Vivianite crystallization is a promising route for phosphorus (P) recovery from P-rich wastewater. However, organic matter (OM) in wastewater may influence vivianite formation. In this study, the effects of four representative OMs, glucose, bovine serum albumin (BSA), humic acid (HA) and sodium alginate (SA), on P recovery by vivianite were investigated. The results showed that P recovery efficiency was inhibited by HA and SA, declining by 3.7% and 12.1% under HA (100 mg/L) and SA (800 mg/L), respectively. BSA, HA and SA affected the aggregated form of vivianite crystals. Vivianite particle size decreased in the presence of HA and SA. Subsequent mechanistic exploration indicated that the complexation between the OM and Fe2+ was the main cause of P recovery efficiency reduction. The coprecipitation of HA and SA with vivianite could reduce the zeta potential on the crystal surface, resulting in a smaller particle size. The nucleation sites provided by BSA and SA could transfer vivianite from single plate-like agglomerate to multilayer plate-like agglomerate. This study provided a better understanding of P recovery by vivianite from OM-rich wastewater.
Glucose, BSA, HA and SA affected vivianite crystallization from wastewater.
OM might reduce P recovery rate by competition adsorption of Fe2+.
The morphology of vivianite crystals were different under SA and BSA.
Negative correlation presented between OM and Fe/P ratios during crystallization.
Phosphorous (P) is an indispensable biogenic element for living matter and plays a vital role in both biogenic growth and modern industry (Venkiteshwaran et al. 2018). Rock phosphate is a limited and nonrenewable resource that might be exhausted in several decades (Cordell et al. 2009; Hao et al. 2013). Therefore, a consensus has been reached regarding the serious shortage of P resources (Chowdhury et al. 2017). However, approximately 1.3 million tons of P are discharged into the environment with wastewater every year (Li & Li 2017). High P emissions have caused increasing crises in aquatic environments, especially for eutrophication (Huang et al. 2015; Park et al. 2017). If this wasted P is recovered, it can meet ∼20% of global P demand (Yuan et al. 2012).
A promising strategy for P recovery (PR) is the production of recyclable compounds, such as calcium phosphates, struvite and vivianite (Desmidt et al. 2015; Shaddel et al. 2019; Wu et al. 2019). In particular, vivianite [Fe3(PO4)2·8H2O] crystallization has shown good application prospects due to its natural ubiquity, easy accessibility, and foreseeable economic value (Wu et al. 2019). Currently, many studies have confirmed the feasibility of applying vivianite crystallization to PR from sludge (Cheng et al. 2015; Wilfert et al. 2016, 2018; Wang et al. 2019). In our previous study, it has been proven that it is possible to release P from the sludge phase into the liquid phase through excess sludge pretreatment followed by reprecipitation to obtain vivianite (Li & Sheng 2020). However, during the P release process, some organic substances and ionic impurities in sludge will be released simultaneously, which may affect vivianite crystallization (Wang et al. 2016; Madsen 2019).
There has been some attempts to delineate the key factors influencing vivianite formation, such as pH, the Fe/P molar ratio, the saturation index (SI) and coexisting metal ions (Liu et al. 2018; Wang et al. 2018). However, the effects of organic matter (OM) interference on vivianite precipitation are scarcely reported (Lin et al. 2020; Zhang et al. 2020). Generally, OM comprises abundant functional groups, e.g., carbonyls, carboxyls, hydroxyls, and ester groups, which may influence the properties of vivianite and the transformation of Fe2+ and orthophosphate (He et al. 2014; Chen et al. 2019). Based on these studies, the effect of OM on the crystallization of calcium phosphates and struvite can be explained by: (1) the adsorption of OM on the crystallite surface and blockage of the active growth sites and (2) the complexation of organic ligands with metal ions in the solution and reduction of the free ions available for precipitation (Zhou et al. 2015). However, notably, the aforementioned studies treated OM as a whole and summarized the effect mechanism. OM in wastewater consists of a variety of large and small molecules. The concentration range, molecular weight (MW) distribution, and dominant functional groups are different for different molecular species. These factors make it difficult to explore the interference mechanism of different OM species. Therefore, using representative compounds might be a viable simulation to understand the interaction between OM and vivianite formation.
