Yagub et al.; adsorption follows pseudo-second-order kinetics in all studies reported therein42.

Ion exchange isotherms

The effect of the initial MB concentration on the equilibrium adsorption capacity was investigated using acetonitrile solutions with initial dye concentrations of 45, 90, 230, 450, and 675 mg L−1 as shown in Fig. 6a. The adsorption capacity increases with increasing initial dye concentration over the whole range, although at a diminishing effect at higher concentrations. Linearized Langmuir, Freundlich, and Temkin adsorption isotherms (see Methods section) were fitted to the adsorption data in Fig. 6a. The corresponding isotherm constants and correlation coefficients (R2) are summarized in Table 3 and the fits are shown in Figs 6b and S23.

Figure 6
figure 6

(a) Saturation adsorption qe of MB at 333 K in acetonitrile as a function of the initial MB solution concentration, Ci. (b) Langmuir isotherm model fitted to data in figure (a); Ce is the equilibrium dye concentration in solution.

Table 3 Langmuir, Freundlich and Temkin isotherm data.

Based on the correlation coefficients (R2), the model describing the experimental data best is the Langmuir isotherm. The parameter qm represents the maximum adsorption capacity in the Langmuir model, and at a calculated value of 45(4) mg g−1, the model is in good agreement with the experimentally determined equilibrium adsorption capacity of 45.7 mg g−1 obtained from an initial concentration of 675 mg L−1. This suggests that the adsorbent has reached saturation, and that an increase in dye concentration would not further increase the adsorption capacity. A Langmuir isotherm model assumes a homogeneous adsorbent surface, where all sites are of equal energy for adsorption, and only a monolayer is formed. This is in good agreement with the fact that the interlayer distance and pore channel dimensions only allow for the presence of a single layer of dye molecules. Moreover, electrostatic interactions would disfavor a multilayer. The Langmuir adsorption is in good agreement with the findings by Qi et al. for Cs+ and Sr2+ exchange in (Me2NH2)4/3(Me3NH)2/3Sn3S7·1.25H2O41.

Dye desorption tests

The potential application of the dye-stained Sn3S7(trenH)2 depends not only on the adsorption capacity, but also on the interactions between organic dyes and thiostannate adsorbent i.e. the material stability. The stability of selected dye-stained materials in solution has been investigated. Ideally, no dye should desorb by dispersing the hybrids in solution. Desorption studies of MB and ST adsorbed onto Sn3S7(trenH)2 were conducted in acetonitrile (see Methods section) revealing a much larger degree of desorption of ST than of MB (Figs S20–S21). From a MB adsorption capacity of 33.3 mg g−1, the desorption just reaches 0.15% of the amount initially adsorbed, while that of ST corresponds to 65% from the adsorption capacity of 1.9 mg g−1. Both experiments reach equilibrium within 60 min. Desorption is only likely to occur in the presence of other cationic species in the solution. Alternatively, it points to deposition of charge neutral species (cationic dye stabilized by a counter ion) on the crystal surface rather than ion exchange. This might be the reason for the large ST desorption, which has not been investigated in larger detail. In conclusion, the MB stained samples are stabile in solution in contrast to the ST functionalized samples.

Optical properties of pristine and dye modified Sn3S7(trenH)2

Diffuse reflectance spectroscopy (DRS) data covering the UV-VIS-nearIR range (200–1200 nm) were collected to study changes in light absorption as a consequence of dye functionalization. Spectra of pristine Sn3S7(trenH)2 and selected stained samples are shown in Fig. 7. The band gaps were calculated based on the reflectance data (Methods section and Fig. S24).

Figure 7: Diffuse reflectance spectroscopy data shown as a function of the wavelength.
figure 7

(1): pristine Sn3S7(trenH)2, Eg = 2.95 eV (black); (2): MB in H2O, 293 K, qe = 38.8 mg g−1; (3): MB in MeCN, 293 K, qe = 4.0 mg g−1, Eg = 3.02 eV (green); (4): MB in MeCN, 333 K, qe = 33.3 mg g−1, Eg = 3.03 eV (olive); (5): ST in MeCN, 333 K, qe = 1.9 mg g−1, Eg = 3.05 eV (red). The band gap of the X-ray amorphous sample (2) was not determined.

