Wenyan
Zhang
*,
Chaoqun
Jiang
,
Hangmin
Guan
,
Yuanyuan
Wang
,
Yingfei
Hu
,
Wei
Wang
,
Wenjie
Tian
and
Lingyun
Hao
College of Material Engineering, Jinling Institute of Technology, Nanjing 211169, China. E-mail: wiseyanyan@jit.edu.cn; Fax: +86-25-86188966; Tel: +86-25-86188966
First published on 5th January 2024
Electrochemical water splitting is an attractive technique for hydrogen production, but its development is constrained due to the sluggish kinetics of the oxygen evolution reaction (OER), limited charge transmission efficiency, and the generation of harmful by-products (like hydrogen peroxide) accompanying the OER process. Herein, we constructed an Fe3O4 film with an inherent chiral structure to demonstrate its chiral induced spin selectivity (CISS) effect on modulating the OER pathway and facilitating the transfer of electrons extracted from the OER. Compared with normal Fe3O4, the chiral Fe3O4 film facilitated the OER pathway for production via the CISS-induced spin alignment of electrons and radicals, while it suppressed the pathway for peroxide by-product generation. Meanwhile, as a half-metallic material, chiral Fe3O4 film promoted the transportation of spin-aligned electrons derived from water oxidation to an external circuit. Compared with normal Fe3O4 film which is not capable of aligning electrons, the potential at 10 mA cm−2 declined by 150 mV, the Tafel slope decreased by 104 mV dec−1, the charge transfer resistance decreased by 50%, the free charge carrier density was amplified by 10-fold, and the electron lifetime was prolonged within the chiral Fe3O4 film.
Electrocatalytic water splitting has emerged as a cost-effective and promising technique for generating hydrogen from water, and it offers the advantage of not requiring extreme conditions like high temperature or pressure.9–13 A myriad of advanced catalysts for splitting water have been developed, such as MOF-derived catalysts,14 nickel oxide and nickel phosphide,15 NiFe selenide,16 CoNi hydrogen phosphate nanotubes,17 nickel nitride,18 and 2D-layered catalysts like NiCo hydroxide nanosheets.19
However, the efficiency of electrochemical water splitting falls short of expectations.20–23 The primary hurdle in this process lies in the sluggish oxygen evolution reaction (OER) that involves a complex four-electron process.24–28 Furthermore, an undesirable by-product, hydrogen peroxide, tends to form at the anodes when electrons derived from water oxidation are not spin-polarized. The presence of this by-product poses a detrimental impact on the OER reaction system, as it tends to poison the surface of electrocatalysts, thereby diminishing their catalytic activity and shortening their operational lifespan.29–31 To facilitate efficient water splitting, it has become imperative to accelerate OER kinetics while mitigating the production of hydrogen peroxide by-products during the OER process.
It is noted that the OER is inherently spin-sensitive, because prior to the formation of OO, the active sites must facilitate the extraction of three out of four electrons with identical spin orientations. Consequently, electrocatalysts that are capable of ensuring spin selectivity at the catalyst/electrolyte interface and subsequently facilitating the seamless transport of these spin-aligned electrons to the external circuit have become highly desirable for enhancing OER efficiency.23–25,32,33
The chiral induced spin selectivity (CISS) effect represents a promising approach to spin control in the OER process. For example, the attachment of organic chiral molecules (such as proteins or DNA) to semiconductors like TiO2 or CdSe, induces a CISS effect, reducing the OER barrier while suppressing the formation of by-products.26,27,34 Similarly, Inorganic materials characterized by intrinsic chiral configurations, such as chiral CuO and chiral CoxO, have showcased the CISS effect on lowering the OER barrier and mitigating the generation of by-products. Notably, their current density can surpass that achieved with semiconductors decorated with organic chiral molecules by up to 1000-fold.35–37
As an inorganic material, magnetite (Fe3O4) is renowned for its exceptional catalytic activity resulting from its redox characteristics, narrow band gap, cost-effectiveness, low toxicity, and remarkable durability.38,39 It is plausible that incorporating Fe3O4 with an inherent chiral structure could lead to a CISS effect on spin control for the OER. Beyond these benefits, Fe3O4 stands out as a half-metallic material, exhibiting nearly 100% spin polarization in the electronic density of states (DOS) near the Fermi energy level. Consequently, the electrical conductivity of Fe3O4 is fundamentally dependent upon the spin states of electrons, with one spin channel exhibiting metallic behavior, while the other spin channel demonstrates insulating properties.40–45 Such a distinguished feature holds potential for enhancing the transfer of spin-aligned electrons from the catalyst to the external circuit.
