Skip to main content

Thank you for visiting nature.com. You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

A novel liquid organic hydrogen carrier system based on catalytic peptide formation and hydrogenation

Abstract

Hydrogen is an efficient green fuel, but its low energy density when stored under high pressure or cryogenically, and safety issues, presents significant disadvantages; hence finding efficient and safe hydrogen carriers is a major challenge. Of special interest are liquid organic hydrogen carriers (LOHCs), which can be readily loaded and unloaded with considerable amounts of hydrogen. However, disadvantages include high hydrogen pressure requirements, high reaction temperatures for both hydrogenation and dehydrogenation steps, which require different catalysts, and high LOHC cost. Here we present a readily reversible LOHC system based on catalytic peptide formation and hydrogenation, using an inexpensive, safe and abundant organic compound with high potential capacity to store and release hydrogen, applying the same catalyst for loading and unloading hydrogen under relatively mild conditions. Mechanistic insight of the catalytic reaction is provided. We believe that these findings may lead to the development of an inexpensive, safe and clean liquid hydrogen carrier system.

Introduction

Containing the highest energy density per unit mass and producing only water upon combustion, hydrogen is a most efficient and environmentally friendly fuel1,2,3,4. In fact, the concept of a ‘hydrogen economy’ was suggested as early as 1972 (ref. 5). However, the low energy density of hydrogen stored in high-pressure tanks or as a liquid in cryogenic tanks, and potential safety issues, presents significant disadvantages. Thus, finding suitable hydrogen carriers is highly desirable1,2,3,4,6,7. For decades, scientists have searched for suitable hydrogen storage materials, such as main-group hydrides, metal organic frameworks, metal clusters and nanostructured materials. Unfortunately, all these systems suffer from significant limitations1,2,3,4.

Recently, organic compounds, such as formic acid8, methanol–water9,10,11,12, formaldehyde–water13, alcohols14 and carbohydrates15, were intensively studied as potential hydrogen storage systems. Of special interest are ‘liquid organic hydrogen carriers’ (LOHCs), which can be readily dehydrogenated as well as regenerated, with considerable hydrogen capacity and that might be used for transportation and stationary purposes7,16,17,18,19,20.

An attractive LOHC of potential commercial interest has been N-ethylcarbazole16,17,18, which upon hydrogenation to perhydro-N-ethylcarbazole consumes 6 equivalents (equiv.) of H2, resulting in a hydrogen storage capacity as high as 5.8 wt%. However, disadvantages of this system include the requirement of high H2 pressure for the hydrogenation step, and high reaction temperature for both the hydrogenation and dehydrogenation steps, for which different catalysts are required17,18. Two other recent examples of LOHCs are 2-methyl-1,2,3,4-tetrahydroquinoline and 2,6-dimethyldecahydro-1,5-naphthyridine, which can be reversibly dehydrogenated to 2-methylquinoline and 2,6-dimethyl-1,5-naphthyridine, respectively, catalysed by Ir complexes. However, these systems suffer from very high catalyst loading (5 mol%), high cost of iridium, relatively expensive liquids and low hydrogen storage capacity of 2-methyl-1,2,3,4-tetrahydroquinoline19,20.

Clearly, discovery of LOHC systems based on inexpensive and abundant organic compounds with high capacity to store and release hydrogen, ideally using the same catalyst for both loading and unloading hydrogen under relatively mild conditions, and compatible with existing infrastructure for transport and refuelling, is a major challenge.

Here we report a promising LOHC system, based on the inexpensive, abundant 2-aminoethanol (AE), that is catalytically converted to a cyclic dipeptide with formation of hydrogen gas by use of a ruthenium pincer catalyst; peptide hydrogenation, using the same catalyst, regenerates AE. Mechanistic information regarding this conceptually new LOHC system is provided.

