Upload
hoangnguyet
View
255
Download
8
Embed Size (px)
Citation preview
PLASMONIC PHOTOCATALYSTS OF
SUPPORTED GOLD NANOPARTICLES FOR
ORGANIC CONVERSIONS
Xingguang ZHANG
[Bachelor of Chemical Engineering and Technology, Guizhou University;
Master of Industrial Catalysis, Nanjing University of Technology]
Thesis completed under the supervision of Dr. Xuebin Ke and Prof. Huaiyong Zhu,
and submitted to Queensland University of Technology, in fulfilment of the
requirements of the degree of
Doctor of Philosophy
School of Chemistry, Physics and Mechanical Engineering
Faculty of Science and Engineering
Queensland University of Technology
February, 2014
i
Keywords
Photocatalysis
Visible light
Gold nanoparticle
Plasmonic photocatalysts
Localised surface plasmon resonance
Electric near-field enhancement
Zeolite
Polarised electrostatic fields
Photooxidation
Selective oxidation
Photoreduction
Selective reduction
Acetalisation
Transesterification
Molecular polarity
Alcohol
Aldehyde
Ketone
Epoxide
ii
Abstract
In photocatalysis, one of the greatest challenges is to design novel photocatalysts
that can efficiently harvest ―green‖ sunlight to drive or enhance chemical reactions.
Compared with traditional TiO2 semiconductors that can only utilise UV light (< 4%
of sunlight), plasmonic photocatalysts of supported gold nanoparticles (Au-NPs)
possess distinct advantages. Au-NPs can absorb visible light (about 43% of sunlight)
owing to the localised surface plasmon resonance (LSPR) effect that amplifies the
electromagnetic field of incident light (|E0|), leading to an intensified electromagnetic
field (|E|). This near-field enhancement phenomenon is well-known as the ―electric
near-field enhancement‖ effect. The two distinct features play an important role in
determining the catalytic performance of plasmonic photocatalysts.
In this thesis, plasmonic photocatalysts of supported Au-NPs were investigated
for several important organic transformations under visible light irradiation at
ambient temperature. The selective reduction of nitroaromatics to azo compounds,
azobenzene to hydroazobenzene, ketones to alcohols, and epoxides to alkenes, the
selective oxidation of aromatic alcohols to aldehydes, and the acetalisation of
aldehydes/ketones to acetals/ketals were studied with the aim to explore the catalytic
performance of new plasmonic photocatalysts.
Firstly, the selective reduction of the aforementioned four types of reduction
reactions proceeded effectively on plasmonic photocatalysts of supported Au-NPs on
Al2O3, CeO2, TiO2, ZrO2, or zeolite Y, in which Au-NPs provided catalytic centres.
The reactive efficiency of the photocatalysts primarily depended on two factors: the
light absorption efficiency and the reduction ability to activate reactants. The light
absorption ability by Au-NPs determined the reduction ability of the photocatalysts;
iii
specifically, light with shorter wavelengths could excite the free conduction electrons
in Au-NPs to higher energy levels, thus inducing reduction with more negative
reduction potentials. Moreover, the photoexcited Au-NPs could grab hydrogen from
the solvent, isopropanol, to form Au-H species on the gold surfaces. These active
Au-H species then reacted with the N=O, N=N, C=O double bonds or epoxide bonds
of reactants to weaken them by the energetic electrons of Au-NPs to produce the
final reductive products. The reduction ability of the Au-H species depended on the
energy of the energetic electrons in Au-NPs: the higher the energy of electrons was,
the stronger the reduction ability of Au-H species was, indicating that the reduction
ability of the photocatalysts could be tuned by controlling the light wavelength.
Secondly, the selective oxidation of aromatic alcohols to aldehydes proceeded
effectively on plasmonic photocatalysts of Au/zeolites with high selectivity (99%), in
which Au-NPs provided catalytic centres. The kinetic study indicated that the
photooxidation under visible light irradiation required much less activation energy to
initiate the reactions compared with that of the thermal-driven reaction. The
molecular polarities of aromatic alcohols were demonstrated to correlate with
photocatalytic performance, because of the different strengths of interaction with
electronically polarised Au-NPs. Moreover, the adsorption capability of zeolite
supports facilitated the concentration of reactants from the solvent.
Thirdly, the acetalisation of aldehydes/ketones to give acetals/ketals exhibited
enhanced catalytic performance on plasmonic photocatalysts of Au/zeolites, in which
zeolites provided catalytic centres. Zeolites possess strong Brønsted acid sites and
polarised electrostatic fields (PEF) created by extra-framework cations. The PEF
could be further intensified by the electric near-field enhancement of Au-NPs. The
acetalisation reaction was chosen as the model reaction performed on Au/MZSM-5
iv
and MZSM-5 (M=H+, Na
+, Ca
2+, or La
3+). Density functional theory (DFT)
calculations confirmed that the intensified PEF played a critical role in stretching the
C=O bonds of the reactants of benzaldehyde and cyclohexanone, to enlarge their
molecular polarities. The reactants with a larger C=O bond polarity could be
activated more easily by active sites of H+, thus boosting the reaction rate.
Overall, this research program illustrates a new way of harvesting visible light
using plasmonic photocatalysts of supported Au-NPs. These findings may evoke
intensive research interests on plasmonic metal nanostructures and diverse catalytic
supports (e.g., zeolites) to take advantage of ―green‖ sunlight for plasmonic devices,
molecular electronics, energy storage, and catalysis.
v
List of publications
Journal publications:
1. Xingguang Zhang, Xuebin Ke*, and Huaiyong Zhu. Zeolite-supported gold
nanoparticles for selective photooxidation of aromatic alcohols under visible-
light irradiation. Chem. Eur. J. 2012, 18, 8048-8056. (Highlighted paper)
2. Xingguang Zhang, Xuebin Ke*, Zhanfeng Zheng, Hongwei Liu, and Huaiyong
Zhu*. TiO2 nanofibers of different crystal phases for transesterification of
alcohols with dimethyl carbonate. Appl. Catal. B 2014, 150-151, 330-337.
3. Xingguang Zhang, Xuebin Ke*, Aijun Du, and Huaiyong Zhu. Plasmonic
nanostructures to enhance catalytic performance of zeolites under visible light.
Sci. Rep. 2014, 4(3805), 1-6.
4. Xuebin Ke*, Xingguang Zhang, Jian Zhao, Sarina Sarina, John Barry, and
Huaiyong Zhu*. Selective reductions using visible light photocatalysts of
supported gold nanoparticles. Green Chem. 2013, 15, 236-244.
5. Xuebin Ke*, Xingguang Zhang, Hongwei Liu, Song Xue, and Huaiyong Zhu*.
Efficient catalysts of zeolite nanocrystals grown with a preferred orientation on
nanofibres. Chem. Commun. 2013, 2013, 49, 9866-9868.
6. Xuebin Ke, Sarina Sarina, Jian Zhao, Xingguang Zhang, Jin Chang, and
Huaiyong Zhu*. Tuning the reduction power of supported gold nanoparticle
photocatalysts for selective reductions by manipulating the wavelength of visible
light irradiation. Chem. Commun. 2012, 48, 3509-3511.
vi
Conference presentation:
1. Xingguang Zhang, Xuebin Ke*, and Huaiyong Zhu. Photocatalysts of zeolite
supported gold nanoparticles for selective oxidation of aromatic alcohols to
aldehydes. The 6th
International Conference on Gold Science, Technology, and
its Applications, 2012, Tokyo, Japan
2. Xuebin Ke, Xingguang Zhang, Sarina Sarina, and Huaiyong Zhu*.
Photocatalytic reductions activated by supported gold nanoparticles. The 6th
International Conference on Gold Science, Technology, and its Applications,
2012, Tokyo, Japan
3. Sarina Sarina, Xuebin Ke, Jian Zhao, Xingguang Zhang, and Huaiyong Zhu*.
Contribution of light irradiation to reduction of activation energy in gold
nanoparticle photocatalysed reactions. The 6th
International Conference on Gold
Science, Technology, and its Applications, 2012, Tokyo, Japan
vii
Table of contents
Keywords……………………………………………………………………….……..i
Abstract…………………………………………………………………………….....ii
List of publications…………………………………………………………………...v
Table of contents…………………………………………………………………….vii
List of figures……….…………………………………………………..……………ix
List of abbreviations..…………………………………………………..……………..I
Statement of original authorship……………………………………………………..II
Acknowledgements……………………………………………………………...…..III
Chapter 1: Introduction……………………………………………………….……1
Chapter 2: Literature review……………………………………………….………9
2.1 Plasmonic gold photocatalysts…………...……………………………………….9
2.1.1 Localised surface plasmon resonance……………………………………...…9
2.1.2 Electric near-field enhancement………………………………………….....11
2.1.3 Applications of plasmonic gold photocatalysts………………...…………..12
2.2 Zeolite catalysts……………………………………………………………..…..17
2.2.1 Zeolite solid-acid catalysts………………………………………...…………..17
2.2.2 Zeolite-based photocatalysts……………...……………………………….…..18
2.2.3 Polarised electrostatic fields…………………………………………….…..20
2.2.4 Applications of zeolite catalysts…………………………………………..…..21
2.3 Summary…………………….…………………………………………………..25
Chapter 3 Selective reduction reaction………………………………………...…35
Introductory remarks……………………………………..………………….………35
Article 1: Selective reductions using visible light photocatalysts of supported gold
viii
nanoparticles.....….…………………………………...…..………………….………39
Chapter 4 Selective oxidation reaction…………………………………………...51
Introductory remarks……………………………………..………………….………51
Article 2: Zeolite-supported gold nanoparticles for selective photooxidation of aromatic
alcohols under visible-light irradiation………………...……………...……….………55
Chapter 5 Acetalisation reaction………………………………………………..64
5.1 Acetalisation reaction on Au/zeolite photocatalysts………………………..64
Introductory remarks……………………………………..………………….………64
Article 3: Plasmonic nanostructures to enhance catalytic performance of zeolites under
visible light………….………………………...…………..………………….………69
5.2 Acetalisation reaction on zeolite catalysts…………….………………..……..85
Introductory remarks……………………………………..………………….………85
Article 4: Efficient catalysts of zeolite nanocrystals grown with a preferred orientation on
nanofibres...………………….....…………………………….………………………90
Chapter 6 Conclusion…………………………………………………………...…96
Chapter 7 Limitations and future work…...………………………………...…99
7.1 Limitations and possible solutions…………………………………………....99
7.2 Future work……………………………………………………….............……101
Appendix
Introductory remarks……………….…………………….………………….……107
Article 5: TiO2 nanofibres of different crystal phases for transesterification of alcohols with
dimethyl carbonate …....……………….……………………….…………….…….112
-
ix
List of figures (in Chapter 2: Literature review)
Figures Page
Figure 1. The scheme of the electromagnetic field of light and its
interaction with Au-NPs: A dipole is induced, which oscillates in phase
with the electromagnetic field of the incoming light.
9
Figure 2: The LSPR bands of (a) Au, Ag, and Cu nanoparticles; (b) Ag
nanostructures with different shapes; (c) Ag nanocubes with different sizes;
and (d) Au-Ag alloy with different compositions.
10
Figure 3 The FDTD (finite-difference time-domain) simulation results of
(a) distribution of the enhanced electric field intensity at the LSPR peak
wavelength (420 nm) around a 75 nm Ag nanocube; (b) quantified electric
field intensity as a function of distance, d, along the dashed line indicated
in (a); (c) distribution of the electric field intensity between two 75 nm Ag
nanocubes separated 1 nm away (one cube is rotated 45°); (d) quantified
value of electric field intensity as a function of dash-indicated d in (c).
11
Figure 4: The proposed mechanism of the photoelectrochemical process
on Au/TiO2. Charges are separated at a visible-light-irradiated gold
nanoparticle-TiO2 system.
13
Figure 5. The schematic mechanism of the photocatalytic reduction of
nitroaromatic compounds. Au-H reacts with N-O bonds to form Au-OH
species that subsequently decompose to release dioxygen molecules and
give Au-H species.
16
Figure 6. The mechanism of the acetalisation of cyclohexanone catalysed
by solid acid catalysts (H+).
23
Figure 7: Visible light induces charge transfer between ethane and oxygen
molecules to form a transient ethane radical and a superoxide species (O2-).
24
I
List of abbreviations
NPs: Nanoparticles
NFs: Nanofibres
LSPR: Localised surface plasmon resonance
PEF: Polarised electrostatic fields
ENFE: Electric near-field enhancement
DFT: Density functional theory
VOCs: Volatile organic compounds
TON: Turnover number
TOF: Turnover frequency
XRD: X-ray diffraction
BET: Brunauer-Emmett-Teller
GC: Gas chromatography
MS: Mass spectrometry
IES: FT-IR emission spectroscopy
ATR: Attenuated total reflectance
NMR: Nuclear magnetic resonance spectroscopy
SEM: Scanning electron microscopy
EDS: Energy dispersive X-ray spectroscopy
TEM: Transmission electron microscopy
TG: Thermogravimetric analysis
UV/Vis: Ultraviolet-visible spectra
XPS: X-ray photoelectron spectroscopy
QUT Verified Signature
III
Acknowledgements
I would love to express sincere gratitude and great appreciation to my
supervisors, Dr. Xubin Ke and Prof. Huaiyong Zhu, for their meticulous guidance,
generous support and great patience towards the completion of this work.
Grateful acknowledgements must go to Dr. Zhanfeng Zheng, Dr. Jian Zhao,
Dr. Sarina Sarina, Mr. Qi Xiao, Miss Fathima Sifani Zavahir, Dr. Hongwei Liu, Prof.
Aijun Du, Prof. Xianliang Sheng, Prof. Jianfeng Jia, Prof. Eric Waclawik, Prof.
Jingyi Li and Dr. Juan Yang, for their kind collaboration, advice and valuable
comments and suggestions, particularly for the method of conducting the research.
Sincere thanks also go to the students: Arixin Bo, Yiming Huang, Chao Chen, who
always give me hands in conducting the laboratory work.
My sincere appreciations also extend to Dr. Wayde Martens, Dr. Llew Rintoul,
Dr. Chris Carvalho, Mr. Eric Martinez, Mrs. Leonora Newby, Dr. Peter Hines, Dr.
Thor Böstrom, Dr. Jamie Riches, Dr. Hui Diao, Dr. Tony Raftery, and other
technicians who have provided assistance with instrumentation. Special thanks go to
Dr. Barry Wood (UQ) for the help with the sample characterisation by XPS spectra.
I wish to thank QUT for offering me the full scholarship. Thanks also go to the
Queensland State Government for the Smart Futures Fellowship and the Australian
Research Council (ARC) for the funding of research.
Finally, I would love to thank my family - my parents and my wife, for their
love, support, encouragement and understanding throughout my work.
1
Chapter 1: Introduction
Catalysis plays an indispensable part in materials science, chemical production,
energy storage, and environmental remediation. Conventional heterogeneous
catalysis heavily relies on high operating temperatures because of large activation
energy barriers and thus suffers from numerous negative side effects: low energy
efficiencies for inherent exothermic reactions, quick deactivation of catalytic centres,
poor selectivity for most partial redox reactions, and dangerous operating
conditions[1-3]
.
Photocatalysis offers great promise in its ability to lower reaction temperature
to the ambient degree thus opens new avenues in developing energy-efficient
catalysts to harvest sunlight - the ―green‖ and abundant solar energy. Photocatalysis
is also a promising approach to fulfil the goals of green chemistry which aims at
designing chemical products or processes to reduce or eliminate the use and
generation of hazardous substances. Solar energy is a clean abundant energy source,
in particular, the energy of sunlight incident on the earth is about 10, 000 times more
than the current energy consumption in the world[4]
. However, the light absorption
efficiency of heterogeneous photocatalysts has long been restricting the
photocatalytic capability for commercial availability. For instance, traditional
photocatalysts almost exclusively focus on TiO2-based semiconductors that can acess
only UV light (< 4% of sunlight)[5]
and thus cannot take advantage of visible light
(400-800 nm in wavelength). Visible light constitutes approximately 43% of solar
energy[6]
; therefore, photocatalysts that can harness visible light are highly desirable.
Recent years have seen development of a new family of plasmonic photocatalysts
of supported gold, silver, or copper nanoparticles, a feature of which is the effect of
2
collective and coherent oscillation between the metal’s free conduction electrons and
the incident photons at the surface of NPs due to the localised surface plasmon
resonance (LSPR) irradiated by visible light[7-9]
. This LSPR effect has been applied
to boost catalytic performance for a variety of important organic transformations
under visible light irradiation, particularly, for the oxidation of organic contaminants
and aromatic alcohols[10]
. However, the neglected photoreduction is rarely reported
by researchers. Given that reduction is one of the major processes for the synthesis of
fine chemicals, it will be of great interest if photocatalytic reduction reactions can be
applied to synthesise fine chemicals under visible light irradiation. Currently, reports
on the topic of photocatalytic reduction are sparse, focusing on the reduction of
nitric-aromatics using cadmium sulphide or modified titania as photocatalysts[11]
.
The core issue regarding photocatalytic reduction is to devise efficient photocatalysts
that can catalyse the reduction reactions with superior product selectivity. Hopefully,
plasmonic photocatalysts of supported Au-NPs can catalyse reduction reactions;
therefore, photocatalytic reactions that are driven by sunlight can be developed.
Moreover, supports play a critical role in modifying the catalytic performance of
supported Au-NPs. For instance, zeolites are crystalline aluminosilicates with rigid
microporous structures and well-defined channels at molecular dimensions. The
contribution of zeolites to the catalytic performance of photocatalysts of supported
Au-NPs has not been clarified, even though the mechanism investigation into their
functions for the aromatic alcohol oxidation in thermal reactions has been
examined[12]
. Li and co-workers report that zeolites supported Au and Au-Pd NPs
can catalyse the oxidation of aromatic alcohols[13]
. The reactions are carried out at
100oC and two-bar O2 pressure, but the conversions are very low and side reactions
are observed. Therefore, under visible light irradiation, zeolites supported Au-NPs
3
probably function more efficiently, because the adsorption ability of zeolites supports
can help concentrate reactants from the solvent.
The plasmon-mediated processes fundamentally differ in their catalytic
mechanisms compared with those occuring on traditional semiconductors or with
processes driven merely by thermal energy. Moreover, the LSPR effect of plasmonic
NPs can amplify the electromagnetic field intensity of incident light (|E0|), resulting
in an enhanced electric field (|E|) on the nanometre scale[7, 9]
. This near-field
enhanced interaction is well-known as the ―electric near-field enhancement (ENFE)‖
effect and has motivated numerous theoretical and experimental studies, and
advanced technological applications, such as surface-enhanced Raman scattering[14]
,
sensors[15, 16]
, plasmonic devices[17, 18]
and photovoltaic solar cells[19, 20]
. In
photocatalysis, Ag-NPs covered by the SiO2 shell and embedded in TiO2 particles
have been tried to degrade methyl blue, and better catalytic performance was
observed as a result of the electric near-field amplitude on the surface of Ag-NPs[21]
.
However, the inert SiO2 shell, which is used to prevent the Ag core from being
oxidised, impedes the light absorption efficiency in photocatalysis.
Zeolites are important catalysts themselves and have extensive applications in
catalysis, separation, and adsorption. Besides possessing regular microporous
structures, high surface areas, shape-selectivity, zeolites possess unique solid acidity.
Moreover, the strong polarised electrostatic fields (PEF, about 1-10 V/nm) created by
extra-framework cations have the power to polarise molecules adsorbed on zeolite
surfaces or confined in the porous matrix (e.g., host-guest structures)[22-24]
. In
principle, the PEF can reduce the energy required to facilitate the electron transfer or
to activate reactants, thereby initiating reactions by moderate heating or visible-light
excitation. The charge-transfer properties from hydrocarbons to molecular oxygen
4
(O2) have been investigated on cation-treated zeolites, such as ZSM-5, Y and beta,
with visible light irradiation in the selective oxidisation of toluene, propane,
cyclohexane, and small alkenes[25-27]
. These studies confirm that the PEF of extra-
framework cations can lower the charge-transfer excitation energy required from
hydrocarbons to O2. However, the products cannot be quantitatively measured, which
results from the low visible light absorption efficiency of zeolites. This triggers a
logical speculation that improved catalytic performance can be expected if the PEF
of cations in zeolites are further intensified to a sufficiently large extent.
In this thesis, three promising findings of plasmonic photocatalysts are reported:
firstly, enhanced catalytic performance of supported Au-NPs for the selective
reduction of four types of reduction reactions, in which Au-NPs provide the catalytic
centres and supports make no contribution to catalytic performance (Article 1:
Selective reductions using visible light photocatalysts of supported gold
nanoparticles); secondly, improved catalytic performance of supported Au-NPs for
the selective oxidation of aromatic alcohols to aldehydes, in which Au-NPs provide
the catalytic centres and the zeolite supports contribute to adsorbing reactants
(Article 2: Zeolite-supported gold nanoparticles for selective photooxidation of
aromatic alcohols under visible-light irradiation); thirdly, boosted catalytic
performance of zeolites for acetalisation of aldehydes/ketones by plasmonic effect of
Au-NPs, in which zeolites provide catalytic centres (Article 3: Plasmonic
nanostructures to enhance catalytic performance of zeolites under visible light). In
addition, the acetalisation is also investigated on zeolite-grafted TiO2 nanofibres
under thermal conditions (Article 4: Efficient catalysts of zeolite nanocrystals grown
with a preferred orientation on nanofibres), showing that the transformation between
aromatic alcohols and dimethyl carbonate can occur on pure TiO2 nanofibres without
5
zeolite nanocrystals. Therefore, the study of ―transesterification of alcohols on TiO2
nanofibres with different crystal phases‖ is also performed as a periphery study and
attached in the ―Appendix‖ section (Article 5: Selective catalysis of alcohols with
dimethyl carbonate using TiO2 nanofibres of different crystal phases).
In Chapter 2 (Literature Review), the theoretical background, the recent
application of plasmonic gold photocatalysts and zeolite catalysts in organic
conversions, and the future development of these fields are summarised to provide an
outline of the scientific novelty and significance of this research program.
