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The concept of micelles was first proposed in 1913 by McBain and has rationalized numerous experimental results of the self-aggregation of surfactants. It is generally agreed that the aggregation number (Nagg) for spherical micelles has no exact value and a certain distribution. However, our studies of calixarene surfactants showed that they were monodisperse with a defined Nagg whose values are chosen from 6, 8, 12, 20, and 32. Interestingly, some of these numbers coincide with the face numbers of Platonic solids, thus we named them “Platonic micelles”. The preferred Nagg values were explained in relation to the mathematical Tammes problem: how to obtain the best coverage of a sphere surface with multiple identical circles. The coverage ratio D(N) can be calculated and produces maxima at N=6, 12, 20, and 32, coinciding with the observed Nagg values. We presume that this “Platonic nature” may hold for any spherical micelles when Nagg is sufficiently small.
Surfactants and lipids comprise of hydrophilic polar head groups and hydrophobic tails, commonly long hydrocarbon chains. When these molecules are dispersed in aqueous solutions, the hydrophobic tails tend to avoid unfavorable interactions with polar water, while the head groups favorably interact with water. This consequently leads to the formation of aggregates with a certain size, called “micelles”. The term of micelle was first used by J. W. McBain in 1913 to describe an aggregate of soap molecules and the first model of the spherical micelles (Supplementary Information Figure S1), which is still widely used today, was proposed by G. S. Hartley1. There are numerous practical applications of micelles such as soaps, detergents, and drug delivery carriers and their chemistry and physics are still a major subject in modern science.
As shown in Hartley’s model, the polar headgroups usually form the exterior of the aggregate and the hydrophobic moieties form the interior. Their volumetric balance is the main determinant of the micelle shape. Israelachvili2 introduced a thermodynamic parameter (ae) related to the equilibrium area per molecule at the aggregate interface and proposed a geometrical criterion that needs to be fulfilled for the micelles to take a spherical shape;
where V and h are the volume and length of the surfactant tails, respectively2. The factor of 1/3 is related to the geometrical relations for the volume and surface area of a sphere made up of N surfactants, subject to the constraint that the radius of the sphere R cannot exceed the extended tail length h. We can imagine that a particular number of cones can assemble to form a spherical shape. This concept is called packing parameter principle and has been widely used because it provides an intuitive insight on the aggregation phenomena of micelles. By the same geometrical analogy, the aggregation number of spherical micelles (Nagg) can be expressed by;
Tanford was the first to formulate the thermodynamics of the micelle formation (S11)3. His theory and its improvements4,5, and additionally recent computer simulations6,7 based on these theories are quite consistent with various experimental results for wide range of materials8. It is generally accepted that Nagg gradually changes with the surfactant concentration and other solvent conditions such as the ionic strength and Nagg has a certain distribution. However, we recently observed an interesting phenomenon that seemingly cannot be rationalized within the above framework. In this paper, we overview our experimental results and propose a possible theoretical explanation for this finding.
We have newly synthesized 18 calixarene-based surfactants as presented in Fig. 1a, whose chemical structures and codes are shown in Table S1. These molecules consist of four headgroups and four alkyl tails, and presumably take a conical shape as presented in Fig. 1a. As a surfactant other than the calixarene ones, we used a bacterial lipopeptide: surfactin, which consists of a heptapeptide unit (Glu-Leu-D-LeulVal-Asp-D-Leu-Leu) and a beta-hydroxy fatty acid, obtained from Kaneka Corporation (SF-S04), Japan. Synchrotron small angle X-ray scattering (SAXS) was carried out at BL40 at SPring 8, Japan to determine the molecule shape as well as Nagg. Analytical ultracentrifugation (AUC) and asymmetric flow field-flow fractionation (aFFF) coupled with multi-angle static light scattering (SLS) were used to determined Nagg and dispersity (see the Supplementary Information). The critical micellar concentrations (CMC) were determined and listed in Table S1, which were in the range 0.4–100μM. Nagg did not change when the concentration was less than approximately 50–100×CMC.
