Open Access

Tuning the Synthesis of Manganese Oxides Nanoparticles for Efficient Oxidation of Benzyl Alcohol

Nanoscale Research Letters201712:23

https://doi.org/10.1186/s11671-016-1777-y

Received: 18 November 2016

Accepted: 9 December 2016

Published: 6 January 2017

Abstract

The liquid phase oxidation of benzyl alcohol is an important reaction for generating benzaldehyde and benzoic acid that are largely required in the perfumery and pharmaceutical industries. The current production systems suffer from either low conversion or over oxidation. From the viewpoint of economy efficiency and environmental demand, we are aiming to develop new high-performance and cost-effective catalysts based on manganese oxides that can allow the green aerobic oxidation of benzyl alcohol under mild conditions. It was found that the composition of the precursors has significant influence on the structure formation and surface property of the manganese oxide nanoparticles. In addition, the crystallinity of the resulting manganese nanoparticles was gradually improved upon increasing the calcination temperature; however, the specific surface area decreased obviously due to pore structure damage at higher calcination temperature. The sample calcined at the optimal temperature of 600 °C from the precursors without porogen was a Mn3O4-rich material with a small amount of Mn2O3, which could generate a significant amount of \( {\mathrm{O}}_2^{-} \) species on the surface that contributed to the high catalytic activity in the oxidation. Adding porogen with precursors during the synthesis, the obtained catalysts were mainly Mn2O3 crystalline, which showed relatively low activity in the oxidation. All prepared samples showed high selectivity for benzaldehyde and benzoic acid. The obtained catalysts are comparable to the commercial OMS-2 catalyst. The synthesis–structure–catalysis interaction has been addressed, which will help for the design of new high-performance selective oxidation catalysts.

Keywords

Manganese oxides Synthesis–structure–catalysis interaction Aerobic oxidation Benzyl alcohol

Background

The liquid phase oxidation of benzyl alcohol is a widely investigated reaction by both academics and engineers as it provides benzaldehyde and benzoic acid [1]. Both products can act as versatile intermediates for the synthesis of fine chemicals or perfume [27]. In the past few years, numerous catalytic systems have been developed to perform this chemo-selective oxidation of alcohols [6]. Both homogeneous and heterogeneous catalysts can perform this benzyl alcohol oxidation. Traditional homogeneous catalytic systems for the oxidation of benzyl alcohols use stoichiometric chemicals such as chromium (VI) reagents, dimethyl sulfoxide, hydrogen peroxide, tert-butyl hydroperoxide (TBHP), nitric acid, and permanganates or other inorganic oxidants [6, 8]. Homogeneous catalysis normally has excellent reactivity and selectivity in a small scale reaction since in homogeneous catalysts every single catalytic entity can act as a single active site [912]. But on an industrial scale and considering environmental and ecological issues, the drawback of homogeneous catalysis is evident, such as catalyst leaking, poisoning, toxic metal waste, difficulty in separation, and recovery of the catalyst from the reaction mixture as well as limited recyclability [1216].

Hence, heterogeneous catalysts are considered to be a promising alternative for the oxidation of benzyl alcohol, and in fact, heterogeneous catalysis participates in almost 90% of industrial practices currently [15]. Recently, a large number of studies on the oxidation of benzyl alcohol to benzaldehyde by molecular oxygen with a solvent, using various transition metal oxide-based and noble metal-based catalysts, have been reported [14, 17]. The noble metal-based catalysts, though highly active for the oxidation of benzyl alcohol, generally suffer from the sintering of surface noble metal particles and high price as well as a low reserve on earth [18]. Although some advancement has been made in the catalytic oxidation of benzyl alcohols over noble metal catalyst, there are only limited literature reports on non-noble metal catalysts, like transition metals or transition metal oxides especially manganese oxides [19]. From the viewpoint of green economy and environmental demand, it is highly attractive to develop new and cost-effective catalysts using non-precious metals or metal oxides such as nickel [20], vanadium [21], copper [3], and manganese [19] that can allow more efficient aerobic oxidation of benzyl alcohol under mild conditions [14].