All samples have a bandgap of 3.0 eV/413 nm corresponding to violet light, which is consistent with the value provided for pristine Sn3S7(trenH)2 in the literature33. Samples stained with MB moreover have significant light absorption around 2 eV/620 nm (orange-red light). The ST functionalized sample also changes its visible light absorption, despite the low adsorbed equilibrium concentration. It shows significant absorption around 2.4 eV/520 nm in addition to the violet light absorption. We suggest the light absorption around 620 nm (MB)/520 nm (ST) and 413 nm correspond to excitation of the dye and the (Sn3S72−)n semiconductor, respectively. The small SnO2 impurity in the samples may contribute to the UV light absorption properties, hence to the potential photocatalytic properties, as SnO2 absorbs light around 300 nm. However, the impurity was found to have a negligible effect on the light absorption (Fig. S25).

The absorption edge at 413 nm is expected to be associated with an intralayer ligand-to-metal charge transfer (LMCT) from the S2− (3p) orbital to the Sn4+ (5d) orbital in the (Sn3S72−)n host layers43,44. Presumably, the higher wavelength light absorption is related to the HOMO-LUMO excitation of the organic dye. More studies are needed to elucidate whether the excitation of the dye leads to charge transfer to the conduction band of the thiostannate layers, similarly to sensitizers in e.g. the Grätzel cell45. Figure S24f,g show Kubelka-Munk plots of pure MB and ST, revealing band gaps of 1.37 eV for MB and 2.08 eV for ST, respectively. The absorption energy of pure MB appears to be approximately 0.2 eV lower than the absorption energy of MB embedded inside the thiostannate. This may be explained by the fact that the excited state gets destabilized when the molecules are embedded between negatively charged layers. This leads to larger HOMO-LUMO separation, hence a higher excitation energy46. The effect seems less pronounced for ST, maybe due to the proposed weaker interaction between ST and the thiostannate.

Not surprisingly, a correlation was found between the amount of MB adsorbed during the adsorption experiments, and the absorption intensity in the high wavelength visible region. The more dye, the larger the orange-red light absorption. Nevertheless, there is a large difference between the samples (2) and (4), for which the saturation adsorption is similar (38.8 mg g−1 for MB staining in H2O and 33.3 mg g−1 for MB staining in MeCN). This may be related to the fact that the water treated sample has lost its long-range order.


This study is a proof-of-concept that R-SnS-1 type materials can be post-synthetically functionalized by ion exchange. Pristine Sn3S7(trenH)2 has been synthesized and modified by ion exchange of the organic dyes Methylene Blue and Safranin T, and detailed insight is given into the sensitization of layered semiconducting Sn3S7(trenH)2. The effects of solvent, temperature and dye concentration were studied in detail revealing that the ion exchange follows pseudo-second order kinetics, and the adsorption follows a Langmuir isotherm. Evidence of size-dependent adsorption of the dyes was found, restricted by the pore size and interlayer distance of the host (Sn3S72−)n layers. The distance between the thiostannate layers decreases with increasing dye loading, but the parent crystal structure remains by performing the functionalization in organic solvents such as acetonitrile.

The adsorption of dyes changed the optical properties of the material, which might pave the way for visible light-responsive Sn3S7(trenH)2-based photocatalysis. The pristine violet light absorber was modified to have significant orange and red light absorption. Thereby, this research may improve the design of cheap, non-toxic dye-sensitized semiconductors for light harvesting as demonstrated by the changes in the light absorption properties of the materials.


The chemical precursors SnO2 (≥99.9%), sulfur (≥99.5%), tris(2-aminoethyl)amine (C6H18N4, tren, 96%), Methylene Blue (MB) chloride, Safranin T (ST) chloride and all solvents were obtained from Sigma-Aldrich. All reagents were used without further purification. As the water content of the salts was not taken into account in the dye adsorption studies, the absolute dye concentrations may be lower than the reported values. The same precursors were used for all experiments which are therefore comparable.

