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Nickel–vanadium monolayer double hydroxide for efficient electrochemical water oxidation

Nature Communications volume 7, Article number: 11981 (2016) | Download Citation


Highly active and low-cost electrocatalysts for water oxidation are required due to the demands on sustainable solar fuels; however, developing highly efficient catalysts to meet industrial requirements remains a challenge. Herein, we report a monolayer of nickel–vanadium-layered double hydroxide that shows a current density of 27 mA cm−2 (57 mA cm−2 after ohmic-drop correction) at an overpotential of 350 mV for water oxidation. Such performance is comparable to those of the best-performing nickel–iron-layered double hydroxides for water oxidation in alkaline media. Mechanistic studies indicate that the nickel–vanadium-layered double hydroxides can provide high intrinsic catalytic activity, mainly due to enhanced conductivity, facile electron transfer and abundant active sites. This work may expand the scope of cost-effective electrocatalysts for water splitting.


Water splitting is considered one of the most promising strategies to produce chemical fuels such as hydrogen. The half reaction of the water splitting process, water oxidation, remains the bottleneck of the whole process at present. Therefore, developing highly efficient water oxidation catalysts is crucial. Some precious metal-based electrocatalysts, such as IrO2 and RuO2, have shown excellent performance for water oxidation; however, they suffer from high-cost and relative scarcity of precious metals, which limits their applications. Although some first-row transition metal oxides (for example, NiOx, NiFeOx, CoOx and MnOx) had been developed as low-cost electrocatalysts for water oxidation, most of them still cannot compete with IrO2 and RuO21,2. Recently, the earth-abundant Ni–Fe double-layered hydroxide (NiFe-LDH) catalysts have attracted attention3,4,5,6,7. From being first reported as an advanced electrocatalyst coupled with carbon nanotubes for water oxidation8, it is nowadays known as one of the most active catalysts with a low overpotential and high electrolysis current. Since, then tremendous efforts have been devoted to further improve the activity of NiFe-LDH, such as exfoliation9 and hybridization6,8,10,11, to the extent that LDH catalysts can now outperform IrO2 in alkaline media6,8,9; however, the aforementioned methods are still too complicated for large-scale applications.

It is already known that Fe(III) incorporated in Ni(II)-based LDH is the key aspect for the high catalytic performance, although the role of Fe in LDH is still ambiguous5,6,12. Besides Fe(III), cobalt is also commonly incorporated in nickel hydroxides to construct NiCo-LDHs for water oxidation13,14,15,16, and the resulting NiCo-LDHs show promising catalytic activities; however, the performance is relatively low compared with the reported NiFe-LDHs under identical conditions9. Besides, more earth-abundant metal elements have been incorporated into Ni(OH)2 to explore novel LDHs for water oxidation, for example, recently Koper and co-workers17 investigated a series of Ni-based double hydroxides with Cr, Mn, Fe, Co, Cu and Zn for water oxidation, and among these candidates NiFe-LDH still appears as the most promising and shows the best activity. Up until now, there has been no reported earth-abundant metal element that can outperform Fe incorporated Ni-based LDHs. Searching for an earth-abundant metal to form efficient Ni-based LDH comparable to NiFe-LDH is still the state-of-the-art in this area of energy research.

In this work, we incorporate another earth-abundant element into Ni(OH)2: vanadium, and succeed in forming NiV-LDH as an efficient catalyst for the water oxidation reaction. A simple one-step hydrothermal method is employed to synthesize NiV-LDH. Without need for exfoliation or hybridization with other materials, the resulting monolayer NiV-LDH catalyst exhibits comparable activity to the best-performing NiFe-LDH for water oxidation in alkaline electrolyte.