Among most of transition metal oxides, manganese oxides attract a broad interest, as they can exist in more than five easily exchangeable transition states with various structural forms over a wide range of temperatures (up 1200 °C) [2224]. Manganese oxides have various catalytic applications due to highly efficient redox properties, and the mixed valence has been confirmed to be important in redox catalysis as well as in energy and electron transfer [23, 25, 26]. Tu and co-workers demonstrated that manganese oxides (II, III, IV, and VII) have significant advantages over other oxidants in removing organic pollutants [25]. Furthermore, it has been confirmed that reduced manganese oxide can readily be reoxidized by dioxygen, meaning that manganese oxide can play as an electron-transfer mediator to generate a rapid electron-transfer path during oxidation reactions [27]. Many factors can affect the performance of manganese oxide catalysts during the oxidation of benzyl alcohols, but there were only a few studies exploring the influence of calcination temperatures of precursors on the physiochemical property and catalytic activity of the final products [28]. Furthermore, plenty of materials with similar gross structure features might have various properties due to different particle sizes and the amount and type of defects formed during different synthesis procedures. So even slight changes of synthetic parameters can result in distinct properties in catalytic, electrochemical, or ion-exchange activity [22]. In this report, transition metal-manganese oxide nanoparticles have been prepared by the variation of precursors and thermally controlled calcination. Their catalytic performance has been addressed by the oxidation of benzyl alcohol under the liquid phase with oxygen. The correlation among synthesis conditions, structure, and catalysis has been formulated based on the characterization and experimental results.

Methods

Catalyst Synthesis

Absolute ethanol, ammonia solution, analytical-grade manganese (II) chloride tetrahydrate, dopamine hydrochloride, and Pluronic® F127 were all purchased from Sigma-Aldrich and used without further purification.

The volumes of 100 mg F127 (7.94 × 10−7 mol), 100 mg dopamine hydrochloride (5.27 × 10−4 mol), and 60 mg manganese (II) chloride tetrahydrate (3.03 × 10−4 mol) were dissolved in a mixture of 10 ml deionized water and 20 ml absolute ethanol. The final mixture was stirred for 2 h (500 rpm) to allow complete dissolution. Then, 0.4 ml ammonia solution was dropwise added into the mixed solution. After stirring for 24 h, the obtained precipitate was sequentially separated from the solution via centrifugation and washed with deionized water and ethanol, and then the black powder was dried at 80 °C overnight in the oven. This was the sample preparation procedure for precursor S1. Totally, three series of samples were made using the control variable method (Table 1).
Table 1

Sample compositions

Sample series

Polymer

Porogen

Mn source

S1

PEO106–PPO70–PEO106 (F127)

C6H3(OH)2–CH2–CH2–NH2 (DA)

MnCl2·4H2O

S2

 

C6H3(OH)2–CH2–CH2–NH2 (DA)

MnCl2·4H2O

S3

PEO106–PPO70–PEO106 (F127)

 

MnCl2·4H2O

The obtained precursors (S1–S3) were thermally treated at temperatures of 400, 600, and 800 °C in air according to the heating procedure as shown in Fig. 1.
Fig. 1

Heating procedure of catalyst precursor

Catalyst Characterization

The crystal structures of the prepared samples were characterized by X-ray diffraction (XRD) on a XRD Siemens D5000 using Cu Kα irradiation with a maximum power of 2200 W. The wide-angle XRD patterns were collected over a 2θ range of 10–80° with a scan step rate of 2°/min and 0.02°/step. The surface area, pore volume, and pore size distribution were characterized by liquid nitrogen adsorption/desorption experiments, performed with a Quantachrome Autosorb-iQ automated adsorption system. The samples were degassed at 150 °C for 12 h under helium prior to each measurement. The surface areas were calculated using the Brunauer–Emmett–Teller (BET) method, and the pore sizes and pore volumes were calculated from the desorption branch of the isotherm using the Barrett–Joyner–Halenda (BJH) method. The manganese oxides was observed by a Zeiss Ultra Plus scanning electron microscope using SEM. High-resolution transmission electron microscopy (HR-TEM) images were recorded on a JEOL 2200FS transmission electron microscope at 200 kV. Each sample was suspended in ethanol, and then a drop or two of the suspension was loaded onto a carbon-coated copper grid and allowed to fully dry. Temperature-programmed reduction (TPR) experiments were conducted to get the sample oxidation reduction profiles. The samples were treated with N2 for 2 h at 150 °C before each experiment. In the experiments, 5% H2 in helium was used at a flow rate of 40 ml/min in the temperature range of 150–900 °C at a ramp of 10 °C/min. Temperature-programmed desorption (TPD) experiments were also done to investigate the surface oxygen activity of the materials in the oxidation reaction using N2 as carrier gas.