Synthesis of Sn3S7(trenH)2

The Sn3S7(trenH)2 samples used for dye adsorption studies were prepared using a solvothermal method: A mixture of SnO2 and sulfur (Sn:S = 3:7) was stirred in tren under ambient conditions for approximately 20 min. The solution was transferred to a Teflon-lined stainless steel autoclave for thermal treatment at 190 °C for 6 days. The resulting pale green-yellow crystals were washed with acetonitrile and subsequently air-dried for at least 24 hours. The samples were found to contain an impurity of SnO2 (Fig. 3). A later synthesis of Sn3S7(trenH)2 was carried out using the same procedure but with a molar ratio of Sn:S = 3:8. This resulted in a phase pure product (Fig. S5).

Powder X-ray diffraction (PXRD)

Powder X-ray diffraction was performed using a SmartLab diffractometer from Rigaku equipped with a Cu source. Cu1 radiation (λ = 1.54056 Å) was used to collect data at room temperature on flat silicon sample holders. Le Bail fitting was performed to extract unit cell parameters and zero-point corrected peak positions from the diffraction data using the FullProf Suite47. The same program was used to fit pseudo-Voigt functions to selected reflections to determine the width of these diffraction peaks and to quantify the SnO2 impurity by Rietveld refinement.

Solid state nuclear magnetic resonance spectroscopy (NMR)

The 13C{1H} CP/MAS NMR spectrum was obtained on a Bruker Avance II 400 MHz (9.4 T) spectrometer using a home-built CP/MAS NMR probe for 7 mm outer-diameter rotors, vR = 4.0 kHz, a 8-s relaxation delay, a CP contact time of 0.5 ms, and 8192 scans.

Diffuse reflectance spectroscopy (DRS)

Diffuse reflectance spectroscopy (DRS) was used to investigate the light absorption properties in the wavelength range (200–1200 nm) using a Shimadzu UV-3600 spectrophotometer. Band gaps were calculated based on DRS data converted to the Kubelka-Munk function, where R is the reflectance:

Scanning electron microscopy (SEM)

Powders were immobilized on conducting carbon tape, and scanning electron microscopy images were acquired on a FEI-Nova NanoSEM 600 scanning electron microscope.

Dye adsorption/ion exchange protocol and quantification

All dye-adsorption experiments were carried out by suspending 0.2 g of Sn3S7(trenH)2 in a 40.0 mL dye-solution and stirring for 3–4 hours in a sealed Erlenmeyer flask. Experiments were performed using different organic dyes (MB and ST), initial dye-concentrations (MB+ or ST+: 45–675 mg L−1), temperatures (293–333 K), and solvents (water and acetonitrile). The resulting dye concentrations were determined by UV-VIS absorption spectroscopy at the maximum absorbance wavelength (i.e. 665 nm for MB in H2O, 655 nm for MB in acetonitrile, and 518 nm for ST in acetonitrile). A Shimadzu UV-1800 spectrophotometer was used for these measurements. The amount of dye adsorbed by the thiostannate, qt (mg g−1), was calculated according to the following equation:

where V is the solution volume (L), C0 is the initial dye concentration (mg L−1), Ct is the concentration at contact time t (mg L−1), and m is the mass of adsorbent (g). As the adsorption reaches equilibrium, the above equation becomes:

where qe is the equilibrium adsorption capacity (mg g−1), and Ce is the equilibrium dye concentration in the solution (mg L−1).

Adsorption kinetics modelling

For each adsorption experiment a series of measurements were conducted at various reaction times. In order to interpret the results, different kinetic models were fitted to data: The pseudo-first order (PFO)48, pseudo-second order (PSO)49, and intraparticle diffusion (IPD)50 models. The linearized forms of these models are as expressed below:

In these equations qt and qe have the same definitions as in Eq. 2 and Eq.3, t is contact time, while K1 (min−1), K2 (g mg−1 min−1), and K3 (mg g−1 min−0.5) are the rate constants of the PFO, PSO, and IPD model, respectively. As the intraparticle model fits do not intersect the origin a constant C was introduced in the fits: qt = K3t1/2 + C.

To compare the adsorption capacity predicted by the models to that found in the experiments, a percent deviation (Δq) was calculated as follows:

where qe,exp and qe,calc are the experimental and calculated equilibrium adsorption capacity, respectively.