Results

Use of AE as LOHC

We reported the PNN ruthenium pincer complexes 14 (Fig. 1a) that efficiently catalyse several C–O and C–N bond forming dehydrogenative coupling reactions, giving pure hydrogen as the sole byproduct21,22,23,24,25, and also the reverse hydrogenation reactions22,26. For example, the dearomatized catalyst 2 directly produces amides from alcohols and amines with the liberation of H2 (ref. 24). Complex 2 can be obtained in situ by the deprotonation of complex 1 with a base. The reverse reaction, hydrogenation of amides to form alcohols and amines, was also achieved under mild hydrogen pressure using the same catalyst (Fig. 1b; ref. 26). These two reactions suggest the potential for loading and unloading H2 using amines and alcohols. A particularly attractive compound is AE; as an amine and an alcohol, one molecule of AE will release two molecules of H2 if piperazine-2,5-dione (glycine anhydride, GA) can be obtained (Fig. 1c), resulting in high potential hydrogen storage capacity of 6.56 wt%. In addition, since it is industrially produced in large amounts (for CO2 scrubbing)27, AE is very inexpensive and readily available.

Figure 1: Dehydrogenative amidation reactions catalysed by PNN ruthenium pincer complexes.
figure1

(a) Complexes 15, (b) reversible dehydrogenative cross-coupling of amines and alcohols to produce amides, (c) unknown dehydrogenation of AE to produce GA and H2, and (d) formation of cyclic dipeptides (1) and oligopeptides (2) from β-aminoalcohols.

Hydrogen generation experiments

We recently reported that aminoalcohols can undergo dehydrogenative coupling to form cyclic dipeptides (diketopiperazines) and/or oligopeptides (Fig. 1d), depending on the substituent R25; in case of R=Me ((S)-2-aminopropan-1-ol), linear oligopeptides are formed, while with larger substituents diketopiperazines are the major products. Density functional theory (DFT) calculations that we have performed show that conversion of AE to GA or to linear oligopeptides are both thermodynamically favourable processes, but the latter is thermodynamically more favoured. For the reaction in Fig. 1c, the calculated Gibbs free energy (ΔG298) is −6.08 kcal mol−1; for reaction (2) in Fig. 1d (R=H), ΔG298 is −10.17 kcal mol−1 (n=3), −18.18 kcal mol−1 (n=6) and −40.19 kcal mol−1 (n=11; see Supplementary Fig. 1, Supplementary Tables 1 and 2, and Supplementary Discussion for full computational details). However, formation of linear oligopeptides as the major products is less beneficial since this lowers the hydrogen storage capacity of AE. On the other hand, the hydrogen storage capacity of linear peptides can also be considerable. For example, in Fig. 1d (R=H), reaction (2), the hydrogen storage capacity for n=6 is 5.46% as compared with 6.56% for AE. Thus, the unknown generation of GA and hydrogen from AE is an important challenge, as is the unknown hydrogenation of GA; hydrogenation of diketopiperazines was never reported, under any conditions, be it under homogeneous or heterogeneous catalysis or any pressure.

Initially, 10 mmol of AE was heated at 135 °C under argon for 12 h in the absence of solvent with 0.05 mol% of 1 and 0.06 mol% of KOtBu (for the in situ generation of the active catalyst 2), resulting in no product formation (Table 1, entry 1). However, using 10 mmol of AE and 0.5 mol% of catalyst 1 with no solvent resulted in 48% conversion to mostly linear peptides, and 25% yield of H2 (entry 2). Adding 0.5 ml dioxane as a solvent to 1 mmol of AE using catalyst loading of 0.5 mol% resulted in 57% conversion of AE to linear peptides as the major products, as observed by nuclear magnetic resonance (NMR) spectroscopy and mass spectrometry (entry 3). Significantly, using 2 ml dioxane as solvent and 0.5 mol% of catalyst 1, 68% conversion was observed, forming GA in 31% yield, the rest being linear peptides (entry 4). Increasing the volume of dioxane led to improvement in both the yield of GA and the amount of linear products (entries 4–6). However, using >4 ml dioxane was not beneficial (entries 10 and 11). Use of the bipyridine-based pincer complexes 3 and 4 resulted in much lower conversion of AE (entries 7 and 8).

Table 1 Selected results of optimization studies for dehydrogenation of 2-aminoethanol.