Catalyst Activity Measurements

In this benzyl alcohol oxidation procedure, 5 ml benzyl alcohol (0.1 M in deionized water) and the catalyst (50 mg) were put in an autoclave reactor under vigorous stirring (around 700 rpm). The sealed reactor was purged by 3 bar molecular oxygen before heating to the reaction temperature. Sampling was taken at every 2 h, and the product mixture was separated from nanocatalysts by centrifugation. Shimazu Ultra 2010 GC-MS and Plus 2010 GC have been used to analyze the products with octane as an internal standard. The conversion of benzyl alcohol (BA) was calculated by the mole ratio of the disappeared BA during the reaction to the total amount of BA before the reaction. The selectivity of the product was obtained by the mole ratio of the produced chemical to the disappeared BA.

Results and Discussion

Structural Characterization of the Manganese Oxides

The surface areas of the manganese oxides prepared with various precursors and calcined at 400, 600, and 800 °C have been listed in Table 2. Along with the increasing of calcination temperature, the surface area was tapering down. Especially for samples S1 and S2, the surface areas dropped down distinctly, while for S3, the increase of the calcination temperature seemed to not have much influence on the surface area. When looking at the compositions of precursors S1 and S2, although the addition of porogen generated larger surface pores (Fig. 5), it also made the precursors unstable and easier to collapse during calcination and then the surface area decreased significantly. The addition of porogen had remarkable effect on the crystallization for precursors S1 and S2 at the calcination temperature 800 °C, which transformed to bixbyite Mn2O3 (Additional file 1: Figure S1 and Additional file 2: Figure S2) phase, while S3 turned into hausmannite (Mn3O4, Fig. 2) phase.
Table 2

Catalytic performance of aerobic oxidation of benzyl alcohol over various samples

Entry

Catalyst

BET surface area (m2 g−1)

Conversion (%)

Selectivity (%)

Benzaldehyde

Benzoic acid

1

S1-400

25.7

6.8

100

0

2

S1-600

16.3

49.8

100

0

3

S1-800

13.5

34.7

100

0

4

S2-400

28.3

7.8

100

0

5

S2-600

22.1

62.0

100

0

6

S2-800

11.7

34.2

100

0

7

S3-400

38.6

32.1

100

0

8

S3-600

35.6

64.5

91.8

8.2

9

S3-800

32.2

40.9

100

0

Reaction conditions: 5 ml benzyl alcohol (0.1 M in deionized water), 50 mg catalyst, T = 140 °C, 3 bar molecular oxygen, reaction time 5 h

Fig. 2

XRD pattern of manganese precursor before and after calcination

The peaks of S3 before calcination (Fig. 2) were similar to the patterns of samples S1 and S2 before calcination (Additional file 1: Figure S1 and Additional file 2: Figure S2). This demonstrates that the prepared manganese precursor was crystalline MnCO3. The patterns of S3-600 and S3-800 in Fig. 2 have three main characteristic peaks, indicating the tetragonal crystalline structure of hausmannite Mn3O4, i.e., (103), (211), and (224), can be observed in both of the XRD patterns (PDF#75-1560). However, the S3 transformed into an amorphous phase after calcination at 400 °C and the other two precursors, S1 and S2, transformed to the body-centered cubic bixbyite Mn2O3 (PDF#76-0150) (Additional file 1: Figure S1 and Additional file 2: Figure S2) after calcination. Based on the Debye–Scherrer equation analysis of the peak width at half height of sample S3-600 and S3-800 in Fig. 2, the size of the obtained particles was estimated to be around 20 nm, which was confirmed by observing the particle size in the SEM image (Fig. 3).
Fig. 3

ad SEM images of manganese precursor S3 calcined at 400, 600, and 800 °C

The SEM images of S3 indicated that there was no obvious morphology change before and after calcination of the precursor except there were more pores formed after calcination. Besides, compared to the SEM images of S1 and S2 (Additional file 3: Figure S3 and Additional file 4: Figure S4), no cubes can be observed in Fig. 3.