Monolayer of Ni0.75V0.25-LDH

Figure 1a shows the typical X-ray diffraction patterns of pure Ni(OH)2 and Ni0.75V0.25-LDH. As can be seen, pure Ni(OH)2 was successfully synthesized in the simple hydrothermal system without addition of V sources, and the X-ray diffraction pattern supports the formation of pure hexagonal α-Ni(OH)2 (JCPDS 380715), which exhibits a layered structure constructed from [NiO6] coordinated octahedra connected by sharing their edges. After incorporation of V into the structure of α-Ni(OH)2, no obvious change can be observed in the X-ray diffraction spectrum, indicating Ni0.75V0.25-LDH is the isomorphous compound as α-Ni(OH)2 with the layered structure. The X-ray diffraction pattern of prepared bare V-based hydroxide without Ni source (Supplementary Fig. 1) shows very low crystallinity that is significantly different from those of the above Ni-based materials. Figure 1b–d shows the Ni 2p, V 2p and O 1s X-ray photoelectron spectroscopy (XPS) core-level spectra of the Ni0.75V0.25-LDH powder. The Ni 2p spectrum presents two main structures, resulting from the spin–orbit splitting of the p orbital that are assigned as Ni 2p3/2 (850−870 eV region) and Ni 2p1/2 (870−890 eV region). The binding energy difference between the 3/2 and 1/2 components is 17.4 eV. Ni 2p3/2 presents a main peak at 855.4 eV with an intense satellite structure at 861.2 eV, (872.8 and 879.6 eV, respectively, for Ni2p1/2), this signature is characteristic of Ni2+ (refs 18, 19, 20, 21). The spectra of O 1s and V 2p are presented in Fig. 1c, the O 1s signal originates from Ni0.75V0.25-LDH, but its main contributions is from the fluorine doped tin oxide (FTO) glass substrate used with an O1s-binding energy 530 eV. The V 2p core-level spectrum is also decomposed into V 2p3/2 and V 2p1/2 due to the spin–orbit splitting that are separated by 7.5 eV. A closer view on the V 2p3/2 region is shown in Fig. 1d. Three components can be distinguished at 515.4 eV (in blue), 516.3 eV (in light grey) and 517.5 eV (in grey) and are in good agreement with respectively V3+, V4+ and V5+ (refs 22, 23, 24). This result indicates that V3+ was partially oxidized by oxygen to V4+ and V5+ during the synthesis.

Figure 1: X-ray diffraction and XPS.
Figure 1

(a) X-ray diffraction patterns of α-Ni(OH)2 and Ni0.75V0.25-LDH. XPS measurements (=1,486.6 eV) on the Ni0.75V0.25-LDH powder deposited on a FTO conductive glass: (b) Ni 2p (c) O 1s and V 2p core-level spectra, and (d) zoom on the V 2p core-level spectrum.

Typical transmission electron microscopy (TEM) images of α-Ni(OH)2 and Ni0.75V0.25-LDH are shown in Fig. 2. Interestingly, as shown in Fig. 2a,b, the pure α-Ni(OH)2 shows a narrow nanosheet morphology with the size of few tens of nanometre. Aggregated by these nanosheet crystals, a porous sphere structure with the diameter of few micrometres was obtained, as observed by scanning electron microscopy (SEM; Supplementary Fig. 2a). After adding the vanadium source to the initial solution for hydrothermal reaction, Ni0.75V0.25-LDH presents a three-dimensional morphology assembled by ultrathin nanosheets as shown in Fig. 2c,d. Selected area electron diffraction pattern in the inset of Fig. 2d confirms the hexagonal phase of Ni0.75V0.25-LDH. The atomic force microscopy (AFM) and height profile of Ni0.75V0.25-LDH in Fig. 2e,f show that the nanosheet is ultrathin with thickness of 0.9 nm, indicating the obtained nanosheet is monolayered. To make a comparison, Ni0.75Fe0.25-LDH was also prepared by a similar protocol in the literature25 and the SEM image of the products obtained is shown in Supplementary Fig. 2b and c. Some large aggregation plates in Ni0.75Fe0.25-LDH can be observed, showing that the size of aggregations by nanosheets in Ni0.75Fe0.25-LDH is bigger than Ni0.75V0.25-LDH. However, the TEM, AFM images and height profile of Ni0.75Fe0.25-LDH in Supplementary Fig. 2d–f exhibit that the nanosheet of Ni0.75Fe0.25-LDH is also ultrathin with thickness of 1.2 nm. Meanwhile, differing from the above nanosheet-based structure, the bare V-based and Fe-based hydroxides (β-FeOOH) without Ni content show mainly ‘nanostick’ morphologies after the hydrothermal processes (Supplementary Fig. 3).

Figure 2: TEM and AFM.
Figure 2

(a,b) TEM images of α-Ni(OH)2. Scale bar, 1 μm (a); 200 nm (b); (c,d) TEM images of Ni0.75V0.25-LDH (inset of d: selected area electron diffraction pattern). Scale bar, 200 nm (c); 100 nm (d); (e) AFM image and (f) height profile of Ni0.75V0.25-LDH nanosheets.