Next, we used the PNN-H complex 5 (ref. 28), bearing an N(H)(tBu) amine group instead of the NEt2 group in 1. It was hoped that the presence of an NH group might allow for metal–ligand cooperation via the well-known Ru-amino/Ru-amido sequence29 in addition to metal–ligand cooperation via aromatization–dearomatization of the pincer ligand22,23,24,25,26. However, use of 1.2 equiv. of base (relative to 5) resulted in similar conversion of AE and lower yield of GA (entry 9). Importantly, increasing the base loading resulted in much higher catalytic efficiency. Thus, using 0.5 mol% of 5 and 1.2 mol% of KOtBu (2.4 equiv. relative to 5) resulted in 85% conversion of AE and 60% yield of GA (entry 14) with formation of 37 ml of H2, corresponding to 77% yield of hydrogen based on the reaction of Fig. 1c. Two equivalents of base relative to 5 likely lead to deprotonation of both the amine group and the benzylic arm (Supplementary Note 1)28. Higher base loadings (entries 15 and 16) and lower temperatures (entries 17 and 18) led to lower GA yields. Increased base loading also led to lower yields of GA when using catalyst 1 (c.f. entries 6 and 19). The dehydrogenation reaction was also tried in a large scale of 20 mmol under the conditions of entry 14, of which give similar results, namely 89% conversion of AE, 55% yield of GA and 74% of H2 (710 ml; entry 20).

Using mixtures of dioxane with polar or nonpolar solvents, including diglyme, dimethylformamide, valeronitrile, dimethylacetamide, N-methylmorpholine and toluene resulted in lower catalytic efficiencies (Supplementary Table 3). Using no solvent or a very small amount of solvent also resulted in lower efficiency of the dehydrogenative coupling reaction, although substantial dehydrogenation was still observed (Supplementary Table 4 and Supplementary Note 2). For example, heating a mixture of only 0.1 ml dimethyl sulfoxide solvent and 10 mmol AE (0.611 ml) with 0.5 mol% catalyst 1 and 0.6 mol% KOtBu at 170 °C for 12 h resulted in 71% conversion of AE, mostly to linear oligopeptides, and 39% yield of H2 (55% relative to converted AE based on the reaction in Fig. 1c and Supplementary Table 4, entry 8).

Hydrogenation experiments

Catalysts 1 and 5 were tested for the hydrogenation of GA, which is unprecedented for any diketopiperazine. No product was obtained under 10 bar of H2 in tetrahydrofuran (THF) using 1 mol% catalyst at 110 °C (Table 2, entries 1 and 2). Applying 50 bar of H2, 2 mol% of catalyst 1 and 2.4 mol% KOtBu in dioxane at 110 °C resulted in quantitative yield of the linear amide 2-amino-N-(2-hydroxyethyl)acetamide (AA; entry 3; ref. 30). Using more base improved the reaction significantly; 61% yield of AE and 34% yield of AA were produced using 4.8 mol% KOtBu and 2 mol% catalyst 1 (entry 4). Importantly, complex 5 was catalytically much more active than 1 and nearly 100% yield of the desired AE was obtained, even when only 0.5 mol% 5 and less solvent were used (entries 5 and 6). However, lower H2 pressure (20 bar) was ineffective (entry 7). The mixed products of GA and linear peptides produced by the dehydrogenative reaction (under conditions of Table 1, entry 14) were also hydrogenated by catalyst 5, leading to 85 wt% yield of AE under 50 bar of H2 (entry 8). Thus, formation of linear peptides does not pose a significant problem regarding regeneration of AE. Higher pressure of H2 was not beneficial (entry 9). A larger amount of GA (5 mmol) was also hydrogenated successfully under 70 bar of H2 in a shorter time (12 h) and less solvent (5 ml dioxane for 5 mmol GA), resulting in full conversion of GA, 96% yield of AE and 4% yield of AA (entry 10).

Table 2 Selected optimization results for the hydrogenation of glycine anhydride.

Repetitive reversal reactions

Repetitive cycles of the dehydrogenation–hydrogenation reactions were also tried without adding new catalyst (Table 3, see Supplementary Methods for procedure details). The cycles began with dehydrogenation, using 1 mol% catalyst 5, 2.4 mol% KOtBu, 1 mmol 2-AE and 4.5 ml dioxane (for an example of applying 0.5 mol% catalyst, see Supplementary Methods and Supplementary Table 5 for details). A catalytic amount of KOtBu (2.4 equiv. relative to complex 5) was added every time after the former reaction, to protect the catalyst from trace amount of water, which may be taken into the system during the course of transfer (catalysed by PNN ruthenium pincer complexes, water and alcohol can produce a carboxylic acid31, which can poison the catalyst in the absence of base). After the first dehydrogenation reaction, of which 86% conversion of AE was achieved, the crude reaction mixture was transferred to a 20-ml Parr apparatus under N2 atmosphere. The Parr apparatus was then filled with H2 and the hydrogenation reaction was performed. Without isolation, the catalytic activity of the system was higher as compared with Table 2, entry 9 and 97% of AE (based on the amount of AE used in the first dehydrogenation reaction) was observed. Following this, the second dehydrogenation step resulted in 79% conversion of AE, while the second hydrogenation step provided 90% of AE. The results of the third cycle were also good, even after using the catalyst for six times, 81% of AE was still observed at the end of the third hydrogenation step.

