Organometallic, Nonclassical Surfactant with Gemini Design Comprising π-Conjugated Constituents Ready for Modification.

Surfactants are functional molecules comprising a water-compatible head group and a hydrophobic tail. One of their features is the formation of self-assembled structures in contact with water, for instance, micelles, vesicles, or lyotropic liquid crystals. One way to increase the functionality of surfactants is to implement moieties containing transition-metal species. Ferrocene-based surfactants represent an excellent example because of the distinguished redox features. In most existing ferrocene-based amphiphiles, an alkyl chain is classically used as the hydrophobic tail. We report the synthesis and properties of 1-triisopropylsilylethynyl-1'-trimethylammoniummethylferrocene (FcNMe3TIPS). In FcNMe3TIPS, ferrocene is part of the head group (Gemini design) but is also attached to a (protected) π-conjugated ethynyl group. Although this architecture differs from that of classical amphiphiles and those of other ferrocene-based amphiphiles, the compound shows marked surfactant properties comparable to those of lipids, exhibiting a very low value of critical aggregation concentration in water (cac = 0.03 mM). It forms classical micelles only in a very narrow concentration range, which then convert into monolayer vesicles. Unlike classical surfactants, aggregates already form at a very low concentration, far beneath that required for the formation of a monolayer at the air-water interface. At even higher concentration, FcNMe3TIPS forms lyotropic liquid crystals, not only in contact with water, but also in a variety of organic solvents. As an additional intriguing feature, FcNMe3TIPS is amenable to a range of further modification reactions. The TIPS group is easily cleaved, and the resulting ethynyl function can be used to construct heterobimetallic platinum-ferrocene conjugates with trans-Pt(PEt3)2X (X = Cl, I) complex entities, leading to a heterobimetallic surfactant. We also found that the benzylic α-position of FcNMe3TIPS is rather reactive and that the attached ammonium group can be exchanged by other substituents (e.g., -CN), which offers additional opportunities for further functionalization. Although FcNMe3TIPS is reversibly oxidized in voltammetric and UV-vis spectroelectrochemical experiments, the high reactivity at the α-position is also responsible for the instability of the corresponding ferrocenium ion, leading to a polymerization reaction.

Introduction

Surfactants are highly important, functional molecules comprising a water-compatible head group and a hydrophobic tail. They are produced by the chemical industry on a mass scale (≈1.6 × 107 t/year) and used in detergents, as emulsification agents, or for phase-transfer catalysis. Their main property is that they reduce the interfacial energy (note that the term “surfactant” represents an abbreviation for “surface-active agent”). One of their most important features is the formation of concentration-dependent, self-assembled structures in contact with water, ranging from micelles or vesicles at low concentrations to lyotropic liquid crystals (LLCs) and inverse phases at higher concentrations. The classical design of a surfactant molecule comprises a water-soluble head group attached to a hydrophobic alkyl tail. The properties and behavior of surfactants strongly depend on the relative proportions of the hydrophilic and oleophilic parts. Concepts like the packing parameter P or the hydrophilic lipophilic balance (HLB) have been developed to describe the influence of such molecular variations.[1−3] For instance, a surfactant equipped with two alkyl chains often has lipid-like character. Compounds with two head groups at the opposite sides of a long hydrophobic chain are called bolaform surfactants.[4] An alternative structure is the so-called gemini architecture with the two heads separated by a relatively short spacer.[5] Because of their special properties, several researchers became interested in asymmetric gemini surfactants.[6−8]

More recently, the portfolio of surfactants was successfully expanded by introducing additional properties such as pH-, CO2-, photo-, magneto-, or thermoresponsive features.[9] Excellent reviews on this topic are available from Eastoe et al. in 2013 or Landfester et al. in 2017.[10,11] A particularly powerful approach in the literature is the generation of hybrid surfactants containing an inorganic, transition-metal-containing building block.[12] One of the most valuable features of such moieties is their rich redox chemistry. The reversible change of head group charge is an intriguing feature for a surfactant system,[13,14] and this requires a redox-active constituent.

Among redox-active building blocks, ferrocene (Fc) has proven to be of eminent importance. Ferrocene is a unique organometallic compound and the prototypical metallocene in modern chemistry.[15−17] It is famous for its efficient methods of synthesis and derivatization, its completely reversible redox properties, and its oxidation state-dependent water solubility.[18−21] Therefore, ferrocene has been widely used in materials science, in particular in polymer chemistry.[22] Amphiphilic copolymers are well known and feature mostly a poly(vinylferrocene) or a poly(ferrocenylsilane) backbone and water solubility-mediating groups. The latter are either incorporated into the backbone or attached to the numerous side chains.[23−25] Various new synthetic procedures have been developed during the recent years, for instance, by Manners et al. or Wurm et al., who provided expanded libraries of polymer-like ferrocene-based amphiphiles with high potential for future applications, for example, in separation methods or for reducing the overall surfactant waste during industrial processes.[26−28] A good overview over ferrocene-based surfactants was provided by Abbot et al.[29] The field of ferrocene-modified amphiphiles was pioneered by Saji in the late 1980s,[30−32] and several related surfactants have been published since then.[33−36] Most of these involve monosubstituted ferrocene derivatives. Because pristine ferrocene is insoluble in water, it is often positioned at the end of the hydrophobic tail. The approach presented by Saji is unique because it solved the latter problem by positioning Fc next to an ammonium group modified by a long alkyl chain in (Fc-CH2)(CH3)2N+(C12H25). The authors reported the redox properties and some preliminary characterization of its colloidal properties, including the formation and redox-triggered disassembly of micelles in water.[30−32]