Oxygen evolution catalysis

It is known that the composition can affect the water oxidation performance of the catalysts significantly. First, we investigated the electrocatalytic activities of NiV-LDHs and NiFe-LDHs on glassy carbon (GC) electrodes with different Ni content to optimize the composition (the measurements were carried out without ohmic-drop correction unless noted otherwise). All the amount of catalyst loadings on GC electrodes were 0.143 mg cm−2. As shown in Supplementary Fig. 4, the Ni content plays an essential role for the catalytic activity in this study (the electrocatalytic activities of pure Ni(OH)2, bare V-based and Fe-based hydroxides are very low, so they are not shown here for clarity). When the molar ratio of Ni/X (X=V or Fe) is 3:1, that is, Ni0.75V0.25-LDH and Ni0.75Fe0.25-LDH, the best water oxidation performances are achieved with the highest catalytic current density (Supplementary Fig. 4a–c) and turnover frequency (TOF) (Supplementary Fig. 4d), and the lowest required overpotential (Supplementary Fig. 4e) in NiV-LDH and NiFe-LDH series, respectively (note that for NiFe-LDH, this optimized molar ratio of Ni/Fe is in a good agreement with the literature reported previously6). Either a lower or higher mole ratio of the two metal elements will decrease the catalytic performances of LDHs. The atomic percentage of Ni, V and Fe in Ni0.75V0.25-LDH and Ni0.75Fe0.25-LDH has been measured by energy-dispersive X-ray spectroscopy (EDS; Supplementary Fig. 5), showing the molar ratios of Ni/V (3.29) and Ni/Fe (2.93) are close to 3:1 that was used in the corresponding solution stoichiometries. The catalytic performances of Ni0.75V0.25-LDH and Ni0.75Fe0.25-LDH are very reproducible (Supplementary Fig. 6) and compared in Fig. 3. A sharp onset catalytic current density can be observed at low overpotential η250 and 300 mV for Ni0.75V0.25-LDH and Ni0.75Fe0.25-LDH, respectively. It is apparent that Ni0.75V0.25-LDH exhibits a better catalytic activity than Ni0.75Fe0.25-LDH, suggesting that substituting Fe entirely by V in Ni-based LDH can improve the water oxidation performance in our case. The improved catalytic activity of Ni0.75V0.25-LDH is not only shown via the higher catalytic current density of linear scan voltammogram (LSV) curves, but also reflected in its lower Tafel slope (Fig. 3b). Ni0.75V0.25-LDH catalyst exhibits a Tafel slope of 50 mV dec−1, which is smaller than that of Ni0.75Fe0.25-LDH catalyst ( 64 mV dec−1). Tafel slopes can be influenced by mass transport and electron transport26,27. Different scan rate ranging from 1 to 5 mV s−1 for LSV have been done, which resulted in negligible change of current densities for Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH catalysts, indicating sufficiently fast mass transport for both LDHs26,27. Therefore, it is reasonable to conclude that the lower Tafel slope of Ni0.75V0.25-LDH is likely ascribed to the facile electron transport through the layers of the catalyst.

Figure 3: Linear scan voltammogram (LSV) curves and Tafel plots.
Figure 3

(a) LSV curves and (b) Tafel plots (with ohmic-drop correction) of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH.

At η of 350 mV, Ni0.75V0.25-LDH can achieve current density of 27.0±1.6 mA cm−2, which is more than twice higher than the one of Ni0.75Fe0.25-LDH (11.7±1.5 mA cm−2). TOF was also calculated at an overpotential of 350 mV in 1 M KOH, assuming all the metal sites were electrochemically active in the water oxidation reaction. Ni0.75V0.25-LDH also shows the better TOF of 0.054±0.003 s−1 compare with 0.021±0.003 s−1 for Ni0.75Fe0.25-LDH. It is worth noting that the above TOFs in this study are obviously underestimated, since some of the metal sites are electrochemically non-accessible. Meanwhile, the overpotential η required to achieve 10 mA cm−2 current density, which is approximately the current expected at the anode in a 10% efficient solar water splitting device under 1-sun illumination28, was also evaluated. Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH show required overpotential 0.347±0.002 and 0.318±0.003 V, respectively, exhibiting the lower required overpotential of Ni0.75V0.25-LDH.

In addition, we compared the durability of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH in 1 M KOH (Fig. 4). When biased galvanostatically at 10 mA cm−2, both of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH electrodes show considerable stability, the slightly decrease of the required potential for Ni0.75V0.25-LDH electrode may be due to the amorphazation during the anodic conditioning process26,29. Obviously, Ni0.75V0.25-LDH electrode requires less overpotential than Ni0.75Fe0.25-LDH, showing its comparable stability and catalytic performance to Ni0.75Fe0.25-LDH for water splitting.

Figure 4: Long-term stability.
Figure 4

Chronopotentiometry curves at current density of 10 mA cm−2 of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH.


To understand the reason behind the high catalytic performance of Ni0.75V0.25-LDH for water splitting, electrochemical active surface areas (ECSA) of Ni0.75V0.25-LDH and Ni0.75Fe0.25-LDH were obtained from cyclic voltammetry (CV) curves in 1 M KOH and compared. Figure 5a shows typical CV curves of Ni0.75V0.25-LDH with different scan rates. By plotting the ΔJ=(JaJc) at 0.25 V versus Ag/AgCl against the scan rate, the linear slope that is twice the double layer capacitance (Cdl) can be obtained, and is normally used to represent the corresponding ECSA1,9,11,26.

Figure 5: ECSA of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH.
Figure 5

(a) Typical cyclic voltammetry curves of Ni0.75V0.25-LDH electrode in 1 M KOH with different scan rates; (b) ΔJ (=JaJc) of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH plotted against scan rates. All the error bars represent the s.d.’s of three replicate measurements. The slopes (2Cdl) were used to represent ECSA. The unit of slopes is mF cm−2.