Table 3 Repetitive cycles of the dehydrogenation–hydrogenation reactions.

Mechanistic experiments

To gain mechanistic understanding, the reaction of the dearomatized complex 2 with AE was studied by NMR spectroscopy (Supplementary Note 3). Addition of 1.5 equiv. of AE to a C6D6 solution of 2 at room temperature (r.t.) rapidly afforded nearly quantitatively the aromatic alkoxo species 6 (Fig. 2), which exhibits a hydride signal (d, −14.22 p.p.m., JPH=18.9 Hz) in 1H NMR and a singlet at 106 p.p.m. in 31P{1H} NMR. The signals of the two NH2 protons appear at very different chemical shifts in 1H NMR (4.58 and 2.83 ppm) as previously observed for related complexes29, while the two methyl groups of NEt2 exhibit a single triplet (6 H, 0.86 p.p.m., JHH=7.1 Hz); both these observations indicate coordination of the NH2 group of AE and decoordination of the NEt2 ‘arm’. Complex 6 is stable below −30 °C and slowly decomposes at r.t. to the known trans-dihydride complex 7 (ref. 23) and to a new species (8). Complex 7 is likely formed by hydride elimination from complex 6 (Fig. 2). Complex 8 exhibits a singlet at 102 p.p.m. in 31P{1H} NMR and a hydride signal at −13.16 p.p.m. (d, JPH=23.2 Hz) in 1H NMR. Crystals of 8 suitable for X-ray analysis were obtained by pentane diffusion into a concentrated benzene solution of 6. Complex 8 has a distorted octahedral geometry around the Ru(II) centre (Fig. 3), with the phosphorus atom coordinated trans to the nitrogen atom of the amide group and the hydride located trans to the NH2 group. The two nitrogen atoms of the N–C–C–N backbone form a five-membered chelate. The C–C bond lengths (C(2)–C(3) 1.388(5), C(3)–C(4) 1.391(5) Å) indicate that complex 8 is aromatized (Fig. 3), consistent with the NMR data. The amide backbone is formed by dehydrogenative coupling of two molecules of AE, illustrating highly selective amide rather than ester formation.

Figure 2: Observed path from complex 2 to complexes 6, 7 and 8.
figure2

Figure 3: X-ray structure of complex 8.
figure3

Hydrogen atoms (except hydride and the hydrogen atoms on C1) are omitted for clarity. tBu and Et groups are presented as wireframe (see Supplementary Fig. 2 for a different perspective). Selected bond lengths (Å) and angles (°): Ru(1)-C(20) 1.809(3), Ru(1)-N(4) 2.147(2), Ru(1)-N(3) 2.232(3), Ru(1)-N(1) 2.248(3), Ru(1)-P(1) 2.2733(8), Ru(1)-H(1) 1.7275, C(1)-C(2) 1.506(4), C(6)-C(7) 1.510(4), C(22)-O(2) 1.273(4), C(24)-O(3) 1.414(4); C(20)-Ru(1)-N(4) 90.33(11), C(20)-Ru(1)-N(3) 100.93(13), N(4)-Ru(1)-N(3) 75.75(9), C(20)-Ru(1)-N(1) 174.84(12), N(4)-Ru(1)-N(1) 94.33(9), N(3)-Ru(1)-N(1) 82.39(10), N(4)-Ru(1)-P(1) 172.46(7), N(3)-Ru(1)-P(1) 98.22(7), N(1)-Ru(1)-P(1) 80.23(7).