Collectively, organic compounds in sludge usually include saccharides (monosaccharides and polysaccharides), proteins and humic substances (Yuan et al. 2019). The polysaccharide released from granular sludge has similar properties to alginate (Lin et al. 2013). Glucose is a common monosaccharide, and the protein and humic substances in synthesizing artificial sewage are usually prepared with bovine serum albumin (BSA) and humic acid (HA) (Yang et al. 2012; Wei et al. 2019). Therefore, glucose, BSA, HA and sodium alginate (SA) could be used as representative OM to identify the effects on vivianite crystallization.
The objectives of this study were to investigate the effects of OM (glucose, BSA, HA, SA) on vivianite crystallization at different concentrations. After the precipitates were recovered, their composition, morphology and other characteristics were analyzed to explore the effects and their mechanisms. The results obtained in this study may provide new insights for PR as vivianite from OM-rich wastewater.
MATERIALS AND METHODS
Preparation of synthetic wastewater
All the inorganic chemicals, glucose and SA used in the experiment were analytical reagent grade and purchased from Sinopharm Chemical Reagent Co., Ltd. HA and BSA (Biotech Grade) were purchased from Shanghai Aladdin Bio-Chem Technology Co., Ltd. Ferrous coagulant of FeSO4·7H2O, which is commonly used in wastewater treatment plants (WTTPs), was selected as the Fe2+ source, and KH2PO4 was selected as the source. The content in the sludge anaerobic digester of WTTPs can range from 75–400 mg/L (Garcia et al. 2012). Therefore, the content of in this study was set at 310 mg/L (0.01 M). Typically, after sludge digestion, different OM concentrations in the wastewater were within the range of tens to thousands of mg/L. According to previous studies, the maximum carbohydrate, protein and HA concentrations can reach 800, 938.33 and 100 mg/L, respectively (Chen et al. 2007; Wei et al. 2019; Zhang et al. 2020). Therefore, the concentrations of glucose, HA, BSA and SA in synthetic wastewater ranged from 0–1,000 mg/L, 0–100 mg/L, 0–1,000 mg/L, and 0–800 mg/L, respectively. Oxygen-free deionized water was used in the experiments, and all the experiments were conducted in an anaerobic glove box with N2 flushing at 25 °C. A stock solution of 0.2 M was prepared from KH2PO4, and a stock solution of 0.3 M Fe2+ was prepared from FeSO4·7H2O. The concentrations of glucose, SA, BSA and HA stock solutions were 20.0, 10.0, 20.0 and 5.0 g/L, respectively. Then, 50 mL stock solution, 50 mL Fe2+ stock solution, and different amounts of OM stock solution were transferred into a 1000 mL volumetric flask for dilution with water and used as synthetic wastewater. The Fe/P molar ratio was 1.5 in the synthetic wastewater samples (Liu et al. 2018).
Prepared synthetic wastewater was transferred to a 1,000 mL beaker and adjusted to pH 7.0 using 2 M NaOH and 2 M H2SO4 under magnetic stirring for 30 min before settling for 30 min. Then, the sample was centrifuged at 4,000 rpm for 10 min. The supernatants were used to measure , Fe2+ and OM concentrations, and the separated solids were dried at 40 °C and ground for further analyses.
Mechanism analysis experiment
Premixing experiments were used to investigate the combination of different OM with Fe2+ or separately. Fifty milliliters of Fe2+ stock solution (0.3 M) or stock solution (0.2 M) were mixed with different amounts of OM stock solution and then transferred to a 1,000 mL volumetric flask for dilution with deionized water. The concentration of OM was similar to that in the vivianite experiments. The mixed solution pH was adjusted to 7.0 under magnetic stirring for 30 min before settling for 30 min (Liu et al. 2018). The concentrations of dissolved Fe2+ and before and after the reaction were measured.
31P nuclear magnetic resonance analyses (31P-NMR) were used to validate the complexes between phosphorus and different OM. OM consisting of 100 mg glucose, 10 mg HA, 100 mg BSA, and 80 mg SA was mixed with 100 mL KH2PO4 solution (0.01 M) individually, and then the mixture was stirred for 2 h at pH 7.0. Then, it was centrifuged, filtered and concentrated to 10 mL at 40 °C for 31P NMR analysis.
To determine the adsorption capacity of vivianite to OM, 0.1 g of pure vivianite was placed in 100 mL centrifuge tubes. Then, 50 mL of solution containing different OM was added (along with 0.01 M NaCl to maintain ionic strength). The gradient concentrations of OM were 0–100 mg/L. The solution pH was adjusted to 7.0 ± 0.2 using 0.1 M NaOH and 0.1 M HCl. The mixture was stirred at 200 rpm for 48 h until adsorption equilibrium was reached. At the end of the adsorption experiments, the OM concentration in the supernatants was determined.
