Light-Triggered Boost of Activity of Catalytic Bola-Type Surfactants by a Plasmonic Metal-Support Interaction Effect.

The maximization of activity is a general aim in catalysis research. The possibility for light-triggered enhancement of a catalytic process, even if the process is not photochemical in nature, represents an intriguing concept. Here, we present a novel system for the exploration of the latter idea. A surfactant with a catalytically active head group, a protonated polyoxometalate (POM) cluster, is attached to the surface of a gold nanoparticle (Au NP) using thiol coupling chemistry. The distance of the catalytically active center to the gold surface could be adjusted precisely using surfactants containing hydrocarbon chains (C n) of different lengths ( n = 4-10). Radiation with VIS-light has no effect on the catalytic activity of micellar aggregates of the surfactant. The situation changes, as soon as the surfactants have been attached to the Au NPs. The catalytic activity could almost be doubled. It was proven that the effect is caused by coupling the surface plasmon resonance of the Au NPs with the properties of the POM head group. The improvement of activity could only be observed if the excitation wavelength matches the absorption band of the used Au NPs. Furthermore, the shorter the distance between the POM group and the surface of the NP, the stronger is the effect. This phenomenon was explained by lowering the activation energy of the transition state relevant to the catalytic process by the strong electric fields in the vicinity of the surfaces of plasmonic nanoparticles. Because the catalytic enhancement is wavelength-selective, one can imagine the creation of complex systems in the future, a system of differently sized NPs, each responsible for a different catalytic step and activated by light of different colors.

Introduction

Surfactant-like compounds are not only key components in the membranes of any biological cell, but the amounts of surfactants prepared by the chemical industry each year (≈2 × 107 t/a) also reflect the enormous importance of this special kind of functional molecules. The classic case is represented by compounds with a water-soluble head group attached to an oil-soluble alkyl tail. The described molecular architecture is responsible for the emergence of amphiphilic properties, self-assembly to higher order structures (e.g., micelles and liquid crystals), and the broad range of applications, such as in detergents, emulsification agents, and in phase-transfer catalysis.[1] Surfactants are also used frequently in nanoscience as capping agents e.g., for the control of nanoparticle growth and colloidal stabilization.[2] The integration of inorganic moieties has proven to be a powerful strategy for the development of novel surfactants equipped with more complex profiles and additional functionalities, for instance, catalytic properties.[3−7] Like for any other catalytic system as well, maximization of activity is one of the main targets in research. An intriguing question is: after the molecular structure of a catalytic surfactant has been optimized if additional measures exist, how to improve the activity further?

A unique way to maximize the activity known in the literature on heterogeneous catalysis is the so-called strong metal–support interaction, a phenomenon describing that certain combinations of metals on immobilized particular metal oxides are orders magnitudes more active than others.[8] Nanoscale dimensions of the metals (e.g., Au) were first and foremost considered important because of the enhanced surface to volume ratio. However, in some recent reports, scientists have discussed the role of plasmonic effects regarding the enhancement of photocatalytic activity in hybrid materials between gold nanostructures and metal oxides.[9−13] Solarska et al. used this concept in polyoxometalate–gold hybrids.[14] Polyoxometalates (POMs) are frequently described as molecular oxides, and one of the numerous, valuable features of POMs is catalytic activity.[15,16] Solarska et al. reported an astonishing improvement of the performance of photoanodes used for the water-splitting reaction, which was modified by Au NPs and POMs. The combination of catalytically active surfactants with gold nanoparticles could be a general and elegant way for optimization of catalytic surfactants as well. Based on the given arguments, surfactants with molecular oxides (POMs) as constituents will be valuable model systems for answering the latter question.[17]