References
1. A. Wittstock, V. Zielasek, J. Biener, C. M. Friend, and M. Bäumer,
―Nanoporous gold catalysts for selective gas-phase oxidative coupling of
methanol at low temperature,‖ Science 327, 319-322 (2010).
2. C. T. Campbell, S. C. Parker, and D. E. Starr, ―The effect of size-dependent
nanoparticle energetics on catalyst sintering,‖ Science 298, 811-814 (2002).
3. Y. Lei, F. Mehmood, S. Lee, J. Greeley, B. Lee, S. Seifert, R. E. Winans, J. W.
Elam, R. J. Meyer, P. C. Redfern, D. Teschner, R. Schlögl, M. J. Pellin, L.A.
Curtiss, and S. Vajda, ―Increased silver activity for direct propylene epoxidation
via subnanometre size effects,‖ Science 328, 224-228 (2010).
4. H. Garcia, and H. D. Roth, ―Generation and reactions of organic radical cations
in zeolites,‖ Chem. Rev. 102, 3947-4008 (2002).
5. A. Fujishima, and K. Honder, ―Electrochemical photolysis of water at a
semiconductor electrode,‖ Nature 238, 37-38 (1972).
6. Z. G. Zou, J. H. Ye, K. Sayama, and H. Arakawa, ―Direct splitting of water
under visible light irradiation with an oxide semiconductor photocatalyst,‖
Nature 414: 625-627 (2001).
6
7. K. Watanabe, D. Menzel, N. Nilius, and H.-J. Freund, ―Gold supported on thin
oxide films: from single atoms to nanoparticles,‖ Chem. Rev. 106, 4301-4320
(2006).
8. S. Linic, P. Christopher, and D. B. Ingram, ―Plasmonic-metal nanostructures for
efficient conversion of solar to chemical energy,‖ Nat. Mater. 10, 911-921
(2011).
9. M. A. El-Sayed, ―Some interesting properties of metals confined in time and
nanometre space of different shapes,‖ Acc. Chem. Res. 34, 257-264 (2001).
10. X. Chen, H. Y. Zhu, J. C. Zhao, Z. F. Zheng, and X. P. Gao, ―Reduction of
nitroaromatic compounds on supported gold nanoparticles by visible and
ultraviolet light,‖ Angew. Chem. Int. Ed. 47, 5353-5356 (2008).
11. B. Pal, T. Torimoto, K. Okazaki, and B. Ohtani, ―Photocatalytic syntheses of
azoxybenzene by visible light irradiation of silica-coated cadmium sulfide
nanocomposites,‖ Chem. Commun. 483-485 (2007).
12. M. Zahmakiran, and S. Ozkar, ―The preparation and characterisation of gold(0)
nanoclusters stabilised by zeolite framework: highly active, selective and
reusable catalyst in aerobic oxidation of benzyl alcohol,‖ Mater. Chem. Phys.
121, 359-363 (2010).
13. G. Li, D. I. Enache, J. Edwards, A. F. Carley, D. W. Knight, and G. J.
Hutchings, ―Solvent-free oxidation of benzyl alcohol with oxygen using zeolite-
supported Au and Au–Pd catalysts,‖ Catal. Lett. 110, 7-13 (2006).
14. S. Nie, and S. R. Emory, ―Probing single molecules and single nanoparticles by
surface-enhanced raman scattering,‖ Science 275, 1102-1106 (1997).
7
15. L. Tang, S. K. Kocabas, S. Latif, A. K. Okyay, D.-S. Ly-Gagnon, K. C. Saraswat,
and D. A. B. Miller, ―Nanometre-scale germanium photodetector enhanced by a
near-infrared dipole antenna,‖ Nat. Photonics 2, 226-229 (2008).
16. X. B. Xu, K. Kim, H. F. Li, and D. L. Fan, ―Ordered arrays of Raman
nanosensors for ultrasensitive and location predictable biochemical detection,‖
Adv. Mater. 24, 5457-5463 (2012).
17. S. A. Maier, P. G. Kik, H. A. Atwater, S. Meltzer, E. Harel, B. E. Koel, and A. A.
G. Requicha, ―Local detection of electromagnetic energy transport below the
diffraction limit in metal nanoparticle plasmon waveguides,‖ Nat. Mater. 2, 229-
232 (2003).
18. R. A. Shelby, D. R. Smith, and S. Schultz, ―Experimental Verification of a
Negative Index of Refraction,‖ Science 292, 77-79 (2001).
19. Q. Q. Gan, F. J. Bartoli, and Z. H. Kafafi, ―Plasmonic-enhanced organic
photovoltaics: breaking the 10% efficiency barrier,‖ Adv. Mater. 25, 2385-2396
(2013).
20. M. Gu, Z. Ouyang, B. H. Jia, N. Stokes, X. Chen, N. Fahim, X. P. Li, M. J.
Ventura, and Z. R. Shi, ―Nanoplasmonics: a frontier of photovoltaic solar cells,‖
Nanophotonics 1, 235-248 (2012).
21. K. Awazu, M. Fujimaki, C. Rockstuhl, J. Tominaga, H. Murakami, Y. Ohki, N.
Yoshida, and T. Watanabe, ―A plasmonic photocatalyst consisting of silver
nanoparticles embedded in titanium dioxide,‖ J. Am. Chem. Soc. 130, 1676-
1680 (2008).
22. S. Bordiga, E. Garrone, C. Lamberti, and A. Zecchina, ―Comparative IR-
spectroscopic study of low-temperature H2 and CO adsorption on Na zeolites,‖ J.
Chem. Soc. Faraday Trans. 90, 3367-3372 (1994).
8
23. Y. Xiang, S. C. Larsen, and V. H. Grassian, ―Photooxidation of 1-alkenes in
zeolites: a study of the factors that influence product selectivity and formation,‖
J. Am. Chem. Soc. 121, 5063-5072 (1999).
24. K. Tsutsumi, and H. Takahashi, ―A study of the nature of active sites on zeolites
by the measurement of heat of immersion. II. effects of silica/alumina ratio to
electrostatic-field strength of calcium-exchanged zeolites,‖ J. Phys. Chem. 76,
110-115 (1972).
25. H. Sun, F. Blatter, and H. Frei, ―Cyclohexanone from cyclohexane and O2 in a
zeolite under visible light with complete selectivity,‖ J. Am. Chem. Soc. 118,
6873-6879 (1996).
26. F. Blatter, and H. Frei, ―Selective photooxidation of small alkenes by O2 with red
light in zeolite Y,‖ J. Am. Chem. Soc. 116, 1812-1820 (1994).
27. H. Frei, ―Selective hydrocarbon oxidation in zeolites,‖ Science 313, 309-310
(2006).
9
Chapter 2: Literature review
2.1 Plasmonic gold photocatalysts
2.1.1 Localised surface plasmon resonance
Materials in the size of nanometre scale (nanomaterials) can exhibit very different
physicochemical properties from bulky ones. Plasmonic metal nanostructures
generally refer to nanomaterials of gold, silver, and copper nanoparticles, nanorods,
nanowires, and nanocubes, because they can strongly interact with the incident light
owing to the localised surface plasmon resonance (LSPR) effect[1-3]
. To illustrate, the
electromagnetic field of incident light can cause the free electrons in gold
nanoparticles (Au-NPs) to oscillate. As the front wave of visible light passes, the
electron density in the Au-NPs are polarised to one side of the surfaces, and the free
conduction electrons collectively and coherently oscillate in resonance with the
light’s frequency, causing a dynamic dipole oscillator, as shown in Figure 1.
Figure 1. The scheme of the electromagnetic field of visible light and its interaction with Au-
NPs: A dipole oscillator is induced, which resonates in phase with the electromagnetic field
of the incoming visible light.
Visible light usually undergoes intraband LSPR absorption (electrons in 6sp
band), which is different from interband absorption irradiated by ultraviolet light
(electrons oscillate from 5d to 6sp)[4]
. These energetic electrons may return to their
Electric field
Magnetic field
Visible light
Electron clouds
Au(δ+-δ-)
dipole oscillator -
E
-
- - -
+ + +
+ + +
- -
+
10
thermal equilibrium states and release heat to the lattice and the surrounding media,
or can be grabbed by reactants to reduce them to initiate chemical reactions.
If the size, shape, and surrounding materials of the Au-NPs change, then the
electric field density of the surface of Au-NPs changes, leading to a change in the
oscillation frequency of electrons and in the LSPR peak positions. For instance, the
free conduction electrons in Au-NPs can readily travel through the material, where
the mean free path is about 50 nm. If the size of Au-NPs prepared is smaller than this
dimension, then no scattering occurs from the gold bulk, and all interactions are on
the gold surfaces. In general, if the size of Au-NPs produced by chemical reduction
of gold salts are smaller than half the wavelength of the incident light, then they can
exhibit the LSPR effect[3]
. Moreover, gold, silver, and copper NPs and their alloys
show different LSPR peak positions, as given in Figure 2. All these properties afford
a variety of adjustable photocatalytic performance of plasmonic nanostructures.
Figure 2: LSPR bands of (a) Au, Ag, and Cu nanoparticles; (b) Ag nanostructures with
different shapes; (c) Ag nanocubes with different sizes; and (d) Au-Ag alloy with different
compositions. Sets (a)-(c) are reproduced from Ref 2, and the set (d) is from Ref 5.
11
2.1.2 Electric near-field enhancement
An important characteristic of the LSPR effect of Au-NPs is that it can amplify
the electromagnetic field intensity of incident light (|E0|) and results in an enhanced
electric field (|E|) on the nanometre scale. This LSPR-induced near-field interaction
is called ―electric near-field enhancement‖ (ENFE). This enhancement effect is
affected by the spatially non-homogeneous distribution of plasmons on NPs and
attenuates exponentially within the spacing range of 10 - 50 nanometres away from
the metal surfaces, relying on the size, shape, and dielectric environments[2]
. The
near-field enhancement factor (|E|/|E0|) is as large as 103 at the surface of individual
NPs, whereas it can reach 106 at the junction of interparticles, as shown in Figure 3
with Ag-NPs being examples[2, 6]
.
Figure 3 FDTD (finite-difference time-domain) simulation results of (a) distribution of the
enhanced electric field intensity at the LSPR peak wavelength (420 nm) around a 75 nm Ag
nanocube; (b) quantified electric field intensity as a function of distance, d, along the dashed
line indicated in (a); (c) distribution of the electric field intensity between two 75 nm Ag
nanocubes separated 1 nm away (one cube is rotated 45°); (d) quantified value of electric
field intensity as a function of dash-indicated d in (c). Reproduced from Ref 2.
12
The nano-gap regions where the maximum ENFE occurs are referred to as ―hot
spots‖, playing a critical role in modifying the physiochemical, optical, and reactive
properties of supports. Thus, the enhancement effect has been successfully applied in
surface-enhanced Raman scattering (SERS), sensitive photodetection[7]
, heat-assisted
magnetic recording[8]
, and photovoltaic solar cells[9]
. In photocatalysis, Awazu and
co-workers embed Ag-NPs in TiO2 particles to degrade the methyl blue, showing
that the electric near-field amplitude on the surface of Ag-NPs affords better catalytic
performance[10]
.
2.1.3 Applications of plasmonic gold photocatalysts
The unique capacity of plasmonic nanostructures to activate molecules by photo-
excited electron clouds, by electric near-field enhancement, by scattering
electromagnetic radiation, or by converting the energy of photons into heat, makes
them suitable for various applications. The applications include fluorescence[11]
,
enhanced Rayleigh (Mie) scattering[12]
, SERS[13]
, water splitting[14]
, degradation of
dye pollutants[15]
, and organic photovoltaics[9]
. Particularly, they can be applied in
the organic conversions that play a critical role in the chemical industry to produce
important precursors/intermediates (e.g., carbonyl compounds of aldehydes/ketones
oxidised from alcohols) for the synthesis of drugs, vitamins, and fragrances. Here the
main focus of the applications of plasmonic gold photocatalysts in this section is the
redox reactions either driven, or enhanced by visible light on plasmonic
photocatalysts of supported Au-NPs.
(1) Selective oxidation reactions
Many studies have been devoted to the mild oxidation ability of supported Au-
NPs, such as thiol to disulfide[16]
, methanol to formic acid[17]
, ethanol to acetic
acid[17]
, isopropanol to acetone[18]
, benzyl alcohol to benzaldehyde[19]
and benzene to
13
phenol[20]
. In contrast to only thermal-energy-driven oxidation with unselective
processes, high selectivity can be obtained under ambient conditions in
photocatalysis.
Among these oxidation reactions, the selective aerobic oxidation of alcohols to
carbonyl compounds with O2 has received attention from the perspective of green
chemistry, particularly on the plasmonic photocatalysts. An early study on the
oxidation of alcohols was Tian and co-workers’ report[17]
, which investigated the
oxidation of methanol and ethanol on Au/TiO2 photocatalysts under visible light
irradiation. The authors stated that the Au-NPs were photoexcited to form the
energetic electrons that were transferred to the TiO2 conduction band. Then
compensating electrons captured from a donor (e.g., Fe2+
Fe3+
) in the solution
transferred to Au-NPs. They also predicted that this system could be potentially
applied in photovoltaic fuel cells. The general mechanism is illustrated in Figure 4.
Figure 4: The proposed mechanism of the photoelectrochemical process on Au/TiO2.
Charges are separated at a visible-light-irradiated gold nanoparticle-TiO2 system.
Reproduced from Ref 17.
On the basis of this system, Naya and co-workers designed heterosupramolecular
photocatalysts consisting of Au/TiO2 and cationic surfactant admicelles. Such
photocatalysts exhibited high activity for the chemoselective oxidation of cinnamyl
alcohol to cinnamaldehyde under visible light irradiation. The authors also
14
demonstrated that the LSPR effect triggered the electron transfer from Au-NPs to
TiO2[16]
. In addition, a recent study on the oxidation of aromatic alcohols on Au-NPs
loaded on the interface of anatase/rutile particles also derived a similar mechanism
whereby Au-NPs located at the anatase/rutile interface facilitated an efficient
electron transfer to TiO2 under visible light irradiation[19]
. All the above-mentioned
studies indicate that TiO2 supports play an essential role in the oxidation of alcohols
under visible light irradiation because of the charge separation and electron transfer
processes, which involve the participation of the electron-hole pairs in TiO2.
However, the aforementioned studies ignore that the Au-NPs themselves are also
efficient photocatalytic materials. For instance, Chen and co-workers’s study
demonstrated that the oxidation of volatile organic contaminants (VOCs), including
CO, CH3OH and HCHO, proceeded effectively on the photocatalysts of Au/ZrO2,
Au/SiO2, and Au/Y zeolite[4, 21]
without using TiO2 photocatalysts. ZrO2 and SiO2
powders were chosen as supports because their band gaps (ca. 5.0 eV and ca. 9.0 eV,
respectively[22]
) are much larger than the energies of photons of visible light (less
than 3.0 eV). It is impossible for the Au-NPs to narrow the band gaps of them
enough for visible light photons to be absorbed or to excite electrons in them.
Therefore, the catalytic activity of these photocatalysts is not caused by the same
mechanism which occurs on semiconductor (TiO2) photocatalysts, but by the LSPR
effect of Au-NPs instead. This phenomenon also applies to other photocatalytic
systems. For instance, plasmonic photocatalysts Au/CeO2 were found to be efficient
for the selective oxidation of aromatic alcohols to aldehydes/ketones in aqueous
suspensions under the irradiation of LED green light[23]
. Au/CeO2 photocatalysts
exhibited high chemoselectivity both in the selective oxidation of aminobenzyl
alcohol (benzyl alcohol with an amino group) to aminobenzaldehyde and in the
15
intermolecular selective oxidation of benzyl alcohol to benzaldehyde in the presence
of aniline. This discovery also confirms that the photocatalytic performance of
Au/CeO2 originates from the LSPR effect of Au-NPs.
(2) Selective reduction reactions
Compared with the selective oxidation processes, the selective reduction reactions
are rarely seen in reports, probably because of the strong ability of Au-NPs to adsorb
and activate O2, thus necessitating the removal of O2 from the reaction system[24]
.
Nevertheless, the unique photocatalytic performance of Au-NPs can always motivate
scientists to explore more applications of plasmonic gold photocatalysts. Zhu and co-
workers found that Au/ZrO2 (3wt%) exhibited high performance in reducing
nitrobenzenes to azobenzene compounds. The overall photocatalytic reaction process
is described as the following[25]
:
8 Ph-NO2 + 2 CH3-CH(OH)-CH3 + Au-NPs
4 Ph-N=N-Ph + 2 CH3-C(=O)-CH3 +2 Au-H + 2 Au-OH +7 O2
As shown in Figure 5, photoexcited Au-NPs can grab hydrogen from the solvent,
isopropyl alcohol, to form Au-H species, in which KOH can assist the abstraction of
the hydrogen atom from isopropyl alcohol. Next, the key step is the cleavage of the
N-O bonds. Under visible light irradiation, the energetic electrons on Au-NPs
induced by the LSPR effect interact strongly with the electrophilic nitro groups of
nitrobenzene, thereby facilitating the breakage of the N-O bonds by Au-H species.
The resulting Au-H species subsequently decompose to give O2 and Au-H species.
Azobenzene is formed as the intermediate in the thermal hydrogenation of
nitrobenzene. This study demonstrated that it is possible to directly transform an
unstable intermediate in a thermal reaction to the wanted product by a photocatalytic
16
process and highlights that the plasmonic Au-NPs can complete all these processes
without the participation of catalyst supports.
Figure 5. The schematic mechanism of the photocatalytic reduction of nitroaromatic
compounds. Au-H species react with N-O bonds to form Au-OH species that subsequently
decompose to release dioxygen molecules and give Au-H species. Reproduced from Ref 25.
On the other hand, Au-NPs supported on TiO2 perform differently. Tanaka and
co-workers report that Au/TiO2 can photocatalytically reduce nitrobenzene to aniline
in the isopropanol suspension under visible light irradiation. The whole process is as
the following[26]
:
Ph-NO2 + 3 CH3-CH(OH)-CH3 Ph-NH2 + 3 CH3-C(=O)-CH3 +2 H2O
They found that the photocatalytic performance (reaction rate and stoichiometry)
was considerably enhanced by functionalisation of Au/TiO2 with Ag-NPs as a co-
catalyst. Ag-free Au/TiO2 sample showed a much lower reaction rate of nitrobenzene
consumption and aniline formation, compared with the Au/TiO2-Ag sample, and this
was probably because the energetic electrons tended to accumulate in the TiO2
particles because of the relatively large rate of hole scavenging by isopropanol. This
process affected the formation of Au-H species that were critical intermediates to
interact with the N-O bonds of nitrobenzene[25]
.
17
All these studies demonstrate that the selective redox reactions can proceed
effectively on plasmonic photocatalysts. Therefore, it should be scientifically
innovative and practically significant to explore more applications of plasmonic
photocatalysts, especially combined with traditional catalysts, such as zeolite solid-
acid catalysts, in other organic conversions.
2.2 Zeolite catalysts
Zeolites are crystalline aluminosilicates with regular porous structures of
molecular dimensions, high surface areas, shape selectivity, and strong adsorptivity,
widely applied in catalysis, separation, adsorption, and ion-exchange. Here the main
focus will concentrate on the solid-acidic properties of zeolites as catalysts in the
acetalisation reactions and the photochemical properties of zeolites as photocatalysts
in the oxidation of hydrocarbons.
2.2.1 Zeolite solid-acid catalysts
Zeolites possess an abundance of Brønsted and Lewis acid sites. The Brønsted
acid sites play a critical role in numerous organic conversions, and the acidity is
influenced by several factors, including the density/concentration, strength,
distribution and location of acid sites[27]
.
The generation of Brønsted solid acidity is related to the terminal and bridging
silanols on the zeolite surfaces, which can be introduced by several approaches.
Firstly, ion-exchange of sodium-form zeolites by ammonium salts followed by
calcinations: NH4+ + Na
+-zeolite NH4
+-zeolite + Na
+ H
+-zeolite + Na
+ + NH3
(the direct ion-exchange of zeolites with mineral acids (e.g., HCl) is unfavoured,
because it damages the zeolite framework by dealumination or even leads to
complete collapse). Secondly, water molecules are adsorbed and electrically
18
polarised owing to the presence of polarised electrostatic fields of the extra-
framework cations, this process helps form bridging hydroxyl groups (Si-O(H)-Al) to
provide Brønsted acid sites (H+): M
n+ + n(T-O-T) + nH2O M(OH)n + n(T-O(H
+)-
T)[28]
. Terminal silanol Si(OH) and extra lattice Al(OH) hydroxyl groups also serve
as weaker Brønsted acid sites and have been investigated in several studies by the
solid-sate IR and 1H-NMR spectroscopy
[29, 30]. In solution, the Brønsted acid sites can
be detected by the colorimetric method that is based on the difference in the
electronic absorption properties of neutral and cationic forms of probe molecules,
such as retinol and retinyl Schiff base. The density of Brønsted acid sites in a given
zeolite host is related to the framework Al sites, and thus a full understanding of
zeolite acidity would involve a detailed analysis of the precise location of the
catalytic centres. For instance, whether they are on external surfaces or inside pores,
whether they are in large pores or small cavities, and whether they are evenly
distributed or concentrated. An increasing number of reports are emerging[31, 32]
, and
given the importance of Brønsted acidity of zeolites, its exploration remains a hot
and important field in the foreseeable future.
2.2.2 Zeolite-based photocatalysts
In recent years, interest has arisen in the employment of zeolites in
photochemistry for several reasons[33, 34]
:
(a) Full photochemical stability, large thermal and chemical inertness, and
transparency to UV/Vis radiations above 240 nm, allow a certain percent of the
excitation light to get into the opaque solid powders and reach the channels and
cages.
(b) Ability of the zeolite framework to actively participate in electron transfer
processes as an either electron acceptor or electron donor[35]
.
19
(c) The possibility of altering the chemical composition of the framework and
surface charges allows the introduction of active sites that make these molecular
sieves photoactive. For instance, one can synthesise zeolites to make them have
photocatalytic activity by incorporation of heteroatoms into the framework, such as
Ti rather than Si or Al.