The systems described above can be developed further by considering the following arguments. Many applications involving surfactants would greatly benefit from charge carrier (electron or hole) transport through the interface, and new perspectives such as micellar batteries, micellar electrocatalysts, or liquid-crystalline semiconductors would open up for such systems.[37,38] Classical surfactants are useless for such purposes, not only because their heads are not redox-active but also because their tails are electrically insulating as well. Ferrocenyl-based head groups represent a promising entry point to charge-conducting surfactants if an additional π-conjugated chain can be introduced into the molecule instead of an alkyl chain. However, in a design analogous to the surfactant by Saji, delocalization of charge carriers would be impeded because the ammonium group interrupts the conjugation between the ferrocene and an N-bonded π-conjugated side chain. Therefore, we aim at ferrocene-based surfactants where a π-conjugated substituent is directly attached to a cyclopentadienide ring at the ferrocene nucleus, leading to a π-conjugation over the entire molecule. We here present FcNMe3TIPS (see Scheme ) as a first successful realization of this concept. As a further advantage, FcNMe3TIPS can be modified in several different ways. Thus, it represents a potential building block for the construction of more complex amphiphilic structures. We describe the synthesis and characterization of FcNMe3TIPS and report on its properties as a surfactant and its redox behavior. Finally, we report first results on exploring possible means for modifying its basic structure.

Scheme 1

Multistep Synthesis of FcNMe3TIPS

Results and Discussion

Molecular Synthesis and Characterization

FcNMe3TIPS was prepared in five steps starting from ferrocene (Scheme ). 1,1′-Dibromoferrocene (2) was obtained as reported by Long and co-workers.[39] It was then converted to 1-bromo-1′-iodoferrocene (3) according to the procedure of Ilyashenko and co-workers.[40] Standard Sonogashira reaction conditions were used to selectively react 1-bromo-1′-iodoferrocene to the 1′-triisopropylsilylethynyl (TIPSA)-substituted derivative (4). Subsequent conversion to 1-triisopropylsilylethynyl-1′-dimethylaminomethylferrocene (5) was performed according to a known procedure published by Widhalm et al. using n-BuLi and Eschenmoser’s salt Me2N=CH2+I– under Mannich-like conditions.[41] Quaternization with methyl iodide in MeOH yielded FcNMe3TIPS (6).[42] Successful synthesis of FcNMe3TIPS was proven by a combination of analytical methods. A section of its electrospray ionization mass spectrum (ESIMS) is shown in Figure (for the full spectrum, see Figure S1 of the Supporting Information). The observed signal at 438.2 g/mol and its isotope pattern are in perfect agreement with the calculated pattern for the M+ peak C25H40FeNSi+. The presence of the triple bond is confirmed by the characteristic stretching vibration νC≡C at 2147 cm–1 in the IR spectrum, in the typical region for internal alkynes.[43]

Figure 1

Experimental ESIMS pattern (black) of FcNMe3TIPS (6) and the spectrum calculated for C25H40FeNSi+ (gray).

Solution UV–vis absorption spectra show an intense absorption band at λmax = 230 nm and a weaker band in the vis region at 400–500 nm (λmax = 443 nm). The latter is characteristic for the highest occupied molecular orbital–lowest unoccupied molecular orbital transition of ferrocene derivatives and is responsible for their typical orange coloration (see Figure a).[44] The density functional theory (DFT)-calculated frontier MOs of FcNMe3TIPS are shown in Figure S2 of the Supporting Information.

Figure 2

(a) Photographic image of a dilute solution of FcNMe3TIPS in water indicating the surface-active properties (foam formation). (b) Geometry-optimized molecular structure of FcNMe3TIPS (see also the Supporting Information Figure S3b) and electrostatic potential surface. (c) Concentration-dependent surface tension measurements. The gray dashed lines indicate the interval for which dynamic light scattering (DLS) measurements were performed. (d) Schematic illustration of the arrangement of molecules of FcNMe3TIPS at the air–water interface according to its overall structure (including its rigid alkyne functionality) and the calculated average area (Am = 43 Å2) occupied per molecule at the interface (blue, water; gray circles, air/foam at the interface).

Surfactant Properties of FcNMe3TIPS

FcNMe3TIPS is slightly soluble in water (0.5 mg/mL) as defined by the United States Pharmacopeia and soluble in nonpolar solvents such as dichloromethane (DCM) (60 mg/mL), which is a first indication for amphiphilic properties. In water, the surfactant exhibits a significant foaming capability (see Figure a), a characteristic feature of surfactants. The calculation of the electrostatic potential surface of FcNMe3TIPS (Figure b) confirms a surfactant-like architecture and shows that all molecular parts except for the ammonium head group are nonpolar. Concentration-dependent surface tension (γ) measurements in water were performed next (Figure c).

It was found that γ remains constant until a concentration of c = 0.007 mM is reached and then decreases. Saturation of the air–water interface is observed at c = 0.79 mM with a minimal surface tension γmin = 28.5 mN/m. This value is lower than those of other ferrocene-based amphiphiles in the literature (γmin = 35–55 mN/m),[9,33,35,45−48] which indicates a very effective stabilization of the interface and a close packing of the surfactant molecules. The surface tension curve can be treated as a Gibbs isotherm, and the surface excess (Γ = 3.90 μmol/m2) and the average area occupied per molecule at the water–air interface (Am = 43 Å2) were calculated. Am fits perfectly the distance between the trimethylammonium head group and the ferrocene at the water–air interface as determined from the calculated, geometry-optimized structure (Figure d; see also the Supporting Information Figure S3b). Classical surfactants start to form micelles only when the interface is covered by a surfactant monolayer. We checked the occurrence of aggregates in solution by dynamic light scattering (DLS) recorded for different concentrations ranging from c = 0.014 to 0.88 mM (Figure ). Even at low concentrations, aggregates could be detected with a hydrodynamic diameter DH (≈5 nm), which is in the range expected for micelles (approx. twice the molecular length of the surfactant). However, the aggregate size increases almost linearly with surfactant concentration (Figure b). Such behavior cannot anymore be explained by the presence of micellar aggregates.