There was already significant activity in the past on POM-organic hybrid materials in general and concerning those with amphiphilic properties in particular.[18−21] A very good introduction to the topic can be found in the seminal review published by Cronin et al.[22] The key for the success was that a variety of strategies have been developed for the organic modification of POM clusters.[16,23] Liu’s group was very successful in using the mentioned modification strategies to achieve multifunctional amphiphiles containing molybdate (Anderson),[24] tungstate (Dawson),[25,26] and also vanadate systems.[27] In the 1990s, Judenstein and Hill’s group established the basis for lacunary W-Keggin clusters as constituents.[28,29] This enabled our group to concentrate on surfactants with an [EW11O39] (lacunary Keggin) head group (E = P, Si, B).[30−33] The hydrophobic entity in the latter surfactants is an alkyl group, and it can thus not interact specifically with inorganic surfaces. However, it is well-known in the literature that organic thiols do strongly interact with metallic surfaces and eventually form the so-called self-assembled monolayers on gold (SAMS).[34] Although the gold surfaces are typically flat for SAMS, organic thiols also bind very well to curved surfaces such as in gold nanoparticles (Au NPs).[35] Cabuil and co-workers or Kapoor et al. used this concept for the immobilization of POMs on Au NPs,[36,37] and later De bruyn et al. reported an extension to Pd NPs.[38] There are further reasons why [SiW11O39]4–-based surfactants modified with alkyl chains containing a terminal thiol group, as shown in Scheme , represent valuable building blocks. The thiol group can undergo various modification reactions like the thiol–ene click reaction,[39] which should enable to introduce several alternative functions as a terminal group of the surfactant. Considering that two thiols can be coupled to disulfide bridges, one can think of POM-surfactant networks. Thiols can also be oxidized to sulfonic acid derivatives, and this would lead to a bolaform surfactant with two highly acidic end groups.

Scheme 1

Synthetic Sequence Leading to the Polyoxometalate-Thiol Surfactants with Bola Design (n = 1–7). TMA ≅ Tetramethylammonium

Here, we will present a systematic series of surfactants with the [SiW11O39] head group and alkylthiol side chain(s) of varying lengths. The surfactant properties of the compounds will be compared to each other, followed by investigating their ability to stabilize the surfaces of Au NPs. Finally, a reaction catalyzed by the protonated [SiW11O39] head will be performed and what the effect of radiation with different wavelengths is will be studied.

Results and Discussion

The surfactants were prepared as shown in Scheme . For further details, see the experimental part. First, an ethoxysilane functionality was introduced into the α-,ω-bromoalkene (1) by catalytic, anti-Markovnikov hydrosilylation. In a second step, bromine was substituted by thioacetate, followed by its reduction to the thiol function. Finally, compound (3) was reacted with a lacunary POM species and tetramethylammonium (TMA) as a counter ion. The nomenclature of the compounds is used as follows: “TMASiC10”, for instance, stands for the compound (N(CH3)4)4[SiW11O40](Si(CH2)10SH)2.

The analysis of TMASiC10 is discussed here as an exemplary case (see also Supporting Information Figure S1 and Table ). In electrospray-ionization mass spectrometry (ESI-MS), several signals can be assigned clearly to the desired compound. Most importantly, at 1092 g/mol, the molecular peak [M5–(TMA)2]3– can be identified. As expected, two signals are found in 29Si NMR spectroscopy, one at −85.09 ppm characteristic for the Si atom bound inside the cluster and one with roughly twice the intensity at −52.18 ppm for the alkylsilane species. The 183W NMR spectrum displays the characteristic pattern of an organically functionalized monolacunary tungstate Keggin species.[40] Since the solubility in water is low for TMA+ compounds and acidic heads are needed for the catalytic experiments, ion exchange chromatography was performed (TMA+ to Na+ or H+). After cation exchange, there is only a small shift in 29Si NMR signals indicating the integrity of the surfactant and the POM head. Analytical data are summarized in Figures S2 and S3. Final evidence for the successful preparation of the target compounds is achieved by ESI-MS. For instance, the signal shown in Figure a can be unambiguously assigned to the doubly charged ion [NaH[SiW11O40](Si(CH2)10SH)2]2–. The acidic character of the compounds with protons as counter ions is proven by recording a titration curve in water as shown in Figure S3. Surfactants with shorter alkyl chains were prepared in analogy and for proof of concept. Figure c shows the ESI-MS pattern of another member of the series with n = 4.

