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Porous Semiconducting Gels and Aerogels from Chalcogenide Clusters

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Science  27 Jul 2007:
Vol. 317, Issue 5837, pp. 490-493
DOI: 10.1126/science.1142535

Abstract

Inorganic porous materials are being developed for use as molecular sieves, ion exchangers, and catalysts, but most are oxides. We show that various sulfide and selenide clusters, when bound to metal ions, yield gels having porous frameworks. These gels are transformed to aerogels after supercritical drying with carbon dioxide. The aerogels have high internal surface area (up to 327 square meters per gram) and broad pore size distribution, depending on the precursors used. The pores of these sulfide and selenide materials preferentially absorb heavy metals. These materials have narrow energy gaps (between 0.2 and 2.0 electron volts) and low densities, and they may be useful in optoelectronics, as photocatalysts, or in the removal of heavy metals from water.

Inorganic porous materials are at the foundation of broad applications such as molecular sieves, ion exchangers, and catalysts (1, 2). Zeolites and aluminosilicate mesoporous materials constitute the vast majority of this class. Aerogels are another kind of porous inorganic amorphous polymer in which nanosized blocks are interconnected to yield high internal surface area, very low densities, and large open pores (3, 4). Although the sol-gel chemistry of oxide-based materials (e.g., SiO2, Al2O3, TiO2) and carbon (5) is well known, successful attempts to apply this approach to non–oxide-based systems are quite rare, especially for chalcogenides. Such systems would be capable of combining the electronic properties of chalcogenides with internal porosity. Aerogels based on aggregated simple binary nanocrystals (e.g., CdS, CdSe) and on amorphous GeS2 have been reported (6, 7).

We report on a strategy to create highly porous semiconducting aerogels derived from chalcogenide-based clusters and platinum as the linking metal ion (8). A family of chalcogenide gels was prepared in aqueous solution with anionic [MQ4]4–, [M2Q6]4–, and [M4Q10]4– (M = Ge, Sn; Q = S, Se) building blocks (Fig. 1A) in the presence of platinum (II) salt, according to the following metathesis reactions: Math(1) Math Math(2) Math Math(3) Math where R= methyl, ethyl; M = Ge, Sn; Q = S, Se; and A = Na, K. In these reactions (e.g., Eq. 1), all chloride ligands of [PtCl4]2– can be replaced by the Q terminal atoms of chalcogenido clusters, generating materials with a formula of Pt2[M4Q10]. Energy-dispersive spectroscopy (EDS) revealed that two platinum atoms per complex anion are incorporated in almost every case, giving a charge-balanced formula (Table 1). K+ or Cl ions, used as counterions in the synthesis, were not detected in the product—a result consistent with complete metathesis. This linking/polymerization reaction produced a continuous, extended Pt/M/Q framework of covalently bonded atoms that encapsulates solvent molecules into their pore system during the process of polymerization and finally makes hydrogels (fig. S1, A to C). Because the gels formed are based on all-chalcogenide species, we term these hydrogels “chalcogels” by analogy to the naming of cyanogels (9). Table 1 lists the six chalcogels we developed and the Zintl anion incorporated in each case.

Fig. 1.

(A) Different building blocks used in chalcogel formation (blue spheres, metal centers; red spheres, chalcogenide atoms). (B and C) Monolithic hydrogel before (B) and after (C) supercritical drying, showing very little volume loss.

Table 1.

Elemental analysis, colors, and optical energy gaps for the chalcogel series.

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After supercritical drying with CO2, these chalcogels yield highly porous aerogels (Fig. 1, B and C) (10). All samples showed consistent Pt/M/Q (M = Ge, Sn; Q = S, Se) ratios very close to those in the starting clusters. However, slight discrepancies were observed for Chalcogel-3 and Chalcogel-6, which might be due to solution equilibrium processes.