Figure 3

(a) Aggregate size distribution curves determined from DLS measurements in aqueous solution of FcNMe3TIPS at c = 0.014 mM (black), 0.22 mM (red), and 0.88 mM (blue). (b) Correlation of the hydrodynamic diameter DH with surfactant concentration.

Transmission electron microscopy (TEM) was performed next (Figure a). In agreement with the DLS data, one notes objects in a size range 100–200 nm separated by a thin membrane. The thickness of the membrane is ≈3 nm, which matches with a double-layer structure composed of molecules of FcNMe3TIPS, and these findings can be supported by small-angle X-ray scattering (SAXS), powder X-ray diffraction, and other TEM micrographs displayed in Figure S3a of the Supporting Information.

Figure 4

(a) TEM of aggregates formed by FcNMe3TIPS in water (c = 0.8 mM). (b) Energy-dispersive X-ray spectroscopy (EDX) data; Cu signals from the TEM grid.

This surfactant has a tendency for the formation of vesicular structures. The vesicles appear to be broken up caused by the high-vacuum conditions in electron microscopy. Area-selected energy-dispersive X-ray spectroscopy (EDX) confirms the presence of Fe (from Fc) and Si (from the TIPS end group) (Figure b) and the signals for iodine originating from the I– counterion (see Scheme ). According to the theory of Israelachvili, surfactants with a packing parameter in the range 0.5–1 are prone to form vesicles instead of micelles.[1] The packing parameter P = 0.87 of FcNMe3TIPS is in full agreement with this expectation (see the Supporting Information, Figure S3b). Vesicle formation is a rather uncommon feature among ferrocene-based amphiphiles known in the literature.[35,36]

However, when comparing Figures and 3, one has to conclude that aggregates form in solution prior to saturation of the air–water interface. This means that the concentration at γmin does not equal the critical aggregation concentration (cac). Therefore, an independent method for the determination of the cac was required. To these ends, FcNMe3TIPS was dissolved in water at different concentrations. The aqueous phase was then layered with n-hexane containing the lipophilic dye azobenzene (see also Figure S4 of the Supporting Information). The optical absorbance of the dye in the oil phase was determined at λ = 316 and 228 nm by UV–vis spectroscopy. At low concentration of the surfactant, the concentration of the dye remains constant (Figure ). Starting at an FcNMe3TIPS concentration of ≈0.01 mM, some azobenzene moves into the aqueous phase, and, as a result, the measured absorption in the oil phase decreases. The concentration of 0.01 mM is identical to that for which we have observed the occurrence of micelles (Figure b). Therefore, it can be concluded that azobenzene-loaded micelles are present in water. Surprisingly, a minimum is reached at c = 0.03 mM, and on increasing the concentration further, the absorption increases again to the original value. In agreement with DLS and TEM (Figures and 4), we explain this behavior by the transition from a micellar state to the vesicular state. Because the inner cavity of the vesicles is also filled with water, azobenzene cannot enter the water phase anymore. This means that the cac (≅the concentration at which the first aggregates form in solution) is very low (at ≈0.01 mM) and that the shape transition commences at a concentration of ≈0.03 mM. Classic surfactants like cetyltrimethylammonium bromide and sodium dodecyl sulfate have a significantly higher cac value of 0.92–1 and 6–8 mM, respectively,[49−51] while the cac of ferrocene-based amphiphiles as they were, for instance, explored by Saji and co-workers is usually in the range of 0.1–2 mM.[30,48,52,53] In contrast, lipids have typically much lower cac’s in the nM region. The cac of FcNMe3TIPS is thus in between those of lipids and classic surfactants.[54,55]

Figure 5

Alternative determination of the cac. Absorption of azobenzene in the cyclohexane phase at different concentrations of the surfactant in the aqueous phase.

Thus, the formation of aggregates commences even before a monolayer is formed at the air–water interface. This unusual behavior can be explained by the peculiar structure of FcNMe3TIPS. The rigid alkyne functionality reduces the flexibility of the overall amphiphile and the possibilities of how the amphiphiles can arrange at the water–air interface. According to Figure d, a close packing of molecules of FcNMe3TIPS leads to an energetic destabilization of the Gibbs monolayer. Notably, the close proximity of the positive charges at the trimethylammonium head groups results in strong Coulombic repulsion. Therefore, the formation of aggregates with a certain degree of curvature (micelles, vesicles) and an increased distance between the positive charges might be energetically favored, thereby decreasing the prevalent charge repulsion, instead of forming a closely packed Gibbs monolayer. Such behavior has rarely been described in the literature but was reported for conical ionic fullerene amphiphiles following the image charge theory by Nitta and co-workers.[51,56,57] Our arguments are also supported by comparison to similar structures as our surfactant, but with alkyl chains.[29] Those compounds have a higher average surface tension (γmin = 35–55 mN/m), and the overall surface activity is reduced. This can be explained by the higher space required by the flexible alkyl chains at the air–water interface.

A surfactant is expected to form lyotropic liquid crystals (LLCs) at higher concentration. We therefore also examined the phases of FcNMe3TIPS formed at high concentration levels in different solvents (water, acetonitrile, a mixture of acetonitrile and isopropanol as well as in apolar solvents like dichloromethane). There are only few reports on LLCs with ferrocene-based amphiphiles.[58,59] Because many LLC phases are optically anisotropic, polarized optical microscopy (POLMIC) is a convenient method to observe LLCs. POLMIC images show that FcNMe3TIPS forms LLC phases not only in polar solvents but also in nonpolar solvents (see Figure a and the Supporting Information Figure S5). Maltese-cross patterns (columnar droplets), giant mosaiclike LLCs, and fanlike textures were observed in polar and apolar solvents, indicating the presence of LLCs in the circular/lamellar and the smectic phase, respectively.[60−62] Small-angle X-ray scattering (SAXS) reveals a signal at a scattering vector q = 2.21 nm–1 corresponding to a lattice plane spacing of d = 2.84 nm. The distance of 2.84 nm equals twice the length of the ferrocene amphiphile as estimated from the geometry-optimized, calculated structure and indicates an end-to-end orientation of the triisopropylsilylethynyl lipophilic tails.