A series of calixarene surfactants designated as QACaLn (which has four quaternary amino headgroups and n is the number carbon atoms of one tail, as shown in Fig. 1b) were examined by use of SAXS, SLS, and AUC (see S3). It was clear that these molecules form spherical micelles in water. We plottedNagg against the number of carbons in the alkyl chain (nC) (Fig. 1b). As nC increases from 3 to 7, Nagg increases discretely from 8 to 12, and then to 20. An increase in Nagg is expected from the packing parameter theory, which predicts that Nagg(nC)2. However, we would have expected a continuous rather than a discrete increment. Figure 1d shows the SLS (green) and UV (red) signals of an aFFF fractogram (see S4) for QACaL5. The micelles show a peak at 8.5min, and the LS and UV signals completely overlap. The SLS intensity is proportional to the sample concentration and molecular weight, whereas the UV absorbance depends only on the concentration. Therefore, the overlap of these signals indicates that the molecular weight is constant over the entire peak. The dispersity index, defined as Mw/Mn, is determined to be 1.0, for this sample, where Mn and Mw are the number and weight averaged molecular weights, respectively. The monodispersity of the sample was confirmed with AUC as Mz/Mw=1.0, also indicated by the linearity of the lnC(r) vs. r2 plot (Fig. 1e), where Mz is the z-averaged molecule weight, and r and C(r) are the distance from the rotating center and the concentration at r after reached equilibrium. When nC≥8, the dispersity index becomes larger than 1.0 and the Nagg distribution widens. As reported for PACaLn, which has a primary amine headgroup9, we observed a similar discrete increment of Nagg and monodispersity (Fig. 1c). Here, as nC increases from 3 to 6, Nagg increases from 6 to 12.
We have synthesized several other calixarene derivatives with sugar (GalCaL3), amino acid (CCaL3 and ECaL3)10, amine dendrimer (G1CaL3), choline phosphate (CPCaL3 and CPCaL6)11, and poly(ethylene oxide)(PEGnCaL5) headgroups as summarized in Table S1. Some examples exhibit similar monodispersity and discreteness of Nagg. So far, such monodispersed aggregation numbers that we have encountered are 6, 8, 12, 20, and 32. It is quite surprising that 6, 8, 12, and 20 coincide with the face numbers of Platonic solids, as illustrated in Fig. 1f. Here, Platonic solids are regular, convex polyhedra and only five polyhedra meet these criteria.
We have examined how the discreteness and monodispersity can be maintained when solvent conditions are continuously changed (Fig. 2). Figure 2b shows the pH dependence of SAXS for ECaL3 (glutamic acid head, Fig. 2a) and the exponent ex in I(q)qex at low q is plotted against pH in Fig. 2c, where I(q) and q are the scattering intensity and magnitude of the scattering vector, respectively. The exponent ex at low q is related to the geometrical dimension of scattering objects; ex=0, −1, and −2 indicate finite sizes for all dimensions, rod-like objects, and disk-like objects, respectively12. As shown in Fig. 2b,c, ex=0 was observed at pH<5.4 and pH=10. This indicates that ECaL3 forms micelles of a finite size, and fitting the SAXS data confirmed the formation of spherical micelles in these pH ranges (see S5). In intermediate pH values, ex decreases, reaching ex=−1 at 7<pH<8.5. Intermediate values of ex between −1 and 0 indicate the cylinder is not long enough to gives ex=−1, meaning short cylindrical micelles with various lengths. Aggregation number analysis with SAXS and SLS (see S5) indicated that v Nagg=6 and=12 at pH<5.4 and pH=10, respectively. Furthermore, we confirmed the monodispersity at both conditions. Spherical micelle formation at both acidic and basic conditions and its transition to cylinders can be explained as follows: ECaL3 has four glutamic acids as headgroups which contain both a primary amine and a carboxyl group; i.e., they have an amphoteric nature. Therefore, the headgroups can be charged and thus create repulsive interactions at both acidic and basic conditions, leading to larger ae in these conditions than in neutral ones. The larger ae values favor the formation of spheres and the smaller ones the formation of cylinders, according to Eq. 1, which can explain the sphere to cylinder transition upon pH change. At low pH when the amino groups are charged, the distance from the hydrophobic core surface at which the charge is located is smaller compared to when the carboxyl groups are charged at high pH. Therefore, the electrostatic repulsions will be smaller for the carboxyl case at high pH compared to the amino case at low pH. The result would be a larger aggregation number for the carboxyl case at high pH compared to the amino case at low pH.
Figure 2e shows the SAXS profiles of G1CaL3 (amido-amine head, Fig. 2d) in water/methanol solvents. As the water volume percent () increases, the intensity minimum of the scattering profiles deepens. It should be noted that the position of the minimum does not change. This behavior contrasts strongly with that of other micelle systems (see S6), where shifts continuously towards smaller q with increasing water content, because of the continuous increase in the micellar size. Knowing that G1CaL3 forms monodisperse octamers in water and remains a unimer in methanol, the unchanged means that the water/methanol solutions contain only unimers and octamers and the smeared scattering profiles at lower is owing to the increase of the unimer content. Based on this assumption, the scattering intensity profile [I(q, )] at an intermediate can be expressed as a linear combination of I(q, =0) and I(q, =1), after multiplying by an appropriate coefficient. The solid lines fitted to the experimental data points are calculated values, showing an excellent agreement, thus supporting our assumption. From the coefficient used, we can estimate the weight fraction ratio of the octamer to the unimer (w.f.) (see S7) and the obtained w.f. is plotted against in Fig. 2f. The increase of water content sigmoidally changes w.f. from 0 to 1 around =50 According to the conventional micellization theory, the distribution of Nagg becomes broader near the CMC due to larger thermal fluctuations2, which is seemingly not the case in the present system.