(d) Property of ion-exchange to change non-framework positions. The net
negative charges on the aluminosilicate framework are balanced by counter ions like
Na+, K
+ or other alkali and alkaline earth metal ions. These counter ions introduced
in the pores play a very important role in introducing photocatalytic properties and
can be readily exchanged by noble or transitional metal ions, providing an
opportunity for modifying the photocatalytic property of zeolites.
(e) Ability of accommodating photoactive guests within the internal voids of
zeolite pores. For instance, semiconductor-incorporated zeolites[36]
, have gained great
importance as potential photocatalysts. Such assembly of multi-component host-
guest systems mainly constitute antenna and relays of natural photosynthetic centres,
including inorganic metal oxide clusters and organic electron-transfer
photosensitisers, since the guest becomes significantly stabilised by incorporation.
(f) High adsorptive ability of zeolites for organic compounds in solution, which
can concentrate reagents in the proximity of the photosensitiser. This strong
adsorptivity contributes to the success of the photocatalytic reactions[37]
. In some
cases, the photosensitiser absorbs light and reaches an excited state, and this state
offers the potential to transfer energy to substrates; hence, the substrates become
electronically excited even if the substrates have not directly absorbed light.
(g) Amphoteric properties which means the co-existence of acid and basic sites.
The three coordinated aluminium sites on the framework and non-framework
20
aluminium sites are normally considered to be Lewis acid sites. Additionally, charge
compensating cations present in the pores of zeolite act as Lewis acids, and the
framework oxygen represents a base. In particular, the oxygen atoms adjacent to Al
(Si–O–Al oxygen) are more basic because of a larger negative charge on the oxygen.
The Lewis acidity is connected to the electron-accepting property and the Lewis
basicity to the electron donating property[34]
.
(h) Modulation of the micropolarity and the polarising strength of zeolite interior
by varying the nature of internal charge balancing cations (charge density) and the
size of channels. The latter factor can lead to dramatic changes and modifications in
the electronic states and conformational mobility of guests within zeolites[38]
.
All these unique characteristics make zeolite-based materials attractive to
scientists in the field of photocatalysis. Particularly, the polarised electrostatic fields
in the proximity of extra-framework cations play a critical role in activating
molecules adsorbed on surfaces, or encapsulated within cavities. This could provide
an opportunity to work cooperatively with the plasmonic Au-NPs because of their
dynamic dipole oscillators induced by the LSPR effect.
2.2.3 Polarised electrostatic field of extra-framework cations in zeolites
Zeolite frameworks feature T-O-T bonds, of which T refers to Si, Al, or other
heteroatoms (no Al-O-Al sequences according to the Loewenstein rule[39]
), and the
T-O-T bonds constitute tetrahedra of [SiO4]4-
and [AlO4]5-
. Isomorphous substitution
of Si with Al creates negative charges on the oxygens of framework and requires
charge-balanced protons or cations of Na+ or K
+ that can be ion-exchanged by other
cations, such as Ag+, Ca
2+ and Ce
3+. Compared with the well-understood mechanism
of reactions catalysed by Brønsted acid sites, the function of extra-framework cations
remains a topic of debate, particularly regarding the polarised electrostatic fields in
21
the vicinity of them (in general, 1-10 V/nm[40]
). In principle, the polarised
electrostatic fields can polarise molecules confined in the microporous matrix (e.g.,
host-guest structures). This could activate adsorbed molecules to initiate reactions
under mild heating or visible light irradiation conditions. In some reports, extra
electrostatic fields have been found to affect the conformational change of flexible
molecules, thus leading to the change in the molecular polarity[41]
. In weak
electrostatic fields compared to the intramolecular fields on the order of volts per
angstrom (V/Å), atoms and molecules can be polarised to form an electrostatic field-
induced dipole moment and a gain in energy; hence, new pathways in chemical
reactions may be established. A study shows that the extra electrostatic field of 12-15
V/nm obviously helps activate the reactants of CO/O2 and enhances the oxidation
process on small gold crystals (20-30 nm). This effect is considered to be associated
with the formation of partially charged gold surfaces induced by the extra
electrostatic field[42]
.
Given the importance of molecular polarity in controlling molecular behaviour
and chemical reactions[43]
, if photocatalysts can modify the molecular polarities, for
instance, by providing a strong electrostatic field, they should offer great promise in
terms of manipulating their photocatalytic performance. Therefore, it is reasonable to
speculate that the electrostatic fields around dipole oscillators of Au-NPs, denoted as
Au(δ+-δ-)
, and the electric near-field enhancement may intensify the polarised
electrostatic fields of zeolites to afford a stronger electrostatic field that can directly
enhance the molecular polarities to improve their reaction rate.
2.2.4 Applications of zeolite catalysts
(1) As solid-acid catalysts for acetalisation reactions
22
Protection of the carbonyl groups is an important technique in multi-step
organic synthesis and can be achieved by employing several types of reagents:
alcohols, diols, orthoesters, oxiranes, or acetals[44]
. Among these, the acetalisation of
aldehydes/ketones with alcohols is a primary step, because products of acetals/ketals
have higher stability towards strong bases or oxidants, Grignard reagent, lithium
aluminium hydride, and esterification reagents[45]
. Moreover, acetals have found
direct applications as fragrances in cosmetics, as additives in food and beverage
industry, and as pharmaceuticals in synthesising enantiometrically pure
compounds[46]
.
The acetalisation is traditionally catalysed by strong/intermediate Brønsted or
Lewis acids, such as HCl, H2SO4, ZnCl2, FeCl3 and p-toluene sulphonic acid[47, 48]
.
These processes involve expensive reagents, tedious work-up procedure,
neutralisation of the strongly acidic media, and production of harmful wastes. These
are disadvantages that make these processes inefficient and uneconomical.
Consequently, there is a demand for environmentally-friendly acid catalysts to
synthesise acetals/ketals under mild conditions. Heterogeneous catalysts offer
promise in these syntheses owing to their ease of separation, high purity,
recyclability, and reusability. Different heterogeneous solid-acid catalysts have been-
developed, such as montmorillonite clay[49]
, sulphated zirconia (SO42-
/ZrO2) and
sulphated titania (SO42-
/TiO2)[50]
. Zeolites are important solid-acid catalysts and
perform efficiently in acetalisation reactions. For example, Al-MCM-41 is for the
acetalisation of cyclohexanone with methanol, ethylene glycol; and pentaerythritol[51]
cation-treated Y zeoiltes are for the acetalisation of cyclohexanone, acetophenone,
and benzophenone with methanol[52]
. The mechanism of the acetalisation of
23
aldehydes/ketones is generally recognised to be the Brønsted-acid catalysed process,
such as the acetalisation of cyclohexanone with methanol, as illustrated in Figure 6.
Despite the obvious advantages that zeolte catalysts have, the catalytic activity
is still not very high and requires elevated operating temperatures and long reaction
times. Thus, optimisation of these processes remains under investigation.
Figure 6. General mechanism of the acetalisation of cyclohexanone catalysed by solid-acid
catalysts (H+). Reproduced from Ref 58.
(2) As photocatalysts for oxidation of hydrocarbons
Partially oxidised hydrocarbons are important building blocks of synthetic fibres
and plastics, and intermediates for manufacturing chemicals[53]
. The present partial
oxidation processes involve O2 which is the best oxidant commercially because of
the very large scale of these processes. Most hydrocarbon merchants give rise to a
wide range of oxidised products because of the high operating temperature; thus,
large amounts of energy are spent on separation of the desired product from side
products. Simultaneously this causes a heavy environmental burden[54]
.
Zeolite photocatalysts hold great promise in the partial oxidation of hydrocarbons,
such as small alkanes, alkenes and aromatics. Hydrocarbons and O2 can be activated
when a gas mixture is loaded into zeolite cages under visible light irradiation[55]
. The
critical oxidation components in this system are extra-framework alkali or alkaline-
earth cations in the zeolites. The highly polarised electrostatic fields in the vicinity of
24
these cations (see Figure 7)[53]
may reduce the activation energy required to activate
hydrocarbon-oxygen charge transfer.
Figure 7: Visible light induces charge transfer between ethane and oxygen molecules to
form a transient ethane radical and the superoxide species (O2-). Reproduced from Ref 53.
Xu and co-workers report that the zeolite Y with different contents of Ca2+
cations
can activate propane oxidation to produce acetone under mild heating[56]
. The
oxidation rate improved considerably when the content of Ca2+
cations increased,
demonstrating that the reaction required hydrocarbon-oxygen encounters in locations
of the high electrostatic fields that are close to the Ca2+
cations. The authors proposed
a mechanism that once charge transfer occurred, the highly acidic hydrocarbon
radical cations are ready to transfer a proton to O2 to form a hydroperoxide molecule
through coupling of the alkyl and HOO* radicals. A water molecule is eliminated
during this process to yield the desired carbonyl product. For the selective oxidation
of ethane (an attractive reaction for commercial use due to the mild C-H bond
activation, see the Figure 7), the intermediate is ethyl hydroperoxide, and the final
product is acetaldehyde. Another reaction accessible by this system is the oxidation
of toluene to benzaldehyde by O2, and this reaction remains a great challenge. Sun
and co-workers tried barium(2+)- and calcium(2+)-exchanged zeolite Y under the
visible light irradiation[57]
; however, like photooxidation of other hydrocarbons, the
products could not be quantitatively measured. The poor yield was primarily due to
25
the low visible light absorption efficiency of zeolites. Therefore, more efforts are
needed to optimise the oxidation of hydrocarbons on zeolite photocatalysts under the
visible light irradiation.
2.3 Summary
These reports mentioned in the literature review demonstrate that plasmonic
nanostructures, particularly Au-NPs, are effective photocatalysts in the selective
oxidation and the selective reduction under visible light irradiation. Their adjustable
size, shape, and their alloys of Ag, Cu, Pt, and Pd, particularly the LSPR effect and
the electric near-field enhancement, make them attractive not only for chemical
production, but also for plasmonic devices, photovoltaic cells, and detectors.
Supports of gold photocatalysts such as zeolites are a class of well-known solid-acid
catalysts that possess strong adsorptivity, singular shape-selectivity, and unique
polarised electrostatic fields near extra-framework cations. Wide applications are
envisaged for these materials in adsorption, separation, ion-exchange, and catalysis.
In catalysis, for instance, the solid-acid catalysed acetalisation of aldehydes/ketones
to acetals/ketals is an important organic transformation to protect carbonyl groups in
multi-step organic synthesis. Zeolite solid-acid catalysts are considered to be ideal
substitutes for liquid-acid catalysts for their ease of separation, minimal waste, and
their reusability. Plasmonic photocatalysts of Au/zeolites offer a great potential to
achieve acetalisation in a photocatalytic way at ambient conditions, thus saving non-
renewable energy. An investigation into the mechanism of these photocatalytic
systems is expected to provide insights into understanding the light-material
interaction mechanism and to promote development of novel photocatalysts for other
important reactions either driven, or enhanced by visible light irradiation.
26
These properties of plasmonic photocatalysts afford a great promise for their
applications in a wide range, such as in materials science, production of fine
chemicals, energy storage, and environmental remediation. Research achievements
on plasmonic photocatalysts may eventually help develop efficient commercial
photocatalysts that can take advantage of sunlight, the most abundant and ―green‖
energy in the world.
References
1. S. Eustis, and M. A. EI-Sayed, ―Why gold nanoparticles are more precious than
pretty gold: noble metal surface plasmon resonance and its enhancement of the
radiative and nonradiative properties of nanocrystals of different shapes,‖ Chem.
Soc. Rev. 35, 209-217 (2006).
2. S. Linic, P. Christopher, and D. B. Ingram, ―Plasmonic-metal nanostructures for
efficient conversion of solar to chemical energy,‖ Nat. Mater. 10, 911-921
(2011).
3. P. Orfanides, T. F. Buckner, and M. C. Buncick, ―Demonstration of surface
plasmons in metal island films and the effect of the surrounding medium-An
undergraduate experiment,‖ Am. J. Phys. 68, 936-942 (2000).
4. H. Y. Zhu, X. Chen, Z. F. Zheng, X. B. Ke, E. Jaatinen, and J. C. Zhao,
―Mechanism of supported gold nanoparticles as photocatalysts under ultraviolet
and visible light irradiation,‖ Chem. Commun. 7524-7526 (2009).
5. M. S. Shore, J. W. Wang, A. C. Johnston-Peck, A. L. Oldenburg, and Joseph B.
Tracy, ―Synthesis of Au(core)/Ag(shell) nanoparticles and their conversion to
AuAg alloy nanoparticles,‖ small, 7, 230-234 (2011).
6. L. Gunnarsson, T. Rindzevicius, J. Prikulis, B. Kasemo, M. Käll, S. Zou, and G.
C. Schatz, ―Confined plasmons in nanofabricated single silver particle pairs:
27
experimental observations of strong interparticle interactions,‖ J. Phys. Chem. B
109, 1079-1087 (2005).
7. L. Tang, S. K. Kocabas, S. Latif, A. K. Okyay, D.-S. Ly-Gagnon, K. C.
Saraswat, and D. A. B. Miller, ―Nanometre-scale germanium photodetector
enhanced by a near-infrared dipole antenna,‖ Nat. Photonics, 2, 226-229 (2008).
8. W. A. Challener, C. B. Peng, A. V. Itagi, D. Karns, W. Peng, Y. G. Peng, X. M.
Yang, X. b. Zhu, N. J. Gokemeijer, Y.-T. Hsia, G. Ju, R. E. Rottmayer, M. A.
Seigler, and E. C. Gage, ―Heat-assisted magenetic recording by a near field
transducer with efficient optical energy transfer,‖ Nat. Photonics 3, 220-224
(2009).
9. Q. Q. Gan, F. J. Bartoli, and Z. H. Kafafi, ―Plasmonic-enhanced organic
photovoltaics: breaking the 10% efficiency barrier,‖ Adv. Mater. 25, 2385-2396
(2013).
10. K. Awazu, M. Fujimaki, C. Rockstuhl, J. Tominaga, H. Murakami, Y. Ohki, N.
Yoshida, and T. Watanabe, ―A plasmonic photocatalyst consisting of silver
nanoparticles embedded in titanium dioxide,‖ J. Am. Chem. Soc. 130, 1676-
1680 (2008).
11. J. Zheng, C. Zhang, and R. M. Dickson, ―Highly fluorescent, water-soluble,
size-tunable gold quantum dots,‖ Phys. Rev. Lett. 93, 077402(1-4) (2004).
12. I. H. El-Sayed, X. Huang, and M. A. El-Sayed, ―Surface plasmon resonance
scattering and absorption of anti-EGFR antibody conjugated gold nanoparticles
in cancer diagnostics: applications in oral cancer,‖ Nano Lett. 5, 829-834
(2005).
13. A. Campion, and P. Kambhampati, ―Surface-enhanced Raman scattering,‖
Chem. Soc. Rev. 27, 241-250 (1998).
28
14. S. C. Warren, and E. Thimsen. ―Plasmonic solar water splitting,‖ Energy
Environ. Sci. 5, 5133-5146 (2012).
15. J. Y. Lan, X. M. Zhou, G. Liu, J. G. Yu, J. C. Zhang, L. J. Zhi, and G. J. Nie,
―Enhancing photocatalytic activity of one-dimensional KNbO3 nanowires by Au
nanoparticles under ultraviolet and visible-light,‖ Nanoscale, 3, 5161-5167
(2011).
16. S.-I. Naya, M. Teranishi, T. Isobe, and H. Tada. ―Light wavelength-switchable
photocatalytic reaction by gold nanoparticle-loaded titanium(IV) dioxide,‖
Chem. Commun. 46, 815-817 (2010).
17. Y. Tian, and T. Tatsuma, ―Mechanisms and applications of plasmon-induced
charge separation at TiO2 films loaded with gold nanoparticles,‖ J. Am. Chem.
Soc. 127, 7632-7637 (2005).
18. E. Kowalska, R. Abe, and B. Ohtani, ―Visible light-induced photocatalytic
reaction of gold-modified titanium(IV) oxide particles: action spectrum
analysis,‖ Chem. Commun. 241-243 (2009).
19. D. Tsukamoto, Y. Shiraishi, Y. Sugano, S. Ichikawa, S. Tanaka, and T. Hirai,
―Gold nanoparticles located at the interface of anatase/rutile TiO2 particles as
active plasmonic photocatalysts for aerobic oxidation,‖ J. Am. Chem. Soc. 134,
6309-6315 (2012).
20. Z. K. Zheng, B. B. Huang, X. Y. Qin, X. Y. Zhang, Y. Dai, and M.-H.
Whangbo, ―Facile in situ synthesis of visible-light plasmonic photocatalysts
M@TiO2 (M = Au, Pt, Ag) and evaluation of their photocatalytic oxidation of
benzene to phenol,‖ J. Mater. Chem. 21, 9079-9087 (2011).
29
21. X. Chen, H.-Y. Zhu, J.-C. Zhao, Z.-F. Zheng, and X.-P. Gao, ―Visible-light-
driven oxidation of organic contaminants in air with gold nanoparticle catalysts
on oxide supports,‖ Angew. Chem. Int. Ed. 47, 5353-5356 (2008).
22. A. Emeline, G.V. Kataeva, A.S. Rudakova, V.K. Ryabchuk, and N. Serpone,
―Spectroscopic and photoluminescence studies of a wide band gap insulating
material: powdered and colloidal ZrO2 sols,‖ Langmuir, 14, 5011-5022 (1998).
23. A. Tanaka, K. Hashimoto, and H. Kominami, ―Preparation of Au/CeO2
exhibiting strong surface plasmon resonance effective for selective or
chemoselective oxidation of alcohols to aldehydes/ketones in aqueous
suspensions under irradiation by green light,‖ J. Am. Chem. Soc. 134, 14526-
14533 (2012).
24. T. A. Baker, C. M. Friend, and E. Kaxiras, ―Atomic oxygen adsorption on
Au(111) surfaces with defects,‖ J. Phys. Chem. C 113, 3232-3238 (2009).
25. H. Y. Zhu, X. B. Ke, X. Z. Yang, S. Sarina, and H. W. Liu, ―Reduction of
nitroaromatic compounds on supported gold nanoparticles by visible and
ultraviolet light,‖ Angew. Chem. 122, 9851-9855 (2010).
26. A. Tanaka, Y. Nishino, S. Sakaguchi, T. Yoshikawa, K. Imamura, K.
Hashimoto, and H. Kominami, ―Functionalisation of a plasmonic Au/TiO2
photocatalyst with an Ag co-catalyst for quantitative reduction of nitrobenzene
to aniline in isopropanol suspensions under irradiation of visible light,‖ Chem.
Commun. 49, 2551-2553 (2013).
27. J. Weitkamp, ―Zeolites and catalysis,‖ Solid State Ionics 131, 175-188 (2000).
28. Y. Xiang, S. C. Larsen, and V. H. Grassian, ―Photooxidation of 1-alkenes in
zeolites: a study of the factors that influence product selectivity and formation,‖
J. Am. Chem. Soc. 121, 5063-5072 (1999).
30
29. J. N. Kondo, E. Yoda, H. Ishikawa, F. Wakabayashi, and K. Domen, ―Acid
property of silanol groups on zeolites assessed by reaction probe IR study,‖ J.
Catal. 191, 275-281 (2000).
30. V. J. Rao, D. L. Perlstein, R. J. Robbins, P. H. Lakshminarasimhan, H-M. Kao,
C. P. Grey, and V. Ramamurthy, ―Detection of low levels of Brønsted acidity in
Na+Y and Na
+X zeolites,‖ Chem. Commun. 269-270 (1998).
31. J. Dědeček, Z. Sobalík, and B. Wichterlová, ―Siting and distribution of
framework aluminium atoms in silicon-rich zeolites and impact on catalysis,‖
Catal. Rev. Sci. Eng. 54, 135-223 (2012).
32. T. Frising, and P. Leflaive. Extraframework cation distributions in X and Y
Faujasite zeolites, Micropor. Mesopor. Mater. 114, 27-63 (2008).
33. A. Corma, and H. Garcia, ―Zeolite-based photocatalysts,‖ Chem. Commun.
1443-1459 (2004).
34. S. Hashimoto, ―Zeolite photochemistry: impact of zeolites on photochemistry
and feedback from photochemistry to zeolite science,‖ J. Photochem. Photobiol.
C 4, 19-49 (2003).
35. P. K. Dutta, and M. Severance, ―Photoelectron transfer in zeolite cages and its
relevance to solar energy conversion,‖ J. Phys. Chem. Lett. 2, 467-476 (2011).
36. S. Corrent, G. Cosa, J. C. Scaiano, M. S. Galletero, M. Alvaro, and H. Garcia,
―Intrazeolite photochemistry. 26. Photophysical properties of nanosized TiO2
clusters included in zeoiltes Y, beta, and mordenite,‖ Chem. Mater. 13, 715-722
(2001).
37. A. Starosud, A. Bhargava, C. H. Langford, and A. Kantzas, ―Development of
new photocatalytic methods and reactors for waste water treatment,‖ Stud. Surf.
Sci. Catal. 122, 219-228 (1999).
31
38. F. Marquez, V. Marti, E. Palomares, H. Garcia, and W. Adam, ―Observation of
azo chromophore fluorescence and phosphorescence emissions from DBH by
applying exclusively the orbital confinement effect in siliceous zeolites devoid
of charge-balancing cations,‖ J. Am. Chem. Soc. 124, 7264-7265 (2002).
39. W. Loewenstein, ―The distribution of aluminum in the tetrahedra of silicates and
aluminates,‖ American Mineralogist, 39, 92-96 (1954).
40. K. Tsutsumi, and H. Takahashi, ―A study of the nature of active sites on zeolites
by the measurement of heat of immersion. II. Effects of silica/alumina ratio to
electrostatic-field strength of calcium-exchanged zeolites,‖ J. Phys. Chem. 76,
110-115 (1972).
41. Y. Xiang, S. C. Larsen, and V. H. Grassian, ―Photooxidation of 1-alkenes in
zeolites: a study of the factors that influence product selectivity and formation,‖
J. Am. Chem. Soc. 121, 5063-5072 (1999).
42. T. Bär, T. Visart de Bocarmé, B. E. Nieuwenhuys, and N. Kruse, ―CO oxidation
on gold surfaces studied on the atomic scale,‖ Catal. Lett. 74, 127-131 (2001).