Equilibrium isotherm modeling

The relationship between the adsorption capacity at equilibrium and the amount of adsorbate (dye) left in solution is important in describing the interaction between adsorbent and adsorbate. Several isotherm models are available51,52,53,54,55,56, and fitting the isotherm equations to equilibrium data can provide insight into the adsorption mechanism. In this paper the Langmuir, Freundlich, and Temkin isotherm models have been fitted to the experimental data.

Langmuir isotherm

The Langmuir model assumes a homogenous adsorbent surface, i.e. all sites are of equal energy for adsorption, and only a monolayer coverage of these sites is possible53. The model is defined by the following equation:

In a linear form (eq. 8) is presented as:

where qe is the equilibrium adsorption capacity (mg g−1), Ce is the equilibrium adsorbate concentration in solution (mg L−1), KL is the Langmuir constant (mg L−1), and qm is the maximum adsorption capacity for a monolayer coverage (mg g−1).

Freundlich isotherm

The Freundlich model describes a heterogeneous adsorbent surface, where the adsorption energy is not equal for all sites55. The Freundlich equation is as expressed below:

This can be written in the linear form:

where KF and n are constants indicating adsorption capacity (mg g−1) and favorableness (unit-less), respectively. The constant n is usually interpreted as a measure of surface heterogeneity; its value ranging between 1 and 10, the lower the value the more heterogeneous the surface.

Temkin isotherm

The Temkin model is based on the Langmuir model, but takes into account indirect adsorbate-adsorbate interactions at the adsorption sites. The model also assumes that the heat of adsorption will decrease linearly with surface coverage56. The model is expressed by the following equation:

which in a linear form is presented as:

where R is the gas constant (8.314 J mol−1 K−1), T is absolute temperature (K), while KT is the Temkin constant corresponding to maximum binding energy (L g−1), and bT is related to the heat of adsorption (J mol−1).

Dye desorption protocol and quantification

The stability of the Sn3S7(trenH)2-organic dye hybrids in solution was analyzed in desorption experiments. Selected dye-stained products were suspended in acetonitrile, and the amount of desorbed dye was determined by UV-Vis absorption spectroscopy. The percentage of desorption was calculated by the following expression:

Additional Information

How to cite this article: Hvid, M. S. et al. Light absorption engineering of a hybrid (Sn3S72-) n based semiconductor – from violet to red light absorption. Sci. Rep. 7, 45822; doi: 10.1038/srep45822 (2017).

Publisher's note: Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.


  1. Huang, Z., Li, F., Chen, B. & Yuan, G. Hydrogen from Water over Openly-Structured Graphitic Carbon Nitride Polymer through Photocatalysis. ChemSusChem 9, 478–484, doi: 10.1002/cssc.201501520 (2016).

    CAS  Article  ADS  PubMed  Google Scholar 

  2. Sayama, K., Mukasa, K., Abe, R., Abe, Y. & Arakawa, H. A new photocatalytic water splitting system under visible light irradiation mimicking a Z-scheme mechanism in photosynthesis. Journal of Photochemistry and Photobiology A: Chemistry 148, 71–77, doi: 10.1016/S1010-6030(02)00070-9 (2002).

    CAS  Article  Google Scholar 

  3. Sasaki, Y., Iwase, A., Kato, H. & Kudo, A. The effect of co-catalyst for Z-scheme photocatalysis systems with an Fe3+/Fe2+ electron mediator on overall water splitting under visible light irradiation. Journal of Catalysis 259, 133–137, doi: 10.1016/j.jcat.2008.07.017 (2008).

    CAS  Article  Google Scholar 

  4. Ahmed, S., Rasul, M. G., Martens, W. N., Brown, R. & Hashib, M. A. Heterogeneous photocatalytic degradation of phenols in wastewater: A review on current status and developments. Desalination 261, 3–18, doi: 10.1016/j.desal.2010.04.062 (2010).

    CAS  Article  Google Scholar 

  5. Chatterjee, D. & Mahata, A. Visible light induced photodegradation of organic pollutants on dye adsorbed TiO2 surface. Journal of Photochemistry and Photobiology A: Chemistry 153, 199–204, doi: 10.1016/S1010-6030(02)00291-5 (2002).