Electrostatic repulsions are not necessary for the creation of discreteness and monodispersity. When we attached long polyethylene glycol chains to calixarene (PEG550CaL5 and PEG1kCaL5), they formed dodecamers and octamers, in accordance with the volume of the PEG head group as shown in Fig. 2g–i. The monodispersity of this system is confirmed with aFFF (S8). One may also suggest that these features are characteristically observed for the above mentioned calixarene systems because of the rigidity and trapezoid-like body of the calixarene building block. However, there have been a few reports in the literature showing similar discreteness and monodispersity for micelles made from surfactants of different building blocks. Khelfallah et al.13 prepared a water-soluble amphiphilic cylindrical brush-coil block copolymer. They observed that their polymer formed micelles consisting of 4 or 5 block copolymers on average and the size distribution was quite narrow. Böttcher et al.14,15 synthesized an amphiphilic fullerene derivative and the molecules showed monodispersity comparable to our systems, and they named their systems shape persistence micelles. They observed their micelles with cryo-electron transmission microscopy and reconstructed the 3D-image. Although electron microscopy does not provide absolute molecular weight, their tomographic image suggested that six molecules of the fullerene derivative make up one micelle.
Surfactin is a bacterial lipopeptide containing large negatively charged cyclic peptides with two carboxyl groups originating from aspartate and glutamate (Fig. 3a)16. When we determined Nagg as a function of CNaCl with AUC (Fig. 3b,c), Nagg changed from 12 and 20 as CNaCl increased. The similar salt concentration dependence of Nagg was observed by another group with small angle neutron scattering17. We confirmed that no peptide conformational change was induced by NaCl using circular dichroism (S9). The SAXS profiles showed a sharp intensity minimum, similar to the calixarene derivatives (S9) and the monodispersity was confirmed with AUC (Fig. 3b). The present surfactin results further confirm that calixarene derivatives are not only the case to show monodispersity with a Nagg chosen from Platonic solid face numbers. It would have been better to demonstrate the existence of “Platonic micelles” with conventional surfactants such as SDS and DTAC. However, these surfactants have rather large Nagg making it experimentally difficult to determine Nagg with accuracy better than ±1 owing to an inevitable error of at least 5%. In another word, for example, we may not be able to distinguish 48 and 49, (although we will discuss later, where Nagg=48 may be a possible configuration of the platonic micelles, but Nagg=49 is not).
There have been no reports for such discreteness and monodispersity in conventional micelles. Here, it should be noted that the classical micellar thermodynamics shows that the dispersity in Nagg can become quite narrow when the hydrophobic interfacial energy is large enough18. In this case, it can be also shown that Nagg becomes almost independent of surfactant concentration. Therefore, the discreteness in Nagg is the most intriguing and peculiar feature of the present system. Hereinafter, we will focus on this discreteness. Generally, normal micelles have larger Nagg than the present systems. Smaller Nagg mean larger ae according to Eq. 2. If ae is large and Nagg is small, the way in which the hydrophobic tails are covered to achieve the minimum free energy may differ from the systems with a large Nagg. This issue may be related to the mathematical problem of how to efficiently cover the surface of a sphere with multiple spherical caps of equal radius. In geometry this is called the “best packing on a sphere” or Tammes problem19,20,21 (see S10). For example, as illustrated in Fig. 4 (right hand), we can have the maximum coverage with three spherical caps when the center of each cap is located on the vertices of an equilateral triangle touching the sphere. In this case, the coverage density D(N) is 0.75. For 12 caps (left), we can have a larger coverage: D(N)=0.879 and the centers of the caps have the same configuration as the vertices of a regular icosahedron. Here, D(N) is defined as the ratio of the sum of the cap areas to that of the sphere surface, as illustrated in the bottom of Fig. 4. It should be noted that D(N) is not a simple monotonic function of N. Figure 5 plots D(N) against the number of caps N. For large N, D(N) is almost constant at 0.82–0.83. On the other hand, for small N, larger D(N) values are obtained at certain numbers such as N=6, 12, and 20. It is surprising that these numbers coincide with our observed values of Nagg. On analogy, it can be reasonably assumed that there are certain numbers of molecules that can more efficiently cover spherical micelles than other numbers (i.e., more decrease in the interfacial free energy originated from unfavorable contact water and the hydrophobic tails). One may think that real molecules do not behave like rigid spherical caps, but the hard-core potential (i.e., Tammes problem) is not a necessary condition for an oscillating D(N) pattern. A similar simulation with the Coulomb potential exhibits local maximums in the same Ns with the Tammes problem (S10). Therefore we can presume that Nagg=6, 12, and 20 are more likely to be encountered in real micelles. The monodispersity can be explained in the same framework. When a certain Nagg is strongly favorable, most aggregates will consist of this number of molecules and the system becomes monodisperse.