The initial Fe/P molar ratios of 1.6–2.0 in synthetic wastewater were chosen to evaluate the effect of Fe/P on vivianite precipitation in the presence of OM. The synthetic wastewater was consistent with the abovementioned methods, and the OM concentrations were 1,000 mg/L glucose, 1,000 mg/L BSA, 100 mg/L HA and 800 mg/L SA. Moreover, the MW distribution of different OM was investigated. Details of the procedures are provided in Figure S1 (Supplementary material).
Analysis and calculation methods
A digital pH meter (PE28-Standard, Mettler) with a combined electrode (LE438) was used to determine the pH values. and Fe2+ were determined following standard methods (APHA 2005). Anthrone-sulfuric acid colorimetry was used to determine glucose. BSA was determined by the Coomassie brilliant blue method. SA and HA were determined using a total organic carbon–nitrogen analyzer (TOC, VCPH, Shimadzu, Japan). For zeta potential measurement, 200 mg vivianite precipitates were dispersed in 100 mL phosphate buffer saline (0.05 M, pH 7.0) by ultrasound for 15 min. The zeta potential of the precipitate surface was measured by a potential analyzer (Zetasizer Nano ZS90, Malvern, UK). The particle size of the precipitates was measured by a laser particle analyzer (2000F, Malvern, UK). The micromorphology of the precipitates was analyzed using a high-resolution field emission scanning electron microscope (SEM, S-4800, Hitachi, Japan). The mineralogical composition was identified by powder X-ray diffraction analysis (XRD-7000, Shimadzu, Japan) with Cu-K radiation (40 kV, 30 mA) in the 2θ range 10°–80°. The functional groups of the precipitates were analyzed by a Fourier transform infrared (FTIR) spectrometer (Nicolet iS10, Thermo Fisher, USA) with a capacity range 4,000–400 cm−1. 31P-NMR analysis was performed using a 500 MHz spectrometer (Advance III Bruker, Germany). D2O was used for the field frequency lock prior to the experiment. All 31P chemical shifts are relative to 85% orthophosphoric acid at 0 ppm.
All tests were conducted in duplicate or triplicate. Analysis of variance was used to evaluate the significance of the results, and p < 0.05 was considered to be statistically significant. Data in this study are presented as the mean ± standard deviation.
RESULTS AND DISCUSSION
Effect of different OM on P recovery efficiency
The effect of OM gradients on PR efficiency is shown in Figure 1. PR reached 99.6% after reaction without added OM. With glucose added, the minimum PR (98.3%) was observed at 600 mg/L, which represented only a 1.3% decrease compared with the control (without OM). This indicated that glucose had almost no effect on PR. The effect of BSA was similar to that of glucose, and PR did not decrease noticeably at different BSA concentration. The maximum residual was 6.3 mg/L, suggesting that 98.0% of P participated after vivianite crystallization. HA inhibition for PR was stronger than that of BSA. Compared with the control, the residual increased from 1.40 to 12.45 mg/L with 100 mg/L HA. Moreover, SA inhibition on PR was not observed at low concentrations, while PR rapidly decreased to 87.7% as SA increased to 800 mg/L. Previous studies have shown that HA and SA had a strong adsorption capacity for divalent metal ions, which could account for the decline in PR in this work (Park & Yoon 2009; Liu et al. 2012). This assumption was supported by the premixing experiments.
In the premixing experiments of OM with Fe2+, the reduction of Fe2+ concentration is shown in Figure 1(c) and 1(d). After glucose and BSA were added to the FeSO4 solution, the soluble Fe2+ was only reduced by 4 and 8 mg/L, respectively. A weak combining capacity was apparent between Fe2+ and glucose/BSA. Fe2+ reduction increased linearly with increasing HA concentration. At low SA concentrations, the reduction of Fe2+ concentration was not obvious, but it had a sharp increase at high SA concentrations. The Fe2+ concentration decreased by 36.5 and 60.8 mg/L at 100 mg/L HA and 800 mg/L SA, respectively. In contrast, the interaction of OM with was not obvious, and the concentration remained stable after OM addition (Figure S2). The 31P NMR spectra of KH2PO4 solution with different OM were investigated separately (Figure S2). Specifically, the single signal of 31P NMR with different OM was observed at 0 ± 0.2 ppm without peak shifting, which was indicative of the weak binding ability between OM and . Both OM solutions and are electronegative, which may be the reason for the weak binding of OM and . To conclude, it was confirmed that by competitive binding of Fe2+, the presence of SA and HA resulted in adverse effects on PR. The OM inhibition of PR was in the following order: SA > HA > BSA > glucose.