An NMR study of the reaction of catalyst 2 with 10 equiv. of AE at r.t. (Fig. 4c) showed formation of complexes 6 and 8 as the major species, and after 10 days 8 became the major product. Compared with reaction of complex 2 with 1.5 equiv. of AE (Fig. 4b), complex 7 was nearly fully consumed when 10 equiv. of AE were used. Complex 8 was also independently prepared by reaction of 2 with AA (Supplementary Methods). In addition, complex 8 was catalytically active for the dehydrogenation of AE under the conditions in which complex 1 was used, resulting in 81% conversion of AE to GA (33% yield) and linear peptides (see Supplementary Methods for details).

Figure 4: Reaction of complex 2 with AE at r.t. in C6D6.
figure4

(a) 1H NMR spectra using 1.5 equiv. of AE, (b) 31P{1H} NMR spectra using 1.5 equiv. of AE and (c) 31P{1H} NMR spectra using 10 equiv. of AE.

Discussion

On the basis of the NMR studies, the isolation of complex 8, and the known chemistry of pyridine-based pincer ruthenium complexes22,23,24,25,26, the mechanism shown in Fig. 5 is proposed. Reaction of the dearomatized complex 2 with AE leads to the aromatic alkoxy complex 6. Following dehydrogenation by metal–ligand cooperation, the 2-amino aldehyde intermediate A is formed and then attacked by another molecule of AE, providing the aromatic hemi-aminoxy intermediate B. Subsequent hydride elimination and H2 generation affords the dearomatized AA-intermediate C. Isomerization of C and activation of the O–H bond produces the aromatic species D, followed by hydride elimination to generate an aldehyde group and release a third molecule of H2 to afford intermediate E. Intramolecular reaction between the amino and aldehyde groups in complex E produces GA via intermediate F, while an intermolecular reaction with AE results in a linear oligopeptide. During formation of D from intermediate C, isomerization followed by amide N–H activation produces complex 8.

Figure 5: Proposed mechanism for dehydrogenative coupling of AE catalysed by complex 2.
figure5

In summary, we have developed a fundamentally new, reversible system that can load and unload H2 with a potentially high hydrogen storage capacity. It is based on a unique acceptorless dehydrogenative coupling process involving cheap and abundant AE, and hydrogenation of the product cyclic dipeptide GA, which takes place with the same catalyst system. Insight into the mechanism is provided, including isolated intermediates. Although there are limitations at this early stage, we believe that this fundamental system provides a sound basis for the development, upon further improvements, such as solvent elimination, of an attractive LOHC system based on inexpensive, abundant and safe AE carrier. The success of this system highlights the possibilities of applying fundamentally new chemical reactions, such as reversible acceptorless peptide bond formation, as a basis for novel LOHCs.

Methods

See Supplementary Methods and Supplementary Fig. 3 for general procedures and further details.

Additional information

Accession codes: The X-ray crystallographic coordinate for the structure (complex 8) reported in this Article has been deposited at the Cambridge Crystallographic Data Centre (CCDC), under deposition number CCDC 1017722. The data can be obtained free of charge from The Cambridge Crystallographic Data Centre via www.ccdc.cam.ac.uk/data_request/cif.

How to cite this article: Hu, P. et al. A novel liquid organic hydrogen carrier system based on catalytic peptide formation and hydrogenation. Nat. Commun. 6:6859 doi: 10.1038/ncomms7859 (2015).

References

  1. 1

    Armaroli, N. & Balzani, V. Energy for a Sustainable World: From the Oil Age to a Sun-Powered Future Wiley-VCH (2011).

  2. 2

    Minić D. (ed.) Hydrogen Energy—Challenges and Perspectives InTech (2012).

  3. 3

    Dalebrook, A. F., Gan, W., Grasemann, M., Moret, S. & Laurenczy, G. Hydrogen storage: beyond conventional methods. Chem. Commun. 49, 8735–8751 (2013).

    CAS  Article  Google Scholar 

  4. 4

    Satyapal, S., Petrovic, J., Read, C., Thomas, G. & Ordaz, G. The U.S. Department of Energy’s national hydrogen storage project: progress towards meeting hydrogen-powered vehicle requirements. Catal. Today 120, 246–256 (2007).

    CAS  Article  Google Scholar 

  5. 5

    O’M Bockris, J. A hydrogen economy. Science 176, 1323 (1972).

    ADS  Article  Google Scholar 

  6. 6

    Crabtree, R. H. Hydrogen storage in liquid organic heterocycles. Energy Environ. Sci. 1, 134–138 (2008).