To verify these hypotheses, we constructed an Fe3O4 film with an inherent chiral structure to investigate its CISS effect on spin alignment for the OER and its effectiveness in transferring spin-aligned electrons to the external circuit. We observed that, compared with normal Fe3O4 film without a chiral structure, the utilization of a chiral Fe3O4 film as an OER electrocatalyst resulted in notable catalytic improvements, encompassing the facilitation of the OER pathway while hindering hydrogen peroxide by-products, a 150 mV reduction in the applied potential required to achieve 10 mA cm−2, a 42% increase in current density at 1.8 V (vs. SCE), a decrease of 104 mV dec−1 in the Tafel slope, a 50% reduction in charge transfer resistance, and a 10-fold amplification in the free charge carrier density. The benefits brought about by the chiral Fe3O4 film are intricately intertwined with the CISS effect induced by its chiral structure and the capabilities of half-metallic materials to facilitate electron transfer.
The Fe 2p XPS spectrum of the chiral Fe3O4 film is presented in Fig. 3. Within this spectrum, the binding energy peak centered at approximately 710.6 eV corresponds to the Fe 2p3/2 state, while the peak at 724.0 eV corresponds to the Fe 2p1/2 state.46–49 These peaks are fitted using a shakeup satellite and two spin–orbit doublets, which originate from the Fe3+ and Fe2+ states.46–48 The area ratio of Fe3+/Fe2+ in the spectrum is approximately 2, indicating that the material deposited on the FTO substrate is Fe3O4.
The chirality of the catalyst surface was assessed through an electrochemical selectivity test, a sensitive technique for discerning the surface chirality of materials (details in ESI†).50,51 As shown in Fig. 4(a), chiral Fe3O4 exhibited a higher current density and smaller reduction potential when it was scanned in a chiral electrolyte comprising 10 mM L-tartaric acid than in a chiral electrolyte containing 10 mM D-tartaric acid. These results confirmed that chiral Fe3O4 exhibited contrasting chiral selectivity responses in electrolytes with opposite chirality, specifically preferring charge exchanges with L-tartaric acid.
To complement the findings from the electrochemical selectivity test, we further elucidated the surface chirality of the chiral Fe3O4 film using circular dichroism spectroscopy (CD) and polarized optical microscopy (POM) measurements performed in reflection mode. Fig. 4(b) demonstrates that the chiral Fe3O4 film prominently displays optical activity within the visible light region, whereas normal Fe3O4 exhibits no discernible optical activity within this region, suggesting inherent chirality with the chiral Fe3O4 film. This observation strongly implies the intrinsic chirality of the chiral Fe3O4 film. The results of POM are shown in Fig. S2 (ESI†), which also support the formation of a chiral film.
The chiral Fe3O4 film, which has inherent chiral structure, demonstrated a CISS effect on spin alignment during the OER. This was verified by monitoring the generation of the singlet-state by-product H2O2 throughout the OER process.32–34 The UV-vis spectra of the electrolyte in the water oxidation system are presented in Fig. 5(a), employing o-tolidine as an indicator to track the production of H2O2. When normal Fe3O4 was used as an electrocatalyst, an absorption peak emerged at approximately 436 nm, as H2O2 oxidized o-tolidine, leading to the formation of a yellow compound. However, this peak was substantially diminished when the chiral Fe3O4 film was utilized as an electrocatalyst, signifying the inhibition of H2O2 generation alongside OER.
As depicted in Fig. 5(b), the OER pathway of Fe3O4 in alkaline media follows the adsorbate evolution mechanism (AEM), involving a sequential series of concerted four-proton-coupled electron transfer (PCET) processes that take place on active sites. These processes create multiple oxygen intermediates, including *OH, *O, and *OOH, to establish the pathway, *OH → *O → *OOH → O2 for the formation of O2. It is recognized that the OER process is spin sensitive, because the four electrons extracted from its four steps should have the same spin direction before the formation of the OO bond. Thereby, the spin orientations of electrons and radicals are beneficial for delivering
.