43. L. C. Richard, H. Wang, J. Kreuzer, M. Grunze, and A. J. Pertsin, ―The effect of
electrostatic fields on an oligo(ethylene glycol) molecule: dipole moments,
polarizabilities and field dissociation,‖ Phys. Chem. Chem. Phys. 2, 1721-1727
(2000).
44. D. M. Clode, ―Carbohydrate cyclic acetal formation and migration,‖ Chem. Rev.
79, 491-513 (1979).
45. T. W. Green, and P. G. M. Wuts, ―Protective groups on organic synthesis,‖ vol.
4, 2nd ed., Wiley, New York, 1991, p. 212.
46. J. H. Kim, I. Čorič, S. Vellalath, and B. List, ―The catalytic asymmetric
acetalisation,‖ Angew. Chem. Int. Ed. 52, 4474-4477 (2013).
32
47. C. A. Mackenzie, and J. H. Stocker, ―Preparation of ketals. A reaction
mechanism,‖ J. Org. Chem. 20, 1695-1701 (1955).
48. J. Bornstein, S. F. Bedell, P. E. Drummond, and C. F. Kosoloski, ―The synthesis
of a-amino-o-tolualdehyde diethylacetal and its attempted conversion to
pseudoisoindole,‖ J. Am. Chem. Soc. 78, 83-86 (1956).
49. J. I. Tateiwa, H. Horiochi, and S. Uemora, ―Ce3+
-exchanged montmorillonite
(Ce3+
-monta) s a useful substrate-selective acetalisation catalyst,‖ J. Org. Chem.
60, 4039-4043 (1995).
50. C. H. Lin, S. D. Lin, Y. H. Yang, and T. P. Lin, ―The synthesis and hydrolysis of
dimethyl acetals catalysed by sulfated metal oxides. An efficient method for
protecting carbonyl groups,‖ Catal. Lett. 73, 2-4 (2001).
51. B. Rabindran Jermy, and A. Pandurangan, ―Al-MCM-41 as an efficient
heterogeneous catalyst in the acetalisation of cyclohexanone with methanol,
ethylene glycol and pentaerythritol,‖ J. Mol. Catal. A 256, 184-192 (2006).
52. B. Thomas, S. Prathapan, and S. Sugunan, ―Synthesis of dimethyl acetal of
ketones: design of solid acid catalysts for one-pot acetalisation reaction,‖
Micropor. Mesopor. Mater. 80, 65-72 (2005).
53. H. Frei, ―Selective hydrocarbon oxidation in zeolites,‖ Science, 313, 309-310
(2006).
54. G. Centi, and M. Misono, ―Modification of the surface reactivity and selectivity
of mixed oxides in oxidation reactions due to coadsorbate species,‖ Catal. Today
41, 287 (1998).
55. F. Blatter, and H. Frei, ―Selective photooxidation of small alkenes by O2 with
red light in zeolite Y,‖ J. Am. Chem. Soc. 116, 1812-1820 (1994).
33
56. J. Xu, B. L. Mojet, J. G. van Ommen, and L. Lefferts, ―Effect of Ca2+
position in
zeolite Y on selective oxidation of propane at room temperature,‖ J. Phys.
Chem. B 108, 15728-15734 (2004).
57. H. Sun, F. Blatter, and H. Frei, ―Selective oxidation of toluene to benzaldehyde
by O2 with visible light in barium(2+)- and calcium(2+)-exchanged zeolite Y,‖ J.
Am. Chem. Soc. 116, 7951-7952 (1994).
35
Chapter 3: Selective reduction reaction - Selective reductions using
visible light photocatalysts of supported gold nanoparticles
Introductory remarks
This chapter reports that Au-NPs supported on Al2O3, CeO2, TiO2, ZrO2, or
zeolite Y enhance the catalytic performance in the selective reduction of
nitroaromatics to azo compounds, azobenzene to hydroazobenzene, ketones to
alcohols, and epoxides to alkenes at ambient temperatures under visible light
illumination (or simulated sunlight). The article describing the discoveries was
published in the journal of ―Green Chemistry” in 2012[1]
.
The selective reduction is an important process in organic synthesis, energy
storage and environmental chemistry, such as production of chemical intermediates,
development of solar panels and degradation of organic pollutants. If these processes
can be achieved in a photocatalytic way, then it will be promising to synthesise
organic chemicals with significant benefits, such as better selectivity to the desired
product via a green approach because the photocatalytic reactions often occur at
ambient conditions. Moreover, it opens a potential way to develop the sunlight-
driven photocatalytic processes in the chemical community[2]
.
This study investigated the reduction activity of photocatalysts of supported Au-
NPs induced by the LSPR effect. Other studies have reported that the same above-
mentioned reactions can be driven by heat energy[3-8]
. However, this study showed
that these reactions exhibited much high conversions of reactants under visible light
irradiation compared with the thermal-driven processes (other reaction conditions
were identical), clearly demonstrating the contribution of visible light irradiation.
36
The reactivity of Au-NPs depended on two basic factors: (i) the light absorption
ability of the photocatalysts to absorb visible light, and (ii) the reduction ability of
the photocatalysts to reduce reactants. The light absorption of Au-NPs resulted from
the LSPR effect under visible light irradiation and was directly correlated to the
reduction ability of Au-NPs. Visible light with shorter wavelengths could excite the
free conduction electrons of Au-NPs to higher energy levels, thereby inducing
reduction of reactants with more negative reduction potentials. This discovery
demonstrated that the reduction capability of the gold photocatalysts could be
adjusted by tuning the wavelength of incident light.
References
1. X. B. Ke, X. G. Zhang, J. Zhao, S. Sarina, J. Barry, and H. Y. Zhu, ―Selective
reductions using visible light photocatalysts of supported gold nanoparticles,‖
Green Chem. 15, 236-244 (2013).
2. I. Kirm, F. Medina, J. E. Sueiras, P. Salagre, and Y. Cesteros, ―Hydrogenation of
styrene oxide in the presence of supported platinum catalysts to produce 2-
phenylethanol,‖ J. Mol. Catal. A 261, 98-103 (2007).
3. X. B. Chen, L. Liu, P. Y. Yu, and S. S. Mao, ―Increasing solar absorption for
photocatalysis with black hydrogenated titanium dioxide nanocrystals,‖ Science,
331, 746-750 (2011).
4. T. Mitsudome, A. Noujima, Y. Mikami, T. Mizugaki, K. Jitsukawa, and K.
Kaneda, ―Supported gold and silver nanoparticles for catalytic deoxygenation of
epoxides into alkenes,‖ Angew. Chem. Int. Ed. 49, 5545-5548 (2010).
37
5. F. Z. Su, L. He, J. Ni, Y. Cao, H. Y. He, and K. N. Fan, ―Efficient and
chemoselective reduction of carbonyl compounds with supported gold catalysts
under transfer hydrogenation conditions,‖ Chem. Commun. 3531 (2008).
6. Y. Zhu, H. F. Qian, B. A. Drake, and R. C. Jin, ―Atomically precise Au25(SR)18
nanoparticles as catalysts for the selective hydrogenation of α, β-unsaturated
ketones and aldehydes,‖ Angew. Chem. Int. Ed. 49, 1295-1298 (2010).
7. E. Merino, ―Synthesis of azobenzenes: the coloured pieces of molecular
materials,‖ Chem. Soc. Rev. 40, 3835-3853 (2011).
8. A. Grirrane, A. Corma, and H. Carcía, ―Gold-catalysed synthesis of aromatic azo
compounds from anilines and nitroaromatics,‖ Science, 322, 1661-1664 (2008).
38
Statement of contribution
The authors listed below have certified that:
1. They meet the criteria for authorship in that they have participated in the
conception, execution, or interpretation, of at least that part of the publication in
their field of expertise;
2. They have public responsibility for their part of the publication, except for the
responsible author who accepts overall responsibility for the publication;
3. There are no other authors of the publication according to these criteria;
4. Potential conflicts of interest have been disclosed to (a) granting bodies, (b) the
editor or publisher of journals or other publications, and (c) the head of the
responsible academic unit, and
5. They agree to the use of the publication in the student’s thesis and its publication
on the Australian Digital Thesis database consistent with any limitations set by
publisher requirements.
In the case of this chapter:
Selective reductions using visible light photocatalysts of supported gold
nanoparticles
Xuebin Ke, Xingguang Zhang, Jian Zhao, Sarina Sarina, John Barry, and Huaiyong Zhu
Published in the journal: Green Chemistry, 2013, 15, 236-244
51
Chapter 4: Selective oxidation reaction - Zeolite-supported gold
nanoparticles for selective photooxidation of aromatic alcohols
under visible-light irradiation
Introductory remarks
This chapter reports that Au-NPs supported on zeolites can oxidise benzyl alcohol
and its derivatives into product aldehydes with high selectivity (99%) under visible
light irradiation at ambient temperature. The article was published in the journal of
―Chemistry – A European Journal”[1]
.
The selective oxidation of aromatic alcohols to corresponding aldehydes is an
important process in the production of fine chemicals, because aldehydes are
valuable components in the industry of perfume, dyes, pharmaceuticals, and
agrochemicals[2, 3]
. In particular, benzaldehyde is the most extensively investigated. It
is traditionally produced by hydrolysis of benzyl chloride or by oxidation of toluene[4,
5]; however, this process often leads to trace of chlorine impurities and a substantial
quantity of waste. If the selective oxidation of aromatic alcohols can be achieved in a
photocatalytic way, then it will be promising to improve the catalytic performance
such as higher selectivity, because the photocatalytic reactions often happen at
ambient conditions.
This study showed that the LSPR effect of Au-NPs, the adsorption capability of
zeolite supports, and the molecular polarities of aromatic alcohols all contributed to
the photocatalytic performance. The kinetic study demonstrated that the
photooxidation under visible light irradiation required less activation energy
compared with that of the thermal-driven reaction. Moreover, the influence of light
52
intensity, wavelength range, and the role of molecular oxygen were investigated in
detail. This study illustrates the potential of Au/zeolite photocatalysts for the
selective oxidation reaction driven by sunlight at ambient temperatures. The
mechanistic study may provide practical guidelines for developing new catalytic
materials for ―green‖ and energy-saving chemical processes.
References
1. X. G. Zhang, X. B. Ke, and H. Y. Zhu, ―Zeolite-supported gold nanoparticles for
selective photooxidation of aromatic alcohols under visible-light irradiation,‖
Chem. Euro. J. 18, 8048-8056 (2012).
2. N. Lingaiah, K. M. Reddy, N. S. Babu, K. N. Rao, I. Suryanarayana, and P. S. S.
Prasad, ―Aerobic selective oxidation of benzyl alcohol over vanadium substituted
ammonium salt of 12-molybdophosphoric acid,‖ Catal. Commun. 7, 245-250
(2006).
3. R. A. Sheldon, and J. K. Kochi, ―Metal-catalysed oxidations of organic
compounds,‖ Academic Press, New York (1981).
4. H. Sun, F. Blatter, and H. Frei, ―Selective oxidation of toluene to benzaldehyde
by O2 with visible light in barium(2+)- and calcium(2+)-exchanged zeolite Y,‖ J.
Am. Chem. Soc. 116, 7951-7952 (1994).
5. Y. Mao, and A. Bakac, ―Photocatalytic oxidation of toluene to benzaldehyde by
molecular oxygen,‖ J. Phys. Chem. 100, 4219-4223 (1996).
53
Statement of contribution
The authors listed below have certified that:
1. They meet the criteria for authorship in that they have participated in the
conception, execution, or interpretation, of at least that part of the publication in
their field of expertise;
2. They have public responsibility for their part of the publication, except for the
responsible author who accepts overall responsibility for the publication;
3. There are no other authors of the publication according to these criteria;
4. Potential conflicts of interest have been disclosed to (a) granting bodies, (b) the
editor or publisher of journals or other publications, and (c) the head of the
responsible academic unit, and
5. They agree to the use of the publication in the student’s thesis and its publication
on the Australian Digital Thesis database consistent with any limitations set by
publisher requirements.
In the case of this chapter:
Zeolite-supported gold nanoparticles for selective photooxidation of aromatic
alcohols under visible-light irradiation
Xingguang Zhang, Xuebin Ke, and Huaiyong Zhu
Published in the journal: Chemistry-A European Journal, 2012, 18, 8048-8056
64
Chapter 5: Acetalisation reaction
5.1 Acetalisation reaction on Au/zeolite photocatalysts - Plasmonic
nanostructures to enhance catalytic performance of zeolites under
visible light
Introductory remarks
This chapter reports an effective way to harvest visible light to boost zeolite
catalysis by using plasmonic Au-NPs supported on the MFI zeolites. Zeolites possess
strong Brønsted acid sites (H+) and polarised electrostatic fields that created by extra-
framework cations as outline in Chapter 2. The polarised electrostatic fields can be
further intensified by the electric near-field enhancement of Au-NPs, which results
from the LSPR effect upon visible light irradiation. The intensified polarised
electrostatic fields play a critical role in polarising or interacting with reactants
adsorbed on zeolite surfaces or confined in zeolite pores. This study demonstrated a
cascade enhancement from visible light to zeolites via the LSPR-induced electric
near-field enhancement which functioned as a ―relay‖ to intensify the polarised
electrostatic fields to boost the catalytic performance of acetalisation reactions. This
research was published in the journal of ―Scientific Reports‖[1]
.
The acetalisation reaction plays an important part in the multi-step organic
synthesis to produce multi-functional organic molecules[2]
. Two acetalisation
reactions were selected as model reactions that were performed on Au/MZSM-5 and
MZSM-5 (M=H+, Na
+, Ca
2+, or La
3+): the condensation of benzaldehyde with 1-
pentanol and the methylation of cyclohexanone with methanol[3, 4]
. Density
functional theory (DFT) calculations confirmed that the intensified polarised
65
electrostatic fields can stretch the C=O bonds of reactants (benzaldehyde and
cyclohexanone), thus allowing them to be activated more efficiently by active sites
(H+) to boost the reaction rates.
This discovery should draw huge attention to plasmonic metal nanostructures
modified zeolitic catalysts, because the enhancement effect holds great potential in
enlarging the molecular polarity of adsorbates. This stretching effect can influence
the activity and the electrostatic behaviour of molecules, which have broad
applications in organic synthesis, ionic liquids, nanofiltration membranes, molecular
electronics, and molecular self-assembly processes[5-7]
. Moreover, new applications
can be expected in sensors, solar panels, water splitting, drug delivery, and
environmental remediation.
References
1. X. G. Zhang, X. B. Ke, A. J. Du, and Huaiyong Zhu, ―Plasmonic nanostructures
to enhance catalytic performance of zeolites under visible light,‖ Sci. Rep.
4(3805), 1-6 (2014).
2. B. Thomas, S. Prathapan, and S. Sugunan, ―Synthesis of dimethyl acetal of
ketones: design of solid acid catalysts for one-pot acetalisation reaction,‖
Micropor. Mesopor. Mater. 80, 65-72 (2005).
3. F. J. Liu, T. Willhammar, L. Wang, L. F. Zhu, Q. Sun, and X. J. Meng, W.
Carrillo-Cabrera, X. D. Zou, and F. S. Xiao, ―ZSM-5 zeolite single crystals with
b-axis-aligned mesoporous channels as an efficient catalyst for conversion of
bulky organic molecules,‖ J. Am, Chem. Soc. 134, 4557-4560 (2012).
66
4. M. Iwamoto, Y. Tanaka, N. Sawamura, and S. Namba, ―Remarkable effect of
pore size on the catalytic activity of mesoporous silica for the acetalisation of
cyclohexanone with methanol,‖ J. Am. Chem. Soc. 125, 13032-13033 (2003).
5. B. Van der Bruggen, J. Schaep, D. Wilms, and C. Vandecasteele, ―Influence of
molecular size, polarity and charge on the retention of organic molecules by
nanofiltration,‖ J. Membrane Sci. 156, 29-41 (1999).
6. P. A. Lewis, C. E. Inman, F. Maya, J. M. Tour, J. E. Hutchison, and P. S. Weiss,
―Molecular engineering of the polarity and interactions of molecular electronic
switches,‖ J. Am. Chem. Soc. 127, 17421-17426 (2005).
7. A. S. Singh, and S.-S. Sun, ―Dynamic self-assembly of molecular capsules via
solvent polarity controlled reversible binding of nitrate anions with C3 symmetric
tripodal receptors,‖ Chem. Commun. 47, 8563-8565 (2011).
67
Statement of contribution
The authors listed below have certified that:
1. They meet the criteria for authorship in that they have participated in the
conception, execution, or interpretation, of at least that part of the publication in
their field of expertise;
2. They have public responsibility for their part of the publication, except for the
responsible author who accepts overall responsibility for the publication;
3. There are no other authors of the publication according to these criteria;
4. Potential conflicts of interest have been disclosed to (a) granting bodies, (b) the
editor or publisher of journals or other publications, and (c) the head of the
responsible academic unit, and
5. They agree to the use of the publication in the student’s thesis and its publication
on the Australian Digital Thesis database consistent with any limitations set by
publisher requirements.
In the case of this chapter:
Plasmonic nanostructures to enhance catalytic performance of zeolites under
visible light
Xingguang Zhang, Xuebin Ke, Aijun Du, and Huaiyong Zhu
Published in the journal: Scientific Reports, 2014, 4(3805), 1-6.
Plasmonic nanostructures to enhancecatalytic performance of zeolites undervisible lightXingguang Zhang, Xuebin Ke, Aijun Du & Huaiyong Zhu
School of Chemistry, Physics and Mechanical Engineering, Queensland University of Technology, QLD 4001, Australia.
Light absorption efficiency of heterogeneous catalysts has restricted their photocatalytic capability forcommercially important organic synthesis. Here, we report a way of harvesting visible light efficiently toboost zeolite catalysis by means of plasmonic gold nanoparticles (Au-NPs) supported on zeolites. Zeolitespossess strong Brønsted acids and polarized electric fields created by extra-framework cations. Thepolarized electric fields can be further intensified by the electric near-field enhancement of Au-NPs, whichresults from the localized surface plasmon resonance (LSPR) upon visible light irradiation. The acetalizationreaction was selected as a showcase performed on MZSM-5 and Au/MZSM-5 (M 5 H1, Na1, Ca21, or La31).The density functional theory (DFT) calculations confirmed that the intensified polarized electric fieldsplayed a critical role in stretching the C5O bond of the reactants of benzaldehyde to enlarge their molecularpolarities, thus allowing reactants to be activated more efficiently by catalytic centers so as to boost thereaction rates. This discovery should evoke intensive research interest on plasmonic metals and diversezeolites with an aim to take advantage of sunlight for plasmonic devices, molecular electronics, energystorage, and catalysis.
Photocatalysis has significantly advanced in developing efficient catalysts to harvest the ‘‘green’’ solar energyat ambient conditions. Recent years have seen a new family of plasmonic photocatalysts of gold, silver, orcopper nanoparticles (NPs), which features a collective and coherent oscillation of the free conduction
electrons with the incident photons at the surface of NPs due to the localized surface plasmon resonance (LSPR)irradiated by visible light1–3. This LSPR effect has been applied to boost catalytic performance in various import-ant organic transformations under the irradiation of visible light: oxidation of organic contaminants and aromaticalcohols, and reduction of nitroaromatic compounds, ketones and epoxides on Au-NPs4–7; epoxidation of ethyl-ene on Ag-NPs and of propylene on Cu-NPs8,9. Very recently, Au-Pd alloys are also founded to be efficientphotocatalysts for Suzuki coupling reactions and oxidation of benzylamine10,11. These discoveries demonstratethat the plasmon-mediated processes fundamentally differ in catalytic mechanisms compared with those ontraditional semiconductors. Moreover, the LSPR effect of plasmonic NPs can amplify the electromagnetic fieldintensity of incident light (jE0j) and results in an enhanced electric field (jEj) of 3–6 orders of magnitude3,12. Thisnear-field enhanced interaction is well-known as the ‘‘electric near-field enhancement (ENFE)’’ effect and hasmotivated numerous intensive studies, such as surface-enhanced Raman scattering13, sensors14–16, plasmonicdevices17–19 and solar cells20,21. In photocatalysis, Ag-NPs covered by the SiO2 shell and embedded in TiO2
particles have been tried to degrade methyl blue and exhibit better catalytic performance owing to the electricfield amplitude effect of Ag-NPs22. However, the inert SiO2 shell, which is used to prevent the Ag core fromoxidation, constraints the light absorption efficiency in photocatalysis.
Zeolites possess regular microporous structures, high surface areas, shape-selectivity, and unique solid acidity,having extensive applications in catalysis, separation, and adsorption. Particularly, the strong polarized electro-static fields (PEF, 1–10 V/nm) created by extra-framework cations have the power to polarize molecules adsorbedon surfaces or confined in the porous matrix (e.g. host-guest structures)23–25. In principle, the PEF can reduce theenergy consumption required to facilitate the electron transfer or to activate reactants, thereby initiating reactionsby moderate heating or visible-light excitation. The charge-transfer properties from hydrocarbons to molecularoxygen (O2) have been investigated on ion-exchanged zeolites, such as ZSM-5, Y and Beta, with visible lightirradiation in the selective oxidization of toluene, propane, cyclohexane, and small alkenes26–29. These studiesverify that the PEF can lower the charge-transfer excitation energy from hydrocarbons to O2. However, the
OPEN
SUBJECT AREAS:PHOTOCATALYSIS
HETEROGENEOUS CATALYSIS
PHOTOCHEMISTRY
CHEMICAL ENGINEERING
Received29 October 2013
Accepted23 December 2013
Published22 January 2014
Correspondence andrequests for materials
should be addressed toX.B.K. ([email protected].
au)
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 1
products cannot be quantitatively measured because of low produc-tivity, which results from the low absorption efficiency of zeolites ofvisible light.