High-resolution transmission electron microscope (TEM) images of the S3 calcined at 600 °C in air are displayed in Fig. 4. Obviously, the manganese oxide nanoparticles (Fig. 4a, b) had an average size between 20 and 30 nm, and the shape of the particle was more like a regular sphere compared to the oval-shaped particles of S1 and S2 after calcination (Additional file 5: Figure S5 and Additional file 6: Figure S6). The two interplanar spacings of 0.46 and 0.26 nm (Fig. 4c) correspond to the (101) and (211) lattice planes of the tetragonal phase Mn3O4, respectively. The highly clear crystal lattice as well as the corresponding well-ordered dot pattern of the fast Fourier transform (FFT) image demonstrates the high-quality single-crystalline nature of Mn3O4.
Fig. 4

ad HR-TEM images of manganese precursor S3 calcined at 600 °C

After calcination at 600 °C in air, the morphologies of precursor S1 and precursor S2 (Fig. 5) were apparently different from that of precursor S3. Mesopores have been observed in the cubic particles, and all the lattice planes in Fig. 5c, d can be indexed to bixbyite Mn2O3. Therefore, crystalline Mn3O4 was formed for S3 and crystalline Mn2O3 was formed for S1 and S2 after the 600 °C calcination. The compositions for the preparation of precursors had significant influence on the structure formation of manganese oxide nanoparticles.
Fig. 5

SEM images of precursor S1 (a) and precursor S2 (b) calcined at 600 °C in air and their corresponding HR-TEM images (c, d)

The reduction profiles of the materials calcined at 600 °C were tested by the temperature-programmed reduction (H2-TPR) studies. From the H2-TPR profile of S2-600 as shown in Fig. 6, two reduction peaks can be observed at 372 and 462 °C, indicating a two-step reduction (Mn2O3 to Mn3O4 and Mn3O4 to MnO). The high-temperature reduction peak appeared at 495 °C for S3-600 and 526 °C for S1-600, indicating the difficulty of reducing S3-600 and S1-600 (Mn3O4 to MnO) comparing to S2-600 (462 °C). However, the low-temperature reduction peak of S3-600 (Mn2O3 to Mn3O4) occurred at 334 °C, which was much lower than those of S1-600 and S2-600 (420 and 372 °C, respectively), suggesting the easily reducible nature of S3-600 (from Mn2O3 to Mn3O4). According to the XRD and HR-TEM results, S3-600 was a Mn3O4-rich material, which only contained a trace amount of Mn2O3 as indicated by a very weak reduction peak at low temperature, while S1-600 still contained a considerable amount of Mn2O3.
Fig. 6

H2-TPR profiles of (black line) S1-600, (red line) S2-600, and (green line) S3-600 catalysts heated in a stream of H2

The temperature-programmed desorption of O2 (O2-TPD) was performed to probe the surface active sites of the catalysts for oxygen adsorption/desorption. A major O2 loss from both S1-600 and S2-600 was observed at temperatures higher than 800 °C (820 °C for S1-600 and 832 °C for S2-600) in the O2-TPD (Fig. 7), which can be ascribed to the loss of lattice oxygen O2−, very strong chemisorbed O, or reticular oxygen (known as β-oxygen) corresponding to different Mn–O bond strengths [8, 2932]. For S3-600, a new and relatively strong desorption peak was observed at 590 °C due to the desorption of active chemisorbed oxygen (species \( {\mathrm{O}}_2^{-} \)) on the surface with the remarkably enhanced oxygen mobility [7, 33]. Only a slightly small peak at 800 °C was observed for S3-600. Lattice oxygen O2−, surface O, or β-oxygen were mainly related to partial oxidation, while the active chemisorbed oxygen \( {\mathrm{O}}_2^{-} \) was very active in the deep oxidation [31]. S3-600, a Mn3O4-rich material with a small amount of Mn2O3, could generate significant amount of \( {\mathrm{O}}_2^{-} \) species on the surface during oxidation that would be responsible for the deep oxidation of alcohols. S1 and S2-600 that were mainly crystalline Mn2O3 could contain the dominant lattice oxygen O2−, surface O, or β-oxygen species on the surface for the partial oxidation.
Fig. 7