The inhibition of H2O2 by-product suggests that the chiral Fe3O4 film filtered the spin orientation of electrons acquired from water oxidation through the CISS effect,29,30,32,33 synchronously ensuring the alignment of spins in the newly generated ˙OH radicals that subsequently attached to the M sites of O–M–O species on the Fe3O4 surface during step 1 and step 3 of the AEM process, as demonstrated in Fig. 5(b). This facilitated the water oxidation pathway for the formation of the triplet-state product, while promoting the alignment of electrons extracted from water oxidation throughout the four steps of AEM. Conversely, the formation of H2O2, which occurs on the singlet potential energy surface, was hindered.29,30,33
In accordance with the CISS-induced preference for the formation pathway during the OER, chiral Fe3O4 exhibited a lower water oxidation barrier than normal Fe3O4. As depicted in the inset of Fig. 6(a), the LSV onset potential was reduced in comparison with normal Fe3O4. Additionally, the potential required to achieve a current density of 10 mA cm−2 decreased by 150 mV when the chiral Fe3O4 film was used as an electrocatalyst.
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Fig. 6 (a) Linear sweep voltammetry characterization of chiral Fe3O4, normal Fe3O4, FTO, and chiral CuO (the LSV of chiral Fe3O4, normal Fe3O4, and FTO were recorded in 0.1 M KOH as electrolyte at room temperature with calomel as reference; the LSV of chiral CuO refers to ref. 31). |
As mentioned above, being a half-metallic material, Fe3O4 should be fundamentally efficient for transferring spin-aligned electrons, even displaying metallic behavior. Here, it is noticed that the chiral Fe3O4 and normal Fe3O4 films demonstrated superior performance in OER current density compared to the chiral CuO film, which is not a half-metal, as shown in Fig. 6(a).
In addition, as seen in Fig. 6(a), the current density generated by the chiral Fe3O4 film at 1.8 V (vs. SCE) was 42% higher than that of normal Fe3O4, indicating that the chiral Fe3O4 film facilitated electron transfer compared to normal Fe3O4 film. Furthermore, as shown in Fig. 6(b), the Tafel slope of the chiral Fe3O4 film was 104 mV dec−1 smaller than that of normal Fe3O4, which suggests that the presence of chirality on the Fe3O4 film enhances OER kinetics and carrier transport. These results demonstrate that, in addition to its CISS effect in promoting the OER pathway for production, the chiral Fe3O4 film facilitates a more efficient transfer of spin-aligned electrons, derived from water oxidation, from the catalyst to the external circuit compared to the normal Fe3O4 film.
In line with the findings from LSV and Tafel characterization, the results from electrochemical impedance spectroscopy (EIS) reveal that the chiral Fe3O4 film exhibited smaller Nyquist circle diameters than normal Fe3O4 (see Fig. 7(a)). To gain further insights from these Nyquist plots, we employed an R(RQ) circuit model for fitting, and the fitting outcomes are summarized in Table 1. Herein, RΩ represents solution resistance, Qd denotes electrochemical double-layer capacitance, and Rct corresponds to charge transfer resistance. The Rct value for normal Fe3O4 was only 6% of that observed for FTO, suggesting the significance of Fe3O4 in promoting electron transfer for the OER. Notably, the chiral Fe3O4 film exhibits a remarkable 50% reduction in Rct compared to normal Fe3O4, suggesting that electron transport across Fe3O4 was enhanced due to its intrinsic chiral structure.
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Fig. 7 (a) Nyquist plots of L-Fe3O4, D-Fe3O4, normal Fe3O4 and FTO. (b) Mott–Schottky plots of L-Fe3O4, D-Fe3O4 and normal Fe3O4. |
R Ω (Ω) | Q d (×10−4 F) | n | R ct (Ω) | |
---|---|---|---|---|
Fe3O4 | 42.95 | 0.2823 | 0.9434 | 3.314 × 105 |
Chiral Fe3O4 | 33.48 | 1.122 | 0.95 | 1.369 × 105 |
FTO | 36.45 | 0.08913 | 0.9642 | 5.135 × 106 |
Simultaneously, Mott–Schottky measurements provided further evidence of the pivotal role played by chirality in enhancing the catalytic activity of Fe3O4 film in the OER. The Mott–Schottky equation, expressed as (Csc)−2 = 2(E − Efb− kT/e)/(εε0A2eNd) (details in ESI†), dictates that the slope of the linear segments in the Mott–Schottky plot correspond to 2/(εε0A2eNd).52,53 These linear segments are associated with the depleted states of majority carriers located within the space charge region.54 As depicted in Fig. 7(b), the slope of the linear segment of normal Fe3O4 was approximately 2.03, while the slope of the chiral Fe3O4 film was around 0.19, merely 10% of that observed for normal Fe3O4. It is calculated that the charge carrier density (Nd) of normal Fe3O4 was about 3.5 × 1028 cm−3, while for the chiral Fe3O4 film, it was approximately 3.7 × 1029 cm−3. This result shows that the majority carrier density within the space charge region of Fe3O4 increased up to 10-fold due to the incorporation of chirality.