    CAS  Article  Google Scholar 

  6. Han, F., Kambala, V. S. R., Srinivasan, M., Rajarathnam, D. & Naidu, R. Tailored titanium dioxide photocatalysts for the degradation of organic dyes in wastewater treatment: A review. Applied Catalysis A: General 359, 25–40, doi: 10.1016/j.apcata.2009.02.043 (2009).

    CAS  Article  Google Scholar 

  7. Jing, D. & Guo, L. A Novel Method for the Preparation of a Highly Stable and Active CdS Photocatalyst with a Special Surface Nanostructure. The Journal of Physical Chemistry B 110, 11139–11145, doi: 10.1021/jp060905k (2006).

    CAS  Article  PubMed  Google Scholar 

  8. Sakulkhaemaruethai, S. & Sreethawong, T. Synthesis of mesoporous-assembled TiO2 nanocrystals by a modified urea-aided sol-gel process and their outstanding photocatalytic H2 production activity. International Journal of Hydrogen Energy 36, 6553–6559, doi: 10.1016/j.ijhydene.2011.03.005 (2011).

    CAS  Article  Google Scholar 

  9. Khan, S. B., Faisal, M., Rahman, M. M. & Jamal, A. Low-temperature growth of ZnO nanoparticles: Photocatalyst and acetone sensor. Talanta 85, 943–949, doi: 10.1016/j.talanta.2011.05.003 (2011).

    CAS  Article  PubMed  Google Scholar 

  10. Park, S., Park, J., Selvaraj, R. & Kim, Y. Facile microwave-assisted synthesis of SnS2 nanoparticles for visible-light responsive photocatalyst. Journal of Industrial and Engineering Chemistry 31, 269–275, doi: 10.1016/j.jiec.2015.06.036 (2015).

    CAS  Article  Google Scholar 

  11. Riegel, G. & Bolton, J. R. Photocatalytic Efficiency Variability in TiO2 Particles. The Journal of Physical Chemistry 99, 4215–4224, doi: 10.1021/j100012a050 (1995).

    CAS  Article  Google Scholar 

  12. Devi, L. G. & Kavitha, R. A review on non metal ion doped titania for the photocatalytic degradation of organic pollutants under UV/solar light: Role of photogenerated charge carrier dynamics in enhancing the activity. Applied Catalysis B: Environmental 140–141, 559–587, doi: 10.1016/j.apcatb.2013.04.035 (2013).

    CAS  Article  Google Scholar 

  13. Kumar, S. G. & Devi, L. G. Review on Modified TiO2 Photocatalysis under UV/Visible Light: Selected Results and Related Mechanisms on Interfacial Charge Carrier Transfer Dynamics. The Journal of Physical Chemistry A 115, 13211–13241, doi: 10.1021/jp204364a (2011).

    CAS  Article  ADS  PubMed  Google Scholar 

  14. Zhang, R.-C., Yao, H.-G., Ji, S.-H., Liu, M.-C. & Ji, M. (H(2)en)(2)Cu(8)Sn(3)S(12): a trigonal CuS(3)-based open-framework sulfide with interesting ion-exchange properties. Chemical communications (Cambridge, England) 46, 4550–4552, doi: 10.1039/b924581b (2010).

    CAS  Article  Google Scholar 

  15. Li, N. et al. Highly Efficient, Irreversible and Selective Ion Exchange Property of Layered Titanate Nanostructures. Advanced Functional Materials 22, 835–841, doi: 10.1002/adfm.201102272 (2012).

    CAS  Article  ADS  Google Scholar 

  16. Takagaki, A., Sasaki, R., Tagusagawa, C. & Domen, K. Intercalation-induced Esterification over a Layered Transition Metal Oxide. Topics in Catalysis 52, 592–596, doi: 10.1007/s11244-009-9194-4 (2009).

    CAS  Article  Google Scholar 

  17. Tagusagawa, C. et al. Effects of Transition-Metal Composition of Protonated, Layered Nonstoichiometric Oxides H1 − xNb1 − xMo1 + xO6 on Heterogeneous Acid Catalysis. The Journal of Physical Chemistry C 113, 17421–17427, doi: 10.1021/jp906628k (2009).