Figure 5 summarizes all the monodisperse systems that we observed so far as well as some examples from the literatures. CPCaL6, which has zwitterion choline phosphate headgroups (Table S1), has Nagg=32. It is notable that there is a local maximum of D(N) at N=32 and its configuration is the same as carbon-60. N=2 gives D(N)=1.0 because two hemispheres can completely cover a sphere. The molecular configuration cannot be identical to hemispheres, but we have two examples for Nagg=2. One is a dimer of bile acids22, and the other is a pillararene based amphiphilic molecule23. We have several examples at Nagg=8, but the coverage D(N) at N=8 is not so large. Although it is much larger than 7, it is slightly smaller than 9. The N=8 configuration is not a regular hexahedron but an augmented triangular prism (i.e, a skewed cube). The symmetry of this configuration is still quite high and this may explain why we encounter Nagg=8. By the way, it is not clear at the moment how large Nagg must be to consider D(Nagg) to be constant. This may depend on the chemical structure. Here, we would like to point out that there are maxima of D(N) at N=32 and 48 and these numbers are normally observed Nagg for conventional surfactants such as alkyl sulfates.
For PACaL3 (Fig. 1c, Nagg=6), we constructed a rigid body model of the hexameric micelle with the program SASREF24 which shows good agreement with the experimental SAXS data (Fig. S12-1). Using this model as a guide, we designed a starting model for molecular dynamics (MD) simulations. SAXS profile was calculated from each MD model and the similarity Jaccard index (Jind.) between the experimental and calculated profiles was also determined. While the total energy oscillated around a constant value (Fig. S12-2), Jind.fluctuated considerably. Probably, our MD simulations overestimate the thermal fluctuations of the atomic positions.
For the models with the largest Jind. (i.e., better agreement between SAXS experiment, Fig. 6a), we evaluated the centers (green) of the four oxygen atoms (red) of each PACaL3 molecule and constructed a polyhedron by connecting thus obtained six centers as shown in Fig. 6b. Interestingly, the obtained six polyhedra are quite similar to the regular octahedron. On the other hand, for the models with the smallest Jind., the positions of the oxygen centers differ significantly from the regular octahedron (Fig. 6c). Consequently, when the micelle conformation determined by MD is in better agreement with the data, each PACaL3 molecule aligns in the same direction from the center to a vertex of the regular octahedron. This implies that the interface of PACaL3 takes the same spatial arrangement with that predicted by the Tammes problem.
The present results indicate that a suitable combination of surfactant tail length, head volume, and sufficiently small Nagg, as well as some rigidity of the building block is necessary to produce the “Platonic micelles”, which are monodisperse with a defined Nagg whose values are chosen from 6, 8, 12, and 32. The specific Nagg values is related to the mathematical Tammes problem, and because of the generality of this mathematical model, we presume that “the Platonic nature” may hold for any spherical micelles when Nagg is sufficiently small.
How to cite this article: Fujii, S. et al. Platonic Micelles: Monodisperse Micelles with Discrete Aggregation Numbers Corresponding to Regular Polyhedra. Sci. Rep. 7, 44494; doi: 10.1038/srep44494 (2017).
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This work is supported by a JST/CREST program and all SAXS measurements were carried out at SPring-8 BL-40B2 [2016A1242, 2015A1782, 2014A1268, 2014A1268, 2013B1203]. This work was supported by the Photon and Quantum Basic Research Coordinated Development Program from the Ministry of Education, Culture, Sports, Science and Technology, Japan. We thank Profs. Shinohara and Amemiya (The University of Tokyo) for the helpful discussions on the best packing on a sphere surface.
The authors declare no competing financial interests.
Author Contributions S.F., S.Y., S.M., R.M., K.Y., G.K., and E.T. carried out the experiments, analyzed and discussed the data. O.T. and E.M. performed computer chemistry. N.O. and H.S. helped for the SAXS measurements. I.A., Y.S., N.Y., and K.S. analyzed and discussed the data. S.F., S.Y., and K.S.wrote the main manuscript text. All authors reviewed the manuscript.