Active surface area is a very important factor for catalysts in water oxidation reaction, as it is well known that an increase of active surface area often leads to enhancement of the catalytic activity. The linear slope (ECSA) of Ni0.75Fe0.25-LDH is 0.199±0.018 mF cm−2, while Ni0.75V0.25-LDH has a higher linear slope of 0.270±0.030 mF cm−2, which means Ni0.75V0.25-LDH has a more electroactive surface than Ni0.75Fe0.25-LDH (Fig. 5b). The bigger ECSA should be attributed to the smaller size of aggregations by nanosheets in Ni0.75V0.25-LDH (as shown in Supplementary Fig. 2). This can contribute to partial enhancement of water oxidation reaction presented here. Nevertheless, it is important to note that comparing to Ni0.75Fe0.25-LDH, Ni0.75V0.25-LDH has just slightly 36% higher ECSA due to the similar nanostructure, with such small increase of ECSA, more than twofold of current density at η=350 mV can be achieved. This improvement of the catalytic activity cannot be merely ascribed to the slightly increased surface area of the catalysts. This result suggests that Ni0.75V0.25-LDH may have higher intrinsic catalytic activity for water oxidation reaction.

To verify this point, the ECSAs of NiV-LDH with different Ni content were further examined in details, as shown in Fig. 6a–c. The slopes (ECSA) of Ni0.25V0.75-, Ni0.5V0.5-, Ni0.75V0.25- and Ni0.83V0.17-LDH electrodes were 0.123±0.009, 0.166±0.012, 0.270±0.030 and 0.144±0.015 mF cm−2, respectively, in Fig. 6a. Obviously, the largest ECSA can be achieved when the Ni content was 0.75 in NiV-LDHs, as shown in Fig. 6b as well. The relationship of ECSA with the current density of different NiV-LDHs is exhibited in Fig. 6c. One can see that the current density of NiV-LDH increases with ECSA, further confirming the active surface area of catalyst is an important contributor for the enhancement of water oxidation reaction. However, investigating this result carefully, the ECSA has more than twofold increase from 0.123 to 0.270 mF cm−2, while the corresponding current density increases from 4.0 to 27.0 mA cm−2, showing significantly almost seven times improvement. This is a strong clue that incorporating V into Ni hydroxide can not only change the active surface area, but also enhance the intrinsic catalytic property. As a comparison, we also investigated current density-dependent ECSA of different NiFe-LDHs in Fig. 6d. For NiFe-LDHs, the current density increases with ECSA as well; however, comparing with the significantly enhanced current density of NiV-LDH, the current density of NiFe-LDH just almost linearly increases to 1.6-fold (from 7.45 to 11.76 mA cm−2) with 1.3-fold increase of ECSA (from 0.157 to 0.199 mF cm−2). This linear correlation indeed indicates that the improvement of catalytic activity of NiFe-LDHs is mainly due to the increase of actively accessible surface area. We attempted to make a comparison of the catalytic activities between NiFe-LDH and NiV-LDH with the same ECSA value. The linear correlation in Fig. 6d for NiFe-LDH is used to predict the current density of NiFe-LDH with 0.270 mF cm−2 of ECSA (the blue solid square in Fig. 6d), which is supposed to have the same ECSA with Ni0.75V0.25-LDH catalyst (the red solid circle in Fig. 6d). The expected current density of NiFe-LDH described above (20.0 mA cm−2) is still lower than Ni0.75V0.25-LDH (27.0 mA cm−2), although they have been estimated to have the same ECSA value. These results suggest in addition to the increased accessible surface area, probably the V in the Ni-based LDHs can also lead to the increased intrinsic catalytic activity than NiFe-LDHs in our case.

Figure 6: ECSA of LDHs.
Figure 6

(a) ΔJ (=JaJc) of NiV-LDH with different Ni contents plotted against scan rates. The unit of slopes is mF cm−2; (b) ECSA (2Cdl) of NiV-LDH with different Ni contents; (c) current density at 350 mV overpotential plotted against ECSA (2Cdl) of NiV-LDH with different Ni contents; and (d) current density at 350 mV overpotential plotted against ECSA (2Cdl) of NiFe-LDH with different Ni contents (black open squares), estimated the activity of NiFe-LDH (blue solid square) with the same ECSA of Ni0.75V0.25-LDH (red solid circle). All the error bars represent the s.d.’s of three replicate measurements.