Table 1

Molecular Characterization of All Synthesized POM-SH-Surfactants by 1H, 29Si NMR, and ESI-MS

	1H NMR (DMSO-d6): δ=	29Si NMR (DMSO-d6): δ=	ESI-MS m/z =
[SiW11O40(SiC4H8SH)2]	2.55 (q, 4H), 1.80–1.60 (m, 8H), 0.68 (t, 4H)	29Si: −52.40 (s, 2Si), −85.10 (s, 1Si)	982.76 (M4– + Na+), 1485.63 (M4– + 2Na+)
[SiW11O40(SiC5H10SH)2]	2.52 (q, 4H), 1.68–1.46 (m, 12H), 0.68 (t, 4H)	29Si: −52.25 (s, 2Si), −85.10 (s, 1Si)	992.10 (M4– + Na+), 1499.65 (M4– + 2Na+)
[SiW11O40(SiC6H12SH)2]	2.49 (q, 4H), 1.65–1.38 (m, 16H), 0.67 (t, 4H)	29Si: −52.23 (s, 2Si), −85.09 (s, 1Si)	1001.11 (M4– + Na+), 1513.17 (M4– + 2Na+)
[SiW11O40(SiC7H14SH)2]	2.48 (q, 4H), 1.62–1.29 (m, 20H), 0.66 (t, 4H)	29Si: −52.23 (s, 2Si), −85.12 (s, 1Si)	1010.79 (M4– + Na+), 1527.68 (M4– + 2Na+)
[SiW11O40(SiC8H16SH)2]	2.47 (q, 4H), 1.61–1.33 (m, 24H), 0.66 (t, 4H)	29Si: −52.21 (s, 2Si), −85.12 (s, 1Si)	1019.82 (M4– + Na+), 1541.22 (M4– + 2Na+)
[SiW11O40(SiC10H20SH)2]	2.47 (q, 4H), 1.58–1.22 (m, 32H), 0.65 (t, 4H)	29Si: −52.22 (s, 2Si), −5.12 (s, 1Si)	1038.48 (M4– + Na+), 1568.72 (M4– + H+ + Na+)

Figure 1

Excerpts of the ESI-MS patterns; black = measured pattern of (a) NaSiC10; gray = signal calculated for the ion [NaHM]2–. (b) HSiC10; gray = signal calculated for the ion [HM]3–. (c) NaSiC4; gray = signal calculated for the ion [Na2M]2–, and light gray = signal calculated for the ion [NaHM]2–. (d) Molecular architecture of the synthesized surfactants; n = 4, 5, 6, 7, 8, 10.

Surface activity and formation of aggregates in solution are two typical features of surfactants. Concentration-dependent surface tension measurements obtained using the Wilhelmy plate method (Figure S4) confirm activity at the air/water interface. Since POM-surfactants tend to interact strongly with the plate used in our set-up,[30,32,33,41,42] which could have an influence on the reliability of the data, we have applied the pendant drop method as an independent method (Figure a). NaSiC4 displays no surface activity. The hydrocarbon chain is obviously too short, so the compound lacks amphiphilic properties. Therefore, SiC4-based compounds were not considered anymore in the following. The drop of surface tension at higher concentrations for compounds NaSiC with n ≥ 5 points to the population of the air/water interface, which is expected for surfactants. However, none of the surfactants could reach minimal surface tension. This is because of the high charge of the head group[33] and the resulting electrostatic repulsion. Nevertheless, dynamic light scattering (DLS) indicates that aggregates are already present in solution (Figure b). The aggregates formed by NaSiC5 have a size in the range expected for micelles. With an increasing packing parameter, the aggregates become significantly larger. For C10, there seems to be a transition, because presumably, a phase with lamellar characteristics becomes more stable. The size of the aggregates was confirmed by transmission electron microscopy (TEM) (Figure c–e) and the presence of tungsten in these aggregates is shown by energy-dispersive X-ray spectroscopy (EDX) given in Figure S5.