    CAS  Article  Google Scholar 

  7. 7

    Makowsky, P., Thomas, A., Kuhn, P. & Goetmann, F. Organic materials for hydrogen storage applications: from physisorption on organic solids to chemisorption in organic molecules. Energy Environ. Sci. 2, 480–490 (2009).

    Article  Google Scholar 

  8. 8

    Enthaler, S., Langermann, J. & Schmidt, T. Carbon dioxide and formic acid—the couple for environmental-friendly hydrogen storage? Energy Environ. Sci. 3, 1207–1217 (2010).

    CAS  Article  Google Scholar 

  9. 9

    Palo, D. R., Dagle, R. A. & Holladay, J. D. Methanol steam reforming for hydrogen production. Chem. Rev. 107, 3992–4021 (2007).

    CAS  Article  Google Scholar 

  10. 10

    Nielsen, M. et al. Low-temperature aqueous-phase methanol dehydrogenation to hydrogen and carbon dioxide. Nature 495, 85–89 (2013).

    ADS  CAS  Article  Google Scholar 

  11. 11

    Rodríguez-Lugo, R. E. et al. A homogeneous transition metal complex for clean hydrogen production from methanol–water mixtures. Nat. Chem. 5, 342–347 (2013).

    Article  Google Scholar 

  12. 12

    Alberico, E. et al. Selective hydrogen production from methanol with a defined iron pincer catalyst under mild conditions. Angew. Chem. Int. Ed. 52, 14162–14166 (2013).

    CAS  Article  Google Scholar 

  13. 13

    Heim, L. E., Schlörer, N. E., Choi, J.-H. & Prechtl, M. H. G. Selective and mild hydrogen production using water and formaldehyde. Nat. Commun. 5, 3621 (2014).

    Article  Google Scholar 

  14. 14

    Trincado, M., Banerjee, H. & Gruetzmacher, H. Molecular catalysts for hydrogen production from alcohols. Energy Environ. Sci. 7, 2464–2503 (2014).

    CAS  Article  Google Scholar 

  15. 15

    Zhang, Y.-H. P. A sweet out-of-the-box solution to the hydrogen economy: is the sugar-powered car science fiction? Energy Environ. Sci. 2, 272–282 (2009).

    CAS  Article  Google Scholar 

  16. 16

    Teichmann, D. et al. Energy storage in residential and commercial buildings via Liquid Organic Hydrogen Carriers (LOHC). Energy Environ. Sci. 5, 9044–9054 (2012).

    CAS  Article  Google Scholar 

  17. 17

    Eblagon, K. M. et al. Hydrogenation of 9-ethylcarbazole as a prototype of a liquid hydrogen carrier. Int. J. Hydrogen Energy 35, 11609–11621 (2010).

    CAS  Article  Google Scholar 

  18. 18

    Sobota, M. et al. Dehydrogenation of dodecahydro-N-ethylcarbazole on Pd/Al2O3 model catalysts. Chem. Eur. J. 17, 11542–11552 (2011).

    CAS  Article  Google Scholar 

  19. 19

    Yamaguchi, R., Ikeda, C., Takahashi, Y. & Fujita, K.-I. Homogeneous catalytic system for reversible dehydrogenation−hydrogenation reactions of nitrogen heterocycles with reversible interconversion of catalytic species. J. Am. Chem. Soc. 131, 8410–8412 (2009).

    CAS  Article  Google Scholar 

  20. 20

    Fujita, K.-I., Tanaka, Y., Kobayashi, M. & Yamaguchi, R. Homogeneous perdehydrogenation and perhydrogenation of fused bicyclic N-heterocycles catalyzed by iridium complexes bearing a functional bipyridonate ligand. J. Am. Chem. Soc. 136, 4829–4832 (2014).

    CAS  Article  Google Scholar 

  21. 21

    Gunanathan, C. & Milstein, D. Applications of acceptorless dehydrogenation and related transformations in chemical synthesis. Science 341, 1229712 (2013).

    Article  Google Scholar 

  22. 22

    Gunanathan, C. & Milstein, D. Metal–ligand cooperation by aromatization–dearomatization: A new paradigm in bond activation and ‘green’ catalysis. Acc. Chem. Res. 44, 588–602 (2011).