Plasmonic Au-NPs are loaded on ion-exchanged ZSM-5 zeolites(Au/MZSM-5, M 5 H1, Na1, Ca21, or La31) as ‘‘antenna’’ to effi-ciently absorb visible light. This study for the first time reports acascade enhancement from visible light to zeolites via the LSPR-induced ENFE which functions as a ‘‘relay’’ to intensify the PEF ofcations in zeolites to boost the catalytic performance. The acetaliza-tion of benzaldehyde with 1-pentanol is selected as the model reac-tion30–34. The present research demonstrated that the ENFE ofAu-NPs could intensify the PEF of MZSM-5 so as to facilitate theeffective activation of the reactant of benzaldehyde by stretching theC5O bonds, thus improving the conversion of the acetalization.
To illustrate this enhancing process, as shown in Figure 1, Au-NPsform dynamic Au(d1, d2) dipole moments owing to the LSPR effectupon visible light irradiation, simultaneously inducing the ENFEaround the surface of Au-NPs2,3. The ENFE intensifies the PEF ofextra-framework cations in MZSM-5, which enables the intensifiedPEF to stretch the C5O bond of reactants of benzaldehyde. Thestretched reactants display larger molecular polarities and can beactivated more efficiently by catalytic active centers of H1, therebyaccelerating reactions with alcohols35. The Brønsted acid sites origin-ate from terminal hydroxyl groups, and extra-framework cations:M21 1 H2O 1 Si-O-Al R M(OH)1 1 Si-O(H1)-Al24,36.
Table 1 revealed that the acetalization between benzaldehyde and1-pentanol proceeded effectively on Au/MZSM-5 under visible lightirradiation. The catalytic conversions improved significantly on Au/NaZSM-5, Au/CaZSM-5, and Au/LaZSM-5; particularly, the conver-sion increased from 21.5% on CaZSM-5 to 62.2% on Au/CaZSM-5(an exception for HZSM-5 will be interpreted later). However, withlight off (see SI, Table S1, Section S1), the catalytic conversions ofMZSM-5 and Au/MZSM-5 showed fewer differences, indicating Au-NPs themselves were not active centers under dark conditions.Moreover, visible light irradiation showed negligible influence onthe activity of MZSM-5 compared with those under dark conditions.These results confirmed that visible light and plasmonic Au-NPswere necessities to sharply boost the acetalization reaction.
The differences in conversions on MZSM-5 indicated that extra-framework cations markedly influenced the catalytic activity.
HZSM-5 exhibited the highest conversion of 53.8%, whereasNaZSM-5, CaZSM-5, and LaZSM-5 exhibited lower conversions(just better than Silicalite-1) primarily because of their relativelyfewer active centers (H1). The change in Brønsted acidity could beproved by the spectra of FT-IR spectroscopy - attenuated total reflec-tance (ATR) which also confirmed that Brønsted acids preserved wellafter loading of gold (see SI, Figure. S1, Section S2).
Moreover, the optical properties of catalysts were investigated byUV/Vis spectra (Figure 2a), showing that MZSM-5 had no mea-surable absorption of visible light (.420 nm), whereas Au/MZSM-5 strongly absorbed visible light owing to the LSPR effect of Au-NPs,with the absorption peaks being about 525–565 nm. The crystalstructures of Au/MZSM-5 were detected by X-ray diffraction(XRD) patterns (Figure 2b), confirming that the MFI structures pre-served well. The oxidation state of gold was analyzed by X-ray photo-electronic spectra (XPS) (Figure 2c) which identified that the bindingenergies of Au4f7/2 electrons (84.1 eV) and Au4f5/2 electrons(87.7 eV) were in agreement with reports for Au-NPs37. In addition,XPS showed that the gold content were similar on Au/MZSM-5, theSi/Al ratio was close to 14, and that the ion-exchange level was highbecause Na1 ions were undetectable in CaZSM-5 and LaZSM-5.Transmission-electron-microscopy (TEM) images provided directinformation of the size (6–18 nm), shape (pseudospherical) and dis-tribution of Au-NPs on zeolites (see SI, Figure. S3, Section S3).
Now one may wonder why visible light coupled with Au-NPscould boost the reaction on Au/MZSM-5. Here we hypothesize thatthe ENFE of Au-NPs directly intensifies the PEF of cations to a largeextent that the intensified PEF can polarize reactants of benzalde-hyde and 1-pentanol to facilitate activation of them by catalytic activecenters of H1. From the experimental perspective, Au/HZSM-5 andHZSM-5 exhibited similar catalytic activities with light on, as shownin Table 1, indicating that Au-NPs neither served as extra activecenters nor interacted directly with the reactants to accelerate thereaction rate even though the LSPR-induced dipole moment ofAu(d1, d2) could in theory interact with the reactants. In this case,there should exist other key factors that affected the interaction withreactants. The density functional theory (DFT, see SI, Section S4)calculations unambiguously demonstrated that increasing thestrength of external electric field stretched the C5O bond of benzal-dehyde, whereas had no effect on 1-pentanol, probably because themolecular polarity of benzaldehyde (dipole momentm5 3.00 Debye)is larger than that of 1-pentanol (1.70 Debye). The relationshipbetween the C5O bond length and the electric field strength waslinear (Figure 3a). In detail, the C5O bond lengths of benzaldehydewere 1.218 A, 1.223 A, 1.229 A, 1.236 A, and 1.245 A, whenthe electric field strengths were 0 V/nm, 2.58 V/nm, 5.16 V/nm,7.74 V/nm, and 10.32 V/nm, respectively. Here the electric fieldstrength used in simulation were on the same order of magnitudeas that reported for HZSM-5 (3.0 V/nm), NaZSM-5 (6.2 V/nm),CaZSM-5 (8.3 V/nm), and LaZSM-5 (10.7 V/nm) (see SI, TableS2, Section S5)23,38. However, the experimental results revealed thatthe PEF of MZSM-5 without Au-NPs had no influence on the con-versions, which indicated that the PEF of MZSM-5 was not strongenough to boost the reaction rate even with light on.
These results trigger a logical deduction that further increasing theelectrostatic field strength may make distinct difference. And it hasbeen underpinned by the experimental evidence that the existence ofan external electric field of 12–15 V/nm obviously helps activate thereactants of CO/O2 and enhances the oxidation process on small goldcrystals (20–30 nm). This effect is considered to be associated withthe formation of partially charged gold surface39. Furthermore, it hasbeen reported that the near-field enhancement factor (jEj/jE0j) ofplasmonic NPs can reach as large as 102 at the surface of individualNPs and 103 at the junction of interparticles (hot spots)40,41, and thatthe ENFE attenuates exponentially within the spacing range of 10–50nanometers away from metal surfaces, depending on the metal
Figure 1 | The acetalization on Au/MZSM-5 (M 5 H1, Na1, Ca21, orLa31) under the irradiation of visible light. ENFE means the electric near-
field enhancement of Au-NPs. PEF means the polarized electro-static fields
of extra-framework cations in zeolites.
www.nature.com/scientificreports
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 2
crystal size and shape, and the dielectric environments1. Therefore, itbecomes convincing that the ENFE may directly intensify the PEF ofcations in MZSM-5 to a large extent so as to stretch the C5O bond ofreactants, thereby boosting the reaction rate.
The intensified PEF of H1, Na1, Ca21, and La31 differed in boost-ing the catalytic activities on Au/MZSM-5. The largest net increase inthe conversion of acetalization reaction, which means the conversionon Au/MZSM-5 deducts the conversion on its counterpart ofMZSM-5, occurred between Au/CaZSM-5 and CaZSM-5, and thelowest between Au/HZSM-5 and HZSM-5 (Figure 3b, calculatedfrom Table 1). It has been reported that the PEF strength of a singlecation within a given zeolite host is influenced by multi-factors, suchas Si/Al ratio, charge/radius ratio, cation charges and cation density(see SI, Table S2, Section S5). As for Au/HZSM-5 and HZSM-5, theoriginal PEF strength of H1 is ca. 3.0 V/nm and the intensified PEFstrength of H1 might be still too weak to stretch the C5O bond ofbenzaldehyde, thus showing the lowest net increase in conversion.The intensified PEF strength of Na1 (originally ca. 6.2 V/nm), Ca21
(originally ca. 8.3 V/nm), or La31 (originally ca. 10.7 V/nm) shouldbe sufficiently strong to extend the C5O bond of benzaldehyde toaccelerate the reaction. Interestingly, La31 ions which had the stron-gest electrostatic field showed a lower net increase of conversion thanNa1 ions and Ca21 ions. This phenomenon probably resulted fromthe difference in cation density within MZSM-5 after ion-exchangebecause one La31 ion corresponds to three Na1 in terms of compens-ating for the negatively-charged framework sites (see SI; Section S5,Table S3, and Section S6); therefore, the number of La31 (La31/Al 5
0.09) was smaller in MZSM-5 compared with the number of Na1
(Na1/Al 5 0.43) or Ca21 (Ca21/Al 5 0.25), thereby exhibiting a lowernet conversion between Au/LaZSM-5 and LaZSM-5. One may arguethat the acidity of zeolites plays a more important role than PEF inthe acetalization reaction because Brønsted acid sites (H1) are thecatalytic centers. However, this study conveys a clear message thatthe intensified PEF by ENFE does contribute to improving the cata-lytic performances of zeolites by affecting the molecular polarities ofreactants.
The impacts of light intensity, the range of wavelength, and reac-tion temperature on the acetalization reaction were investigated onCaZSM-5 and Au/CaZSM-5 with light on. As shown in Figure 4a, theincrease of light intensity improved the catalytic activity on Au/CaZSM-5, but not on CaZSM-5. This result indicated that raisingthe light intensity could afford a much stronger ENFE on Au/CaZSM-5 thus contributing more to boosting the catalytic activity.The light wavelength was also investigated using glass filters to blockphotons with wavelengths below the filter threshold. For example,the cut-off wavelength of 420 nm means that the light with wave-length smaller than 420 nm was blocked. Figure 4b showed that thelight wavelength significantly influenced the catalytic activity of Au/CaZSM-5, but not on CaZSM-5. This result demonstrated a wave-length-selective enhancement on Au/CaZSM-5, and proved that vis-ible light that could induce the ENFE effect of Au-NPs made a largercontribution to boost the catalytic activity. Raising the reaction tem-perature increased the conversions both on CaZSM-5 and Au/CaZSM-5 (Figure 4c). The conversion on Au/CaZSM-5 was muchhigher than that on CaZSM-5 at the same temperature. The slightdecrease in selectivity could be ascribed to the oxidation of
Table 1 | Catalytic performances of the acetalization between benzaldehyde and 1-pentanol on MZSM-5 and Au/MZSM-5 (M 5 H1, Na1,Ca21, or La31) under visible light irradiation
Catalyst Conv.a (%) Sele.b (%) Yield (%) Reaction rate (1023 molg21 h21)
CaZSM-5 21.5 .99 21.3 4.37Au/CaZSM-5 62.2 99.1 61.6 12.79NaZSM-5 30.9 .99 31.6 6.28Au/NaZSM-5 52.5 97.8 51.3 10.80LaZSM-5 48.7 .99 48.2 9.90Au/LaZSM-5 58.4 96.5 56.4 12.01HZSM-5 53.8 .99 53.3 10.93Au/HZSM-5 55.8 98.7 55.1 11.48Silicalite-1 9.3 .99 9.2 1.91Au/Silicalite-1 11.5 96.5 11.1 2.37a: the conversion of benzaldehyde.b: the selectivity towards pentyloxy(phenyl)methanol. Reaction conditions: benzaldehyde (0.65 g), 1-pentanol (4.40 g); temperature (60uC), time (6 h); light intensity (0.5 W/cm2), wavelength range(420–800 nm); catalyst (0.05 g); atmosphere (air). No detectable reaction without catalysts.
Figure 2 | Characterizations of Au/Silicalite-1 and Au/MZSM-5 (M 5 H1, Na1, Ca21, or La31): (a) UV/Vis spectra, (b) XRD patterns, and (c) XPSspectra.
www.nature.com/scientificreports
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 3
benzaldehyde by oxygen inevitably adsorbed on catalysts42,43. Theseresults suggested the boosting effect of ENFE of Au-NPs held atdifferent temperatures, and that the largest net increase of conversionwas at 60uC. The reusability test shows that CaZSM-5 and Au/CaZSM-5 were very stable with above 95% retentions of originalconversions after five runs (see SI, Section S7). Furthermore, theacetalization reaction between cyclohexanone and methanol showedsimilar cascade enhancement effect from visible light to zeoiltes (seeSI, Section S8)31,44.
In summary, the present study unravels a cascade enhancementeffect from visible light to zeolite catalysts bridged via the ENFE ofAu-NPs. The enhancement effect holds great potential in modifyingthe molecular polarities which affect the activity and electrostaticbehavior of molecules and have broad applications in organicsynthesis, ionic liquids, nanofiltration membranes, molecular elec-tronics, and molecular self-assembly technology by means of non-covalent interactions45–47. This study should draw attention to anumber of critical issues following this topic, considering more than200 types of zeolites (IZA Framework Type Codes), and variousplasmonic metal (or alloy) nanostructures together with their wideapplications in sensing, solar panels, solar water splitting, photoche-mical synthesis, drug delivery, industrial processes of cracking andisomerization, and environmental remediation.
MethodsPreparation and ion-exchange of zeolites. All chemicals used for preparing zeoliteswere purchased from Sigma-Aldrich without further treatment. Silicalite-1 and ZSM-5 were synthesized by hydrothermal methods and were calcined at 550uC for 5 h withthe step of increasing temperature being 5uC/min to remove organic templates.
MZSM-5 (M 5 H1, Na1, Ca21, or La31) were obtained by standard ion-exchangeprocedures from the as-synthesized zeolites at 90uC for 3 h for each run, three timesin total, under continuous stirring with 0.1 mol/L NH4NO3 aqueous solution toprepare HZSM-5, 0.1 mol/L sodium chloride (NaCl) aqueous solution to prepareNaZSM-5, 0.1 mol/L calcium chloride (CaCl2) aqueous solution to prepare CaZSM-5, or 0.1 mol/L lanthanum(III) chloride (LaCl3) aqueous solution to prepare LaZSM-5. After each run of ion-exchange, the samples were washed thoroughly withdeionized water and then calcinations were conducted at 400uC for 3 hours.
Preparation of zeolites supported gold catalysts. Zeolites supported catalysts (Au/zeolite) catalysts were prepared by a reduction method. Typically, 1.25 g of zeolitefine powders were dispersed into 50 mL of 3.8 3 1023 mol/L aqueous solution ofchloroauric acid (HAuCl4). Then 0.125 g of poly(vinyl alcohol) (PVA) was dispersedin 10 mL of deionized water; and the PVA solutions were added into the mixture ofzeolite and HAuCl4 solution under stirring for 0.5 h. To this suspension, 0.5 mL of0.38 mol/L aqueous solution of tetrakis(hydroxymethyl) phosphonium chloride(THPC) was added drop by drop as the reducing agent, followed by adding 2.25 mLof 0.38 mol/L sodium hydroxide aqueous solution (NaOH). The mixture was stirredcontinuously for 2 h and aged statically for 24 h. Finally, the solid was washed withdeionized water three times and ethanol once; and the obtained solids were dried at60uC for 16 h. The dried solids were used directly as photocatalysts, denoted as Au/zeolite catalysts.
Characterization of catalysts. X-ray diffraction (XRD) patterns of the samples weredetected on a Philips PANalytical X’Pert PRO diffractometer using Cu Ka radiation(l 5 1.5418 A) at 40 kV and 40 mA. The diffraction data were collected from 5u to75uwith a resolution being 0.01u (2h). UV/Visible (UV/Vis) spectra were recorded ona Cary 5000 UV/Vis-NIR Spectrophotometer in the wavelength range of 200–800 nm. The XPS data were recorded on an ESCALAB 250 spectrometer and Al Karadiation was used as the X-ray source. The C1s peak at 284.8 eV was used as areference for the calibration of the binding energy scale. Transmission electronmicroscopy (TEM) images were taken with a Philips CM200 Transmission electronmicroscope employing an accelerating voltage of 200 kV. The specimens were finepowders deposited onto a copper microgrid coated with a holey carbon film. Thediffuse reflectance The FT-IR spectra were recorded on Nicolet Nexus 870 IR
Figure 3 | (a) The relationship between the C5O bond length (Angstrom) of benzaldehyde and the intensity of extra electrostatic fields simulated by the
density functional theory (DFT) method. (b) The net increase of the conversion of the condensation reaction between benzaldehyde and 1-pentanol was
calculated from Table 1. The net increase means the conversion on Au/MZSM-5 deducts the conversion on its counterpart of MZSM-5 (M 5 H1, Na1,
Ca21, or La31).
Figure 4 | The trend of conversion and selectivity of the acetalization between benzaldehyde and 1-pentanol varies as the function of light intensity (a),
cut-off wavelength (b) (e.g. 420 nm means the light wavelength ,420 nm is cut off, so the light used is from 420–800 nm), and the reaction temperature.
(c) Reaction conditions: benzaldehyde (0.65 g), 1-pentanol (4.40 g), Au/ZSM-5 (0.05 g), atmosphere (argon), reaction temperature 60uC, and reaction
time 6 h.
www.nature.com/scientificreports
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 4
spectrophotometer equipped with a deuterated triglycine sulfate (DTGS) detectorand a Diamond Attenuated Total Reflectance (ATR) Smart Accessory. 128 scans werecollected for each measurement over the spectral range of 4000–650 cm21 with aresolution of 4 cm21.
Catalytic test of Au/zeolites. All the raw chemicals were purchased from Sigma-Aldrich and used without further treatment. The batch reactions were conducted in around-bottomed 50-mL transparent glass flask equipped with a sealed spigot and amagnetic stirrer. The reaction temperature was controlled by a portable air-conditioner in a sealed box. The flask was irradiated with a 500-Walt Halogen lamp,the UV light was removed by using a glass filter to cut off the light with the wavelengthbeing shorter than 420 nm to avoid the possibility of direct inter-band transition ingold. The intensity of light source was from 0 (light off) to 0.505 W/cm2. Aliquots(0.5 mL) were collected at given time intervals and filtrated through a Millipore filter(pore size 0.45 mm) to remove the catalyst particles. Control experiments wereperformed without light irradiation, maintaining the other conditions identical. Thefiltrates were analyzed by a Gas Chromatography (HP6890, HP-5 column) and GC-MS (6890-5793, HP-5MS column) was used to determine the components.Quantification of the products was obtained from the peak area ratios of the productand its corresponding reactant. The typical details of the chosen two reactions were asthe following: the acetalization between benzaldehyde and 1-pentanol. Typically,0.65 g of benzaldehyde was added into 4.40 g of 1-pentanol, and then 0.05 g catalystwas involved. The reaction temperature was controlled at 60uC. The acetalization ofcyclohexanone with methanol produced dimethyl acetals. Typically, 1.0 g ofcyclohexanone was mixed with 10 mL of methanol, and then 0.05 g of catalyst wasadded into this mixture. The reaction temperature was controlled at 40uC, andsamples were withdrawn every 2 h.
1. El-Sayed, M. A. Some interesting properties of metals confined in time andnanometer space of different shapes. Acc. Chem. Res. 34, 257–264 (2001).
2. Watanabe, K., Menzel, D., Nilius, N. & Freund, H.-J. Photochemistry on metalnanoparticles. Chem. Rev. 106, 4301–4320 (2006).
3. Linic, S., Christopher, P. & Ingram, D. B. Plasmonic-metal nanostructures forefficient conversion of solar to chemical energy. Nat. Mater. 10, 911–921 (2011).
4. Chen, X., Zhu, H. Y., Zhao, J. C., Zheng, Z. F. & Gao, X. P. Visible-light-drivenoxidation of organic contaminants in air with gold nanoparticle catalysts on oxidesupports. Angew. Chem. Int. Ed. 47, 1–5 (2008).
5. Zhang, X. G., Ke, X. B. & Zhu, H. Y. Zeolite-supported gold nanoparticles forselective photooxidation of aromatic alcohols under visible-light irradiation.Chem. Euro. J. 18, 8048–8056 (2012).
6. Zhu, H. Y., Ke, X. B., Yang, X. Z., Sarina, S. & Liu, H. W. Reduction ofnitroaromatic compounds on supported gold nanoparticles by visible andultraviolet light. Angew. Chem. Int. Ed. 49, 9657–9661 (2010).
7. Ke, X. B. et al. Tuning the reduction power of supported gold nanoparticlephotocatalysts for selective reductions by manipulating the wavelength of visiblelight irradiation. Chem. Commun. 48, 3509–3511 (2012).
8. Christopher, P., Xin, H. L. & Linic, S. Visible-light-enhanced catalytic oxidationreactions on plasmonic silver nanostructures. Nat. Chem. 3, 467–472 (2011).
9. Marimuthu, A., Zhang, J. W. & Linic, S. Tuning selectivity in propyleneepoxidation by plasmon mediated photo-switching of Cu oxidation state. Science29, 1590–1593 (2013).
10. Wang, F., Li, C. H., Chen, H. J., Jiang, R. B., Sun, L.-D., Li, Q., Wang, J. F., Yu, J. C.& Yan, C.-H. Plasmonic harvesting of light energy for Suzuki coupling reactions.J. Am. Chem. Soc. 135, 5588–5601 (2013).
11. Sarina, S. et al. Enhancing catalytic performance of palladium in gold andpalladium alloy nanoparticles for organic synthesis reactions through visible lightirradiation at ambient temperatures. J. Am. Chem. Soc. 135, 5793–5801 (2013).
12. Xiao, M. D. et al. Plasmon-enhanced chemical reactions. J. Mater. Chem. A 1,5790–5805 (2013).
13. Nie, S. & Emory, S. R. Probing single molecules and single nanaoparticles bysurface-enhanced Raman scattering. Science 275, 1102–1106 (1997).
14. Xu, X. B., Kim, K., Li, H. F. & Fan, D. L. Ordered arrays of Raman nanosensors forultrasensitive and location predictable biochemical detection. Adv. Mater. 24,5457–5463 (2012).
15. Tang, L. et al. Nanometer-scale germanium photodetector enhanced by a near-infrared dipole antenna. Nat. Photonics 2, 226–229 (2008).