Figure 2

(a) Concentration-dependent surface tension measurements determined by the pendant drop method. Gray squares = NaSiC4, black circles = NaSiC5, triangles = NaSiC6, hashes = NaSiC7, hexagons = NaSiC8, pentagons = NaSiC10. (b) Representative aggregate size distribution curves (black) determined from DLS of NaSiC5 (solid line) and NaSiC10 (dashed line). Dependence of aggregate size on hydrocarbon chain length C (gray). TEM micrographs of a solution of NaSiC5 (c), NaSiC6 (d), and NaSiC10 (e) deposited on a carbon-coated grid.

There are two ways for obtaining the required Au NPs covered by SiC surfactants. Either the surfactants act as a capping agent during nucleation and growth of Au0 [37] or they can exchange the capping agent from preformed Au NPs. Figure S6 shows the result of a photoreduction synthesis approach using AuCl4– as a precursor and NaSiC10 as a surfactant. Because the particles are still polydisperse in size and shape, and even in an ideal case, each surfactant would lead to differently sized Au NPs, we decided that it is not worth investing substantial work in optimizing the nanoparticle synthesis protocol further. Instead, we prepared Au0 nanoparticles by a known, citrate-based method.[43] Afterward, Na/HSiC was added and the success of the required exchange process is proven by high-resolution (HR) TEM/EDX as shown in Figure . Each of the Au nanoparticles is surrounded by a thin, noncrystalline layer. The substantial imaging contrast is a first sign for the presence of heavy atoms such as W. In images with lower magnification (Figure a), one can even see a dark rim caused by the high electron density of W in the head group region. Unfortunately, in the HRTEM image (Figure b), the head group zone is not imaged anymore, because the focus has been set on the lattice planes of the Au NP and the electron beam penetrates multiple surfactant heads simultaneously due to imperfect alignment of the particle. Final confirmation comes from line-scan EDX (Figure c), showing the presence of W, and thus the surfactants at the surfaces. Because the thickness of the layer fits to a monolayer of NaSiC10, we can assume that the surfactant binds by means of the thiol group to the gold surface. Decorating the Au NPs with the surfactant is also confirmed by a small shift (Δλ = 6 nm) of the surface plasmon resonance band (λmax = 528 nm) after the exchange process. This shift is expected because the dielectric constant of the ligand shell is now different and the electron density of the W-containing surfactants is much higher than for citrate.

Figure 3

TEM (a; scale bar 50 nm) and HRTEM (b; scale bar 2.5 nm) images of Au nanoparticles obtained after surface exchange with NaSiC10. (c) Line-scan EDX analysis (black = Au; gray = W).

Protonated forms of POMs can act as Brønsted acid catalysts for diverse reactions.[44] Therefore, and because the protonated forms of the surfactants have also proven to be acidic (Figure S3), we have used HSiC10 for the Fischer esterification of 3-phenylpropionic acid with methanol as a test reaction (Figure a). The conversion was monitored by quantitative analysis of 1H NMR spectra (Figure S8). The importance of the protic form is also documented by the fact that only HSiC10 is able to catalyze the reaction, whereas NaSiC10 is inactive. HSiC10 remains active when immobilized at the surfaces of the Au NPs (Figure b). The high charge of the POM (−4; Figure ) makes sure that the protons remain in close vicinity of the head group region even in water.

Figure 4

(a) Catalytic test reaction (isothermal conditions). (b) Turnover numbers (TONs) of HSiC10@AuNPs (squares) and free HSiC10 (triangles) as a reference; dark conditions (black symbols) and the irradiated sample (yellow symbols). The arrows indicate the light-induced enhancement. (c) TONs after 6 days of HSiC@AuNPs. (d) Surfactant chain length dependence of TONs after 6 days for HSiC@AuNPs as a catalyst irradiated by red (630 nm), green (530 nm), and blue (470 nm) light. The inset shows the optical plasmon absorption band with respect to these three wavelengths. (e) Catalytic enhancement factor as a function of hydrocarbon length in HSiC surfactants (n = 5–10).