Figure 6

POLMIC (a) and SAXS (b) of an LLC phase of FcNMe3TIPS.

Functionalization of FcNMe3TIPS and Redox Properties

As it was mentioned before, the new surfactant FcNMe3TIPS has the potential advantage that it can be modified further such as to endow it with even superior levels of functionality. The most attractive position for such modification is obviously the TIPS-protected ethynyl end group. The TIPS group is easily cleaved from (5) using tetrabutylammonium fluoride (Scheme ). The resulting H-terminated alkyne (7) is now amenable to a wide range of further functionalizations. For proof of concept, the square-planar platinum fragment trans-Pt(PEt3)2Cl was attached to (7) to give the neutral complex (8). The latter was converted to the heterobimetallic surfactant (9) by subsequent quaternization of the amine function with concomitant substitution of the chloro by an iodo ligand at the platinum ion. The success of these reactions was unambiguously proven by NMR spectroscopy (see the Experimental Section and Figure S6 of the Supporting Information). Two-dimensional (2D) NMR spectroscopic investigations confirmed the purity of complexes (8) and (9). In particular, Pt satellites for the ethynyl-carbon atoms of (9) were observed in its 13C NMR spectrum. The triplet at −4823 ppm (JPtP = 2337 Hz) in the 195Pt NMR spectrum indicates the formation of a trans-Pt(PEt3)2I(−C≡CR) fragment, while the 31P NMR spectrum accordingly shows a singlet at 8.57 ppm with Pt satellites with an identical JPtP = 2337 Hz.

Scheme 2

Preparation of a New Heterobimetallic Surfactant

According to the report of Lindsay et al.,[42] it should also be possible to exchange the ammonium group in α-position to the ferrocene ring by nucleophiles. We adapted the procedure according to Scheme and obtained the corresponding nitrile compound (10). The 1H NMR spectrum shown in Figure S7 proves the upfield shift of the resonance signal for the methylene protons in α-position upon substitution of the trimethylammonium group by the nucleophile cyanide and underlines the successful synthesis of FcCNTIPS (10). Compound (10) itself can be further functionalized to the respective carboxamides, the carboxylic acid, or to amines.

Scheme 3

Nucleophilic Attack at the Ammonium Group

An important feature of ferrocene-based amphiphiles is their reversible one-electron oxidation to the corresponding ferrocenium species (Fc+). In the case of FcNMe3TIPS, the charge of the surfactant increases from +1 to +2. More importantly, the formerly neutral ferrocene nucleus changes to cationic ferrocenium and hence may become a part of the hydrophilic head as opposed to the oleophilic part of the molecule (c. f. Figure b). Both effects should cause a major change of the packing parameter P. We first investigated the redox properties of the iodide salt of the cationic FcNMe3TIPS surfactant by cyclic voltammetry (CV). As shown in Figure S8 in the Supporting Information, CVs recorded in dichloromethane (DCM) show three consecutive redox waves. Comparison with tetrabutylammonium iodide indicates that the first two processes at E = −165 and 88 mV are due to the I–/I3–/I2 redox couples[63,64] and that the most anodic wave at a half-wave potential E1/2 of 332 mV is assignable to the Fc/Fc+ redox couple. To avoid this interference, the iodide counterions were replaced by nitrate using an ion-exchange resin, and the corresponding nitrate salt was used further on in the electrochemical investigations. The latter showed only the reversible Fc/Fc+ couple at an E1/2 of 332 mV (see Figure a) in organic solvents. In water as the solvent, oxidized FcNMe3TIPS is obviously immobilized at the electrode surface as revealed by the typical, sharp and nondiffusive anodic adsorption peak. The presence of a normal diffusion-controlled reverse peak on the cathodic scan suggests that oxidized FcNMe3TIPS is chemically (at least partially) stable on the short CV time scale.

Figure 7

CV of the nitrate salt of FcNMe3TIPS in DCM/0.1 M NBu4PF6 (a) and in water (b). Repetitive scans of the Fc/Fc+ wave in the presence of “magic blue” (c), and changes in the UV–vis spectra on electrochemical oxidation of FcNMe3TIPS (d).

More detailed investigations of the oxidation process using UV–vis spectroelectrochemistry (SEC, 0.1 M NBu4PF6 in DCM) revealed a more complex behavior on longer time scales. When employing a rather high overpotential to ensure rapid oxidation, the vis band of the neutral compound at λmax = 443 nm decreased upon oxidation and two new bands with similar or higher intensity at λmax = 585 and 782 nm develop (Figure d). Both are typical of ferrocenium species.[65,66] Rapid rereduction at likewise high overpotential reproduced the spectrum of the neutral compound almost quantitatively (see Figure S9a). When, however, the electrolysis was conducted at a slower rate and with a gradual, stepwise increase of the applied potential, no ferrocenium formation was observed. Rather, a filming of the working electrode was encountered (see Figure S9b). Chemical oxidation of the nitrate salt of FcNMe3TIPS in a CV cell (0.1 M NBu4PF6 in DCM) using tris(4-bromophenyl)aminium hexachloridoantimonate (magic blue) as the oxidizing agent[67,68] (0.5 or 1 eq., respectively) likewise suggests rapid degradation and polymerization, leading to the deposition of an insulating film on to the electrode surface on repeated scanning (see Figure c). In water as the solvent, oxidized FcNMe3TIPS degrades at an even faster rate. Thus, oxidizing FcNMe3TIPS with dropwise addition of an aqueous solution of cerium ammonium nitrate led to an instantaneous, greenish-blue coloration and then to a rapid discoloration to pale orange with the concomitant formation of a yellow-orange, insoluble precipitate (see Figure S9c of the Supporting Information for UV–vis data).