16. Liu, W. J. et al. Gold nanorod@chiral mesoporous silica core2shell nanoparticleswith unique optical properties. J. Am. Chem. Soc. 135, 9659–9664 (2013).
17. Challener, W. A. et al. Heat-assisted magenetic recording by a near fieldtransducer with efficient optical energy transfer. Nat. Photonics, 3, 220–224(2009).
18. Maier, S. A. et al. Local detection of electromagnetic energy transport below thediffraction limit in metal nanoparticle plasmon waveguides. Nat. Mater. 2,229–232 (2003).
19. Shelby, R. A., Smith, D. R. & Schultz, S. Experimental verification of a negativeindex of refraction. Science 292, 77–79 (2001).
20. Gan, Q. Q., Bartoli, F. J. & Kafafi, Z. H. Plasmonic-enhanced organicphotovoltaics: breaking the 10% efficiency barrier. Adv. Mater. 25, 2385–2396(2013).
21. Gu, M. et al. Nanoplasmonics: a frontier of photovoltaic solar cells. Nanophotonics1, 235–248 (2012).
22. Awazu, K. et al. A plasmonic photocatalyst consisting of silver nanoparticlesembedded in titanium dioxide. J. Am. Chem. Soc. 130, 1676–1680 (2008).
23. Bordiga, S., Garrone, E., Lamberti, C. & Zecchina, A. Low-temperature Fouriertransform infrared study of the interaction of CO with cations in alkali-metalexchanged ZSM-5 zeolites. J. Chem. Soc. Fraday Trans. 90, 3367–3372 (1994).
24. Xiang, Y., Larsen, S. C. & Grassian, V. H. Photooxidation of 1-alkenes in zeolites: astudy of the factors that influence product selectivity and formation. J. Am. Chem.Soc. 121, 5063–5072 (1999).
25. Tsutsumi, K. &Takahashi, H. A study of the nature of active sites on zeolites by themeasurement of heat of immersion. II. Effects of silica/alumina ratio toelectrostatic-field strength of calcium-exchanged zeolites. J. Phys. Chem. 76,110–115 (1972).
26. Sun, H., Blatter, F. & Frei, H. Selective oxidation of toluene to benzaldehyde by O2
with visible light in Barium(21)- and Calcium(21)-exchanged zeolite Y. J. Am.Chem. Soc. 116, 7951–7952 (1994).
27. Sun, H., Blatter, F. & Frei, H. Cyclohexanone from cyclohexane and O2 in a zeoliteunder visible light with complete selectivity. J. Am. Chem. Soc. 118, 6873–6879(1996).
28. Blatter, F. & Frei, H. Selective photooxidation of small alkenes by O2 with red lightin zeolite Y. J. Am. Chem. Soc. 116, 1812–1820 (1994).
29. Frei, H. Selective hydrocarbon oxidation in zeolites. Science 313, 309–310 (2006).30. Liu, F. J. et al. ZSM-5 zeolite single crystals with b-axis-aligned mesoporous
channels as an efficient catalyst for conversion of bulky organic molecules. J. Am,Chem. Soc. 134, 4557–4560 (2012).
31. Iwamoto, M., Tanaka, Y., Sawamura, N. & Namba, S. Remarkable effect of poresize on the catalytic activity of mesoporous silica for the acetalization ofcyclohexanone with methanol. J. Am. Chem. Soc. 125, 13032–13033 (2003).
32. Kim, J. H., Coric, I., Vellalath, S. & List, B. The catalytic asymmetric acetalization.Angew. Chem. Int. Ed. 52, 4474–4477 (2013).
33. Ogura, M. et al. Alkali-treatment technique–new method for modification ofstructural and acid-catalytic properties of ZSM-5 zeolites. Appl. Catal. A 219,33–43 (2001).
34. Xu, J., Mojet, B. L., van Ommen, J. G. & Lefferts, L. Effect of Ca21 position in zeoliteY on selective oxidation of propane at room temperature. J. Phys. Chem. B 108,15728–15734 (2004).
35. Khatri, O. M., Murase, K. & Sugimura, H. Structural organization of goldnanoparticles onto the ITO surface and its optical properties as a function ofensemble size. Langmuir 24, 3787–3793 (2008).
36. Jin, F. & Li, Y. D. A FTIR and TPD examination of the distributive properties ofacid sites on ZSM-5 zeolite with pyridine as a probe molecule. Catal. Today 145,101–107 (2009).
37. Cho, H., Park, H., Russell, T. P. & Park, S. Precise placements of metalnanoparticles from reversible block copolymer nanostructures. J. Mater. Chem.20, 5047–5051 (2010).
38. Dunne, J. A., Rao, M., Sircar, S., Gorte, R. J. & Myers, A. L. Calorimetric heats ofadsorption and adsorption isotherms. 2. O2, N2, Ar, CO2, CH4, C2H6, and SF6 onNaX, H-ZSM-5, and Na-ZSM-5 zeolites. Langmuir 12, 5896–5904 (1996).
39. Bar, T., Visart de Bocarme, T., Nieuwenhuys, B. E. & Kruse, N. CO oxidation ongold surfaces studied on the atomic scale. Catal. Lett. 74, 127–131 (2001).
40. Wustholz, K. L. et al. Structure-activity relationships in gold nanoparticle dimersand trimers for surface-enhanced raman spectroscopy. J. Am. Chem. Soc. 132,10903–10910 (2010).
41. Large, N., Abb, M., Aizpurua, J. & Muskens, O. L. Plasmonic near-electric fieldenhancement effects in ultrafast photoelectron emission: correlated spatial andlaser polarization microscopy studies of individual Ag nanocubes. Nano Lett. 10,1741–1746 (2010).
42. Bulanin, K. M. & Lobo, R. F. Low-temperature adsorption of N2, O2, and D2 onLiX, NaX, and NaLiX zeolites studied by FT-IR spectroscopy. J. Phys. Chem. B104, 1269–1276 (2000).
43. Xu, J., Mojet, B. L., van Ommen, J. G. & Lefferts, L. Formation of M21(O2)(C3H8)species in alkaline-earth-exchanged Y zeolite during propane selective oxidation.J. Phys. Chem. B 109, 18361–18368 (2005).
44. Shetti, V. N., Kim, J., Srivastava, R., Choi, M. & Ryoo, R. Assessment of themesopore wall catalytic activities of MFI zeolite with mesoporous/microporoushierarchical structures. J. Catal. 254, 296–303 (2008).
45. Van der Bruggen, B., Schaep, J., Wilms, D. & Vandecasteele, C. Influence ofmolecular size, polarity and charge on the retention of organic molecules bynanofiltration. J. Membrane Sci. 156, 29–41 (1999).
46. Lewis, P. A., Inman, C. E., Maya, F., Tour, J. M., Hutchison, J. E. & Weiss, P. S.Molecular engineering of the polarity and interactions of molecular electronicswitches. J. Am. Chem. Soc. 127, 17421–17426 (2005).
47. Singh, A. S. & Sun, S.-S. Dynamic self-assembly of molecular capsules via solventpolarity controlled reversible binding of nitrate anions with C3 symmetric tripodalreceptors. Chem. Commun. 47, 8563–8565 (2011).
AcknowledgmentsThis research is supported by the Australian Research Council (ARC) and X. Ke is indebtedto QUT and the Queensland State Government for a Smart Futures Fellowship.
www.nature.com/scientificreports
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 5
Author contributionsX.Z. conducted the experiments, sample characterization and data analysis. X.K. designedthe experiments and prepared parts of the materials. A.D. conducted DFT calculations andhelped revise the manuscript. H.Z. proposed the study and contributed importantsuggestions. The manuscript was written by X.Z. and X.K.
Additional informationSupplementary information accompanies this paper at http://www.nature.com/scientificreports
Competing financial interests: The authors declare no competing financial interests.
How to cite this article: Zhang, X.G., Ke, X.B., Du, A.J. & Zhu, H.Y. Plasmonicnanostructures to enhance catalytic performance of zeolites under visible light. Sci. Rep. 4,3805; DOI:10.1038/srep03805 (2014).
This work is licensed under a Creative Commons Attribution-NonCommercial-NoDerivs 3.0 Unported license. To view a copy of this license,
visit http://creativecommons.org/licenses/by-nc-nd/3.0
www.nature.com/scientificreports
SCIENTIFIC REPORTS | 4 : 3805 | DOI: 10.1038/srep03805 6
p1
Supporting Information
Plasmonic nanostructures to enhance catalytic performance of zeolites under visible
light
Xingguang Zhang, Xuebin Ke,* Aijun Du, and Huaiyong Zhu
Table of Contents
Section 1. Control experiments of the acetalization between benzaldehyde and 1-pentanol (Table S1) p2
Section 2. Analysis of Brønsted acid sites on catalysts from the IR-ATR results (Figure. S1, Figure. S2) p2
Section 3. TEM images and the distribution of Au-NPs (Figure. S3) p4
Section 4. The computer simulation method p4
Section 5. Polarized electrostatic fields (PEF) of zeolites p5
5.1 Calculation of the PEF of cations in zeolites (Table S2)
5.2. Influential factors on the PEF of cations in zeolites
Section 6. XPS analyses of the gold content, the Si/Al ratio, and the cation contents (Table S3) p6
Section 7 Reusability test of the catalyst CaZSM-5 and Au/CaZSM-5 (Figure. S4) p7
Section 8. The acetalization between cyclohexanone and methanol (Table S4, Table S5, Figure. S5) p7
References p9
p2
Section S1. Control experiments of the acetalization between benzaldehyde and 1-pentanol
Typically, 0.65 g of benzaldehyde was added into 4.40 g of 1-pentanol, and then 0.05 g catalyst was added. The reaction
temperature was kept at 60oC in a silicone oil bath. The results were listed in Table S1.
Table S1 | Catalytic performances for acetalization between benzaldehyde and 1-pentanol on MZSM-5 and Au/MZSM-5 (M=H+, Na
+, Ca
2+, or La
3+)
with light off.
Catalyst Conversiona (%) Selectivity
b (%) Yield (%) Reaction rate (10
-3 molg
-1h
-1)
CaZSM-5 19.7 >99 19.5 4.00
Au/CaZSM-5 22.3 >99 22.1 4.53
NaZSM-5 31.7 >99 31.4 6.44
Au/NaZSM-5 36.9 >99 36.5 7.50
LaZSM-5 49.8 >99 49.3 10.12
Au/LaZSM-5 47.7 >99 47.2 9.69
HZSM-5 55.2 >99 54.6 11.21
Au/HZSM-5 54.3 >99 53.8 11.03
Silicalite-1 8.6 >99 8.5 1.75
Au/Silicalite-1 9.7 >99 9.6 1.97
a: Conversion refers to the conversion of benzaldehyde.
b: Selectivity refers to the selectivity towards pentyloxy(phenyl)methanol. Reaction
conditions: of benzaldehyde (0.65 g) and 1-pentanol (4.40 g); catalyst (0.05 g); atmosphere (air); temperature (60oC); time (6 h). No reaction was
detectable without catalysts.
Section S2. Analysis of Brønsted acid sites on catalysts from the IR-ATR results
The Brønsted acid sites of MZSM-5 and Au/ZSM-5 were investigated by the adsorption of 2-(hydroxymethyl) pyridine
(2-pyridinemethanol) on IR-ATR (attenuated total reflectance). The samples were prepared as the following. Typically,
0.025 g sample was heated to 400oC for 2 h in a clean crucible with a lid, and then the sample was cooled automatically to
150oC at which 0.1 mL 2-pyridinemethanol (Sigma-Aldrich) was added directly into the sample for adsorption. After
adsorbing, the IR-ATR spectra of these treated samples, untreated MZSM-5 and Au/MZSM-5, and pure 2-pyridinemethanol
were collected.
Based on the literature reports,s1, s2, s3 the band at 1530 cm-1 represented the Brønsted acid sites on which the adsorbed
species were 2- (hydroxymethyl) pyridinium ions and the band at 1415 cm-1 was assigned to Lewis acid sites on which the
adsorbed species were 2- (hydroxymethyl) pyridine complexes, as shown in Figure. S1a and S1b. Therefore, the IR-ATR
spectra could give four conclusions based on Figure. S1c and S1d) Silicalite-1 and Au/Silicalite-1 had nearly undetectable
Brønsted acids; 2) MZSM-5 had Brønsted acids with their peaks centered at around 1530 cm-1; 3) HZSM-5 had more
Brønsted acids than CaZSM-5 as indicated by the peak areas; 4) The acid sites preserved well after loading of Au-NPs.
p3
1700 1600 1500 1400 130050
60
70
80
90
100
110
(a)1415
Tra
nsm
itance (
%)
Wavenumber (cm-1)
1530
2-(hydroxymethyl)pyridine
Au/HZSM-5 + 2-(hydroxymethyl)pyridine
Au/Silicalite-1 + 2-(hydroxymethyl)pyridine
Silicalite-1 + 2-(hydroxymethyl)pyridine
HZSM-5 + 2-(hydroxymethyl)pyridine
HZSM-5
Silicalite-1
Au/Slicalite-1
Au/HZSM-5
1700 1600 1500 1400 130050
60
70
80
90
100
110
(b)14151530
Tra
nsm
itta
nce (
%)
Wavenumber (cm-1)
2-(hydroxymethyl)pyridine
Au/CaZSM-5 + 2-(hydroxymethyl)pyridine
Au/Silicalite-1 + 2-(hydroxymethyl)pyridine
Silicalite-1 + 2-(hydroxymethyl)pyridine
CaZSM-5 + 2-(hydroxymethyl)pyridine
CaZSM-5
Silicalite-1
Au/Slicalite-1
Au/CaZSM-5
1575 1550 1525 1500 1475
(c) 1530
CaZSM-5
NaZSM-5
HZSM-5
LaZSM-5
Silicalite-1
Tra
nsm
itance
Wavenumber (cm-1)
1575 1550 1525 1500 1475
(d) 1530
Au/CaZSM-5
Au/NaZSM-5
Au/HZSM-5
Au/LaZSM-5
Au/Silicalite-1
Tra
nsm
itta
nce
Wavenumber (cm-1)
Figure S1 | The ATR results of (a) Silicalite-1, Au/Silicalite-1, HZSM-5, Au/HZSM-5, pure 2-(hydroxymethyl)pyridine, and these catalysts treated
by absorbing 2--(hydroxymethyl)pyridine; (b) Silicalite-1, Au/Silicalite-1, CaZSM-5, Au/CaZSM-5, pure 2-(hydroxymethyl)pyridine, and these
catalysts treated by absorbing 2--(hydroxymethyl)pyridine; (c) and (d) Comparison of peaks centerd at 1530 cm-1
which showed the Brønsted
acids on MZSM-5 and Au/MZSM-5 (M=H+, Na
+, Ca
2+, or La
3+).
Under the same experimental schedule, pyridine was also used as the probe molecules to detect the Brønsted acids, but
no peaks of Brønsted acids were observed, probably because the interaction between pyridine and MZSM-5 was too weaker
to be detected by IR-ART at room temperature and in air atmosphere.
1700 1600 1500 1400 130020
30
40
50
60
70
80
90
100
110
Pyridine
Au/HZSM-5 + Pyridine
Au/Silicalite-1 + Pyridine
Silicalite-1 + Pyridine
HZSM-5 + Pyridine
HZSM-5
Silicalite-1
Au/Slicalite-1
Au/HZSM-5
(a)1415
Tra
nsm
itance (
%)
Wavenumber (cm-1)
1530
1700 1600 1500 1400 130020
30
40
50
60
70
80
90
100
110
(b)14151530
Tra
nsm
itta
nce (
%)
Wavenumber (cm-1)
Pyridine
Au/CaZSM-5 + Pyridine
Au/Silicalite-1 + Pyridine
Silicalite-1 + Pyridine
CaZSM-5 + Pyridine
CaZSM-5
Silicalite-1
Au/Slicalite-1
Au/CaZSM-5
Figure S2 | The ATR results of (a) Silicalite-1, Au/Silicalite-1, HZSM-5, Au/HZSM-5, pure 2-(hydroxymethyl)pyridine, and these catalysts treated
by absorbing 2--(hydroxymethyl)pyridine; (b) Silicalite-1, Au/Silicalite-1, CaZSM-5, Au/CaZSM-5, pure 2-(hydroxymethyl)pyridine, and these
catalysts treated by absorbing 2--(hydroxymethyl)pyridine.
p4
Section S3. TEM images and the distribution of Au-NPs
4 6 8 10 12 14 16 18 20 22 24 260
5
10
15
20
25
30Au/Silicalite-1
Pe
rcen
tage
(%
)
Particle size (nm) 2 4 6 8 10 12 14 16 18
0
5
10
15
20
25
30Au/CaZSM-5
Pe
rcen
tage
(%
)
Particle size (nm)
Figure S3 | TEM analyses of two typical catalysts: Au/Silicalite-1 and Au/CaZSM-5.
The Transmission-Electron-Spectroscopy (TEM) was conducted to determine the size, shape and distribution of Au-NPs
on two typical catalysts of Silicalite-1 and CaZSM-5. Figure. S3 indicated that the shape of Au-NPs was generally spherical
and that they were distributed better on Silicalite-1 and formed clusters on CaZSM-5. The size distributions were also
provided, showing that the size of Au-NPs on Silicalite-1 and CaZSM-5 was in the range of 6-18 nm.
Section S4. The computer simulation method
All the ab initio calculations were performed with the Gaussian09 package.s4 The Density Functional Theory level
method B3lYP with basis set of 6-31G(d,P) was employed.s5, s6 Geometry optimizations are first performed in the absence of
electric field for benzaldehyde and -pentanol, respectively. Then a finite field at various sizes was added along a specific axis
and all the geometries were fully relaxed in the presence of an electric field until a tight convergence reached.
Section S5. Polarized electrostatic fields (PEF) of zeolites
S5.1 Calculation of the PEF of cations in zeolites
Several reported values of the PEF of ion-exchanged ZSM-5 were given in Table S2, and two methods were used to
estimate the PEF of the other cation-treated ZSM-5.
The first method was based on the low-temperature CO adsorption bands:s7
Equation (1):E = 6.1764 × 10-4·v(CO)2 – 2.4976·v(CO) + 2516, in which:
The CO frequencies (v(CO)) was in wavenumber (for free CO, it was at 2143 cm-1)
The second method was based on the equation reported in Rybakov and coworkers study:s8
Equation (2):E = q/rn, in which:
q is the charge, for Na+, q=1, for Ca2+, q=2, and for La3+, q =3;
r is the distance from the site to the point charge q (here the radius of cation was used for simplification);
n is a factor that can be calculated from a reported zeolite. For example, NaZSM-5 is used for calculating the n factor of
the monovalent cations, and BaZSM-5 for the divalent cations. (http://boomeria.org/chemlectures/textass2/firstsemass.html).
p5
Table S2. Reported and calculated polarized electrostatic field (PEF) strength of ion-exchanged ZSM-5.
MZSM-5 Reported
PEF (V/nm)
Calculated PEF from
Equation (1) (V/nm)
v(CO)
cm-1
Calculated PEF from
Equation (2) (V/nm)
Ion Radius
(Å)
HZSM-5 3.0 s9
3.8 2170 s11
unsuitable s14
0.53
LiZSM-5 7.2 2188 s11
8.1 0.68
NaZSM-5 6.2 s9
5.3 2178 s11
6.2 0.95
KZSM-5 3.1 2166 s11
4.9 1.33
MgZSM-5 11.9 0.65
CaZSM-5 8.3 2193 s12
9.1 0.99
SrZSM-5 7.7 2190 s12
8.3 1.13
BaZSM-5 7.4 s10
7.0 2187 s12
7.4 1.35
La(III)ZSM-5 10.7 1.06
Ce(III)ZSM-5 10.9 1.03
Pd(III)ZSM-5 14.7 2221 s13
14.7 0.64
S5.2. Influential factors on the PEF of cations in zeolites
The data of PEF listed in the above Table S2 might not be absolutely precise; however, they could qualitatively reflect
the tendency of the PEF in a given zeolite host. According to the literature reports, four general conclusions can be
summarized (to be clear, these tendencies apply to a single cation in zeolite pores, namely, even though a cation has a strong
PEF, it does not necessarily mean that the net PEF within the whole zeolite host is strong because the content of cations may
be very low, depending on the Si/Al ratio).
Point 1: the PEF increases with increasing cation charges, for instance, ECaZSM-5 > ENaZSM-5. It is reported that divalent
cations generally have stronger electrostatic fields than monovalent cations because the monovalent cations, e.g. H+, or Na+
balanced the negatively charged Al sites one to one. As for divalent cations, Kazansky and co-workers propose a model for
localization of bivalent cations of zinc cations (Zn2+) in high silica zeolites with distantly placed Al atoms in the framework.
The model indicates that some of the bivalent cations Mg2+ and Ca2+ can be localized at the isolated singly negatively
charged Al occupied oxygen tetrahedra. In parallel the equivalent number of the isolated framework Al atoms remains
without compensating protons or bivalent cations, and their negative charges are compensated indirectly by coulomb
interaction with the surrounding excessively charged cationic sites. The partially compensated positive electric charges
possess unusually high chemical activity.s15, s16
Point 2: the PEF increases with increasing the charge/radius ratio for a given zeolite, for instance, EMg/ZSM-5 > ECaZSM-
5 > EBaZSM-5. Xu and co-workers find that the electrostatic field of alkaline-earth cation increases with decreasing cation
radius, which results in an increased polarization of adsorbed oxygen in the order BaY < SrY < CaY. According to this
conclusion, the electrostatic field strength of CaZSM-5 should be larger than BaZSM-5 (7.4 V/nm, reported) with other
conditions be identical. Therefore, the calculated value 8.3 V/nm is reasonable.s17, s18
Point 3: the PEF increases with increasing Si/Al ratios. The correlation between the Si/Al ratio and the PEF of zeolites
has been investigated by measurements of the heats of immersion into various organic liquids as for Na- and Ca-exchanged
zeolites. The PEF of Na-form zeolites is not much affected by the Si/Al ratio. However, as for Ca-exchanged zeolites, raising
Si/Al ratio increases the PEF, probably because univalent cations like Na+, the number of the cation and the number of the
site that form the electrostatic field decrease with an increase in the Si/Al ratio, the net PEF becomes smaller. On the other
hand, in the case of bivalent cations like Ca2+, parts of cation sites in the large cavity become to be positively charged and
others to be negatively charged with an increase in the Si/Al ratio. The polarization thus occurs, and a strong net electrostatic
p6
field is formed. This tendency seems remarkable when the Si/Al ratio is high. Nevertheless, if the Al sites are too few, e.g.