The catalytic tests were repeated while irradiating the sample with light for both systems (free surfactants and immobilized to Au NPs). The design of the self-made photoreactor design is shown in Figure S9 and the calculation procedure of turnover numbers (TON) is described in Figure S10. It is important to note that the reaction was performed under strict isothermal conditions for excluding any heating effect caused by radiation (see experimental details). The conversion does not differ for the free HSiC10 as a catalyst, whether the reaction is performed in light or not (Figure a). This result is expected since HSiC10 does not absorb light in the VIS region (Figure S3d). The behavior changes when HSiC10 is attached to the Au NPs (HSiC10@AuNP). VIS radiation (white light) of the latter system leads to a large increase in catalytic efficiency (Figure b). We have checked that the catalyst remains unaltered during the catalytic reaction (Figure S11). UV/vis spectra and line-scan EDX measurements are the same before and after catalysis, showing that the POM-surfactant is still attached to the Au NPs. The turnover number (TON) is a linear function of time in both cases, “dark” and “bright” (Figure S12). Thus, the catalytic activity for each system probably does not change over time, but the difference in slopes is caused by higher catalytic activity in the presence of light.

For testing the hypothesis, the noted effects are caused by an interaction with the plasmonic nanoparticle, we also tested if similar effects are observed and if Au NPs and a reference heteropoly acid H8SiW11O39 is present, but the latter is not attached to the particles (see Supporting Information Figure S13c). Because the esterification reaction is catalyzed by protons, there is slow conversion, but the values remain in a region comparable to Figure b for HSiC10 in the absence of Au NPs. Two further parameters were addressed: (i) distance—there must be an effect of the surfactant chain length because this will alter the distance of the catalytically active POM head group to the surface of the Au NPs. (ii) Light—because the plasmon resonance band of the Au NPs used here is found at 528 nm (Figure d-inlet), green light lead to a maximal enhancement, whereas other wavelengths should not influence the catalytic efficiency at all or at least to a much lower extent.

The catalytic tests were repeated for a series of compounds differing systematically in the hydrocarbon chain length (Figure c–e; Table S1). The catalytic activity difference in the presence of light becomes more marked for shorter chains C. For HSiC5, the light-induced catalytic enhancement reaches 150%, meaning that it is more than two times more active than in the dark. For final proof of our hypothesis, the experiments were repeated using monochromatic red (630 nm), green (530 nm), or blue (470 nm) instead of white light (Figure d,e). Red light has led to almost no catalytic improvement and the system is independent of the surfactant chain length (Figure e). There is a small contribution of blue light to the catalytic enhancement, but the effect does not differ for surfactants with different chain-length. In contrast to this, there is a significant effect for green light and the strongest increase in catalytic activity compared to the dark situation (182%) can be observed for the shortest POM surfactants. Thus, an enhancement by interactions of plasmonic effects and the catalytically active POM clusters was proven.