O2-TPD profiles of (black line) S1-600, (red line) S2-600, and (green line) S3-600 catalysts heated in a stream of N2

Catalytic Reactions

The benzyl alcohol oxidation activities of all samples obtained at different calcination temperatures were studied under identical conditions [14]. Their catalytic performances are listed in Table 2 with their surface areas.

All prepared samples exhibited target selectivity for benzyl alcohol oxidation, with only benzaldehyde and benzoic acid produced. No over oxidation occurred and no CO or CO2 was observed by GC/TCD. As shown in Table 2, it is clearly illustrated that samples calcined at 400 °C did not have much oxidation activity as the conversion was quite low. Although samples calcined at 800 °C performed better than those calcined at 400 °C, their conversions were still lower than samples calcined at 600 °C. So in general, the relationship between oxidation activity and calcination temperature followed the order of 400 °C < 800 °C < 600 °C. The oxidation activities of the samples were not increased proportionally with the surface area. For samples calcinated at 400 °C with the highest surface areas, no crystalline Mn oxides were generated resulting in the lowest catalytic activity. Therefore, the oxidation activity should be based on both crystal structure and surface sites.

Among samples calcined at 600 °C, S3-600 performed the best compared to S1-600 and S2-600 in 5 h under the same conditions as shown in Table 2. Figure 8 illustrates benzyl alcohol conversion over precursors S1–S3 calcined at 600 and 800 °C after 10-h reaction as the reaction would reach an equilibrium if the reaction time is prolonged. It was evident that conversions of precursors calcined at 800 °C did not increase much after another 5-h reaction. However, precursors calcined at 600 °C still had high activity. Among all the catalysts calcined at 600 °C, S3-600 has the best performance as its conversion can reach as high as 82% and further oxidation from benzaldehyde to benzoic acid also confirmed its excellent oxidation activity. Therefore, the activity of the manganese oxides can be linked to their specific surface property. S3-600, a Mn3O4-rich material with a small amount of Mn2O3, could generate significant amount of \( {\mathrm{O}}_2^{-} \) species on the surface during oxidation that would lead to the high catalytic activity in the oxidation of alcohols. S1 and S2-600 with mainly crystalline Mn2O3 could contain the dominant lattice oxygen O2−, surface O, or β-oxygen species on the surface for the relatively lower activity in the oxidation. It was proposed that Mn3O4 with coexistence of a mix-valence state such as Mn2O3 can create defects in the materials and contribute unique and more activity in certain redox reactions [19, 34, 35]. The defects promoted the adsorption of the oxygen as indicated by O2-TPD, which would enhance the catalytic activity. Furthermore, the structure and crystallinity of samples obtained were similar to what Sourav and his group reported recently [6], and the manganese oxides they made still have good performance in benzyl alcohol oxidation after being recycled four times. So we believe that our catalysts could also have excellent reusability.
Fig. 8

Influence of sample calcination temperatures on benzyl alcohol conversion to benzaldehyde and benzoic acid over catalysts S1, S2, and S3 calcined at 600 and 800 °C, respectively; reaction time 10 h