Although it is difficult to correctly normalize the catalytic current to the number of active sites in the LDH electrocatalysts to compare the intrinsic catalytic performances accurately, the kinetic parameters of the Tafel slope and onset potential can be selected to reflect the intrinsic activity of catalysts30,31. Thus, we investigated the Tafel slopes and onset potentials of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH in Fig. 3 again. The Tafel slope is only affected by the kinetics of the reaction, which involves the type of active sites but not its quantity, surface area, morphology or electrical resistance30. Therefore, the lower Tafel slope of Ni0.75V0.25-LDH (50 mV dec−1) than that of Ni0.75Fe0.25-LDH (64 mV dec−1) indicates the higher catalytic activity and superior type of the active sites in Ni0.75V0.25-LDH. In addition, Ni0.75V0.25-LDH also shows lower onset potential (250 mV overpotential) than that of Ni0.75Fe0.25-LDH (300 mV overpotential), implying the facile kinetics of Ni0.75V0.25-LDH for the water oxidation reaction, which is consistent with the Tafel slope investigation. These results indicate that Ni0.75V0.25-LDH possesses superior intrinsic catalytic activity in our case.

The higher intrinsic catalytic activity of Ni0.75V0.25-LDH may be due to the higher conductivity than Ni0.75Fe0.25-LDH. To test the conductivity, electrochemical impedance spectroscopies (EIS) of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH electrodes were carried out in the three-electrode configuration in 1 M KOH. The Nyquist diagrams of both electrodes show an apparent semicircle in the high frequency range (Fig. 7a), which should be mainly associated with charge transfer resistance (Rct) in the LDH catalysts32,33. The diameter of the semicircle in Nyquist diagram of Ni0.75V0.25-LDH decreases comparing to that of Ni0.75Fe0.25-LDH, indicating lower charge transfer resistance, that is, improved conductivity in LDH catalysts. A reported electrical analogue was used to fit the EIS data32, and the Rct of Ni0.75V0.25-LDH is estimated to be 62 Ω cm2, lower than that of Ni0.75Fe0.25-LDH (94 Ω cm2). This is also reflected in the Bode plots in Fig. 7b, where Ni0.75V0.25-LDH shows smaller resistance than Ni0.75Fe0.25-LDH. It is known that the LDHs suffer from their low conductivity, in the current case, the higher electron conductivity of Ni0.75V0.25-LDH benefits the charge transfer efficiently, which is also in a good agreement with the lower Tafel slope in Fig. 3b.

Figure 7: EIS measurements.
Figure 7

(a) Nyquist diagram and (b) Bode plots of Ni0.75Fe0.25-LDH and Ni0.75V0.25-LDH with bias of 350 mV overpotential.

On the other hand, comparing to the relatively planar structure in Ni0.75Fe0.25-LDH, the slightly more three-dimensional structured Ni0.75V0.25-LDH can expose more edges of the nanosheets to the electrolyte (see TEM images in Fig. 2c,d and Supplementary Fig. 2). The edges are expected to contain open coordination sites that can be the active sites for water oxidation. Therefore, from this point, Ni0.75V0.25-LDH exposes more active sites than Ni0.75Fe0.25-LDH in electrolyte, while maintaining a similar active surface area. This may be another important factor contributing to the highly catalytic activity of Ni0.75V0.25-LDH. Meanwhile, investigating Fig. 6c again, it is also noted that the increases in ECSA produce large changes in current density up to ECSA=0.17 (2Cdl), but after that the trend is much less pronounced. This change of trend of the activity dependent on ECSA for NiV-LDHs indicates that there should be other factors that can influence the activity of NiV-LDHs besides ECSA. It was reported that the catalytic performance of the layered catalyst for water splitting more strongly depends on the edge-state length than ECSA. The catalytic activity can be linear to the edge-state length34. Therefore, as shown in Fig. 6c, a plausible explanation is that it can be speculated that at small ECSA (<0.17 in our case), the active sites on the edge-state length can be exposed to the electrolyte sufficiently, increasing with ECSA, and dominate the catalytic activity, so the modest increases in ECSA can produce large changes in current density by the edge-state length. However, when the ECSA increases to a large value, due to the aggregation, ESCA will cover numerous edges of the nanosheets from the electrolyte, which makes ECSA show more significant effect than the edge-state length, resulting in a slower increase rate. This result also indicates the important role that the edge state of LDHs plays in the catalytic activity. More investigations into the detailed mechanism are in progress.

To further understand the advantages of Ni0.75V0.25-LDH, density functional theory (DFT) calculations were performed based on the following mechanism for water oxidation:

Here ‘*’ presents the adsorption site that is usually on the top of the doping element. The calculation of the reaction free energy with the zero-point energy and entropy corrections followed the same procedure in ref. 35. Reaction free energies of reaction 1–5 are denoted as ΔG1–ΔG5, ΔG5 is defined as 4.92 eV–ΔG1–ΔG2–ΔG3–ΔG4 to avoid the calculation of the energy of O2 molecule. The overpotential η is defined in equation (1):

