Theodore
Lazarides‡
a,
Milan
Delor
b,
Igor V.
Sazanovich
b,
Theresa M.
McCormick
c,
Irene
Georgakaki
a,
Georgios
Charalambidis
a,
Julia A.
Weinstein
*b and
Athanassios G.
Coutsolelos
*a
aLaboratory of Bioinorganic Chemistry, Chemistry Department, University of Crete, PO Box 2208, 71003 Heraklion, Crete, Greece. E-mail: coutsole@chemistry.uoc.gr; Fax: +30 2810 545161; Tel: +30 2810 545045
bDepartment of Chemistry, University of Sheffield, Sheffield S3 7HF, UK. E-mail: julia.weinstein@sheffield.ac.uk; Fax: +44 (0)114 222 9346; Tel: +44 (0)114 222 9408
cDepartment of Chemistry, University of Rochester, Rochester, New York 14627, USA
First published on 22nd July 2013
A combination of noble-metal free components, a water soluble porphyrin photosensitizer zinc meso-tetrakis(1-methylpyridinium-4-yl)porphyrin chloride [ZnTMPyP4+]Cl4 (1) with cobaloxime complex [CoIII(dmgH)2(py)Cl] (2) as a catalyst, creates an efficient system for photochemical hydrogen production acting under visible light with 280 TONs. This is the first example of a water soluble porphyrin acting as a photosensitizer for cobaloxime catalysed H2 production.
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Fig. 1 Structures of photosensitizer 1, [ZnTMPyP]4+(Cl−)4, and catalyst2, [CoIII(dmgH)2(py)Cl] (dmgH = dimethylglyoximate and py = pyridine). |
Fig. 2 shows the amount of hydrogen produced over time upon irradiation (λ > 440 nm) at two different pH values of systems containing 1, 2 and triethanolamine (TEOA) in MeCN–H2O (1:
1).
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Fig. 2 Plots of hydrogen production upon irradiation (λ > 440 nm) of solutions (1![]() ![]() |
At pH 8, the initial rate of H2 generation is maintained for approximately 3 h before starting to decline until it finally ceases in about 5 h. At pH 7, hydrogen production is observed only after an induction period of 1 h with the initial hydrogen production rate being considerably slower than that at pH 8. However, at pH 7, the system shows considerably improved stability as it maintains its photocatalytic activity for more than 20 h producing in total about 280 TONs of hydrogen.
These pH values were selected on the basis of observations in related photocatalytic systems involving 2 as the catalyst and TEOA as a sacrificial donor, which show their maximum rate of hydrogen production at neutral to slightly basic pH values (7 < pH < 8.5).10–12,14 Cessation of hydrogen production coincides, in all cases, with bleaching of the photolysis solutions. To regenerate the catalytic activity of the system, addition of both 1 and 2 is necessary, suggesting that both the photosensitizer and the catalyst undergo at least partial decomposition in the course of the reaction.10–12 Control experiments at pH 7 and 8 with λ > 440 nm irradiation showed that the presence of all three components (1, 2 and TEOA) is necessary in order to observe H2 production. Photolysis experiments performed under identical conditions but in the presence of 2 mL of Hg, in order to suppress any heterogeneous catalytic sites, show no appreciable change in the H2 production rate confirming that catalysis is of truly homogeneous nature.10 It is worth mentioning that H2 production was also observed in experiments in which ascorbate was used as a sacrificial donor at pH 4 albeit with lower TON (50) (detailed comments are provided in ESI†).
Importantly, selective excitation of the porphyrin Q-band with 572 nm light (through a band-pass filter of ∼10 nm FWHM) in the solution containing 1, 2 and TEOA in MeCN–H2O (1:
1) at pH 7 also resulted in H2 production with 90 TONs after 120 h of irradiation.§ This experiment unambiguously confirms that the porphyrin acts as a photosensitizer for H2 production in this system.
Addition of 25 equivalents of [CoIII(dmgH)2(py)Cl] or up to 700 equivalents of TEOA into a solution of 1 in MeCN–H2O (1:
1) at pH 7 results in quenching of the porphyrin-based fluorescence by only 5% and no appreciable quenching, respectively (Fig. S1 and S2, ESI†). No change is observed in the UV-Vis absorption spectra of 1 in both of the above cases.
These results are in agreement with what was observed in other diffusion-controlled photocatalytic systems11,12,17 and indicate that intermolecular electron transfer to/from the singlet excited state of 1 is not favourable due to its short lifetime (τ = 1.6 ns fluorescence lifetime in MeCN–H2O (1:
1) at pH 7). This observation is consistent with previous transient absorption studies, which showed that reductive and oxidative electron transfer occurs via the lowest-lying triplet excited state of 1.18,19
To shed more light on the mechanism of photocatalytic H2 production by the system {1 + 2 + TEOA}, the UV-Vis absorption spectra at pH 8 and 11 before and after irradiation with visible light (λ > 440 nm) were recorded (Fig. 3). At pH 8 under H2 producing conditions, the absorption spectrum of the initial solution is simply the sum of the spectra of its components (see individual spectra in Fig. S3, ESI†). After 4 min of irradiation the porphyrin Soret band shows considerable broadening accompanied by an increase in intensity. This can be attributed to the formation of the absorption band at 450 nm characteristic of the CoII species.8,12 When the same experiment is conducted at pH 11, where H2 generation is greatly suppressed, a new broad absorption at 500–600 nm appears within 7 min due to the accumulation of a CoI species.12,20
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Fig. 3
UV-Vis
spectra at pH 8 and pH 11 before and after irradiation of degassed solutions (1![]() ![]() |
It had been proposed previously that this CoI species leads to H2 generation, via protonation yielding a CoIII hydride.21,22 Variation of the concentration of 2 in systems {1 + 2 + TEOA} at pH 8 reveals a linear relationship between the concentration of 2 and the initial rate of hydrogen production (Fig. S4, ESI†).
