Thank you for visiting nature.com. You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

# Hydrodynamic assembly of two-dimensional layered double hydroxide nanostructures

## Abstract

Formation mechanisms of two-dimensional nanostructures in wet syntheses are poorly understood. Even more enigmatic is the influence of hydrodynamic forces. Here we use liquid flow cell transmission electron microscopy to show that layered double hydroxide, as a model material, may form via the oriented attachment of hexagonal nanoparticles; under hydrodynamic shear, oriented attachment is accelerated. To hydrodynamically manipulate the kinetics of particle growth and oriented attachment, we develop a microreactor with high and tunable shear rates, enabling control over particle size, crystallinity and aspect ratio. This work offers new insights in the formation of two-dimensional materials, provides a scalable yet precise synthesis method, and proposes new avenues for the rational engineering and scalable production of highly anisotropic nanostructures.

## Introduction

Two-dimensional (2D) structured materials, such as graphene, metal chalcogenides, and layered double hydroxides (LDHs), have been suggested as next-generation materials in catalysis1, energy storage2,3, and electronics4. While some 2D materials are made via vapor-phase deposition, many scalable and low-cost syntheses take place in the liquid phase. The current state of fundamental understanding of how highly anisotropic nanoparticles crystallize and how synthesis conditions affect crystal morphology, size, and structure is rather limited, yet such knowledge is crucial to our ability to rationally design new materials and processes for large-scale manufacturing and applications.

A key problem in identifying the crystallization mechanism of nanostructures is that classical models are overly simplistic, assuming constant surface and bulk energies, while disregarding particle interactions, mass transfer effects, competing kinetics, and external forces. Non-classical mechanisms, including oriented attachment (OA) and two-step nucleation pathways, may dominate when molecular and interparticle interactions are anisotropic. These are important not only in materials synthesis but also in biogenic and geologic environments, for example, in the mineralization of complex calcium carbonate structures in aquatic organisms5.

In wet syntheses, hydrodynamics govern mixing, residence time, and particle interactions but are often neglected in laboratory studies. Reactor geometry and agitation influence the rates of mass transfer, nucleation and growth, residence time distribution, and the resulting particle size distribution6,7. Hydrodynamic shear stress, which is introduced by agitation or pumping, can decrease kinetic interaction barriers to accelerate nucleation and aggregation8,9. Shear also induces the alignment of anisotropic particles by stabilizing angular orientations in the direction of flow10,11. Conversely, by introducing strain, shear may also inhibit crystallization and causes breakup12,13. Depending on its intensity, shear may be used to exfoliate 2D materials like LDH14 and graphene15 or induce structuring16. The effects of shear on non-classical mechanisms of growth such as self-assembly have yet to be fully elucidated, though recent simulations have shown that the OA of patchy trimer particles is accelerated under certain shear rates17.

LDHs are cationic 2D metal hydroxides intercalated with anions and possess applications in catalysis18, drug delivery19, and energy storage20. Colloidal LDH is synthesized via hydrothermal treatment or co-precipitation, usually followed by thermal aging to improve crystallinity21. The crystallization process is not well understood and is thought to proceed via local dissolution and crystallization of amorphous LDH22,23 or via the physical rearrangement of nanocrystalline domains24,25. Surfactant-assisted methods26 and continuous flow reactors have recently been used to generate monolayer LDH nanoplatelets27,28,29, though the control of particle size, crystallinity, and thickness remains difficult.

Hydrodynamics also play a key role in the synthesis of LDH. Reactor geometries (e.g., the T-micromixer30, flow hydrothermal reactor31, and inline dispersion precipitator27), flowrates, and mixing speed have pronounced effects on the crystallite size, surface area, and aspect ratio. However, the physical mechanism behind these effects has not been rigorously investigated. The obscure crystallization mechanism, observed sensitivity to hydrodynamics, and relative ease of synthesis via co-precipitation make LDH a perfect model system for the study of 2D structures under controlled shear.

In this study, we seek to identify the crystallization mechanism of 2D LDHs and examine the effect of hydrodynamics, particularly shear rate. For this, we develop a scalable microreactor, in which a high shear microfluidic environment with microsecond mixing is generated using two-phase annular flow. We observe particle dynamics using liquid transmission electron microscopy (LTEM), a powerful tool for characterizing nanoparticle crystallization and self-assembly32,33,34 and reveal that 2D LDH nanoparticles may crystallize via OA. We mechanistically explain the effects of shear on nucleation, growth, and oriented assembly using insights gleaned from LTEM, atomic force microscopy (AFM), powder X-ray diffraction (XRD) and shear-induced aggregation kinetic modeling. At high shear rates, crystallization of 2D nanoplatelets via OA may be accelerated, affecting the resulting particle size distribution and shape.