Silicalite-1 has no Al sites; the net electrostatic field strength decreases dramatically.s7,s19-s21
Therefore it is easy to understand that the electrostatic field strength of rare-earth ions of La3+ or Ce3+ is generally higher
than that of alkaline-earth ions of Ca2+or Ba2+, but the total quantity of La3+ ions is quite low because one La3+ ion
corresponds to three Na+ ions, and one and a half Ca2+ ions, thus the net electrostatic strength of the whole zeolite particle
may be not strong. To illustrate, if a zeolite had six negatively-charged sites, it required six H+/Na+ cations, or three Ca2+
cations, or two La3+ cations to compensate/balance the framework negative charges (please see the illustration below,
Scheme s1). The change from H+, Na+, Ca2+, to La3+ is not only in valences (cation charges) and strength of PEF, but also in
the number of cations (cation density), and cation/radius ratio. Therefore, the net effect of enhancement on boosting the
catalytic performance of a zeolite should be a synergetic effect of these factors. Even though the original PEF of La3+ (10.7
V/nm) is higher than that of Ca2+ (8.3 V/nm), the number of La3+ on ZSM-5 is smaller, thus leading to a lower net
enhancement effect over a given zeolite catalyst.
Scheme s1: Illustration of the compensation relationship between negatively-charged framework sites and extra-framework cations of Na+,
Ca2+
, and La3+
.
Point 4: The PEF is affected by the location cations. ZSM-5 with is characterized by a 2D pore system with straight,
parallel channels intersected by zigzag channels (the detailed 3D structure can be found on the website: http://www.iza-
structure.org/databases). Both channels consist of 10-membered rings with a diameter of 0.53 × 0.56 nm (straight channels)
and 0.51 × 0.5 nm (sinusoidal channels). IR studies of H2 and CO adsorption indicate that the cations are preferentially
located at the intersections of the sinusoidal and straight channels at the edge of a four-membered ring (site I). Additionally,
small cations, like Na+ ions are also found in small cavities above the sinusoidal channel (site II), but MAS-NMR studies
showed a low occupancy of this site (10%).s22,s23
Section S6. XPS analyses of the gold content, the Si/Al ratio, and the cation contents
The XPS results of the gold content, the Si/Al ratio, and the cation contents were given in Table S3. The MZSM-5 used
in the experiment might not have a 100% ion-exchange and might contain residual Na+, or H+ ions, but these residual ions
were negligible and undetectable. The Si/Al ratios of MZSM-5 and Au/MZSM-5 were generally remained stable and the
average value of Si/Al ratio was 13.95 for MZSM-5, and 14.00 for Au/MZSM-5. Therefore, the influence of Si/Al ratio on
the electric field strength of zeolites could be ruled out. The gold contents on MZSM-5 were similar, with the average value
Si
O O
o
O O
o Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Na+
Na+
Na+
Na+
Na+
Na+
Si
O O
o
O O
o Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Ca2+
Ca2+
Ca2+
Si
O O
o
O O
o Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
Al
O
O
Si
O
O
La3+
La3+
Radii of La3+
0.106 nm
Radii of Ca2+
0.099 nm
Radii of Na+
0.095 nm (-) (-) (-) (-) (-) (-)
(-) (-) (-) (-) (-) (-)
(-) (-) (-) (-) (-) (-)
p7
being 2.19%. Likewise, the influence of the content of gold was negligible. Therefore, the primary influential factor on the
electric field strength boiled down to the extra-framework cations: charges, charge/radius ratio, and density (amount).
Table S3. The gold content on MZSM-5, Si/Al ratio of catalysts, and the content of cations on catalysts detected or calculated from the XPS
results.
Catalyst Au (wt%) Si/Al (Ratio) Cation (At%)
HZSM-5 --a 12.94 --
NaZSM-5 -- 13.32 (Na) 0.85 (Na+/Al = 0.47)
CaZSM-5 -- 14.94 (Ca) 0.41 (Ca2+
/Al = 0.23)
LaZSM-5 -- 14.66 (La) 0.17 (La3+
/Al = 0.10)
Slicalite-1 -- -- --
Au/HZSM-5 2.09 15.26 --
Au/NaZSM-5 2.40 12.70 (Na) 0.76 (Na+/Al = 0.43)
Au/CaZSM-5 2.28 14.89 (Ca) 0.38 (Ca2+
/Al = 0.25)
Au/LaZSM-5 1.98 13.16 (La) 0.15 (La3+
/Al = 0.09)
Au/Silicalite-1 2.13 -- --
a: -- refers to “undetected”
Section S7. Reusability of the catalyst CaZSM-5 and Au/CaZSM-5
The reusability of the CaZSM-5 and Au/CaZSM-5 for the acetalization between benzaldehyde and 1-pentanol was
conducted by recycling the catalyst solids after reaction and then washed thoroughly with deionized water. The recycled
catalysts were dried overnight at 60°C in a vacuum oven and used as such. These two catalysts showed quite slight changes
in the activity; meanwhile, the selectivity remained excellent (>99%) after five runs. These results indicated that CaZSM-5
and Au/CaZSM-5 were stable and reusable.
1 2 3 4 510
20
30
40
50
60
70
Au/CaZSM-5
CaZSM-5Co
nve
rsio
n (
%)
Run
Figure S4 | Test of the reusability of CaZSM-5 and Au/CaZSM-5 in the acetalization reaction between benzaldehyde and 1-pentanol after five
runs.
Section S8. The acetalization between cyclohexanone and methanol
Typically, 1.0 g of cyclohexanone was mixed with 10 mL of methanol, and then 0.05 g of catalyst was added into this
mixture. The reaction temperature was controlled at 40oC in an oil bath. The results were listed in Table S4 and S5.
With light on, the conversion on Au/NaZSM-5, Au/CaZSM-5, and Au/LaZSM-5 improved considerably compared with
their counterparts without Au-NPs (Table S4). The boosting mechanism should resemble the aforementioned acetalization
reaction, as the DFT calculation clearly demonstrated that the C=O bond of cyclohexanone (3.25 Debye) could be stretched
p8
by extra electric fields, but the methanol molecule (1.72 Debye) was unaffected. The maximum net conversions also
appeared on Au/CaZSM-5.
Table S4 | Catalytic performances of and the acetalization between cyclohexanone and methanol on MZSM-5 and Au/MZSM-5 (M=H+, Na
+, Ca
2+,
or La3+
) under the irradiation of visible light.
Catalyst OCH3
OCH3CH3OHO
Conversiona
(%)
Selectivityb
(%)
Yield
(%)
Reaction rate
(10-3
molg-1
h-1
)
CaZSM-5 20.1 >99 19.9 20.94
Au/CaZSM-5 61.3 >99 60.7 63.85
NaZSM-5 38.9 >99 38.5 40.52
Au/NaZSM-5 56.9 >99 56.3 59.27
LaZSM-5 37.6 >99 37.2 39.16
Au/LaZSM-5 48.2 >99 47.7 50.21
HZSM-5 52.3 >99 51.8 54.48
Au/HZSM-5 53.6 >99 52.1 54.78
Silicalite-1 5.2 >99 5.2 5.42
Au/Silicalite-1 7.3 >99 7.2 7.60
a: Conversion refers to the conversion of cyclohexanone.
b: Selectivity refers to the selectivity towards dimethyl acetal (dimethoxycyclohexane).
Reaction conditions: cyclohexanone (1.0 g), methanol (10 mL), temperature, (40oC), time (6h), light intensity (0.505 W/cm
2), wavelength range
(420-800 nm); catalyst (0.05 g), atmosphere (air). No reaction was detectable without catalysts.
With light off, the conversion on Au/HZSM-5, Au/NaZSM-5, Au/CaZSM-5, and Au/LaZSM-5 did not improve much
compared with their counterparts without Au-NPs (Table S5).
Table S5 | Catalytic performances for the acetalization of cyclohexanone with methanol (ACM) on MZSM-5 and Au/MZSM-5 (M=H+, Na
+, Ca
2+, or
La3+
) with light off.
Catalyst Conversiona (%) Selectivity
b (%) Yield (%) Reaction rate (10
-3 molg
-1h
-1)
CaZSM-5 18.4 >99 18.2 19.17
Au/CaZSM-5 17.6 >99 17.4 18.34
NaZSM-5 39.7 >99 39.3 41.35
Au/NaZSM-5 38.3 >99 37.9 39.89
LaZSM-5 38.3 >99 37.9 39.89
Au/LaZSM-5 41.8 >99 41.4 43.54
HZSM-5 51.8 >99 51.3 53.96
Au/HZSM-5 50.9 >99 50.4 53.02
Slicalite-1 3.7 >99 3.7 3.79
Au/silicalite-1 5.8 >99 5.7 6.04
a: Conversion refers to the conversion of cyclohexanone.
b: Selectivity refers to the selectivity towards dimethyl acetal (dimethoxycyclohexane).
Reaction conditions: cyclohexanone (1.0 g) methanol (10 mL); catalyst (0.05 g); atmosphere (air), temperature (40oC); time (6 h). No reaction was
detectable without catalysts.
p9
0 2 4 6 8 10 121.215
1.220
1.225
1.230
1.235
1.240
1.245 (a)
O
Electric-field Strength (V/nm)
C=
O B
ond L
ength
(Å
)
H Na Ca La
0
10
20
30
40(b)
Cations
Ne
t con
ve
rsio
n (
%)
Figure S5 | (a) The relationship between the C=O bond length (Angstrom) of cyclohexanone and the intensity of extra electrostatic fields
simulated by the density functional theory (DFT) method. (b) The net conversion of the acetalization reaction between cyclohexanone and
methanol was calculated from Table 2 in the main text. The net conversion means the conversion on Au/MZSM-5 deducts the conversion on
MZSM-5 (M=H+, Na
+, Ca
2+, or La
3+).
The DFT calculations demonstrated that the C=O bond length of cyclohexanone extended with increasing the extra
electric field strength. In detail, the C=O bond lengths of benzaldehyde were 1.223 Å, 1.227 Å, 1.232 Å, 1.237 Å, and 1.242
Å, when the electric field strengths were 0 V/nm, 2.58 V/nm, 5.16 V/nm, 7.74 V/nm, and 10.32 V/nm, respectively.. The
relationship between the C=O bond length and the electric field strength was linear (see Figure. S1a). The highest net
conversion appeared on the Ca2+ (see Figure. S1b).
References
s1. Barzetti, T., Selli, E., Moscotti, D. & Forni, L. Pyridine and ammonia as probes for FTIR analysis of solid acid catalysts. J. Chem. Soc. Faraday Trans. 92,
1401-1407 (1996).
s2. Zhao, G. L., Teng, J. W., Xie, Z. K., Jin, W. Q., Yang, W.M., Chen, Q. L. & Tang, Y. Effect of phosphorus on HZSM-5 catalyst for C4-olefin cracking
reactions to produce propylene. J. Catal. 248, 29-37 (2007).
s3. Jin, F. & Li, Y. D. A FTIR and TPD examination of the distributive properties of acid sites on ZSM-5 zeolite with pyridine as a probe molecule. Catal.
Today, 145, 101-107 (2009).
s4. Frisch, M. J., Trucks, G., Schlegel, H., Scuseria, G., Robb, M., Cheeseman, J., Scalmani, G., Barone, V., Mennucci, B. & Petersson, G. Gaussian 09;
Gaussian. Inc., Wallingford, CT 2009.
s5. Becke, A. D. Density-functional thermochemistry. III. the role of exact exchange. J. Chem. Phys. 98, 5648-5652 (1993).
s6. Lee, C. & Yang, W. Parr, R. G. Development of the Colle-Salvetti correlation-energy formula into a functional of the electron density. Phys. Rev. B 37, 785-
789 (1988).
s7. Panov, A. G., Larsen, R. G., Totah, N. I., Larsen, S. C. & Grassian, V. H. Photooxidation of toluene and p-xylene in cation-exchanged zeolites X, Y, ZSM-5,
and Beta: the role of zeolite physicochemical properties in product yield and selectivity. J. Phys. Chem. B 104, 5706-5714 (2000).
s8. Rybakov, A. A., Larin, A. V. & Zhidomirov, G. M. Computational differentiation of Brønsted acidity induced by alkaline earth or rare earth cations in
zeolites. Inorg. Chem. 51, 12165-12175 (2012).
s9. Dunne, J. A., Rao, M., Sircar, S., Gorte, R. J. & Myers, A. L. Calorimetric heats of adsorption and adsorption isotherms. 2. O2, N2, Ar, CO2, CH4, C2H6, and
SF6 on NaX, H-ZSM-5, and Na-ZSM-5 zeolites. Langmuir 12, 5896-5904 (1996).
s10. Xiang, Y., Larsen, S. C. & Grassian, V. H. Photooxidation of 1-alkenes in zeolites: a study of the factors that influence product selectivity and formation. J.
Am. Chem. Soc. 121, 5063-5072 (1999).
s11. Zecchina, A., Bordiga, S., Lamberti, C., Spoto, G. & Carnelli, L. Low-temperature Fourier transform infrared study of the interaction of CO with cations in
alkali-metal exchanged ZSM-5 zeolites. J. Phys. Chem. 98, 9577-9582 (1994).
s12. Kamble, V. S. & Gupta, N. M. On the role of balancing cations in the entrapment of CO in ZSM-5 zeolite at room temperature: FTIR study. Phys. Chem.
Chem. Phys. 2, 2661-2665 (2000).
s13. Chakarova, K., Ivanova, E., Hadjiivanov, K., Klissurski, D. & Knözinger, H. Co-ordination chemistry of palladium cations in Pd-H-ZSM-5 as revealed by
FTIR spectra of adsorbed and co-adsorbed probe molecules (CO and NO). Phys. Chem. Chem. Phys. 6, 3702-3709 (2004).
s14. According to Ref. s11, there is a strong interaction between H+ and the framework of ZSM-5 because hydrogen is partially covalently bonded to the
framework oxygen. As a consequence, only a part of the H+ positive charge is available, and the electric field around the proton is consequently reduced.
s15. Kazansky, V. & Serykh, A. A new charge alternating model of localization of bivalent cations in high silica zeolites with distantly placed aluminum atoms
in the framework. Micropor. Mesopor Mater. 70, 151-154 (2004).
s16. Xu, J., Mojet, B. L. & Lefferts, L. Effect of zeolite geometry for propane selective oxidation on cation electrostatic field of Ca2+ exchanged zeolites.
Micropor. Mesopor. Mater. 91, 187-195 (2006).
s17. Xu, J., Mojet, B. L., van Ommen, J. G. & Lefferts, L. Propane selective oxidation on alkaline earth exchanged zeolite Y: room temperature in situ IR study.
Phys. Chem. Chem. Phys. 5, 4407-4413 (2003).
p10
s18. Xu, J., van Ommen, J. G., Mojet, B. L. & Lefferts, L. Formation of M2+(O2)(C3H8) species in alkaline-earth-exchanged Y zeolite during propane selective
oxidation. J. Phys. Chem. B 109, 18361-18368 (2005).
s19. Tsutsumi, K. & Takahashi, H. A study of the nature of active sites on zeolites by the measurement of heat of immersion. II. Effects of silica/alumina ratio to
electrostatic-field strength of calcium-exchanged zeolites. J. Phys. Chem. 76, 110-115 (1972).
s20. Xiang, Y., Larsen, S. C. & Grassian, V. H. Photooxidation of 1-alkenes in zeolites: a study of the factors that influence product selectivity and formation. J.
Am. Chem. Soc. 121, 5063-5072 (1999).
s21. Rybakov, A. A., Larin, A. V. & Zhidomirov, G. M. Computational differentiation of Brønsted acidity induced by alkaline earth or rare earth cations in
zeolites. Inorg. Chem. 51, 12165-12175 (2012).
s22. Tsutsumi, K. & Takahashi, H. A study of the nature of active sites on zeolites by the measurement of heat of immersion. II. effects of silica/alumina ratio to
electrostatic-field Strength of calcium-exchanged zeolites. J. Phys. Chem. 76, 110-115 (1972).
s23. Xu, J., Mojet, B. L., van Ommen, J. G. & Lefferts, L. Effect of Ca2+ position in zeolite Y on selective oxidation of propane at room temperature. J. Phys.
Chem. B 108, 15728-15734 (2004).
85
5.2 Acetalisation reaction on zeolite catalysts – Efficient catalysts of
zeolite nanocrystals grown with a preferred orientation on nanofibres
Introductory remarks
This chapter reports an innovative structure—nanozeolites (as shell) grown with a
preferred orientation on ceramic nanofibres (as core). The Y-zeolite nanocrystals on
TiO2 nanofibres exhibited superior ability to catalyse acetalisation and
transesterification reactions, achieving high conversions to desired products with
selectivity of 100% under moderate conditions. This research was published in the
journal of ―Chemical communication‖[1]
.
Zeolites are important industrial catalysts that have been extensively applied in
the manufacture of fine chemicals and petrochemicals[2]
. The diffusion of reactants
within zeolite pores and the accessibility of active centres of zeolites determine the
catalytic performance of zeolite catalysts. The intra-crystalline diffusion of reactants,
intermediates, and products often adversely affects the performance when large
zeolite particles are used, especially in liquid-phase catalytic systems. Therefore,
zeolite nanocrystals have obvious advantages because more active sites can be
accessed by reactant molecules and the diffusion pathways are short[3]
. However, it is
difficult to synthesise discrete zeolite nanocrystals without aggregation, which
necessitates new synthetic methods to be developed to solve this problem.
This study demonstrated that the zeolite Y nanocrystals could be grafted on TiO2
nanofibres without aggregation[4, 5]
and that the zeolite@NFs composites exhibited
superior catalytic performance in the acetalisation reaction of cyclohexanone with
86
methanol and the transesterification of dimethyl carbonate with alcohols compared
with bulky zeolite particles and TiO2 nanofibres. Moreover, the orientation of the
zeolite nanocrystals with respect to the TiO2 substrate and the openings of the
nanozeolite micropore systems were certain, namely, with a preferred orientation
which was confirmed by the HRTEM analyses, so that the active sites of zeolites
were exposed to the reactants with a certain orientation. TiO2 NFs have a large aspect
ratio and a large external surface area[6]
, and can be easily dispersed and recovered
from in a liquid-phase system. All these advantages demonstrate that zeolite@NFs
structures are promising catalysts for the acetalisation and transesterification
reactions.
Although this study involves no plasmonic effects on enhancing the catalytic
performance, it does help further understand the influential factors, such as the size
of zeolite nanocrystals, on the acetalisation reactions and provides guidance to design
new (plasmonic) photocatalysts for the acetalisation reactions. Moreover, because of
the catalytic capacity of pure TiO2 (without zeolite Y nanocrystals) to catalyse the
transesterification of dimethyl carbonate with alcohols, we have done further work
on the transesterification on TiO2 nanofibres with different crystal phases, and the
results can be seen in the "Appendix – Transesterification reaction‖[7]
.
References
1. X. B. Ke, X. G. Zhang, H. W. Liu, S. Xue and H. Y. Zhu, ―Efficient catalysts of
zeolite nanocrystals grown with a preferred orientation on nanofibres,‖ Chem.
Commun. 49, 9866-9868 (2013).
2. B. Smit, T. L. M. Maesen, ―Towards a molecular understanding of shape
selectivity,‖ Nature 451, 671-678 (2008).
87
3. K. Varoon, X. Y. Zhang, B. Elyassi, D. D. Brewer, M. G. S.; Kumar, J. A. Lee, S.
Maheshwari, A. Mittal, C. Y. Sung, M. Cococcioni, L. F. Francis, A. V.
McCormick, K. A. Mkhoyan, M. Tsapatsis, ―Dispersible exfoliated zeolite
nanosheets and their application as a selective membrane,‖ Science 334, 72-75
(2011).
4. M. Iwamoto, Y. Tanaka, N. Sawamura, and S. Namba, ―Remarkable effect of
pore size on the catalytic activity of mesoporous silica for the acetalisation of
cyclohexanone with methanol,‖ J. Am. Chem. Soc. 125, 13032-13033 (2003).
5. P. Tundo, and M. Selva, ―The chemistry of dimethyl carbonate ,‖ Acc. Chem
Res. 35, 706-716 (2002).
6. H. Y. Zhu, X. P. Gao, Y. Lan, D. Y. Song, Y. X. Xi, and J. Cai. Zhao, ―Hydrogen
titanate nanofibres covered with anatase nanocrystals: a delicate structure
achieved by the wet chemistry reaction of the titanate nanofibres,‖ J. Am. Chem.
Soc. 126, 8380-8381 (2004).
7. X.G. Zhang, X.B. Ke, Z.F. Zheng, H.W. Liu, and H.Y. Zhu, ―TiO2 nanofibres of
different crystal phases for transesterification of alcohols with dimethyl
carbonate,‖ Appl. Catal. B 150-151 330-337 (2014).
88
Statement of contribution
1. The authors listed below have certified that:
2. They meet the criteria for authorship in that they have participated in the
conception, execution, or interpretation, of at least that part of the publication in
their field of expertise;
3. They have public responsibility for their part of the publication, except for the
responsible author who accepts overall responsibility for the publication;
4. There are no other authors of the publication according to these criteria;
5. Potential conflicts of interest have been disclosed to (a) granting bodies, (b) the
editor or publisher of journals or other publications, and (c) the head of the
responsible academic unit, and
6. They agree to the use of the publication in the student’s thesis and its publication
on the Australian Digital Thesis database consistent with any limitations set by
publisher requirements.
In the case of this chapter:
Efficient catalysts of zeolite nanocrystals grown with a preferred orientation on
nanofibres
Xuebin Ke, Xingguang Zhang, Hongwei Liu, Song Xue, and Huaiyong Zhu
Published in the journal: Chemical Communications, 2013, 49, 9866-9868
96
6 Conclusions
In this Ph.D thesis, several new applications of plasmonic photocatalysts of
supported Au-NPs have been found in the selective reduction, the selective
oxidation, and the acetalisation reaction under visible light irradiation, and a
theoretical outline has been established on the basis of the LSPR effect and the
concurrently induced electric near-field enhancement of plasmonic nanostructures.