Transfer of OM
During vivianite crystallization, OM might transfer to the solid phase through adsorption or coprecipitation with crystals, which would affect the purity of the harvested products. The residue of OM in the supernatant and the removal efficiency (OR) variation are illustrated in Figure 2. At different glucose concentrations, the OR values were less than 10.0%, indicating that most of the glucose remained in the liquid phase after vivianite crystallization. This result indicated that nearly no glucose reacted with Fe2+ and , and glucose was not involved in the precipitates. However, for BSA and HA, OR remained above 85% for all concentration gradients. These results showed that most of the BSA or HA in the liquid phase was transferred to the solid phase during the reaction. When the SA concentration was below 200 mg/L, most SA was fixed by precipitates, and the OR reached 83.6%. However, ∼30.0% SA remained in the supernatant with an SA concentration of 800 mg/L. The remaining SA could not be transferred to precipitates by centrifugation or filtrated through a 0.45 μm membrane. The synthetic wastewater after crystallization remained viscous.
The transfer of OM to the solid phase includes two pathways, coagulation by Fe2+ and coprecipitation after adsorption on the vivianite surface. In vivianite adsorption experiments, the calculated maximum adsorption capabilities of glucose, BSA, HA and SA were 3.22, 7.69, 5.07 and 16.80 mg/g, respectively, which were far below the OM concentration reduction (Table S1, Supplementary material). BSA, HA and SA solution properties are similar to those of colloids. Charge neutralization of Fe2+ could destabilize the colloid, which might be the main cause of OM transfer to the solid. OM precipitation with vivianite would inhibit the crystal process and then the PR. According to Figure 1, the PR changing with HA and SA bore this out. Interestingly, however, BSA coprecipitation had little effect on PR, which needs further explanation.
Effect of OM on recovered precipitates
The XRD patterns of precipitates with different OM are shown in Figure 3. Without OM addition, the recovered vivianite crystals showed strong and sharp diffraction peaks at 11.05°, 13.05°, 18.05°, 23.14°, 27.85°, 30.06° and 33.02° corresponding to Miller indices (110), (020), (200), (−201), (−131), (201) and (041), respectively. The result was consistent with the standard spectra of vivianite crystals (PDF#79-1928), indicating that the product was vivianite (Li et al. 2020). After addition of different OM, no significant difference was observed in the positions of the obtained precipitate peaks. This proved that the type of recovered product was not changed by the addition of OM. However, the presence of BSA and SA changed the relative intensity of the crystal diffraction peaks (Figure 3). The lattice plane relative strength of vivianite crystals (020) and (201) decreased by degrees with increasing BSA. This result suggested that BSA could alter the morphology of vivianite crystals. When the SA concentration ranged from 50 to 200 mg/L, the XRD patterns of the precipitates corresponded to the vivianite pattern. In comparison, when the SA concentration was increased to 800 mg/L, the intensity of the peak at 13.05° decreased significantly, and the increasing strength of the characteristic peaks at 30.06° showed that the crystals presented long dimensions in the (201) direction (Zhang et al. 2020).
Usually, crystallization can be divided into homogeneous and heterogeneous crystallization, which is related to the SI. When the SI was in the metastable zone, heterogeneous crystallization occurred, that is there was a growth of small crystals. When the SI was above the metastable zone, homogeneous crystallization occurred, namely, small crystal aggregation (Wang et al. 2014). A previous study has shown that the suitable supersaturation level for efficient vivianite crystallization could be in SI 4–11 (Liu et al. 2018). In this study, the initial SI was 15.1, so the aggregation of small crystals was dominant during crystallization. This result was further confirmed by SEM images of vivianite crystals with different OM (Figure 4 and Figure S3). In the absence of OM, the harvested crystal was an agglomerate of a single plate with a roughly spherical morphology. Zelibor et al. (1988) reported that vivianite occurs as spherical aggregates of platy-, lath- and needle-shaped crystals in different environments. However, in this study, with the presence of different OM, only plate crystals were observed. Although the surface of any individual crystal in the aggregates appeared to be randomly oriented, the crystals showed a definite crystal orientation, as if they generally radiated from a common center. Moreover, there were some amorphous substances on the crystal surface, and it was presumed to be adsorbed OM or Fe-P precipitation. The crystal transformed from a single plate-like agglomerates to a multilayer plate-like agglomerates with increasing BSA concentration (Figure 4). In contrast, with the addition of 800 mg/L SA, the products formed multiple layers of cumulative compounds rather than crystals with clear boundaries. Such changes in morphology were consistent with the XRD results. A likely explanation was that BSA and SA could penetrate into the interior of crystals and play a bonding role in the aggregate process.