The optimized structures of the intermediates in the free-energy landscape are shown in Fig. 8. The intermediate *OH and *OOH bind to the surface through oxygen with a single bond. The difference of their binding energies has been shown to be a constant (3.2±0.2 eV) for various materials, such as metals and oxides36. In our case, the constant is calculated to be 3.22 eV. Because this binding energy difference equals to the sum of the reaction free energies of reaction 3 and 4 (ΔG3G4)35,37, the rate-limiting step is either the formation of *O from *OH (ΔG3) or formation of *OOH from *O (ΔG4). The calculated free-energy landscape shows that the rate-limiting step is the formation of *OOH when the sample is doped with V with η=0.62 V, whereas the rate-limiting step becomes the formation of *O when the sample is doped with Fe with η=1.28 V. Because ΔG3G4=3.22 eV, the lower limit of the η can be reached when ΔG3G4=1/2 × 3.22 eV=1.61 eV if a proper element was doped. Then η=1.61–1.23=0.38 V, which suggests it has a large space to further optimize the activity of Ni-based LDH by doping with other elements.

Figure 8: DFT calculation.
Figure 8

Adsorption geometries of the intermediates H2O, *OH, *O and *OOH in a,b,c and d, respectively. The red, blue, white, grey atoms represent the O, Ni, H and V atoms, respectively. The adsorption structures are similar to these when one Ni is substituted by Fe instead of V; (e) the free-energy landscape.

Besides being better than the prepared NiFe-LDH in our case, Ni0.75V0.25-LDH shows superior catalytic performance than other reported LDHs as well, to the best of our knowledge. Supplementary Table 1 compares the activity of Ni0.75V0.25-LDH with recently reported state-of-the-art LDH catalysts without exfoliation or coupling with other materials, which were loaded on GC electrodes for water splitting, including NiFe-, NiCo-, ZnCo-, CoCo- and MnCo-LDHs. Although the catalytic performances of LDH electrodes are strongly dependent on the preparation methods in literatures, to make a general overview, the current density at 350 mV overpotential and the corresponding mass activity (A g−1) are still used to compare the intrinsic activities between different LDH catalysts. To make the comparison more reasonable, ohmic-drop correction was also performed for Ni0.75V0.25-LDH, as most of the literature has done (Supplementary Fig. 7)8,9,26,29,38. In our case, without ohmic-drop correction, at 350 mV overpotential, Ni0.75V0.25-LDH can achieve 27 mA cm−2 current density with 190 A g−1 mass activity. After ohmic-drop correction, the current density and mass activity can be as high as 57 mA cm−2 and 400 Ag−1, respectively. Those results are even better than some exfoliated NiFe-, NiCo- and CoCo-LDHs. It is worthy to note that Ni0.75V0.25-LDH shows even higher activity than MnCo-LDH (43 mA cm−2 and 301 A g−1) before long-term anodic conditioning that was reported as one of the most active LDH catalyst for water oxidation26.

It is worth pointing out that although Ni0.75V0.25-LDH outperforms Ni0.75Fe0.25-LDH in our case, we cannot claim Ni0.75V0.25-LDH has higher catalytic activity than all the NiFe-LDHs in the literature. For instance, Louie and Bell reported NiFe-LDH that requires <300 mV overpotential to deliver current densities of 10 mA cm−2 with a Tafel slope of 40 mV dec−1 (with ohmic-drop correction), which outperforms our Ni0.75V0.25-LDH probably due to the different preparation method12. Nevertheless, from Supplementary Table 1, our Ni0.75V0.25-LDH is still highly efficient among the listed catalysts, and comparable to the best-performing NiFe-LDHs12, which indicates our Ni0.75V0.25-LDH is one of the best water oxidation catalysts.

To confirm the O2 evolution and Faradaic efficiency of Ni0.75V0.25-LDH electrode, the experimental and theoretical O2 evolution amount by Ni0.75V0.25-LDH at a constant oxidative current of 1 mA in 1 M KOH were performed as shown in Supplementary Fig. 8. The experimental O2 evolution determined by gas chromatography exhibited 101±7% Faradaic efficiency, when the electrolysis time was 60 min. Moreover, to further explore the highly catalytic activity of Ni0.75V0.25-LDH, we drop-casted Ni0.75V0.25-LDH suspension onto Ni foam as well, which can supply excellent conductivity and very high surface area for the electrode, and tested the catalytic activity of resulted electrode in 1 M KOH for water oxidation. The Ni0.75V0.25-LDH on Ni foam exhibits the promising activity for practical applications, with 44 mA cm−2 at 350 mV overpotential, and just 300 mV overpotential required to reach 10 mA cm−2 (Supplementary Fig. 9) without ohmic-drop correction. Such catalytic activities of Ni0.75V0.25-LDH on Ni foam indicate attractive prospects for large-scale and practical applications.

In summary, Ni0.75V0.25-LDH has been prepared by a simple hydrothermal method, which is monolayered and shows high catalytic activity for the water oxidation reaction comparable to the best-performing NiFe-LDHs. The high intrinsic catalytic activity of Ni0.75V0.25-LDH is mainly due to the good conductivity, facile electron transfer and abundant active sites in the nanolayers of Ni0.75V0.25-LDH, showing potential to be one of the most effective Ni-based LDH electrocatalysts. Our study reveals the promising catalytic properties of vanadium incorporated Ni-based LDHs, and expands the scope of non-precious metal catalysts with the highly intrinsic activity for the water oxidation reaction.