Conclusions

This research aimed to tune the precursors and calcination temperature to synthesize manganese oxide nanocatalysts for the aerobic oxidation of benzyl alcohol in the liquid phase with molecular oxygen. Three groups of samples have been synthesized by Mn source with both F127 polymer (PEO106–PPO70–PEO106) and DA porogen (C6H3(OH)2–CH2–CH2–NH2) (S1), with only DA porogen (S2), and with only F127 polymer (S3). The crystalline MnCO3 has been observed for all samples before calcination. After calcination at 400 °C, the S3 transformed into an amorphous phase while S1 and S2 transformed to the body-centered cubic bixbyite Mn2O3. Upon further heating to 600 and 800 °C, S1 and S2 kept their crystalline Mn2O3 structure; S3, however, changed from the amorphous state to the tetragonal crystalline structure of hausmannite Mn3O4 with the average particle size of around 20 nm. Along with the increasing of the calcination temperature, the surface area was tapering down. Especially for samples S1 and S2, their surface areas dropped down distinctly, while for S3, the increase of the calcination temperature seemed to not have much influence on the surface area. The addition of porogen (to precursors S1 and S2) had a remarkable effect on the structure formation after calcination. TEM images (Fig. 4) show regular spherical-shaped particles of S3 compared to the oval-shaped particles of S1 and S2 after calcination at 600 °C. The temperature-programmed reduction (H2-TPR) indicated the existence of a small amount of Mn2O3 in the Mn3O4-dominated S3-600 sample.

The compositions for the preparation of precursors had significant influence on the structure formation of the manganese oxide nanoparticles and their surface properties. S3-600 was a Mn3O4-rich material with a small amount of Mn2O3 that could generate significant amount of \( {\mathrm{O}}_2^{-} \) species on the surface after adsorption of oxygen. S1 and S2-600 with mainly crystalline Mn2O3 could contain the dominant lattice oxygen O2−, surface O, or β-oxygen species on the surface. All the prepared samples showed target selectivity for benzyl alcohol oxidation, generating benzaldehyde and benzoic, which are essential materials in the pharmaceutical and perfumery industries. No over oxidation occurred and no CO or CO2 was observed during the reaction. The samples calcined at 400 °C with higher surface areas did not display much oxidation activity as the conversions were quite low. The oxidation activities of the samples were not increased proportionally with the surface area but were correlated to the crystal structure and surface sites. S3-600 with the significant amount of \( {\mathrm{O}}_2^{-} \) species on the surface during oxidation exhibited the highest catalytic activity in the oxidation of alcohols. S1 and S2-600 with mainly crystalline Mn2O3 could contain the dominant lattice oxygen O2−, surface O, or β-oxygen species on the surface that led to the relatively lower activity in the oxidation.

Declarations

Acknowledgements

We thank the Australian Research Council for the funding support (ZL DP130104231) and the Australian Research Council (JH DP150103842) and AINST Accelerate Scheme (JH and ZL), the Early Career Research Scheme (JH), and MCR (JH and ZL) from the University of Sydney.

Authors’ Contributions

JF contributed ideas and carried out main part of the experiment work. LS contributed to the structure and context. CZ contributed to the SEM and TEM part. HL contributed ideas and training of alcohol oxidation experiment. FY contributed to data analysis and figure processing. XZ and JS helped with samples preparation and calcination. YL helped the background writing. JH and ZL both made the coordination of the whole project and helped revise the manuscript. All authors read and approved the final manuscript.

Competing Interests

The authors declare that they have no competing interests.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

(1)
School of Chemical and Bimolecular Engineering, The University of Sydney
(2)
School of Materials Science and Engineering, Guilin University of Electronic Technology
(3)
School of Environment, Tsinghua University