The particle size changes of the products after OM addition are shown in Figure 5. The particle sizes of the precipitates presented two centralization distributions: one-micron and ten-micron scales. These bimodal distributions were consistent with the aggregative growth theory (Wang et al. 2014); small particles were formed in solution with supersaturation as the driving force, and large particles were formed by continued growth or direct fusion of small crystals. There was no significant effect on the particle size of the product from glucose addition. BSA addition could result in a 10-micron scale increase for the particle size, while a 1-micron scale increase was observed for HA addition. These results indicated that HA inhibited the further growth of small crystals. For SA (<800 mg/L), the product particle size was uniformly distributed from one to tens of microns, while it decreased significantly for concentrations over 800 mg/L (Figure 5). This result suggested that the increased solution viscosity might reduce the aggregation of small particles.
Figure 5 also illustrates the zeta potential variation of vivianite with different OM. It was noteworthy that larger vivianite particles had settled before zeta potential measuring. Therefore, the zeta potential reflects the surface potential of the remaining small particles (10 microns and below). Generally, a higher zeta potential (absolute value) on the particle surface results in less particle bonding. The dispersion system of agglomeration was more stable (Zhang et al. 2020). Compared with HA and SA, the effect of glucose and BSA addition on crystal surface potential changes was not significant. The zeta potential of the control was −15.5 mV, and it fluctuated with increasing concentrations of glucose and BSA. The minimum zeta potentials were −25.3 and −21.4 mV, respectively. After HA and SA addition, the zeta potential of the products was reduced to −44.2 and −56.1 mV, respectively. Lower zeta potential on the surface of the products inhibited the aggregative growth of small crystals and thus affected the distribution of particle size.
Mechanisms of different OM affecting the vivianite formation
The inhibition of PR by OM was mainly caused by OM competing with for Fe2+. This was examined by increasing the molar Fe/P ratio in synthetic wastewater. In the presence of OM, Fe2+ was consumed by OM and became a limiting factor for PR. The PR was significantly improved (>97.0%) after Fe/P increased to 1.8, which supported the above deduction (Figure S4). In addition to competing for Fe2+, OM might decrease the crystal growth rate through its adsorption on surface active growth sites of the crystals (Akin et al. 2008; Wei et al. 2017).
To validate the interaction of OM with vivianite, the precipitated products were analyzed by FTIR spectroscopy. As shown in Figure 6, without OM addition, the bands of products appeared at 3,480, 3,148, 1,622, 1,042, 970, 938, and 815 cm−1. These absorption bands were consistent with vivianite crystals in the Sadtler standard spectra (Frost et al. 2002). Specifically, the broad peak between 3,480 and 3,148 cm−1 was attributed to the stretching vibration of hydroxyl groups. The band at 1,622 cm−1 was assigned to the bending mode of water hydrogen bonded to water. Three bands at 1,042, 970 and 938 cm−1 were attributed to the PO-stretching region. The band observed at 815 cm−1 was assigned to the water vibrational modes of strongly hydrogen bonded water molecules (Frost et al. 2002). In the presence of glucose and HA, no new absorption peaks were observed for the product (Figure 6). Bands of HA at 1,385 and 1,577 cm−1 were assigned to the asymmetric and symmetric carboxylate stretch (Wei et al. 2019). However, regardless of the dosage of HA, no bands of product at 1,385 and 1,577 cm−1 were detected, indicating that HA was not directly involved in vivianite formation. The interaction between HA and vivianite was weakly physical coprecipitation. In contrast with HA, the products with both BSA and SA addition exhibited new absorption bands. For BSA, the band located at 1,646 cm−1 came from C = O stretching and was attributed to the amide group of BSA (Liu et al. 2017). For SA, the bands that appeared at 1,416 and 1,543 cm−1 were assigned to the symmetric and asymmetric stretching vibrations of carboxyl groups (Cao et al. 2019). These results indicated that Fe2+ initially forms a binary complex with BSA or SA and then forms an insoluble vivianite-BSA or vivianite-SA complex.
