Birth of a class of nanomaterial

Nearly 30 years ago, a simple chemical principle was reported that enabled the synthesis of a plethora of porous materials — some of which might enable applications ranging from biomedicine to petrochemical processing.
Ryong Ryoo is at the Center for Nanomaterials and Chemical Reactions, Institute for Basic Science, Daejeon 34141, South Korea, and in the Department of Chemistry, KAIST, Daejeon.

Search for this author in:

In 1992, Kresge et al.1 reported a breakthrough in materials science. They described multimolecular templates that guide the assembly of ordered mesoporous molecular sieves — materials that contain uniform, regularly arranged pores with mesoscopic diameters (between 2 and 50 nanometres). Their findings triggered an explosion of research into mesoporous materials, which have since been intensively studied for applications as diverse as catalysis, molecular adsorption, drug delivery and molecular separations using membranes.

When Kresge and colleagues published their work, materials known as zeolites — crystalline aluminosilicate compounds with uniform pores usually less than 2 nm in diameter — had long been used as catalysts in petroleum refining and for molecular separations. However, large molecules, such as those found in the heavy fractions of crude oil, were unable to diffuse through the small pores of these molecular sieves, and so could not be processed efficiently. There had been many attempts to obtain zeolite-like materials with enlarged pores and ordered structures, but the large-pore materials commonly available at that time all had a broad distribution of pore diameters, making them unsuitable for many applications.

In 1990, it was reported2 that the spaces between the layers of a silicate material called kanemite could be expanded by adding organic molecules containing long hydrocarbon chains to a suspension of kanemite powder in water. This process could generate pores of up to 4 nm in diameter, but worked only with kanemite.

Enter Kresge and colleagues, whose method for making mesoporous materials began with the formation of layers of silica, a few nanometres thick, in between the surfaces of cylindrical supramolecular assemblies called micelles (Fig. 1). The micelles consisted of numerous detergent-like molecules, known as surfactants, that were packed together to form a liquid-crystal structure reminiscent of a honeycomb. Once silica layers had formed between the micelles, the researchers heated the resulting material in air to remove the surfactant, thereby producing a silica product that retained a honeycomb-like array of nanometre-scale pores. The researchers named their material Mobil Composition of Matter No. 41 (MCM-41), after the oil company that they worked for.

Figure 1 | Synthesis of the porous solid MCM-41. In 1992, Kresge et al.1 reported the use of cylindrical molecular aggregates, called micelles, as templates for the synthesis of porous materials. a, In the first step, they formed a silicate layer between micelles stacked in a hexagonal array; the individual molecules in the micelles are shown as blue spheres with ‘tails’ attached. The authors then destroyed the micelles using heat, thereby producing the porous silicate MCM-41. b, This micrograph1 of MCM-41 reveals its uniform, honeycomb-like porous structure. Kresge and colleagues’ template-based strategy has since enabled the synthesis of a wide range of potentially useful materials that contain ordered pores of 2–50 nanometres in diameter (mesopores). Scale bar, 100 ångströms.

The most impressive feature of Kresge and colleagues’ strategy was that the diameter, shape and connectivity of the pores could, in principle, be controlled by manipulating the structure and size of the surfactant molecules. The authors demonstrated only a few examples of this: they showed that the pore diameter could be controlled within a narrow range of about 3–10 nm. Nevertheless, their approach was later shown to be applicable to the full range of mesopore sizes3.

Researchers in the field initially regarded Kresge and colleagues’ work as simply extending the pore sizes of the existing family of molecular sieves. However, it soon became apparent that the surfactant-based strategy could be used to synthesize many types of ordered mesoporous material, including ones made from metal oxides4, organic polymers5 and even transition metals6. Having the ability to make a variety of mesoporous materials that contain highly ordered arrangements of pores opened up many avenues of research for nanoscience.

A key development in 1998 was the use of polymeric surfactants7, which increased the size of mesopores that could be made to 30 nm. Polymeric surfactants used in the synthesis of such large-pored materials, as well as other organic surfactants (including the one used to make MCM-41) are now classified as soft templates, which reflects the somewhat deformable nature of the micelles that act as the mould. An advantage of using soft templates is that mesoporous materials can be made in solution at relatively low temperatures. Moreover, the porous structure of the resulting material can easily be controlled by making simple modifications to the template molecules.

Another breakthrough, reported in 1999, was the discovery of hard templating (also known as nanocasting)8,9. In this process, mesoporous materials are fabricated from precursor molecules using another solid mesoporous material as a mould, in a manner analogous to the casting of concrete pipes or bricks. Nanocasting has two somewhat cumbersome requirements: the precursors must infiltrate the pores of the mould uniformly, without accumulating on the external surface; and the precursors must convert completely into the desired product. The method does, however, work particularly well when high temperatures (of the order of 500 °C or more) are needed to synthesize a mesoporous material. This contrasts with the use of surfactant-based soft templates, which typically decompose at temperatures above 200 °C.