## Results

### Microreactor fluid dynamics

The reactor consists of three quartz tubes placed in a staggered, coaxial configuration; see Fig. 1a and Methods. A high velocity gas is pumped through the innermost tube, with liquid reagent streaming through the two outer tubes, creating two regions of two-phase annular flow. The mixing region forms by the collision and hydrodynamic focusing of two-liquid annular flows, which then stabilize into a wavy annular thin film. As the thin film thickness stabilizes, the shear rate $$\dot \gamma$$ in an annular thin film approaches a constant value, which may be determined from the film thickness and velocity or gas and liquid flowrates35.

The liquid profile, mixing dynamics, and mixing time were measured with high-speed fluorescence confocal microscopy. As seen in Fig. 1b, the annular film thickness decreases from 100 to 10 µm with increasing $$\dot \gamma$$, indicating a highly confined reaction environment at shear rates up to 106 s−1. These measurements agree with modeled predictions35. Further discussion of the velocity flow field and decomposition of the gradient and rate-of-strain tensors is included in Supplementary Discussion – Gradient Tensor Decomposition.

When Liquid 1 stream is laced with a fluorescent tracer, as seen in Fig. 1c, micro-vortices are seen originating at the tip of the first annular flow outlet, likely generated by Kelvin–Helmholtz instabilities at the high shear interface, and by secondary flows as the flow suddenly accelerates in the radial direction. These vortices grow and dissipate in a mixing process known as vortex engulfment, a well-described mode of micromixing36,37. After the transient mixing section, the liquid profile stabilizes into wavy striations. High-speed video footage is available in Supplementary Movie 1.

The measured characteristic micromixing times, which range from 11 to 0.4 ms, are in close agreement with those predicted by an engulfment mixing model36, as seen in Fig. 1d, confirming that the engulfment of microscale eddies is the dominant mixing mechanism. The energetic efficiency of mixing is on average 53% of the theoretical efficiency, an improvement over rotor-stator mixers (~35%) and serpentine micromixers (~14%)38, which could reduce power consumption at the industrial scale. A comparison with other mixing technologies is given in Supplementary Table 1, where the annular microreactor is one of the fastest mixing techniques for the synthesis of nanoparticles. It is slower than highly confined single-phase microreactors such as the turbulent tangential mixer and capillary ball mixer, though it has significantly less clogging risk and a lower pressure drop.

Macromixing times, which were determined from the concentration of fluorescent tracer, decrease from milliseconds to microseconds as $$\dot \gamma$$ increases; the fastest mixing time measured was 288 µs, as seen in Fig. 1d. These are in the same range as micromixing times determined by Villermaux–Dushman chemical test method39,40 and in agreement with predictions from the engulfment mixing model. Rapid micromixing and macromixing timescales ensure that parallel reaction systems with different rates, such as nucleation (fast) and growth (slow), may be segregated and that the residence time distribution should be narrow, ensuring a product with small size and low polydispersity.

There are several key advantages that make this reactor amenable for rapid scale-up and precise manufacturing of nanostructures: (1) with microsecond mixing, fast kinetics such as nucleation, surface growth, and aggregation during high supersaturation precipitation may be controlled; (2) with high wall shear and only one non-slip boundary, scaling and clogging are reduced; (3) increasing throughput can be achieved by increasing the number of reactors or the flowrate, in accordance with previously determined reaction conditions; and (4) as a continuous reactor, space–time yield is high, which reduces capital and operating costs during scale-up41,42, integration with downstream processes is simplified, and inline characterization/optimization is possible43,44. This flexibility provides a means of precisely controlling hydrodynamic shear, mixing time, and residence time from the laboratory bench to the industrial scale and may be used to intensify the development of colloid synthesis techniques of nanomaterials.

### LDH synthesis and characterization

Colloidal dispersions of MgAl LDH (hydrotalcite) were co-precipitated from an aqueous solution of metal nitrates and a basic solution of sodium hydroxide and sodium carbonate at a supersaturation ratio of 3 × 104 at 21 °C. Reagents and air were injected at flowrates corresponding to shear rates ranging from 7.26 × 104 to 3.16 × 106 s−1. The suspensions consisted of fine, white, translucent precipitate, which formed a thick gel after centrifugation. After rinsing with deionized (DI) water, the colloidal stability of the material was increased, as has been observed in previous studies27.

AFM measurements were conducted to determine the particle size distribution in dry samples, measuring both height (H) and area-averaged diameter (D). AFM height maps showed nanoplatelets of 28.1 ± 5.5 nm in diameter, ranging from 0.7 to 1.5 nm in height, corresponding to monolayer and bilayer LDHs. These nanoplatelets would also form clusters, seen in Fig. 2a. The aspect ratios (AR = D/H), measured for each particle and cluster strongly correlate with their height. The slope of this correlation varied non-monotonically with $$\dot \gamma$$; at 8.4 × 105 s−1 “flat” clusters of maximum anisotropy formed, while at lower or higher shear rates “round” clusters of lower anisotropy formed, which is shown in Fig. 2b.