Scheme offers a possible explanation for these observations. Oxidation to the ferrocenium ion is expected to increase the electrophilicity of the methylene carbon, which links the ferrocene and the adjacent trimethylammonium head group. The latter is now even more readily attacked by external nucleophiles to release NMe3 or may attack a nearby, unoxidized molecule of FcNMe3TIPS, most likely at the more electron-rich TIPS–C≡C-substituted Cp ring (note that ferrocenes are by a factor of ca. 106 more reactive toward electrophiles than benzene). The resulting methylene-bridged diferrocenium cation with one oxidized and one reduced ferrocene unit might then undergo homogeneous charge-transfer with yet another molecule of FcNMe3TIPS, thereby triggering an electrocatalytic process, or follow reactions such as the substitution of the ammonium head group. We note here again that nucleophilic substitution of the NMe3 leaving group of trimethylammoniummethylene-substituted ferrocenes is a standard procedure for preparing Fc–CH2Nu derivatives (Nu = OH, OR, CN, SR, etc.).[36,41,42] Thus, substitution at the trimethylammonium head group offers another way to further modify the surfactant properties of FcNMe3TIPS, and work along these lines is presently being pursued in our laboratories.

Scheme 4

Redox-Triggered Polymerization of FcNMe3TIPS

Conclusions and Outlook

We present the synthesis of 1-triisopropylsilylethynyl-1′-trimethylammoniummethylferrocene (FcNMe3TIPS). FcNMe3TIPS features a trimethylammonium head group and an oleophilic part constituted by the ferrocene nucleus and the attached TIPS-protected ethynyl functionality at the other cyclopentadienide ring. This unusual architecture sets the title compound apart from other ferrocene-based amphiphiles in the literature. FcNMe3TIPS has typical features of a surfactant and shows colloidal behavior similar to lipids. It packs very efficiently at the air–water interface, leading to a very low value of the minimum surface tension (γmin = 28.5 mN/m). In agreement with its packing parameter, it has a high tendency for the formation of vesicles instead of micelles. The critical aggregation concentration was determined by two independent methods. It could be confirmed that aggregates are already present in solution at significantly lower concentrations as required for the formation of a full monolayer at the air–water interface. This behavior also differs from that of classical surfactants.

As an additional advantage, FcNMe3TIPS can be modified in various different ways. We demonstrated that the protective TIPS group is easily cleaved to yield complex 7 with an unprotected ethynyl functionality (see Scheme ). Complex 7 was then used to prepare the heterobimetallic Fe–Pt complexes (8) and (9), where the ethynyl linker connects the ferrocenyl group to a trans-configured Pt(PEt3)2Cl or Pt(PEt3)2I entity. The latter could endow them also with additional catalytic function in addition to their (as-yet unexplored) surfactant properties. Its terminal ethynyl functionality makes 7 also an ideal precursor for the incorporation of other functionalities, for example, via Sonogashira coupling or click chemistry reactions. We also found that the terminal α-position next to the aromatic system of Fc is highly reactive and can be transformed by nucleophilic substitution. As expected, FcNMe3TIPS is reversibly oxidized to the corresponding ferrocenium species at a half-wave potential of 332 mV in CH2Cl2/NBu4PF6. In water, the corresponding redox process is compromised by the strong adsorptive behavior of the ferrocenium species. On a longer time scale, FcNMe3TIPS is chemically reactive with the release of NMe3, which initiates a polymerization reaction. Because the presence of the ammonium group is essential for securing solubility and the function as a surfactant, we aim at modifying this position, for example, by introducing an ethylene spacer or by employing a different, charged head group, for example, a carboxylate, in order to fully exploit the inherent redox activity of such ferrocene-based gemini surfactants.

Experimental Section

Chemicals and Materials

The reactions were performed using standard Schlenk techniques under a N2 atmosphere. Solvents were dried according to standard procedures and stored under argon atmosphere. Water was deionized by Millipore Milli-Q. C6D6, CD2Cl2, and CDCl3 were supplied from Eurisotop. Starting materials for synthesis were purchased from commercial sources unless stated otherwise. Compounds were synthesized according to literature procedures and follow the representative synthesis protocols provided below. FcNMe2Pt(PEt3)2Cl was obtained as reported by Schanze and co-workers.[69] The atom numbering pertinent to the NMR discussion is provided in the Supporting Information together with the corresponding NMR spectra.

Preparation of 1,1′-Dibromoferrocene (FcBr2) (2)

A solution of ferrocene (10 g, 53.75 mmol, 1 equiv) in n-hexane (400 mL) and tetramethylethylenediamine (19 mL, 125.24 mmol, 2.33 equiv) was stirred in a dried 1 L Schlenk flask and cooled to 0 °C. Then, 1.6 M n-BuLi in hexane (72 mL, 125.24 mmol, 2.33 equiv) was added dropwise. The temperature of the suspension was allowed to raise to room temperature overnight. The orange precipitate was filtered, resuspended in diethyl ether (350 mL), and cooled to −78 °C. Then, a solution of 13.5 mL of tetrabromoethane (115.56 mmol, 2.15 equiv) in 80 mL of diethyl ether was added dropwise. The solution was stirred overnight while slowly warming to ambient temperature. The dark red solution was decanted and quenched with 100 mL of distilled water. After solvent removal, the dark orange solid was dissolved in 300 mL of n-hexane, filtered through Celite, and then washed with sat. aq FeCl3 (ca. 3 × 100 mL). The organic phase was extracted with water and dried over MgSO4, and the solvent was removed in vacuo. Pure orange, crystalline FcBr2 was obtained after recrystallization from MeOH in 59% yield (10.89 g, 31.67 mmol). 1H NMR (400 MHz, CDCl3): δ 4.42 (vt, 3JHH = 1.9 Hz, 4H), 4.17 (vt, 3JHH = 1.9 Hz, 4H).