Transmission electron microscopy (TEM) images of our aerogel samples revealed empty mesopores with no long-range order (Fig. 2, A to C). Indeed, they appear to be morphologically similar to the silica aerogels where particles are connected to each other, making continuous amorphous (Fig. 2D) networks. The micro- and mesoporosity were confirmed by nitrogen physisorption measurements. The adsorption-desorption isotherms show a type IV adsorption branch with a combination of H1- and H3-type hysteresis loops characteristic of an interconnected mesoporous system (Fig. 3) (11). This indicates that the mesopores have cylindrical and slit-shaped geometries. Pore size distribution plots calculated by the Barrett-Joynes-Halenda (BJH) method (11) from the desorption branch suggest the presence of a broad range of pore sizes in the meso region (fig. S1, D and E). Additionally, the absence of saturation in the adsorption isotherm implies the simultaneous presence of macropores (pore diameter >50 nm) in the samples, which would be consistent with the aerogel nature of these chalcogenides.

Fig. 2.

(A and B) TEM images of Chalcogel-1 (A) and Chalcogel-2 (B). Pores between the particles in the meso- and macrophase regime are clear from these pictures, although they are not ordered. (C) TEM image of Chalcogel-2 shows small pores inside the particle. Large macropores are absent here. (D) Wide-angle powder x-ray diffraction data for Chalcogel-1. The amorphous nature of the aerogel and the lack of other crystalline phases are obvious.

Fig. 3.

Nitrogen adsorption-desorption isotherms of (A) Chalcogel-1 and (B) Chalcogel-2 at 77 K (solid circles, adsorption data; open circles, desorption data). Samples were degassed overnight at 348 K before testing.

Brunauer-Emmett-Teller (BET) surface areas obtained from the aerogels range from 108 to 327 m2/g, depending on the chalcogenido cluster (Table 2). The surface area of 327 m2/g obtained from [Ge4Se10]4– in Chalcogel-2 is the highest of the six chalcogels, followed by 323 m2/g for [Ge4S10]4– in Chalcogel-1. The smallest cluster, [SnS4]4– in Chalcogel-6, gave the lowest BET surface area value of 117 m2/g. Given that the formula weights of these chalcogels are high, on a per-mole basis the surface area values are actually very large. The silica equivalence (12) BET surface area of Chalcogel-2 is 1674 m2/g and that of Chalcogel-3 is 1580 m2/g (Table 2). Values for silica aerogels range from 100 to 1600 m2/g and typical values are 600 m2/g. The bulk density of these chalcogels is very low; for example, Chalcogel-1 showed 0.12 to 0.17 g/cm3 with a skeletal density of 3.1 g/cm3.

Table 2.

Nitrogen adsorption-desorption data for the chalcogel series.

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To probe the local structure of the amorphous aerogels, we used the atomic pair distribution function (PDF) (13) technique, which analyzes both diffuse and Bragg scattering by recovering atom-atom correlations in real space in the form of a radial distribution function. A single correlation occurring at 2.36 Å is evident in the PDF of Chalcogel-1 (Fig. 4A), corresponding to the first-neighbor Ge-S and Pt-S bond distances. A clustering of correlations is evident around 3.52 Å, which corresponds to the second-neighbor Ge···Ge, S···S, and Pt···Ge distances. The PDF of Chalcogel-2 is remarkably similar to that of Chalcogel-1, although it exhibits a shift in correlations to longer interatomic distances r as a result of the larger atomic radius of Se versus S. Again a single correlation is evident in the PDF of Chalcogel-2 at 2.49 Å (Ge-Se and Pt-Se bond distances), and several appear centered around 3.75 Å. The higher intensity of the first correlation in Chalcogel-2 arises from the larger scattering factor of Se over that of S. Both PDFs show a lack of well-defined features past 6 Å that suggests a lack of long-range translational symmetry. However, a well-defined local structure is evident from the PDF and clearly shows that the adamantane clusters remain intact. The splitting of the correlations (3.52 Å and 3.75 Å) is likely due to subtle distortions, arising from linking of the adamantane clusters, that ultimately disrupt the long-range translational symmetry. The PDF data, together with the complete metathesis chemistry, elemental analysis, and x-ray photoelectron spectroscopy (XPS) (fig. S2), suggest a nonperiodic structure of the type shown in Fig. 4B. Further support for the integrity of the starting clusters in the final aerogels was provided by nuclear magnetic resonance (NMR) (fig. S3), electrospray ionization mass spectroscopy (ESI-MS) (fig. S4), and infrared spectroscopy (fig. S5).