Several possibilities exist on how promoting the catalytic activity by plasmons can occur.[45] The first possibility is a local photothermal effect.[46−48] The plasmonic particles heat up because of the absorption of radiation. Because dissipation of heat has to occur by means of transport through the surfactant shell attached to the gold particles, the thermal conductivity of surfactants is not high,[48] and they are located in the direct vicinity of the particle surface, one cannot exclude the local temperature at the POM head group that is different from the surrounding solution. An elevated temperature at the POM head could explain the enhancement in catalytic activity. Another alternative is the occurrence of a photoelectrocatalytic effect.[49] Electrons from the metallic nanoparticle are able to tunnel to suitable acceptor orbitals inducing an electrocatalytic reaction.[50,51] The POM head does indeed offer such electronic levels,[42,52] and the WVI centers can be reduced to WV. However, we could not observe the corresponding change in the UV–VIS spectrum of the surfactant, and the mechanism of the esterification reactions involves the activation of the carboxylic group by protonation. Some reports describe that positive charge carriers (holes) can also be transferred by plasmonic particles,[53] but because the POM-surfactant can hardly be oxidized, we believe that this alternative is unlikely. Besides, it was shown by our experiments that only the protonated form of the surfactant is active in catalysis. Therefore, the effect cannot be caused by a hole-mediated mechanism. The direct energy transfer from a plasmonic nanoparticle is possible by Förster resonance energy transfer or surface energy transfer,[54] but because of the HOMO–LUMO gap in the UV of the POM-surfactant species, it is also unlikely that this process occurs here. Finally, the absorption of light also leads to strong electric fields directly at the surface of the plasmonic nanoparticle. The transition state of the esterification reaction was reached after protonation of the carboxylic group that has ionic character and is thus highly polar. Therefore, the dipolar coupling of this transition state can alter its energy, similar to solvent effects known for such type of reactions in organic chemistry.[55] To visualize the size and shape of the plasmonic optical mode in our hybrid system, we applied finite-time-domain-difference simulations with the 0.4 nm grid size. We found that a gold radius of 8 nm and a cover layer of 2 nm at an effective refractive index of n = 1.2 can approximately reproduce the measured resonance wavelength and shift. Figure shows the resulting spatial intensity distribution. It covers the surfactants and adjacent reactants with the expected light concentration to a few nanometer dimensions; the peak intensity is enhanced by a factor of 7. Lowering the energy of the transition state would result in a change of the activation barrier for the process and, consequently, an increase in the rate constant of the reaction.

Figure 5

Plasmonic field enhancement around the nanoparticle at the resonance wavelength. A plane wave with amplitude E_0 = 1 is propagating in the y-direction with polarization along the x-direction. Plotted is the magnitude |E| of the electric field E at peak time (see also the movie attached in the Supporting Information).

From the arguments above, the two most likely candidates for explaining the observed catalytic effects are local heating effects and electric field effects. To shed some more light onto the phenomenon, we have performed a series of additional experiments. The reaction was repeated with HSiC5@AuNP as a catalyst without light but at different temperatures (see Supporting Information Figure S13a). As expected, raising the temperature leads to an increase in TON as well up to 711 at 55 °C. This is much smaller than the effect observed for the photopromoted reaction (TON = 1700). Assuming that the temperature dependency of the reaction rate follows an Arrhenius law (k ∝ exp (−Ea/kT)), the corresponding extrapolation of the experimental data leads to a temperature of ≈80 °C for reaching a comparable TON. This means that the local temperature present at the POM heads would have to be of the order of 75 °C. We also checked the effect of the light intensity (see Supporting Information Figure S13b). It is seen that for doubling the light intensity, the TON is directly proportional, whereas for electric field-induced effects, the proportionality should only be of the order of √2. Therefore, we believe that the most likely explanation for the increase of catalytic activity during irradiation with light is a photothermal effect. However, it should be underlined that a precise photophysical characterization requires the application of a much more extended set of analytical techniques and theoretical calculations, which is beyond the scope of the current manuscript.

Conclusions

We have presented the synthesis of organic inorganic surfactants with an anionic polyoxometalate head group and bolaform-type architecture. A thiol group attached on the opposite side of the surfactant enabled bonding to the surface of gold nanoparticles. The acidity of the surfactants with protons as counter ions was sufficiently high to enable chemical reactions catalyzed by a Brønsted acid. The new POM-surfactant Au NP composites show catalytic activity as well, and it could be enhanced significantly by radiation with light. The cooperation between the plasmonic properties of the Au NP and the catalytic activity of the POM head group was proven because the features of the system depend strongly on the distance between POM and the surface of the nanoparticle adjusted by means of the surfactant length. Furthermore, catalytic enhancement strongly increased when the correct wavelength was used for radiation. There were first hints that this is because of a photothermal effect. Experiments for further photophysical characterization of the phenomenon are underway. Since the spectral position of the surface plasmon band depends on the nanoparticle size, in future, the generation of complex catalytic systems triggered by light of a particular wavelength seems achievable.