    CAS  Article  Google Scholar 

  18. Dias, A. S. et al. Exfoliated titanate, niobate and titanoniobate nanosheets as solid acid catalysts for the liquid-phase dehydration of d-xylose into furfural. Journal of Catalysis 244, 230–237, doi: 10.1016/j.jcat.2006.09.010 (2006).

    CAS  Article  Google Scholar 

  19. Hosogi, Y., Kato, H. & Kudo, A. Photocatalytic Activities of Layered Titanates and Niobates Ion-Exchanged with Sn2+ under Visible Light Irradiation. The Journal of Physical Chemistry C 112, 17678–17682, doi: 10.1021/jp805693j (2008).

    CAS  Article  Google Scholar 

  20. Shangguan, W. & Yoshida, A. Synthesis and photocatalytic properties of CdS-intercalated metal oxides. Solar Energy Materials and Solar Cells 69, 189–194, doi: 10.1016/S0927-0248(01)00020-4 (2001).

    CAS  Article  Google Scholar 

  21. Jiang, T., Lough, A., Ozin, A. G. & Bedard, L. R. Intermediates in the formation of microporous layered tin(IV) sulfide materials. Journal of Materials Chemistry 8, 733–741, doi: 10.1039/A706042D (1998).

    CAS  Article  Google Scholar 

  22. Marking, G. A. & Kanatzidis, M. G. Encapsulation of Cyclooctasulfur Molecules in an Open Metal-Sulfide Framework. Isolation of the Host-Guest Complex Cs2Sn3S7∙1/2S8 from Molten Cesium Polysulfide Fluxes. Chemistry of Materials 7, 1915–1921, doi: 10.1021/cm00058a024 (1995).

    CAS  Article  Google Scholar 

  23. Sheldrick, W. S. & Schaaf, B. Darstellung und Kristallstruktur von Rb2Sn3S7·2H2O und Rb4Sn2Se6. Zeitschrift für anorganische und allgemeine Chemie (1950) 620, 1041–1045, doi: 10.1002/zaac.19946200616 (1994).

    CAS  Article  Google Scholar 

  24. Parise, J. B. et al. Novel layered sulfides of tin: synthesis, structural characterization and ion exchange properties of TMA-SnS-1, Sn3S7∙(NMe4)2∙H2O. Journal of the Chemical Society, Chemical Communications 527–527, doi: 10.1039/C39940000527 (1994).

  25. Bowes, C. L., Petrov, S., Vovk, G., Young, D. & Ozin, G. A. Microporous layered tin sulfide, SnS-1: molecular sieve or intercalant? Journal of materials chemistry 8, 711–720, doi: 10.1039/a706278h (1998).

    CAS  Article  Google Scholar 

  26. Jiang, T., Lough, A., Ozin, A., Bedard, G. L. R. & Broach, R. Synthesis and structure of microporous layered tin(IV) sulfide materials. Journal of Materials Chemistry 8, 721–732, doi: 10.1039/A706279F (1998).

    CAS  Article  Google Scholar 

  27. Liu, G.-N. et al. Different Effects of a Cotemplate and [(Transition-Metal)(1,10-Phenanthroline)m]2 + (m = 1–3) Complex Cations on the Self-assembly of a Series of Hybrid Selenidostannates Showing Combined Optical Properties of Organic and Inorganic Components. Inorganic Chemistry 50, 9660–9669, doi: 10.1021/ic201413h (2011).

    CAS  Article  PubMed  Google Scholar 

  28. Rogez, G., Massobrio, C., Rabu, P. & Drillon, M. Layered hydroxide hybrid nanostructures: a route to multifunctionality. Chemical Society Reviews 40, 1031–1058, doi: 10.1039/C0CS00159G (2011).

    CAS  Article  PubMed  Google Scholar 

  29. Genna, D. T., Wong-Foy, A. G., Matzger, A. J. & Sanford, M. S. Heterogenization of Homogeneous Catalysts in Metal–Organic Frameworks via Cation Exchange. Journal of the American Chemical Society 135, 10586–10589, doi: 10.1021/ja402577s (2013).