Furthermore, evidence from the Bode and phase angle plots serves to reinforce the enhanced electron transport capabilities observed in the chiral Fe3O4 film. In Fig. 8(a), the Bode plots illustrate that the chiral Fe3O4 film displays lower impedance modulus values compared to normal Fe3O4 and FTO. This observation signifies an increase in carrier mobility on the chiral Fe3O4 film.55 Moreover, as depicted in Fig. 8(b), the phase angle plot for chiral Fe3O4 shifts towards lower frequencies compared to normal Fe3O4. This red shift indicates accelerated carrier mobility across the chiral Fe3O4 film. Furthermore, Fig. 8(b) also reveals that the electron lifetime within the chiral Fe3O4 film is prolonged compared to that within the normal Fe3O4 film, taking into account that the electron lifetime (τe) can be calculated with the equation τe =
1/2πfmax, where fmax represents the peak frequency.49,56 The elongated electron lifetime implies lower charge recombination probability in chiral Fe3O4 film than in normal Fe3O4 film.
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Fig. 8 (a) Bode plots of chiral Fe3O4 film and normal Fe3O4 and FTO. (b) Phase angle plots of chiral Fe3O4 film and normal Fe3O4 and FTO. |
Additionally, hydrogen production in water splitting systems with different OER catalysts was demonstrated, as shown in Fig. 9(a) with chiral Fe3O4 film and normal Fe3O4 film as OER catalysts. The hydrogen production rate with chiral Fe3O4 film as OER catalyst was approximately 20% higher than that with normal Fe3O4 film as OER electrocatalyst and about 5 times of that with chiral CuO film as OER electrocatalyst. Furthermore, chiral Fe3O4 film exhibited robust electrocatalytic activity during the three experimental trials, as shown in Fig. S1 (ESI†). In each trial, the hydrogen production rate was enhanced by at least 20% when chiral Fe3O4 was employed as electrocatalyst rather than normal Fe3O4 as electrocatalyst. The growth of the hydrogen production rate is associated with the elevation of water oxidation kinetics and decline of the OER barrier, which was induced by the chiralization of the Fe3O4 catalyst. The stability also suggests the robustness of the chiral Fe3O4 film for the OER, as shown in Fig. S4 (ESI†).
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Fig. 9 (a) Hydrogen production recorded in a water splitting system with chiral Fe3O4 and normal Fe3O4 as OER catalysts (conducted at a voltage of 1.5 V (vs. SCE) in 0.1 M KOH electrolyte, at room temperature, with calomel as reference, Pt wire as counter). The hydrogen production of chiral CuO refers to ref. 37. (b) Scheme of the CISS effect in conjunction with the half-metallic nature of chiral Fe3O4 film for aligning the spins of electrons and radicals for the OER and the transportation of spin-oriented electrons. |
The evidence presented above coherently demonstrates the advantages offered by the chiral Fe3O4 film compared to normal Fe3O4 film and chiral CuO. As illustrated in Fig. 9(b), during the OER, the CISS effect of the chiral Fe3O4 film aligned the spins of electrons and radicals. This spin-controllable process improved the possibility for the formation of the triplet-state product , promoted the AEM water oxidation pathway, and thereby reduced the barrier for the OER. Meanwhile, the half-metallic nature of Fe3O4 facilitated the transfer of spin-aligned electrons. The combined and synergistic influence of these factors plays a pivotal role in unlocking the catalytic potential of Fe3O4 film for the OER.
Footnote |
† Electronic supplementary information (ESI) available. See DOI: https://doi.org/10.1039/d3ma00854a |
This journal is © The Royal Society of Chemistry 2024 |