Nanocasting was first used to make ordered mesoporous carbon8, but has since been developed as a general approach for synthesizing nanowires and nanoporous materials of various compositions, including metal oxides, organic polymers and metals10. Mesoporous carbons have garnered much interest because of their high electrical conductivity11, and because they can accommodate a large volume of guest atoms, molecules or particles inside the mesopores. For this reason, mesoporous carbons are considered to be particularly attractive candidates for electrode materials in chemical sensors12, supercapacitors13 and high-performance batteries14.

Mesoporous materials are also gaining attention for biomedical applications such as drug or gene delivery15,16. Mesoporous silicas, in particular, can be synthesized in various shapes and sizes, are often biocompatible and spontaneously degrade in human tissues — a property that could be used to release drugs trapped in the silica. Moreover, the ability to accurately control the diameters of mesopores in silica is expected to provide tremendous advantages in biomedical applications, because the pore sizes directly affect the loading and release kinetics of drugs in delivery systems.

The main uses envisaged for mesoporous materials include as adsorbents in industrial processes for separating chemicals, and as catalysts in petrochemical refinery processes. Indeed, the original motivation for Kresge and colleagues’ MCM-41 research was to synthesize catalytic materials for petroleum refining17. But although MCM-41 had sufficiently large pores for this purpose, its glass-like amorphous framework showed poor catalytic activity.

Ever since, enormous efforts have been made to synthesize mesoporous materials that contain crystalline, microporous, zeolite-like frameworks, which exhibit high catalytic performance. A breakthrough was made ten years ago, with the report of a specially designed surfactant molecule that enables the synthesis of such materials18,19. The catalytic properties of the resulting mesoporous zeolites have not been fully explored for industrial processes, because the required surfactant is costly and not yet commercially available. However, I expect that mesoporous zeolites will trigger the next explosion of research in this field, by opening up many opportunities for catalytic applications.

Nature 575, 40-41 (2019)

doi: 10.1038/d41586-019-02835-7


  1. 1.

    Kresge, C. T., Leonowicz, M. E., Roth, W. J., Vartuli, J. C. & Beck, J. S. Nature 359, 710–712 (1992).

  2. 2.

    Yanagisawa, T., Shimizu, T., Kuroda, K. & Kato, C. Bull. Chem. Soc. Jpn 63, 988–992 (1990).

  3. 3.

    Cao, L., Man, T. & Kruk, M. Chem. Mater. 21, 1144–1153 (2009).

  4. 4.

    Stein, A. et al. Chem. Mater. 7, 304–313 (1995).

  5. 5.

    Zhang, F. et al. J. Am. Chem. Soc. 127, 13508–13509 (2005).

  6. 6.

    Attard, G. S. et al. Angew. Chem. 109, 1372–1374 (1997).

  7. 7.

    Zhao, D. et al. Science 279, 548–552 (1998).

  8. 8.

    Ryoo, R., Joo, S. H. & Jun, S. J. Phys. Chem. B 103, 7743–7746 (1999).

  9. 9.

    Joo, S. H. et al. Nature 412, 169–172 (2001).

  10. 10.

    Yang, H. & Zhao, D. J. Mater. Chem. 15, 1217–1231 (2005).

  11. 11.

    Liang, C., Li, Z. & Dai, S. Angew. Chem. Int. Edn 47, 3696–3717 (2008).

  12. 12.

    Nengqin, J., Wang, Z., Yang, G., Shen, H. & Zhu, L. Electrochem. Commun. 9, 233–238 (2007).

  13. 13.

    Li, W. et al. Carbon 45, 1757–1763 (2007).

  14. 14.

    Ji, X., Lee, K. T. & Nazar, L. F. Nature Mater. 8, 500–506 (2009).

  15. 15.

    Vallet-Regi, M., Balas, F. & Arcos, D. Angew. Chem. Int. Edn 46, 7548–7558 (2007).

  16. 16.

    Han, Y., Stucky, G. D. & Butler, A. J. Am. Chem. Soc. 121, 9897–9898 (1999).

  17. 17.

    Kresge, C. T. & Roth, W. J. Chem. Soc. Rev. 42, 3663–3670 (2013).

  18. 18.

    Choi, M. et al. Nature 461, 246–249 (2009).

  19. 19.

    Na, K. et al. Science 333, 328–332 (2011).

Download references

Nature Briefing

An essential round-up of science news, opinion and analysis, delivered to your inbox every weekday.