Preparation of 1-Iodo-1′-bromoferrocene (FcBrI) (3)

FcBr2 (10.7 g, 31.12 mmol, 1 equiv) was dissolved in 750 mL of anhydrous tetrahydrofuran (THF), and the solution was cooled to −78 °C. A solution of 2.5 M n-BuLi in n-hexane (12.5 mL, 31.12 mmol, 1 equiv) was added dropwise, and the temperature was maintained at −78 °C for 4 h. Then, a solution of I2 (21.32 g, 84 mmol, 2.7 equiv) in THF (120 mL) was added dropwise. After complete addition, the reaction temperature was stirred with gradual warming to room temperature overnight. Aqueous sodium thiosulphate (20% w/v, 300 mL) was added to the reaction vessel, followed by diethyl ether (100 mL), and the organic layer was separated and subsequently washed with aqueous sodium thiosulphate (3 × 100 mL) and dried over MgSO4, and the solvent was removed in vacuo. The product was isolated in 86% yield (10.42 g, 26.66 mmol). The product was contaminated with some minor impurities, which could not be removed via flash column chromatography. 1H NMR (400 MHz, CDCl3): δ 4.42 (vt, 3JHH = 1.9 Hz, 2H), 4.38 (vt, 3JHH = 1.9 Hz, 2H), 4.22 (vt, 3JHH = 1.9 Hz, 2H), 4.13 (vt, 3JHH = 1.9 Hz, 2H).

Preparation of 1-Triisopropylsilylethynyl-1′-bromoferrocene (FcBrTIPS) (4)

FcBrI (8.21 g, 21 mmol, 1 equiv), CuI (40 mg, 0.21 mmol, 0.01 equiv), PdCl2(PPh3)2 (147.4 mg, 0.21 mmol, 0.01 equiv), and PPh3 (110.2 mg, 0.42 mmol, 0.02 equiv) were dissolved in 50 mL of degassed NEt3/THF (1:1 v/v), 7.1 mL of TIPSA (31.5 mmol, 1.5 equiv) was added, and the reaction vessel was sealed and heated to 60 °C for 60 h. Then, the solvent was removed in vacuo, and the residue was resuspended in hexane and filtered over Celite. After removal of the solvent, the product was obtained following purification by flash column chromatography (PE) as a brown-red oil (5.50 g, 12.35 mmol, 59%). 1H NMR (400 MHz, CDCl3): δ 4.44 (vt, 3JHH = 1.9 Hz, 2H), 4.39 (vt, 3JHH = 1.9 Hz, 2H), 4.23 (vt, 3JHH = 1.9 Hz, 2H), 4.14 (vt, 3JHH = 1.9 Hz, 2H), 1.14–1.12 (m, 21H).

Preparation of 1-Triisopropylsilylethynyl-1′-dimethylaminomethylferrocene (FcNMe2TIPS) (5)

First, 1.92 g of FcBrTIPS (4.3 mmol, 1 equiv) were dissolved in 120 mL of THF, and the solution was cooled to −78 °C. Then, 1.72 mL of a 2.5 M solution of n-BuLi in hexane (4.3 mmol, 1 equiv) was added dropwise. The solution was stirred for further 20 min at −78 °C. Freshly sublimed Eschenmoser salt (0.88 g, 4.73 mmol, 1.1 equiv) was added, and the reaction temperature was kept at −78 °C for an hour. The reaction mixture was stirred overnight while allowing to warm up to room temperature. Next, 100 mL of distilled water and 200 mL of ethyl acetate were added. The organic layer was separated, washed three times with saturated NaCl solution, and dried over MgSO4. The solvent was removed in vacuo, and the residue was purified by column chromatography (PE/NEt3 = 95:5%) yielding 1.18 g of FcNMe2TIPS (2.79 mmol, 65%) as a brown oil. 1H NMR (400 MHz, CDCl3): δ 4.35 (vt, 3JHH = 1.9 Hz, 2H, H-6), 4.18–4.12 (m, 6H, H-9, H-7, H-8), 3.33 (s, 2H, H-11), 2.17 (s, 6H, H-12), 1.14–1.12 (m, 21H, H-1, H-2). 13C NMR (101 MHz, CDCl3): δ 105.56 (s, C-4), 86.88 (s, C-3), 84.87 (s, C-10), 72.35 (s, C-6), 72.19 (s, C-9), 69.85 (s, C-8), 69.03 (s, C-7), 65.85 (s, C-5), 58.39 (s, C-11), 44.76 (s, C-12), 18.75 (s, C-1), 11.30 (s, C-2). ESIMS: M+ (C24H38FeNSi+) = 424.21, M+–NMe3 (C22H31FeSi+) = 379.15. Anal. Calcd for C24H37FeNSi: C, 68.07; H, 8.81; N, 3.31. Found: C, 67.97; H, 9.11; N, 3.80.