References

  1. Kumar A, Kumar VP, Kumar BP, Vishwanathan V, Chary KV (2014) Vapor phase oxidation of benzyl alcohol over gold nanoparticles supported on mesoporous TiO2. Catal Lett 144:1450–1459View ArticleGoogle Scholar
  2. Sun H y, Hua Q, Guo F f, Wang Z y, Huang W x (2012) Selective aerobic oxidation of alcohols by using manganese oxide nanoparticles as an efficient heterogeneous catalyst. Adv Synth Catal 354:569–573View ArticleGoogle Scholar
  3. Hamza A, Srinivas D (2009) Selective oxidation of benzyl alcohol over copper phthalocyanine immobilized on MCM-41. Catal Lett 128:434–442View ArticleGoogle Scholar
  4. Ali R, Nour K, Al-warthan A, Siddiqui MRH (2015) Selective oxidation of benzylic alcohols using copper-manganese mixed oxide nanoparticles as catalyst. Arabian J Chem 8:512-517Google Scholar
  5. Arena F, Gumina B, Lombardo AF, Espro C, Patti A, Spadaro L, Spiccia L (2015) Nanostructured MnO x catalysts in the liquid phase selective oxidation of benzyl alcohol with oxygen: part I. Effects of Ce and Fe addition on structure and reactivity. Appl Catal B Environ 162:260–267View ArticleGoogle Scholar
  6. Biswas S, Poyraz AS, Meng Y, Kuo C-H, Guild C, Tripp H, Suib SL (2015) Ion induced promotion of activity enhancement of mesoporous manganese oxides for aerobic oxidation reactions. Appl Catal B Environ 165:731–741View ArticleGoogle Scholar
  7. Chen Y, Zheng H, Guo Z, Zhou C, Wang C, Borgna A, Yang Y (2011) Pd catalysts supported on MnCeOx mixed oxides and their catalytic application in solvent-free aerobic oxidation of benzyl alcohol: support composition and structure sensitivity. J Catal 283:34–44View ArticleGoogle Scholar
  8. Makwana VD, Son Y-C, Howell AR, Suib SL (2002) The role of lattice oxygen in selective benzyl alcohol oxidation using OMS-2 catalyst: a kinetic and isotope-labeling study. J Catal 210:46–52View ArticleGoogle Scholar
  9. Habibi D, Faraji A, Arshadi M, Fierro J (2013) Characterization and catalytic activity of a novel Fe nano-catalyst as efficient heterogeneous catalyst for selective oxidation of ethylbenzene, cyclohexene, and benzylalcohol. J Mol Catal A Chem 372:90–99View ArticleGoogle Scholar
  10. Burri DR, Shaikh IR, Choi K-M, Park S-E (2007) Facile heterogenization of homogeneous ferrocene catalyst on SBA-15 and its hydroxylation activity. Catal Commun 8:731–735View ArticleGoogle Scholar
  11. Cole-Hamilton D, Tooze R (2006) Homogeneous catalysis—advantages and problems. In Catalyst Separation, Recovery and Recycling; Springer Netherlands, pp 1-8Google Scholar
  12. Larhed M, Moberg C, Hallberg A (2002) Microwave-accelerated homogeneous catalysis in organic chemistry. Acc Chem Res 35:717–727View ArticleGoogle Scholar
  13. Mallat T, Baiker A (2004) Oxidation of alcohols with molecular oxygen on solid catalysts. Chem Rev 104:3037–3058View ArticleGoogle Scholar
  14. Su Y, Wang L-C, Liu Y-M, Cao Y, He H-Y, Fan K-N (2007) Microwave-accelerated solvent-free aerobic oxidation of benzyl alcohol over efficient and reusable manganese oxides. Catal Commun 8:2181–2185View ArticleGoogle Scholar
  15. Ali ME, Rahman MM, Sarkar SM, Hamid SBA (2014) Heterogeneous metal catalysts for oxidation reactions. J Nanomater 2014:209Google Scholar
  16. Clark JH, Macquarrie DJ (1997) Heterogeneous catalysis in liquid phase transformations of importance in the industrial preparation of fine chemicals. Org Process Res Dev 1:149–162View ArticleGoogle Scholar
  17. Enache DI, Knight DW, Hutchings GJ (2005) Solvent-free oxidation of primary alcohols to aldehydes using supported gold catalysts. Catal Lett 103:43–52View ArticleGoogle Scholar