Fig. 4.

(A) Reduced atomic pair distribution function G(r) of Chalcogel-1 (black line) and Chalcogel-2 (red dashed line) as a function of interatomic distance r. (B) Interatomic distances (in angstroms) are shown for the [Ge4S10]4– cluster in the proposed Chalcogel-1 structure. (C) Ultraviolet-visible electronic absorption spectra of (a) Chalcogel-1 (red dashed line), (b) Chalcogel-2 (blue dash-dot line), (c) Chalcogel-3 (magenta dashed line), (d) Chalcogel-4 (purple dotted line), (e) Chalcogel-5 (green dashed line), and (f) Chalcogel-6 (violet dash-dot line).

The chalcogels showed a remarkably high capacity for removing heavy metals from contaminated water. For example, starting with water contaminated by 645 parts per million (ppm) Hg2+, 10 mg of Chalcogel-1 removed Hg2+ down to concentration levels of ∼0.04 ppm (14). Whereas mesoporous silicates need to be functionalized with surface-modified thiolate ligands before application toward environmental remediation (15), the chalcogels work directly as potential adsorbents for Hg2+ (16) without prior modification of their surface. The detailed mechanism of metal ion removal is not known.

The chalcogels also efficiently absorb organic hydrophobic aromatic molecules from solution. In contrast to the unmodified silica aerogels—which generally have hydrophilic surfaces and tend to be unstable under a humid atmosphere—the chalcogels present hydrophobic surfaces lined with chalcogen atoms and are immune to high humidity (17). Thermal gravimetric analysis indicates that the aerogels are stable to 180°C (fig. S6). As a demonstration of its high affinity for hydrophobic species, Chalcogel-1 absorbed quantitatively all of porphyrin I from a 5.67 μmol/liter ethanolic solution within 24 hours (30 mg of Chalcogel-1 was shaken continuously in 16 ml of the porphyrin solution).

The chalcogels absorb light in the visible and infrared regions, exhibiting sharp energy gaps from 2.0 eV to 0.8 eV (Table 1) as determined by diffuse-reflectance solid-state ultraviolet-visible/near-infrared spectroscopy (Fig. 4C). Only Chalcogel-5 gave a broad absorption with a band gap of 0.2 eV. The optical properties of the highly porous semiconducting aerogels can be tuned by changing the building block. Going from the S to the Se analogs of the adamantane cluster, the energy gap decreases as expected. Also, by changing the group IV metal in the cluster from Ge to Sn, the energy gap is decreased by 0.3 eV. Similarly, the band gap can also be changed by varying the chalcogenide content per metal in the starting clusters. This is well reflected in the observed band gaps of Chalcogel-3, -4, and -5, where the Se content per Sn atom is increased gradually and shows a narrowing of the energy gap.

Given that it is difficult to remove surfactants from mesostructured chalcogenide materials (1822), the strategy reported here represents a convenient and general route for making porous materials with chalcogenide-based clusters. Because of the availability of a large number of soluble chalcogenido clusters, together with various linking transition and main-group metal ions, our approach seems to offer a general technique for preparing broad classes of porous chalcogenides.

Supporting Online Material

www.sciencemag.org/cgi/content/full/317/5837/490/DC1

Materials and Methods

Figs. S1 to S6

References

References and Notes

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