In the selective reduction (Article 1: Selective reductions using visible light
photocatalysts of supported gold nanoparticles), four reduction reactions:
nitroaromatics to azo compounds, azobenzene to hydroazobenzene, ketones to
alcohols, and epoxides to alkenes, proceed efficiently on the Au/CeO2 photocatalysts
under visible light irradiation or simulated sunlight. The reduction power of the
photocatalysts can be manipulated by the light wavelength. Irradiation with shorter
wavelengths can induce a more negative reduction by creating a more negative
potential. The efficiency of the photocatalytic reductions increases with the
increasing light intensity under ambient conditions. The kinetic study shows that the
activation energy can be significantly reduced under visible light irradiation
compared with that in the thermal-driven processes. The photocatalytic reduction on
Au/CeO2 follows a mechanism distinctly different from that on the semiconductor
photocatalysts and provides insights into the formation of Au-H species and their
interaction with the reactants. Such photocatalytic syntheses are sustainable and
clean as these production processes have the potential to utilise sunlight for chemical
synthesis.
In the selective oxidation (Article 2: Zeolite-supported gold nanoparticles for
selective photooxidation of aromatic alcohols under visible-light irradiation),
97
photooxidation of aromatic alcohols can proceed well on Au/zeolite catalysts with
high selectivity towards aldehydes under visible light irradiation at ambient
temperature. Experimental results show that the catalytic activities of Au/zeolite
photocatalysts are influenced by the adsorptive properties of zeolites, the particle size
and specific surface areas of Au-NPs, and the molecular polarity of aromatic
alcohols. The kinetic study shows that the visible light irradiation significantly
reduces the activation energy of the photooxidation reaction compared with the
thermal-driven reaction. The role of molecular oxygen is the hydrogen remover from
the gold surfaces. Finally, a possible mechanism based on the LSPR effect of Au-
NPs and the adsorptivity of zeolite supports is proposed. This study illustrates the
potential of Au/zeolite photocatalysts for the selective oxidation reaction driven by
sunlight at ambient temperature. The mechanistic study can provide practical
guidelines for development of new catalytic materials for ―green‖ and energy-saving
chemical processes.
The study on the acetalisation reaction unravels a cascade enhancement effect
from visible light to zeolite catalysts bridged via the electric near-field enhancement
of Au-NPs (Article 3: Plasmonic nanostructures to enhance catalytic performance of
zeolites under visible light). The polarised electrostatic fields of extra-cations in
zeolites can be further intensified by the electric near-field enhancement of Au-NP,
and the intensified polarised electrostatic fields can stretch the C=O bond of the
reactants of benzaldehyde and cyclohexanone to enlarge their molecular polarities,
thus allowing them to be activated more efficiently by catalytic centres of H+ to
boost the reaction rate. This enhancement effect offers promise in modifying the
molecular polarities which affect the activity and electrostatic behaviour of
molecules and have broad applications in organic synthesis, ionic liquids,
98
nanofiltration membranes, molecular electronics, and molecular self-assembly
processes through non-covalent interactions.
Overall, the findings in this thesis demonstrate that plasmonic photocatalysts
based on plasmonic (gold) nanostructures have great potential in the selective
reduction, the selective oxidation, and the acetalisation owing to their singular
characteristics of the LSPR effect and the electric near-field enhancement around the
particle surfaces. Considering various plasmonic metals or alloys, and numerous
catalytic supports, such as zeoiltes (213 framework types, IZA), other solid-acid
catalysts, semiconductor photocatalysts and metal/acid bifunctional catalysts, the
findings in this research thesis may inspire scientists to explore more applications of
plasmonic photocatalysts in sensing, solar panels, solar water splitting,
photochemical synthesis, drug delivery, industrial processes of cracking and
isomerisation, and environmental remediation.
99
7 Limitations and future work
7.1 Limitations and possible solutions
Even though considerable achievements have been made on plasmonic
photocatalysts, there still exist limitations and knowledge gaps in the field of
plasmonic photocatalysis, and more work needs to be done in the future to improve
the photocatalytic performance and to clarify the photocatalytic mechanism.
As for plasmonic gold photocatalysts, though significant progress has been
made, to fully unravel the LSPR effect and the induced electric near-field
enhancement, several challenges need to be addressed: (i) the electron transfer
processes are still ambiguous and under debate. Scientists are uncertain whether the
electron transfer is from metals to supports and then to reactants, or from metals to
reactants directly, or whether the interaction between catalysts and reactants is
through electron transfer or merely excitation of reactants by electron clouds without
electron migration; (ii) the measurement of the contribution of heat released by
energetic electrons that return to ground states is still challenging. The excited free
conduction electrons will release heat when they return to the ground states, and this
plasmonic photothermal effect can usually cause the temperature to increase around
metal NPs. Because the reaction rate constant exponentially depends on reaction
temperature, the plasmon-excitation-induced heat may also accelerate chemical
reactions. How to measure the contribution of heat on the surface of metal
nanocrystals remains a great challenge; and (iii) obviously the cost of plasmonic
metals is still high. The practical application of plasmonic photocatalysts is a big
issue, because the plasmonic photocatalysts heavily depend on the use of gold or
silver nanostructures. The aforementioned problems (i) and (ii) are quite difficult at
100
present, scientists are struggling to develop new techniques to detect and quantify the
electron or heat transferred in reactions. A feasible approach to measure the electron
transfer is reported in Wang and co-workers’ study[1]
; they use tetracyanoethylene
(TCNE), which is a strong electron abstractor and changes its colour after grabbing
electrons, to quantify the electrons released from the molybdenum oxides (MoOx)
supports to evaluate the catalytic activity of Au/MoOx in the oxidation of aromatic
alcohols. For the problem (iii), the practical applications of plasmonic photocatalysts
in chemical reactions necessitate inexpensive and earth-abundant metals, such as iron,
aluminium and copper. Therefore, developing photocalalysts with alloy structures
will be promising. Moreover, it is also meaningful to explore non-metal
nanomaterials that can exhibit the LSPR effect, such as indium tin oxide[2]
, tungsten
oxide[3]
and copper chalcogenide[4, 5]
. Exploration of these non-metal nanomaterials
for plasmon-enhanced chemical reactions will be interesting and worthwhile.
As for zeolite catalysts, there are also several problems for solid-acid catalysed
reactions: (i) the high operating temperature due to the large activation barriers of
reactions. To address this problem, I speculate that if the traditional reactions (e.g.,
acetalisation) could be achieved in a photocatalytic way, better catalytic performance
or low reaction temperature can be expected; (ii) the polar products/intermediates are
strongly bound to the zeolite catalysts, impeding rapid desorption of them and thus
reducing the reaction rate[6]
. Hence, fast removal of the final products/intermediates
from catalytic centres is essential. To combat this issue, a more detailed
understanding is necessary about how reactant molecules arrange themselves in
zeolite pores, for instance, around the strong electrostatic-field cations to change
their molecular polarities. Moreover, insights into the location/geometry of cation
sites may guide the design of new zeolite-based catalysts[7]
; and (iii) the mass
101
transfer limitations because of the large catalyst particles aggregated after
calcinations. A possible solution is to graft zeolite nanocrystals on a substrate (e.g.,
TiO2 nanofibres, as reported in Article 4: Efficient catalysts of zeolite nanocrystals
grown with a preferred orientation on nanofibres) to alleviate the aggregation
problem[8]
.
7.2 Future of work
The LSPR effect and the electric near-field enhancement of plasmonic
nanostructures allow for development of novel plasmonic photocatalysts that can
take advantage of visible light and show better catalytic performance than these
photocatalysts perform in reactions driven only by thermal energy under the same
conditions. More efforts need to be made on the basis of the above-mentioned
―limitations and possible solutions‖. Given the importance and phenomenal progress
that has been achieved, development of novel plasmonic photocatalysts based on
―plasmonic metal (Au or Ag) nanostructures modified traditional catalysts‖ should
be promising. To be specific, the following topics can be developed in the future:
(i) Plasmonic metal (Au or Ag) nanostructures to modify traditional TiO2-based
photocatalysts for water splitting[9]
. Production of hydrogen from water in a
photocatalytic way is a promising technology and has long been a hot topic.
However, the photo efficiency of traditional TiO2 photocatalysts is still low,
scientists are striving to modify photoelectrochemcial properties of these
conventional photocatalysts, for instance, by narrowing the band gaps, but this
decreases the driving force of a photocatalyst for redox reactions. Meanwhile,
scientists are making great efforts to develop novel photocatalytic materials, such as
porous LaTiO2N[10]
, GaN:ZnO[11]
and Ta3N5[12]
, for their enhancement of the
electrode conductivity. Recently (2011-present), the contribution of the LSPR effect
102
to enhancing water splitting receives huge attention, and photocatalysts based on
plasmonic metals include Au/TiO2[13]
, Au/N-TiO2[14]
, Au/Fe2O3[15]
, Au/ZnO2[16]
,
Au/ZnFe2O4/ZnO[17]
and Au/ZnO-CdTe[18]
. However, the light-harvesting capacity,
the enhancement effect, and the oxidation activity are still limited, probably owing to
the inefficient electronic contact between electrodes and reactants. Therefore, there is
great demand for developing new photocatlytic materials based on plasmonic
nanostructures or techniques to address those problems.
(ii) Plasmonic metal (Au or Ag) nanostructures to modify traditional zeolite-based
solid acid catalysts for the selective oxidation of hydrocarbons[19]
, alkylation of
alcohols, methylation of phenols, and carbonylation of aldehydes. I will explore
whether the dipole oscillators of Au(δ+-δ-)
can further polarise reactants to affect its
adsorption or activation to boost the reaction rate; whether the electric near-field
enhancement can function as a ―relay‖ to affect the polarised electrostatic fields of
cations in zeolites to intensify them and then to affect the photocatalytic performance
of zeolites; and whether the molecular polarities and orientations of reactions can be
controlled at moderate conditions in the zeolite pores.
(iii) Plasmonic metal (Au or Ag) nanostructures to modify traditional
metal/acid bifunctional catalysts for the isomerisation of n-paraffins in industrial
catalysis[20]
. In refineries, skeletal isomerisation of n-paraffins to give branched
isomers is an important process to enhance the octane number in the gasoline pool.
The isomerisation of C5/C6 has been used as a commercial approach to light
isoparaffins, whereas the isomerisation of C7-C9 n-paraffins remains challenging
because of concurrent cracking. The isomerisation of n-heptane usually serves as a
model on the bifunctional catalyst of Pt/Hbeta or Pt/HY, on which the mechanism
involves Pt-catalysed dehydrogenation of alkane to alkene and reversible
103
hydrogenation of branched alkenes to alkanes, and the acidity of the zeolites
promotes protonation of the intermediate alkenes and subsequent rearrangement to
form branched alkenes (the mechanism is still controversial). A big disadvantage of
this process is that n-heptane cracks largely (low selectivity) because the operating
temperature is high (200-300oC). However, the report that the catalytic performance
of epoxidation of ethylene on supported Ag-NPs and propylene on Cu-NPs can be
enhanced by visible light irradiation[21]
inspires me to improve the catalytic
performance of the isomerisation of n-heptane. Alloy structures of Au-Pt or Ag-Pt
will be supported on zeolites; I wonder whether the reaction temperature can be
lowered by using these plasmonic alloy nanostructures under the visible-light
irradiation.
References
1. F. Wang, W. Ueda, and J. Xu, ―Detection and measurement of surface electron
transfer on reduced molybdenum oxides (MoOx) and catalytic activities of
Au/MoOx,‖ Angew. Chem. Int. Ed. 51, 3883-3887 (2012).
2. M. Kanehara, H. Koike, T. Yoshinaga, and T. Teranishi, ―Indium tin oxide
nanoparticles with compositionally tunable surface plasmon resonance
frequencies in the near-IR region,‖ J. Am. Chem. Soc. 131, 17736-17737 (2009).
3. K. Manthiram, and A. P. Alivisatos, ―Tunable localised surface plasmon
resonances in tungsten oxide nanocrystals,‖ J. Am. Chem. Soc. 134, 3995-3998
(2012).
4. D. Dorfs, T. Härtling, K. Miszta, N. C. Bigall, M. R. Kim, A. Genovese, A.
Falqui, M. Povia, and L. Manna, ―Reversible tunability of the near-infrared
valence band plasmon resonance in Cu2-xSe nanocrystals,‖ J. Am. Chem. Soc.
133, 11175-11180 (2011).
104
5. S.-W. Hsu, K. On, and A. R. Tao, ―Localised surface plasmon resonances of
anisotropic semiconductor nanocrystals,‖ J. Am. Chem. Soc. 133, 19072-19075
(2011).
6. J. Xu, B. L. Mojet, J. G. van Ommen, and L. Lefferts, ―Effect of Ca2+
position in
zeolite Y on selective oxidation of propane at room temperature,‖ J. Phys.
Chem. B 108, 15728-15734 (2004).
7. J. Dědeček, Z. Sobalík, and B. Wichterlová, ―Siting and distribution of
framework aluminium atoms in silicon-rich zeolites and impact on catalysis,‖
Catal. Rev. Sci. Eng. 54, 135-223 (2012).
8. T. Cao T. Pham, H. S. Kim, and K. B. Yoon, ―Growth of uniformly oriented
silica MFI and BEA zeolite films on substrates,‖ Science, 334, 1533-1538
(2011).
9. A. Fujishima, and K. Honder, ―Electrochemical photolysis of water at a
semiconductor electrode,‖ Nature, 238, 37-38 (1972).
10. F. X. Zhang, A. Yamakata, K. Maeda, Y. Moriya, T. Takata, J. Kubota, K.
Teshima, S. Oishi, and K. Domen, ―Cobalt-modified porous single-crystalline
LaTiO2N for highly efficient water oxidation under visible light,‖ J. Am. Chem.
Soc. 134, 8348-8351 (2012).
11. K. Maeda, A. K. Xiong, T. Yoshinaga, T. Ikeda, N. Sakamoto, T. Hisatomi, M.
Takashima, D. L. Lu, M. Kanehara, T. Setoyama, T. Teranishi, and K. Domen,
―Photocatalytic overall water splitting promoted by two different co-catalysts for
hydrogen and oxygen evolution under visible light,‖ Angew. Chem. Int. Ed. 49,
4096-4099 (2010).
105
12. Y. B. Li, T. Takata, D. Cha, K. Takanabe, T. Minegishi, J. Kubota, and K.
Domen, ―Vertically Aligned Ta3N5 nanorod arrays for solar-driven
photoelectrochemical water splitting,‖ Adv. Mater. 25, 125-131 (2013).
13. Z. W. Liu, W. B. Hou, P. Pavaskar, M. Aykol, and S. B. Cronin, ―Plasmon
resonant enhancement of photocatalytic water splitting under visible
illumination,‖ Nano Lett. 11, 1111-1116 (2011).
14. D. B. Ingram, and S. Linic, ―Water splitting on composite plasmonic-
metal/semiconductor photoelectrodes: evidence for selective plasmon-induced
formation of charge carriers near the semiconductor surface,‖ J. Am. Chem. Soc.
133, 5202-5205 (2011).
15. E. Thimsen, F. L. Formal, M. Grätzel, and S. C. Warren, ―Influence of
plasmonic Au nanoparticles on the photoactivity of Fe2O3 electrodes for water
splitting,‖ Nano Lett. 11, 35-43 (2011).
16. H. M. Chen, C. K. Chen, C.-J. Chen, L.-C. Cheng, P. C. Wu, B. H. Cheng, Y. Z.
Ho, M. L. Tseng, Y.-Y. Hsu, T.-S. Chan, J.-F. Lee, R.-S. Liu, and D. P. Tsai,
―Plasmon inducing effects for enhanced photoelectrochemical water splitting: X-
ray absorption approach to electronic structures,‖ ACS Nano, 6, 7362-7372
(2012).
17. A. Sheikh, A. Yengantiwar, M. Deo, S. Kelkar, and S. Ogale, ―Near-field
plasmonic functionalisation of light harvesting oxide–oxide heterojunctions for
efficient solar photoelectrochemical water splitting: the AuNP/ZnFe2O4/ZnO
system,‖ small 9, 2091-2096 (2013).
18. C. K. Chen, H. M. Chen, C.-J. Chena, and R.-S. Liu, ―Plasmon-enhanced near-
infrared-active material in photoelectrochemical water splitting,‖ Chem
Commun. 10.1039/C3CC42567C.
106
19. H. Frei. Science, ―Selective hydrocarbon oxidation in zeolites,‖ 313, 309-310
(2006).
20. X. G. Zhang, P. Liu, Y. J. Wu, Y. Yao, and J. Wang, ―Synthesis and catalytic
performance of the framework-substituted manganese β zeolite,‖ Catal. Lett.
137, 210-215 (2001).
21. A. Marimuthu, J. W. Zhang, and S. Linic, ―Tuning selectivity in propylene
epoxidation by plasmon mediated photo-switching of Cu oxidation state,‖
Science 339, 1590-1593 (2013).
107
Appendix – Transesterification reaction
TiO2 nanofibres of different crystal phases for transesterification of
alcohols with dimethyl carbonate
Introductory remarks
This chapter reports the novel catalysts for the transesterification of dimethyl
carbonate with alcohols using TiO2 nanofibres of different crystal phases. This study
is derived from the report (Article 4: Efficient catalysts of zeolite nanocrystals grown
with a preferred orientation on nanofibres)[1]
, in which the transesterification of
dimethyl carbonate with alcohols was discovered to occur on pure TiO2 nanofibres
without zeolite nanaocrystals. TiO2 crystals have three different crystal structures:
anatase, TiO2(B), and rutile. TiO2 with different crystal structures should have
different catalytic performances or catalytic mechanisms, and thus we dived into
details on the transesterification reaction on TiO2 as a periphery study. This research
was published in the journal of ―Applied Catalysis B: Environmental‖[2]
.
In organic conversions, methylation, carbonylation, and transesterification are
important reactions, for instance, the conversion of alcohols to methyl ethers or
methyl carbonates plays a critical role in producing organic carboxylated
intermediates[3]
. However, the traditional processes heavily hinge on the base-
promoted reactions that involve toxic, hazardous, or corrosive agents or wastes[4]
.
Therefore, new catalysts are highly demanded because of raised severe concerns on
safety and environments.
This study demonstrated that TiO2 nanofibres of different crystal phases could
effectively catalyse the transesterification of alcohols with dimethyl carbonate to
108
produce corresponding methyl carbonates. The catalytic activities correlated with the
crystal phases and adsorption of benzyl alcohol. It is interesting that the light (UV or
visible) irradiation had a negative influence on the catalytic performance of TiO2
catalysts, because partial benzyl alcohol underwent photocatalytic reaction to
produce benzaldehyde[5]
. The kinetic isotope effect (KIE) study identified the rate-
determining step and the reaction pathway. Finally, a new mechanism was proposed
on the basis of the experimental results and literature reports.
Advantages of this catalytic system included excellent selectivity (>99%), general
suitability to alcohols, convenient preparation and reusability of fibrous catalysts.
Moreover, the proposed mechanism is new, compared with those reactions occur on
the traditional zeolite-based catalysts or acid-base catalysts[5, 6]
. More significantly, It
is discovered that TiO2-based catalysts have great potential in non-photo involved
reactions even though TiO2 catalysts have been exclusively investigated as
photocatalysts after the finding of water splitting[7]
.
References
1. X. B. Ke, X. G. Zhang, H. W. Liu, S. Xue, and H. Y. Zhu, ―Efficient catalysts of
zeolite nanocrystals grown with a preferred orientation on nanofibres,‖ Chem.
Commun. 49, 9866-9868 (2013).
2. X. G. Zhang, X. B. Ke, Z. F. Zheng, H. W. Liu, and H. Y. Zhu. ―TiO2 nanofibers
of different crystal phases for transesterification of alcohols with dimethyl
carbonate,‖ Appl. Catal. B 150-151, 330-337 (2014).
3. O. Haba, I. Itakura, M. Ueda, and S. Kuze, ―Synthesis of polycarbonate from
dimethyl carbonate and bisphenol-A through a non-phosgene process,‖ J. Polym.
Sci. Part A: Polym. Chem. 37, 2087-2093 (1999).
109
4. A.-A. G. Shaik, S. Sivaram, ―Organic carbonates,‖ Chem. Rev. 96, 951-976
(1996).
5. M. Zhang, Q. Wang, C. C. Chen, L. Zang, W. H. Ma, and J. C. Zhao, ―Oxygen
atom transfer in the photocatalytic oxidation of alcohols by TiO2: Oxygen isotope
studies,‖ Angew. Chem. 68, 6081-6084 (2009).
6. P. Tundo, and M. Selva, ―The chemistry of dimethyl carbonate ,‖ Acc. Chem
Res. 35, 706-716 (2002).
7. A. Fujishima, and K. Honder, ―Electrochemical photolysis of water at a
semiconductor electrode,‖ Nature 238, 37-38 (1972).
110
Statement of contribution
1. The authors listed below have certified that:
2. They meet the criteria for authorship in that they have participated in the
conception, execution, or interpretation, of at least that part of the publication in
their field of expertise;
3. They have public responsibility for their part of the publication, except for the
responsible author who accepts overall responsibility for the publication;
4. There are no other authors of the publication according to these criteria;
5. Potential conflicts of interest have been disclosed to (a) granting bodies, (b) the
editor or publisher of journals or other publications, and (c) the head of the
responsible academic unit, and
6. They agree to the use of the publication in the student’s thesis and its publication
on the Australian Digital Thesis database consistent with any limitations set by
publisher requirements.
In the case of this chapter:
TiO2 nanofibers of different crystal phases for transesterification of alcohols
with dimethyl carbonate
Xingguang Zhang, Xuebin Ke, Zhanfeng Zheng, Hongwei Liu, and Huaiyong Zhu
Published in the journal: Applied Catalysis B, 2014, 150-151, 330-337