Preparation of NiV- and NiFe-LDHs

A one-step hydrothermal method was employed to synthesize the bulk LDHs. In brief, for preparation of NiV-LDH, different mole ratios of Ni/V solution (1:0, 5:1, 3:1, 1:1, 1:3 and 0:1 for the synthesis of pure Ni(OH)2, Ni0.83V0.17-LDH, Ni0.75V0.25-LDH, Ni0.5V0.5-LDH, Ni0.25V0.75-LDH and bare V-based hydroxide, respectively) was obtained by mixing NiCl2 and VCl3 in 80 ml H2O, while the total amount of metal ions (Ni2++V3+) was kept to 3.2 mmol. Afterwards, 0.3 g of urea was added, and the above mixture solution was transferred to a stainless-steel Teflon-lined autoclave, and heated in an oven at 120 °C for 12 h. After cooling the autoclave to room temperature, the resulting powder was washed by deionized water and ethanol three times, collected and then dried at 70 °C overnight. As a reference, for preparation of NiFe-LDH, the same processes were followed except FeCl3 was used as iron source instead of VCl3, which was analogous to the literature25.

Electrode preparation

A measure of 5 mg of the obtained LDH powders were dispersed in the mixture solution of 1 ml H2O, 0.25 ml 2-propanol and 10 μl 5% Nafion (ethanol solution) by sonication for >1 h. A measure of 2.5 μl of the above suspension were drop-casted to a pre-polished GC electrode (diameter: 3 mm), and dried at 50 °C for 15 min to evaporate the solvent.

Structure and surface characterization

X-ray diffraction measurements were carried out on Bruker X-ray diffraction diffractometer D5000 with Cu Kα radiation. SEM images were taken on JEOL JSM-7000F instrument with energy-dispersive X-ray spectroscopy (EDS). TEM images were taken on JEOL JEM2100 TEM. Tapping mode AFM was performed to examine the surface morphology by a Dimension Icon AFM (Bruker, Santa Barbara, USA) on silicon wafer. Rectangular cantilevers with approximate dimensions of 125 μm in length and 40 μm in width (BudgetSensors Tap300Al-G) were used to perform the tapping mode experiments. The NanoScope Analysis software (version 1.50, Bruker) was used to analyse the recorded AFM data. A first-order polynomial-flattening algorithm was employed to remove surface tilt from height images. XPS measurements were conducted with an in-house spectrometer (PHI 5500) using monochromatized Al Kα radiation (1,486.6 eV). The pressure in the analysis chamber was 5 × 10−9 mbar during the measurement. Core peaks were analysed using a nonlinear Shirley-type background. The peak positions and areas were optimized by a weighted least-squares fitting method using 70% Gaussian/30% Lorentzian lineshapes. The powder was grinded and deposited on a conductive FTO glass. An electron flood gun was used to compensate the charging effects. The XPS spectra were energy calibrated by setting the adventitious carbon peak to 285 eV.

Electrochemical measurements

Electrolysis experiments were carried out in a polytetrafluoroethylene cell with an Autolab potentiostat with GPES electrochemical interface (Eco Chemie) in a standard three-electrode configuration, which was composed of working electrode (LDHs deposited on GC electrodes), counter electrode (Pt net) and reference electrode (Ag/AgCl). The electrolyte was 1 M KOH, and the applied potentials were converted with respect to reversible hydrogen electrode (RHE), ERHE=EAg/AgCl+0.059 pH+0.197 V, and overpotential η=ERHE–1.23 V.

First, before all the electrochemical measurements, a galvanostatic measurement at a fixed current density of 5 mA cm−2 was performed until a stable potential was obtained. Then LSV were measured from 0.2 to 0.7 V versus Ag/AgCl with a slow scan rate of 2 mV s−1. By plotting overpotential η against log (J) from LSV curves, Tafel slopes can be obtained. To test the stability of LDHs, a galvanostatic measurement at a fixed current density (J) of 10 mA cm−2 was performed. ECSA were measured by CV at the potential window 0.2–0.3 V versus Ag/AgCl, with different scan rates of 20, 40, 60, 80, 100 and 120 mV s−1. By plotting the ΔJ=(JaJc) at 0.25 V versus Ag/AgCl against the scan rate, the linear slope that is twice of the double layer capacitance (Cdl) is used to represent ECSA. All the above measurements were carried out without ohmic-drop correction unless noted otherwise.