Preparation of 1-Triisopropylsilylethynyl-1′-trimethylammoniummethylferrocene Iodide (FcNMe3TIPS) (6)

FcNMe2TIPS (1.18 g, 2.79 mmol, 1 equiv) was dissolved in absolute MeOH (5 mL) and cooled to 0 °C. Then, an excess of MeI (0.5 mL, 8.03 mmol, 2.9 equiv) was added dropwise, and the clear solution was stirred for 1 h. After heating to reflux for 5 min, 500 mL of diethyl ether were added, and the resulting shiny orange precipitate was filtered via cannula and washed with diethyl ether until the washings were colorless. The quaternary FcNMe3TIPS was obtained as the iodide salt in 93% yield (1.47 g, 2.6 mmol). 1H NMR (400 MHz, CDCl3): δ 4.82 (s, 2H, H-11), 4.55–4.53 (m, 4H, H-9, H-7), 4.41 (vt, 2H, 3JHH = 1.9 Hz, H-8), 4.39 (vt, 2H, 3JHH = 1.9 Hz, H-6), 3.31 (s, 9H, H-12), 1.10–1.14 (m, 21H, H-1, H-2). 13C NMR (101 MHz, CDCl3): δ 104.67 (s, C-4), 88.84 (s, C-3), 74.06 (s, C-8), 73.44 (s, C-9), 73.36 (s, C-7), 72.48 (s, C-10), 70.79 (s, C-6), 67.50 (s, C-11), 66.92 (s, C-5), 52.86 (s, C-12), 18.95 (s, C-1), 11.40 (s, C-2). ESIMS: M+ (C25H40FeNSi+) = 438.23, M+–NMe3 (C22H31FeSi+) = 379.15. Anal. Calcd for C25H40FeINSi: C, 53.10; H, 7.13; N, 2.48. Found: C, 53.21; H, 6.93; N, 2.73. IR (powder): 2942, 2863, 2147 cm–1.

Preparation of 1-Ethynyl-1′-dimethylaminomethylferrocene (FcNMe2H) (7)

FcNMe2TIPS (0.300 g, 0.71 mmol, 1 equiv) was dissolved in 40 mL of anhydrous THF, and 1.06 mL (1.06 mmol, 1.5 equiv) of a 1 M solution of tetrabutylammonium fluoride in THF was added dropwise. After the reaction mixture was stirred for 2 h, the solvent was removed in vacuo and the product was purified by column chromatography (PE/EA = 100:0 to 75:25%). The product was isolated in quantitative yield (190 mg, 0.71 mmol). 1H NMR (400 MHz, CDCl3): δ 4.37 (vt, 3JHH = 1.9 Hz, 2H), 4.18–4.14 (m, 6H), 3.29 (s, 2H), 2.74 (s, 1H), 2.17 (s, 6H).

Preparation of FcNMe2Pt(PEt3)2Cl (8)

FcNMe2H (80 mg, 0.3 mmol, 1 equiv) was dissolved in 35 mL of diethylamine and degassed for 15 min. Then, 165.8 mg (0.33 mmol, 1.1 equiv) of trans-Pt(PEt3)2Cl2 were added, and the reaction mixture was heated to reflux for 24 h. Next, 20 mL of CH2Cl2 were added, and the reaction mixture was extracted with water (30 mL) and brine (30 mL). The combined organic phases were dried over MgSO4, and the solvent was removed in vacuo. The crude product was washed with diethylamine (20 mL) at −20 °C to remove the remaining unreacted Pt-precursor complex by precipitation from diethylamine. The solvent was removed under reduced pressure, and the crude product was purified by column chromatography (DCM/MeOH/NEt3 87:10:3%) to give FcNMe2Pt(PEt3)2Cl in 82% yield (180 mg, 0.25 mmol). 1H NMR (400 MHz, C6D6): δ 4.30–4.26 (m, 4H, H-4, H-7), 4.14 (vt, 3JHH = 1.6 Hz, 2H, H-6), 4.00 (vt, 3JHH = 1.6 Hz, 2H, H-5), 3.59 (s, 2H, H-9), 2.22 (s, 6H, H-10), 1.99–1.89 (m, 12H, H-P1), 1.09 (dt, 3JHH = 8.0 Hz, 3JPH = 15.8 Hz, 18H, H-P2). 13C NMR (101 MHz, C6D6): δ 96.82 (t, 3JPC = 2.51 Hz, C-2), 81.75 (s, C-8), 79.41 (t, 2JPC = 14.5 Hz, C-1), 74.52 (s, C-3), 72.24 (s, C-7), 71.31 (s, C-4), 70.30 (s, C-6), 68.33 (s, C-5), 58.39 (s, C-9), 43.84 (s, C-10), 15.10 (t, JPC = 14.5 Hz, with shoulders, C-P1), 8.31 (s, with shoulders, C-P2). 31P NMR (162 MHz, C6D6): δ 14.55 (s, with satellites, JPtP = 2417 Hz). 195Pt NMR (86 MHz, C6D6): δ -4435 (t, JPtP = 2417 Hz).

Preparation of FcNMe3Pt(PEt3)2I (9)