    CAS  Article  Google Scholar 

  23. 23

    Zhang, J., Leitus, G., Ben- David, Y. & Milstein, D. Facile conversion of alcohols into esters and dihydrogen catalyzed by new ruthenium complexes. J. Am. Chem. Soc. 127, 10840–10841 (2005).

    CAS  Article  Google Scholar 

  24. 24

    Gunanathan, C., Ben-David, Y. & Milstein, D. Direct synthesis of amides from alcohols and amines with liberation of H2 . Science 317, 790–792 (2007).

    ADS  CAS  Article  Google Scholar 

  25. 25

    Ganaprakasam, B., Balaraman, E., Ben-David, Y. & Milstein, D. Synthesis of peptides and pyrazines from β-amino alcohols through extrusion of H2 catalyzed by ruthenium pincer complexes: ligand-controlled selectivity. Angew. Chem. Int. Ed. 50, 12240–12244 (2011).

    Article  Google Scholar 

  26. 26

    Balaraman, E., Gnanaprakasam, B., Shimon, L. J. W. & Milstein, D. Direct hydrogenation of amides to alcohols and amines under mild conditions. J. Am. Chem. Soc. 132, 16756–16758 (2010).

    CAS  Article  Google Scholar 

  27. 27

    Rochelle, G. T. Amine scrubbing for CO2 capture. Science 325, 1652–1654 (2009).

    ADS  CAS  Article  Google Scholar 

  28. 28

    Fogler, E. et al. System with potential dual modes of metal-ligand cooperation: highly catalytically active pyridine-based PNNH-Ru complexes. Chem. Eur. J. 20, 15727–15731 (2014).

    CAS  Article  Google Scholar 

  29. 29

    Zhao, B., Han, Z. & Ding, K. The N-H functional group in organometallic catalysis. Angew. Chem., Int. Ed. 52, 4744–4788 (2013).

    CAS  Article  Google Scholar 

  30. 30

    Kashima, C., Harada, K., Fujioka, Y., Maruyama, T. & Omote, Y. Amino alcohols as C-terminal protecting groups in peptide synthesis. J. Chem. Soc. Perkin Trans. I 535–539 (1988).

  31. 31

    Balaraman, E., Khaskin, E., Leitus, G. & Milstein, D. Catalytic transformation of alcohols to carboxylic acid salts and H2 using water as the oxygen atom source. Nat. Chem. 5, 122–125 (2013).

    CAS  Article  Google Scholar 

Download references

Acknowledgements

This research was supported by the European Research Council under the FP7 framework (ERC no. 246837) and by the Israel Science Foundation. We thank the Planning and Budgeting Committee of the Council for Higher Education in Israel for a fellowship to P.H.

Author information

Affiliations

Authors

Contributions

P.H. made the initial discovery, carried out experiments and wrote the manuscript. E.F. planned and developed complex 5. Y.D.-P. performed the X-ray structural study of complex 8. M.A.I. performed the DFT calculations. D.M. designed and directed the project and wrote the manuscript.

Corresponding author

Correspondence to David Milstein.

Ethics declarations

Competing interests

The authors declare no competing financial interests.

Supplementary information

Supplementary Information

Supplementary Figures 1-3, Supplementary Table 1-5, Supplementary Notes 1-3, Supplementary Discussion, Supplementary Methods and Supplementary References (PDF 561 kb)

Rights and permissions

This work is licensed under a Creative Commons Attribution-NonCommercial-NoDerivs 4.0 International License. The images or other third party material in this article are included in the article’s Creative Commons license, unless indicated otherwise in the credit line; if the material is not included under the Creative Commons license, users will need to obtain permission from the license holder to reproduce the material. To view a copy of this license, visit http://creativecommons.org/licenses/by-nc-nd/4.0/

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Hu, P., Fogler, E., Diskin-Posner, Y. et al. A novel liquid organic hydrogen carrier system based on catalytic peptide formation and hydrogenation. Nat Commun 6, 6859 (2015). https://doi.org/10.1038/ncomms7859

Download citation

Further reading

Comments

By submitting a comment you agree to abide by our Terms and Community Guidelines. If you find something abusive or that does not comply with our terms or guidelines please flag it as inappropriate.

Search

Quick links

Nature Briefing

Sign up for the Nature Briefing newsletter — what matters in science, free to your inbox daily.

Get the most important science stories of the day, free in your inbox. Sign up for Nature Briefing