Turnover frequency

The TOF of LDH catalysts were calculated according to the following equation (2)9,

where J is the current density at a given overpotential, for example, in our cases η=350 mV, A is the surface area of the electrode (0.07 cm2), F is Faraday constant (96,485 s A mol−1) and m is the number of moles of the metal on the electrodes. In our cases, we assumed all the metal sites were actively involved in the electrochemical reaction.

To compare the conductivities of LDHs, EISs were carried out in 1 M KOH with a three-electrode configuration, the frequency ranged from 0.1 to 105 Hz, with an a.c. amplitude of 10 mV and overpotential bias of 350 mV.

The measurements of O2 were performed in an air-tight H shape cell, which was divided by a glass frit to two chambers. The working electrode, the Ag/AgCl reference electrode and a magnetic stirring bar were inserted in one chamber of the cell, the Pt counter electrode was inserted in the other chamber. The cell was filled with 1 M KOH and degassed with helium for >1 h. The headspace of the compartment containing the working electrode was 23.6 ml. The electrolysis was carried out with a constant oxidation current of 1 mA for 60 min. A measure of 500 μl of the gas sample in the compartment containing the working electrode was transferred by a specific syringe to the gas chromatography, (Shimadzu) where the amount of O2 evolution was determined. The Faradaic efficiency was determined from the total amount of charge Q (C) passed through the cell and the total amount of the produced O2 nO2 (mol): Faradaic efficiency=4F × nO2/Q, where F is the Faraday constant, assuming the four electrons are needed to produce one oxygen molecule.

DFT calculation

Calculations were carried out with DFT implanted in the Vienna Ab initio Simulation Package (VASP)39,40,41,42 to give a better understanding for the superior activity of Ni0.75V0.25-LDH. Perdew-Burke-Ernzerhof (PBE)43 exchange-correlation functional and projector augmented-wave (PAW)44 pseudo-potential were adopted. An energy cutoff of 400 eV was applied for the plane-wave basis set. A 2 × 2 supercell was used with one of the Ni atom substituted by Fe or V. A 7 × 7 Monkhorst–Pack K-point grid was applied for the sampling of Brillouin zone. To describe the transition metal elements, DFT+U45 method have been used with the U values from ref. 35, U−J=3.8 eV for Ni2+ and U−J=4.3 eV for Fe3+ and U−J=3.4 eV for V3+ species. One proton of the material is removed to create the metal ion at 3+ oxidation state. The structures were optimized until the maxima force on the atoms was smaller than 0.02 eV/Å.

Data availability

The data that support the findings of this study are available from the corresponding author upon request.

Additional information

How to cite this article: Fan, K. et al. Nickel–vanadium monolayer double hydroxide for efficient electrochemical water oxidation. Nat. Commun. 7:11981 doi: 10.1038/ncomms11981 (2016).


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We thank Beatrice Johansson from KTH, Dr Valentina Leandri, Chao Xu and Sareh Ahmed from Uppsala University for their help in characterizations of materials. We acknowledge the financial support of this work by Swedish Energy Agency, the Knut and Alice Wallenberg Foundation, the Swedish Research Council, the National Natural Science Foundation of China (21120102036, 91233201) and the National Basic Research Program of China (973 program, 2014CB239402).

Author information


  1. Department of Chemistry, Organic Chemistry, KTH Royal Institute of Technology, 10044 Stockholm, Sweden

    • Ke Fan
    • , Hong Chen
    • , Quentin Daniel
    • , Fusheng Li
    •  & Licheng Sun
  2. State Key Laboratory of Advanced Technology for Materials Synthesis and Processing, Wuhan University of Technology, Wuhan 430070, China

    • Ke Fan
  3. Division of Theoretical Chemistry and Biology, School of Biotechnology, KTH Royal Institute of Technology, SE-106 91 Stockholm, Sweden

    • Yongfei Ji
    •  & Yi Luo
  4. Department of Chemistry, Surface and Corrosion Science, KTH Royal Institute of Technology, SE-10044 Stockholm, Sweden

    • Hui Huang
    •  & Per Martin Claesson
  5. Department of Physics and Astronomy, Uppsala University, Box 516, 751 20 Uppsala, Sweden

    • Bertrand Philippe
    •  & Håkan Rensmo
  6. State Key Laboratory of Fine Chemicals, DUT-KTH Joint Education and Research Center on Molecular Devices, Dalian University of Technology (DUT), Dalian 116024, China

    • Licheng Sun


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K.F. and H.C. contributed equally to this paper. K.F. designed the experiments, fabricated and measured the devices, and wrote the paper. H.C. carried out the X-ray diffraction, SEM and TEM characterization, analysed the data and helped to revise the paper. Y.J. and Y.L. did the DFT calculation; H.H. and P.C. carried out the AFM measurement; and B.P. and H.R. carried out and analysed the XPS measurements. Q.D. and F.L. contributed to the discussion of the paper. L.S. supervised the project and wrote the paper.

Competing interests

The authors declare no competing financial interests.

Corresponding author

Correspondence to Licheng Sun.

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