This observation is consistent with the results obtained with related photocatalytic systems and favours a H2-generating mechanism that is first order in cobalt.11,12,14 Thus, taking into account recent results from transient absorption studies,21,23 we propose the mechanism shown in Scheme 1 involving the generation of a CoIIhydride which decomposes giving H2via a monometallic pathway.
The metal-free analogue of 1, [H2TMPyP]4+(Cl−)4, was also tested as a sensitizer for H2 production under the same conditions. At pH 8, only a relatively modest amount of H2 was produced (ca. 60 TONs) after 9 h of irradiation (λ > 440 nm). The system containing [H2TMPyP]4+(Cl−)4 + 2 + TEOA at pH 8 (Fig. S5, ESI†) shows the formation of a CoII species within the first 3 min of irradiation. The considerably slower rate of H2 production with the metal free photosensitizer, PS, can possibly be attributed to the higher oxidation potential of the first triplet excited state of [H2TMPyP]4+ compared to that of [ZnTMPyP]4+ [(−0.14 V) and (−0.45 V) in aqueous solution, respectively].24
To elucidate the role of the porphyrin as a photosensitizer, picosecond–microsecond transient absorption studies have been undertaken. Picosecond transient absorption studies of {1 + 2 + TEOA} at pH 7 show the formation of the characteristic spectrum of the singlet excited state of the porphyrin and its decay to that of the triplet excited state of 1, 3*PS, with a 1.0 ± 0.1 ns lifetime (Fig. S6, ESI†). The observed 1 ns lifetime of the singlet state is similar to that previously reported for 1*1,18,19 indicating that this state is not participating in the photoinduced processes, and that any PS contribution to H2-production must originate from its triplet state. No further processes have been detected on the time scale up to 4 ns.
The transient absorption spectrum of {1 + 2 + TEOA} at pH 7 on the microsecond time scale (Fig. 4) shows characteristic features of 3*1. The decay kinetics of 3*1 in the PBS–MeCN mixture are best fitted with double-exponential functions (Table 1), probably due to concentration self-quenching, or different solvation environments. If both 1 and 2 are present, addition of TEOA or a change in pH does not affect the lifetime of 3*1. Excitation at different wavelengths (438 nm, the Soret band of 1; 560 nm, Q-band, or 490 nm, cobaloxime) to explore different 1(PS)/2(Co) absorption ratios consistently produced the same results in the transient absorption experiments. 1 in the presence of TEOA alone is extremely photo-unstable and instantaneously photobleaches upon excitation, as has been reported previously.18,19
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Fig. 4 Nanosecond transient absorption decay kinetics at 470 nm for {1 + 2 + TEOA} (black) and {1 in PBS} (blue) following 438 nm excitation. Inset: spectrum of {1 + 2 + TEOA} at representative delay times 0.5, 0.8, 1.7, 4.1 and 9.2 μs (black, red, green, blue and cyan, respectively). |
For all systems containing 1 and 2, decay traces of the transient signals can be satisfactorily fitted with a single-exponential function, indicating that only one process, that of the triplet state decay, is observable on this timescale. The addition of 2 decreases the 3*1 lifetime from over a hundred μs to ∼2 μs (Table 1 and Fig. 4), indicating that 2 efficiently quenches 3*1. This fact directly supports the participation of 3*1 in the hydrogen production pathway.
We have shown for the first time that a combination of a water soluble porphyrin ZnTMPyP4+ (1) photosensitizer and the cobaloxime catalyst [CoIII(dmgH)2(py)Cl] (2) is effective in photoinduced H2 production in MeCN–water (1:
1) with TEOA as a sacrificial donor. The maximum performance occurs at neutral to slightly basic pH, with ca. 300 TONs of H2 after 25 h of irradiation with >440 nm light.
We thank the European Commission FP7-REGPOT-2008-1, BIOSOLENUTI No 229927, Heraklitos and Thales MIS 377252 grant from Ministry of Education, GSRT; EPSRC (UK), E-Futures DTC and the University of Sheffield and its Strategic Development fund for support. Prof. R. Eisenberg is gratefully acknowledged for fruitful discussions and encouragement of this work.
Footnotes |
† Electronic supplementary information (ESI) available. See DOI: 10.1039/c3cc45025b |
‡ Laboratory of Physical Chemistry, Department of Chemistry, University of Ioannina, Ioannina 45110, Greece. |
§ The lower rate of H2 production observed under 572 nm excitation in comparison to the λ > 440 nm cut off filter is due to the considerably reduced amount of light delivered to the sample. |
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