Methods

Unless stated differently, synthesis was performed using general Schlenk techniques under an argon atmosphere. The solvents were dried according to the standard literature[56] and stored under argon. All starting materials used for synthesis were purchased from commercial sources (Sigma-Aldrich or ABCR chemicals).

The lacunary polyoxometalate (POM) cluster [SiW11O39]8– was synthesized according to the literature.[57]

Synthesis of Organic Precursor (EtO)3SiCHSH (x = 4–10; y = 2x)

(EtO)3SiCHBr (1)[41]

(41)In a 250 mL Schlenk flask, 20 mmol (1.0 equiv) of X-bromo-1-alkene was dissolved in 100 mL of dichloromethane (DCM). Next 22 mmol (1.1 equiv) of triethoxysilane and 5 droplets of Karstedt’s catalyst were added to the stirring solution. The reaction was stirred for 7 days at 40 °C. Following, the solvent was removed by reduced pressure to yield a yellowish oil. The pure product was obtained by removing the residual starting materials by reduced pressure (∼1 mbar) and at 90 °C for 8 h.

Yield: 55–90%, yellowish oil.

1H NMR (400 MHz, CDCl3) δ (ppm) = 3.79 (q, 6H), 3.39 (t, 2H); 1.90–1.30 (m, 4–16H); 1.20 (t, 9H), 0.61 (t, 2H).

(EtO)3SiCHSAc (x = 4–10; y = 2x) (2)[58]

In a 100 mL Schlenk flask, 10 mmol (1.0 equiv) of (1) and 17 mmol (1.7 equiv) of potassium thioacetate were dissolved in 40 mL of DMF. The reaction solution was heated up to 40 °C for 2 h with vigorous stirring. Next, the solution was cooled to room temperature and 30 mL of water was added. The aqueous solution was extracted three times with pentane and dried over anhydrous magnesium sulfate. The solvent of the combined organic layers was removed by reduced pressure.

Yield: 90–100%, brownish oil.

1H NMR (400 MHz, CDCl3) δ (ppm) = 3.77 (q, 6H), 2.84 (t, 2H); 2.30 (s, 3H); 1.60–1.30 (m, 4–16H); 1.20 (t, 9H), 0.61 (t, 2H).

(EtO)3SiCHSH (x = 4–10; y = 2x) (3)

In a 100 mL Schlenk flask, 8 mmol (1.0 equiv) of (2) was dissolved in 60 mL of ethanol. With vigorous stirring, 10.4 mmol (1.3 equiv) of sodium borohydride was added. The reaction was heated to 40 °C for 2 h. Next, the solution was cooled to room temperature and 30 mL of water was added. The aqueous solution was extracted three times with pentane and dried over anhydrous magnesium sulfate. The solvent of the combined organic layers was removed by reduced pressure.

Yield: 80–95%, yellowish oil.

1H NMR (400 MHz, CDCl3) δ (ppm) = 3.80 (q, 6H), 2.49 (t, 2H); 1.60–1.30 (m, 4–16H); 1.20 (t, 9H), 0.61 (t, 2H).

Synthesis of POM-Surfactants

[SiW11O40(SiCHSH)2] (x = 4–10, y = 2x) (4)[41]

(41)In a 2L beaker, 1 mmol (1.0 equiv) of powdered lacunary POM-cluster (K8[SiW11O39]) and 7.5 mmol (7.5 equiv) of tetramethylammonium chloride were suspended in 800 mL of acetonitrile. To the resulting suspension, 4.4 mmol (4.4 equiv) of 1 M hydrochloric acid and 2.2 mmol (2.2 equiv) of (3)—dissolved in 10 mL of DCM—were dripped into the solution. The reaction was stirred vigorously for 1d at room temperature. The suspension was filtered and the solvent of the filtrate was removed by reduced pressure. The precipitate was washed with water, methanol, and diethyl ether.