  18. Ji H, Wang T, Zhang M, She Y, Wang L (2005) Simple fabrication of nano-sized NiO 2 powder and its application to oxidation reactions. Appl Catal A Gen 282:25–30View ArticleGoogle Scholar
  19. Dhanalaxmi K, Singuru R, Kundu SK, Reddy BM, Bhaumik A, Mondal J (2016) Strongly coupled Mn 3 O 4–porous organic polymer hybrid: a robust, durable and potential nanocatalyst for alcohol oxidation reactions. RSC Adv 6:36728–36735View ArticleGoogle Scholar
  20. Choudary B, Kantam ML, Rahman A, Reddy C, Rao KK (2001) The first example of activation of molecular oxygen by Nickel in Ni-Al hydrotalcite: a novel protocol for the selective oxidation of alcohols. Angew Chem Int Ed 40:763–766View ArticleGoogle Scholar
  21. Velusamy S, Punniyamurthy T (2004) Novel vanadium-catalyzed oxidation of alcohols to aldehydes and ketones under atmospheric oxygen. Org Lett 6:217–219View ArticleGoogle Scholar
  22. Brock SL, Duan N, Tian ZR, Giraldo O, Zhou H, Suib SL (1998) A review of porous manganese oxide materials. Chem Mater 10:2619–2628View ArticleGoogle Scholar
  23. Suib SL (2008) Structure, porosity, and redox in porous manganese oxide octahedral layer and molecular sieve materials. J Mater Chem 18:1623–1631View ArticleGoogle Scholar
  24. Tian Z-R, Tong W, Wang J-Y, Duan N-G, Krishnan VV, Suib SL (1997) Manganese oxide mesoporous structures: mixed-valent semiconducting catalysts. Science 276:926–930View ArticleGoogle Scholar
  25. Tu J, Yang Z, Hu C (2015) Efficient catalytic aerobic oxidation of chlorinated phenols with mixed-valent manganese oxide nanoparticles. J Chem Technol Biotechnol 90:80–86View ArticleGoogle Scholar
  26. Ohsaka T, Mao L, Arihara K, Sotomura T (2004) Bifunctional catalytic activity of manganese oxide toward O 2 reduction: novel insight into the mechanism of alkaline air electrode. Electrochem Commun 6:273–277View ArticleGoogle Scholar
  27. Oishi T, Yamaguchi K, Mizuno N (2011) Conceptual design of heterogeneous oxidation catalyst: copper hydroxide on manganese oxide-based octahedral molecular sieve for aerobic oxidative alkyne homocoupling. ACS Catal 1:1351–1354View ArticleGoogle Scholar
  28. Li X, Hu B, Suib S, Lei Y, Li B (2010) Manganese dioxide as a new cathode catalyst in microbial fuel cells. J Power Sources 195:2586–2591View ArticleGoogle Scholar
  29. Genuino HC, Dharmarathna S, Njagi EC, Mei MC, Suib SL (2012) Gas-phase total oxidation of benzene, toluene, ethylbenzene, and xylenes using shape-selective manganese oxide and copper manganese oxide catalysts. J Phys Chem C 116:12066–12078View ArticleGoogle Scholar
  30. Doornkamp C, Ponec V (2000) The universal character of the Mars and Van Krevelen mechanism. J Mol Catal A Chem 162:19–32View ArticleGoogle Scholar
  31. Paredes JR, Díaz E, Díez FV, Ordóñez S (2008) Combustion of methane in lean mixtures over bulk transition-metal oxides: evaluation of the activity and self-deactivation. Energy Fuel 23:86–93View ArticleGoogle Scholar
  32. Morales MR, Barbero BP, Cadús LE (2007) Combustion of volatile organic compounds on manganese iron or nickel mixed oxide catalysts. Appl Catal B Environ 74:1–10View ArticleGoogle Scholar
  33. Du Y, Wang Q, Liang X, He Y, Feng J, Li D (2015) Hydrotalcite-like MgMnTi non-precious-metal catalyst for solvent-free selective oxidation of alcohols. J Catal 331:154–161View ArticleGoogle Scholar
  34. Bai Z, Sun B, Fan N, Ju Z, Li M, Xu L, Qian Y (2012) Branched mesoporous Mn3O4 nanorods: facile synthesis and catalysis in the degradation of methylene blue. Chem Eur J 18:5319–5324View ArticleGoogle Scholar
  35. Duan J, Chen S, Dai S, Qiao SZ (2014) Shape control of Mn3O4 nanoparticles on nitrogen-doped graphene for enhanced oxygen reduction activity. Adv Funct Mater 24:2072–2078View ArticleGoogle Scholar

Copyright

© The Author(s). 2017