    CAS  Article  PubMed  Google Scholar 

  30. Qi, X.-H., Du, K.-Z., Feng, M.-L., Li, J.-R. & Du, C.-F. A two-dimensionally microporous thiostannate with superior Cs and Sr ion-exchange property. Journal of materials chemistry. A, Materials for energy and sustainability 3, 5665–5673, doi: 10.1039/C5TA00566C (2015).

    CAS  Article  Google Scholar 

  31. Pienack, N. & Bensch, W. (dienH)2Sn3S7 - ein Thiostannat des R-SnS-1-Typs mit interessantem Verhalten gegenüber Cs+ -Kationen. Z. Anorg. Allg. Chem. 634, 1 (2008).

    Article  Google Scholar 

  32. Manos, M. J. & Kanatzidis, M. G. Metal sulfide ion exchangers: superior sorbents for the capture of toxic and nuclear waste-related metal ions. Chemical Science 7, 4804–4824, doi: 10.1039/C6SC01039C (2016).

    CAS  Article  PubMed  PubMed Central  Google Scholar 

  33. Pienack, N., Schinkel, D., Puls, A., Ordolff, M.-E. & Luehmann, H. New Thiostannates Synthesized Under Solvothermal Conditions: Crystal Structures of (trenH)2Sn3S7 and {[Mn(tren)]2Sn2S6}. Zeitschrift für Naturforschung. B, A journal of chemical sciences 67, 1098–1106, doi: 10.5560/znb.2012-0126 (2012).

    CAS  Article  Google Scholar 

  34. Tan, K., Ko, Y. & Parise, J. B. Trimethylammonium Tin Sulfide. Acta Crystallographica Section C 51, 398–401, doi: 10.1107/S0108270194010437 (1995).

    Article  Google Scholar 

  35. Li, L., Quinlivan, P. A. & Knappe, D. R. U. Effects of activated carbon surface chemistry and pore structure on the adsorption of organic contaminants from aqueous solution. Carbon 40, 2085–2100, doi: 10.1016/S0008-6223(02)00069-6 (2002).

    CAS  Article  Google Scholar 

  36. Pelekani, C. & Snoeyink, V. L. Competitive adsorption between atrazine and methylene blue on activated carbon: the importance of pore size distribution. Carbon 38, 1423–1436, doi: 10.1016/S0008-6223(99)00261-4 (2000).

    CAS  Article  Google Scholar 

  37. Wu, Q.-y., Liang, H.-q., Li, M., Liu, B.-t. & Xu, Z.-k . Hierarchically porous carbon membranes derived from PAN and their selective adsorption of organic dyes. Chinese Journal of Polymer Science 34, 23–33, doi: 10.1007/s10118-016-1723-6 (2015).

    CAS  Article  Google Scholar 

  38. Akasaka, H. et al. Selective adsorption of biladien-ab-one and zinc biladien-ab-one to mesoporous silica. Microporous and Mesoporous Materials 120, 331–338, doi: 10.1016/j.micromeso.2008.11.025 (2009).

    CAS  Article  Google Scholar 

  39. Sarma, G. K., SenGupta, S. & Bhattacharyya, K. G. Methylene Blue Adsorption on Natural and Modified Clays. Separation Science and Technology 46, 1602–1614, doi: 10.1080/01496395.2011.565012 (2011).

    CAS  Article  Google Scholar 

  40. Gupta, V. K. & Suhas Application of low-cost adsorbents for dye removal – A review. Journal of Environmental Management 90, 2313–2342, doi: 10.1016/j.jenvman.2008.11.017 (2009).

    CAS  Article  PubMed  Google Scholar 

  41. Qi, X.-H. et al. A two-dimensionally microporous thiostannate with superior Cs+ and Sr2+ ion-exchange property. Journal of Materials Chemistry A 3, 5665–5673, doi: 10.1039/C5TA00566C (2015).

    CAS  Article  Google Scholar 

  42. Yagub, M. T., Sen, T. K., Afroze, S. & Ang, H. M. Dye and its removal from aqueous solution by adsorption: a review. Advances in colloid and interface science 209, 172–184 (2014).

    CAS  Article  PubMed  Google Scholar 

  43. Jiang, T. A., Ozin, G., Verma, A. & Bedard, L. R. Adsorption and sensing properties of microporous layered tin sulfide materials. Journal of Materials Chemistry 8, 1649–1656, doi: 10.1039/A801501E (1998).