Yield: 75–90% (based on the 3), white solid.

Ion exchange to the corresponding H- and Na-[SiW11O40(SiCHSH)2] (x = 4–10; y = 2x):

Cations were exchanged to Na+ or H+ by slow filtration of a 2 mg/mL solution of TMA–POM through a column packed with Amberlite-IR120-H/Na. Complete exchange was confirmed via 1H NMR (absence of a signal at δ = 3.23 ppm).

Synthesis of POM-Surfactant Gold Nanoparticle Hybrid Systems

Gold nanoparticles were synthesized by the Turkevich method.[43]

Ion Exchange to the Corresponding H-catalyst

The cations of the functionalized gold nanoparticles were changed by ion exchange chromatography. A concentrated methanol solution was filtered slowly through a column packed with Amberlite-IR120-H. The resulting suspension was concentrated by centrifugation. The nanoparticles were resuspended in 5 mL of methanol.

1H NMR (400 MHz, CDCl3) δ (ppm) = 7.15 (m, 5H), 3.58 (s, 3H), 2.86 (t, 2H); 2.57 (t, 2H).

Analytical Methods

NMR measurements (1H, 11B, 13C, 29Si, and 31P) were performed on a Varian Unity INOVA 400 Spectrometer. The 183W NMR-spectra were recorded on a Bruker Avance III 600 MHz Spectrometer with 10 mm NMR tubes. ESI-MS data were acquired on a Bruker microtof II system. The solutions were injected directly into the evaporation chamber. SAXS was acquired on a Bruker Nanostar system equipped with pinhole collimation and Cu Kα radiation. The samples were placed between X-ray transparent mylar foils and were measured in an evacuated chamber. For avoiding the contamination of the measurement chamber, samples were dried prior to use. TEM was acquired on a Zeiss Libra 120 system and a JEOL JEM-2200FS. The dry sample was placed directly on carbon-coated copper grids. HRTEM images have been taken with a JEOL JEM-2200FS with an acceleration voltage of 200 kV. The individual surfactant samples have been prepared from aqueous solutions on copper TEM grids with a carbon coating and a net distance of 400 mesh. Dynamic light scattering (DLS) measurements were performed using a Malvern ZEN5600. UV/VIS spectroscopy was performed on a Varian Cary 100. Pictures obtained by polarization microscopy were photographed with an Olympus CX41 light microscope. Surface tensions between aqueous surfactant solutions and air were measured at 25 ± 1 °C using a Krüss drop shape analysis DSA1 apparatus. This instrument obtains spatial coordinates of a drop edge (shape and size), which are used to calculate the surface tension. The calibration used the surface tension of pure water. Surface Tension measurements were performed using a Krüss K100 tensiometer.

Catalytic Measurements (Esterification of 3-Phenylpropionic Acid)

Seventy milligrams of 3-phenylpropionic acid (0.5 mmol) were solved in 5 mL of catalyst. The suspension was stirred during the reaction. The reaction was irradiated by white light (power = 100 W, λ = 400–800 nm), red light (power = 50 W, λ = 630 nm), green light (power = 50 W, λ = 530 nm), or blue light (power = 50 W, λ = 470 nm). Reference samples were prepared without any light irradiation. All measurements were performed at isothermal conditions. All conversions were measured by 1H NMR spectroscopy.

Photochemical Experiments

The experiments were performed using a self-constructed reactor setup. Ten day-light chip light emitting diodes (LEDs) (voltage = 29 V, current = 350 mA) were used for irradiation with white light. A double-walled reaction vessel and a cryostat were used for assuring isothermal conditions. The temperature of all solutions was monitored by a thermometer, for isothermal conditions. For an irradiation by red (630 nm), green (530 nm), or blue (470 nm) light also, a self-constructed reactor setup was used. Therefore, 30 RGB chip LEDs were used. These were cooled by air. Overall a power of 50 W was used (voltage = 9 V, current = 5.5 A) for the experiments. The temperature of all solutions was monitored by a thermometer, for isothermal conditions.