First, 80 mg of FcNMe2Pt(PEt3)2Cl (0.11 mmol, 1 equiv) was dissolved in 5 mL of abs. MeOH and 0.02 mL of MeI (0.32 mmol, 2.9 equiv) were added dropwise. The reaction mixture was stirred at room temperature for 2 h. Then, 150 mL of diethyl ether were added, resulting in a suspension with an orange precipitate. The solution was filtered via cannula, and the orange solid was washed with diethyl ether (3 × 30 mL), dried in vacuo, and FcNMe3Pt(PEt3)2I was obtained as an orange, shiny solid (101 mg, 0.10 mmol, 91%). 1H NMR (600 MHz, C6D6): δ 5.21 (s, 2H, H-9), 4.67 (vt, 2H, 3JHH = 1.8 Hz, H-7), 4.63 (vt, 2H, 3JHH = 1.8 Hz, H-4), 4.54 (vt, 2H, 3JHH = 1.8 Hz, H-5), 4.27 (vt, 2H, 3JHH = 1.8 Hz, H-6), 3.11 (s, 9H, H-10), 2.19–2.14 (m, 12H, H-P1), 1.11 (dt, 3JHH = 8.2 Hz, 3JPH = 15.8 Hz, 18H, H-P2). 13C NMR (151 MHz, C6D6): δ 95.33 (s, with satellites, 2JPtC = 401.06 Hz, C-2), 87.34 (t, 2JPC = 14.5 Hz, with satellites, 1JPtC = 1437.97 Hz, C-1), 74.95 (s, with satellites, 3JPtC = 31.68 Hz, C-3), 73.44 (s, C-6), 73.33 (s, C-7), 73.33 (s, C-8), 71.85 (s, C-4), 70.00 (s, C-5), 66.42 (s, C-9), 52.10 (s, C-10), 17.20 (t, JPC = 17.7 Hz, with shoulders, C-P1), 8.71 (s, with shoulders, C-P2). 31P NMR (162 MHz, C6D6): δ 8.57 (s, with satellites, JPtP = 2337 Hz). 195Pt NMR (86 MHz, C6D6): δ -4823.57 (t, JPtP = 2337 Hz).

Preparation of FcCNTIPS (10)

FcNMe3TIPS (35 mg, 0.062 mmol, 1 equiv) was dissolved in a mixture of absolute acetonitrile/methanol (20:10 mL), and 40.33 mg (0.62 mmol, 10 equiv) of KCN  were added. The reaction mixture was stirred at reflux for 48 h and then cooled to room temperature. The solvent was removed in vacuo, and the resulting brown solid was extracted with diethyl ether (3 × 50 mL). The organic phase was washed with water (3 × 30 mL) and dried over MgSO4, and the solvent was removed under reduced pressure. FcCNTIPS was obtained as a brown solid (17.50 mg, 0.043 mmol, 70%). 1H NMR (400 MHz, CDCl3): δ 4.48 (t, 3JHH = 1.9 Hz, 2H), 4.28–4.24 (m, 4H), 4.21 (t, 3JHH = 1.9 Hz, 2H), 3.49 (s, 2H), 1.15–1.10 (m, 21H).

Ion-Exchange Procedure for Electrochemical Investigations (FcNMe3TIPS_NO3)

First, 500 mg of the iodide salt of FcNMe3TIPS (0.88 mmol) was dissolved in 50 mL of MeOH and flushed through a plug of freshly activated, KNO3-loaded Amberlite IRA-402. This procedure was repeated 10 times, and then the solvent was removed in vacuo, resulting in a yellow solid with white impurities (KNO3). The precipitate was dissolved in dichloromethane and washed two times with 30 mL of distilled water. The organic phase was dried over MgSO4, and the solvent was removed in vacuo. CV measurements confirmed the complete displacement of I– by NO3–. The ion-exchange proceeded quantitatively.

Characterization

NMR experiments were carried out on a Varian Unity Inova 400, a Bruker Avance III DRX 400, or a Bruker Avance DRX 600 spectrometer. 1H and 13C spectra were referenced to the respective solvent signal, whereas 31P and 195Pt spectra were referenced to external standards (85% H3PO4) and saturated K2[PtCl6] in D2O, respectively. Two-dimensional (2D) NMR experiments were used to assign unequivocal signals. Numbering of the nuclei can be seen in the Supporting Information in the respective NMR data. Combustion analysis was performed with an Elementar vario MICRO cube CHN-analyzer from Heraeus. ESIMS data were acquired on a Bruker microtof II system. Cyclic voltammetry was performed in a one-compartment cell with 5–7 mL of DCM or deionized water as the solvent and NBu4PF6 (0.1 M) or KNO3 (0.1 M) as the supporting electrolyte. A platinum electrode (⌀ = 1.1 mm, BASI) was used in DCM and a glassy carbon electrode (⌀ = 3 mm, BASI) in water as the working electrode. A computer-controlled BASi EPSILON potentiostat was used for recording of the voltammograms. A Ag/AgCl wire pseudoreference electrode in DCM and a Ag/AgCl (3 M KCl) reference electrode in water were used in combination with a platinum wire auxiliary electrode. UV–vis spectroelectrochemistry was performed in a self-built OTTLE cell according to the design of Hartl et al.[70] A platinum grid as the working and counter electrode was welded in a polyethylene spacer, incorporated into a Teflon surrounded with electrical connectors in between the CaF2 plates of a liquid IR cell. Next, 0.1 M of NBu4PF6 in DCM was used as the supporting electrolyte. IR/NIR spectra were recorded on an Fourier transform infrared Bruker Tensor II instrument. UV–vis spectroscopy and spectroelectrochemical measurements were performed on a diode-array unit TIDAS by J&M ANALYTIK. In the latter experiments, a WENKING potentiostat POS3 was used. Attenuated total reflection (ATR)-IR spectra were measured on a Perkin Elmer 100 Spectrum Spectrometer equipped with an ATR unit. DLS measurements were done on Malvern Zen5600. Liquid-crystal pictures were performed with an Olympus CX41 light microscope. High-resolution transmission electron microscopy (TEM) observations were done on JEOL JEM-2200FS. For surface tension measurements, Krüss K100 was used. SAXS was acquired on a Bruker Nanostar system equipped with pinhole collimation and Cu Kα radiation. Geometry optimization and orbital calculations were performed using DFT with the TURBOMOLE program package for ab initio electronic structure calculation using the BP86/def2-TZVP level of theory. TURBOMOLE V7.1 2016, a development of the University Karlsruhe and Forschungszentrum Karlsruhe GmbH, 1989-2007, TURBOMOLE GmbH, since 2007; available from http://www.turbomole.com.