    CAS  Article  Google Scholar 

  44. Jiang, T. A., Ozin, G. & Bedard, L. R. Spectroscopic properties of microporous layered tin sulfide materials. Journal of Materials Chemistry 8, 1641–1648, doi: 10.1039/A801602J (1998).

    CAS  Article  Google Scholar 

  45. O’Regan, B. & Gratzel, M. A low-cost, high-efficiency solar cell based on dye-sensitized colloidal TiO2 films. Nature 353, 737–740, doi: 10.1038/353737a0 (1991).

    Article  ADS  Google Scholar 

  46. Qu, W., Chen, F., Zhao, B. & Zhang, J. Preparation and visible light photocatalytic performance of methylene blue intercalated K4Nb6O17. Journal of Physics and Chemistry of Solids 71, 35–41, doi: 10.1016/j.jpcs.2009.10.005 (2010).

    CAS  Article  ADS  Google Scholar 

  47. Rodríguez-Carvajal, J. Recent advances in magnetic structure determination by neutron powder diffraction. Physica B: Condensed Matter 192, 55–69, doi: 10.1016/0921-4526(93)90108-I (1993).

    Article  ADS  Google Scholar 

  48. Lagergren, S. Zur Theorie der sogenannten Adsorption gelöster stoffe. Kungliga Svenska Vetenskapsakademiens . Handlingar 24, 1–39, doi: 10.1007/bf01501332 (1898).

    Article  Google Scholar 

  49. Ho, Y. S. & McKay, G. Pseudo-second order model for sorption processes. Process Biochemistry 34, 451–465, doi: 10.1016/S0032-9592(98)00112-5 (1999).

    CAS  Article  Google Scholar 

  50. Weber, W. J. J. & C. M. Kinetics of adsorption on carbon from solutions. J. Sanit. Eng. Div. Am. Soc. Civ. Eng. 89, 31–60 (1963).

    Google Scholar 

  51. Sips, R. On the Structure of a Catalyst Surface. The Journal of Chemical Physics 16, 490–495, doi: 10.1063/1.1746922 (1948).

    CAS  Article  ADS  Google Scholar 

  52. Redlich, O. & Peterson, D. L. A Useful Adsorption Isotherm. The Journal of Physical Chemistry 63, 1024–1024, doi: 10.1021/j150576a611 (1959).

    CAS  Article  Google Scholar 

  53. Langmuir, I. The Adsorption of Gases on Plane Surfaces of Glass, Mica and Platinum. Journal of the American Chemical Society 40, 1361–1403, doi: 10.1021/ja02242a004 (1918).

    CAS  Article  Google Scholar 

  54. Dubinin, M. M. The Potential Theory of Adsorption of Gases and Vapors for Adsorbents with Energetically Nonuniform Surfaces. Chemical Reviews 60, 235–241, doi: 10.1021/cr60204a006 (1960).

    CAS  Article  Google Scholar 

  55. Freundlich, H. Concerning adsorption in solutions. Zeitschrift Fur Physikalische Chemie–Stochiometrie Und Verwandtschaftslehre 57, 385–470 (1906).

    CAS  Google Scholar 

  56. Temkin, M. & Pyzhev, V. Kinetics of ammonia synthesis on promoted iron catalysts. Acta Physicochimica Urss 12, 327–356 (1940).

    CAS  Google Scholar 

Download references


We gratefully acknowledge financial support by the Villum Foundation Young Investigator Programme (VKR023449) and the Danish National Research Foundation (DNRF 118). J. Skibsted is kindly acknowledged for acquisition of the NMR spectrum.

Author information

Authors and Affiliations



M.S.H. and N.L. designed and conducted the material synthesis, modification and kinetics studies. All authors contributed to the materials characterization and to the manuscript preparation.

Corresponding author

Correspondence to Nina Lock.

Ethics declarations

Competing interests

The authors declare no competing financial interests.

Supplementary information

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

Hvid, M., Lamagni, P. & Lock, N. Light absorption engineering of a hybrid (Sn3S72−)n based semiconductor – from violet to red light absorption. Sci Rep 7, 45822 (2017).

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