Does this complexation affect the crystallization rate? According to Equation (3), SI was determined by the ionic activity of Fe2+ and . The initial SI with different OM additions was the same before crystallization, so the difference in SI after the reaction can be used to evaluate the effect of OM on the crystallization rate. Based on Visual MINTEQ calculations, after crystallization, the SI with different OM are shown in Table S2. After reaction, the SI of the control, 1,000 mg/L glucose, 1,000 mg/L BSA, 100 mg/L HA and 800 mg/L SA were 5.85, 5.84, 6.46, 6.19 and 6.11, respectively. Compared with the initial SI (15.1), the SI after the reaction experienced rapid declines at different OM concentrations. It was indicated that crystallization rates were not significantly different. Therefore, the potential OM absorption on the vivianite active site was not the main reason for PR reduction.
Based on the above discussion, a schematic diagram of OM reaction pathways during vivianite crystallization is illustrated in the graphical abstract. There was no inhibitory effect on the formation, morphology and structure of vivianite precipitates after glucose addition. BSA could combine with Fe2+, but this part of Fe2+ could still react with to form vivianite. Therefore, the presence of BSA could serve as a template and regulate the morphology of the crystals. This process is similar to biomimetic synthesis, which simulates the biomineralization process (Liu et al. 2017). The amide groups in BSA could enrich Fe2+ and provide nucleation sites. Then, the enriched Fe2+ would attract , resulting in local supersaturation and increasing the growth rate. HA could bind with Fe2+ and inactivate it. Moreover, HA could coprecipitate on the vivianite surface and reduce the surface zeta potential, which would impede crystal aggregation growth. The mechanism of SA was similar to that of BSA, namely, it would precipitate during vivianite formation by direct physical precipitation and indirect chemical coprecipitation. In addition, SA would increase the solution viscosity and inhibit the aggregation growth and sedimentation of products.
The consumption of and resulted in a change in pH. The decrease in pH and the consumption of Fe2+ might cause a lower descent rate of SI. The ionic activity mainly depends on ionic strength of the solution. According to Visual MINTEQ calculations, at the same concentration of Fe2+ and , a lower pH resulted in a smaller SI. To ensure a high recovery rate, keeping a stable reaction pH and raising the Fe/P ratio appropriately to obtain a higher SI may be a feasible approach. However, it is worth noting that with the decrease in SI, the rate of crystal formation also decreased. Therefore, to harvest vivianite efficiently within a limited crystallization time (100 min), the P concentration should be maintained at an optimum range (>5.0 mg/L).
The MW of organic substances is much larger than that of inorganic ions. The MW distribution of different OM is shown in Figure S5. It was found that OM with a lower MW weakly inhibited PR. Thus, another feasible approach to enhance PR is selectively removing high MW substances (HA and SA). From the perspective of morphology, reducing the concentration of HA and SA in wastewater helps to harvest larger vivianite crystals, which facilitates further separation.
Glucose, BSA, HA and SA were used to evaluate the effect of OM on vivianite crystallization. The results showed that glucose had no effect on PR and vivianite morphology; BSA changed the vivianite morphology; HA reduced the PR efficiency; and SA reduced the PR efficiency with morphological changes. Mechanistic exploration indicated that Fe2+ inactivation by OM adsorption caused a reduction in PR efficiency. The coprecipitation of HA on the vivianite surface decreased the vivianite particle size. The BSA and SA involved in vivianite internal provided nucleation sites and regulated vivianite aggregate morphology.
This work was supported by the Strategic Priority Research Program of the Chinese Academy of Sciences (CAS) (Grant No. XDA23,050,203). Additional support was provided by the Regional Key Project of STS of CAS (Grant No. KFJ-STS-QYZX-057), the Key Project of Shandong Provincial Natural Science Foundation (Grant No. ZR2020KE048) and the Key Research and Development Program of Shandong Province (Grant No. 2019GSF109002).
DATA AVAILABILITY STATEMENT
All relevant data are included in the paper or its Supplementary Information.