The correlation between aspect ratio and height indicates that the particles assemble in an ordered manner, which directly verifies previous studies that have suggested that LDH particles may preferentially orient epitaxially, edge-to-edge45 and face-to-face24. More interestingly, the non-monotonic dependence of aspect ratio and shear suggests that shear not only influences the kinetics of OA but also has competing effects that enhance or decrease particle anisotropy.

XRD and high-resolution TEM (HRTEM) were performed to identify the scale at which shear governs cluster anisotropy. XRD patterns showed the characteristic peaks of hydrotalcite structure at 2θ = 11.5°, 22.9°, and 61.8°, corresponding to the (003), (006), and (110) lattice planes, as seen in Supplementary Figure 1. The crystallite size in the [110] direction (the basal crystal plane) as determined using the Scherrer equation, varied non-monotonically with $$\dot \gamma$$, similarly to the trend in aspect ratio observed with AFM, as shown in Fig. 2c. From 7.26 × 104 to 4.11 × 105 s−1, the crystallite size increased from 15 to 27 nm, approximately the observed diameter of the primary platelets, and decreased to 13 nm at 3.16 × 106 s−1. This suggests that shear affects particle crystallinity, which then governs their oriented aggregation and anisotropy. Highly crystalline particles synthesized at 4.11 × 105–8.4 × 105 s−1 align readily, whereas less crystalline particles do not.

HRTEM images, exhibited in Fig. 3a, b, showed that LDH synthesized at 4.11 × 105 s−1 were indeed highly crystalline. The LDH synthesized at 3.16 × 106 s−1 was polycrystalline, with domain sizes in the order of 5 nm, seen in Fig. 3c. The meso-crystalline structure of the densely packed aggregates was also resolved. Displayed in Fig. 3d are layers of LDH primary particles separated by 0.8 nm, indicative of the (003) spacing. A fast-Fourier transform shows visible (003) and (106) peaks, revealing that not only are the particles stacked but are also epitaxially attached in the basal plane.

### Liquid transmission electron microscopy

LTEM was performed to visualize the mechanism of platelet aggregation and the mechanism by which hydrodynamic shear may affect crystallization kinetics. Immediately after synthesis, suspensions were diluted, loaded into a 150-nm-thick silicon nitride cell using a Protochips liquid holder, and imaged within an hour (see Methods). Dispersed hexagonal disks ≤10 nm in diameter adhered to the silicon nitride membrane surface. These were predominantly oriented face down, most likely due to Coulombic attraction between the positively charged hydrotalcite and negatively charged silicon nitride, limiting Brownian motion. We speculate that these LDH particles most likely aggregate to form the ~30 nm nanoplatelets measured in AFM during the post-processing steps of centrifugation, rinsing, and drying.

Under static conditions, particles at close distances aggregated by “walking” to each other, rotating until crystal facets were aligned, and attaching edge-to-edge, as seen in Fig. 4a and Supplementary Movie 2. As seen in Fig. 4b, the speed of approach was correlated to the alignment of facets, clearly indicating a mechanism of OA. In one interesting scenario seen in Supplementary Movie 3 and Supplementary Figure 2, six particles with diameters of approximately 5 nm are loosely packed in a pentagonal configuration. These six particles undergo much slower rates of aggregation, despite their proximity. While the high local concentration of particles can decrease Brownian diffusivity, OA is also likely hindered by the pentagonal configuration of these particles, which limits facet alignment with the neighboring particles. This also indicates that misalignment, in addition to electrostatic repulsion, is a significant barrier to aggregation where van der Waals forces are the main driving force.

The introduction of flow accelerated particle aggregation. Local particle motion was difficult to induce with an external syringe pump; however, when a bubble was created via radiolysis under an intensified electron beam46, the de-wetting of the silicon nitride membrane created a local flow strong enough to convect particles. The approach rates of two colliding particles, which was determined by tracking interparticle distances, were compared for static and bubble-induced flow conditions. The approach velocity in aggregation events between two ~8 nm particles in a static liquid environment and in a flowing liquid are detailed in Fig. 5 and Supplementary Movies 4 and 5. The average approach velocity was about four times faster in a flowing liquid as it was in a static liquid at interparticle distances under 25 nm.

This acceleration may be explained by two factors: flow-induced convection and rotation. Flow increases mass transport via advection and the dissipation of energy into heat, which enables particles to overcome the electrostatic barrier to aggregation. This can be modeled as a lowered effective kinetic barrier12,47,48,49. In static conditions, attraction to the TEM cell membrane surface limits rotation. When hydrodynamic forces overcome this adhesive force, particles rotate more easily and as a result will orient more quickly. This effect seems to be important at very close distances, at the order of the particle size. The added barrier to aggregation from misalignment may perhaps be included in models as a modified collision frequency parameter.

These are, to the best of our knowledge, the first direct observations of LDH crystallization via OA of nanoplatelets and of hydrodynamically accelerated OA via bubble-induced flow in LTEM. We speculate that this is the dominant mechanism in concentrated, rapidly mixed conditions and may be a significant crystallization pathway during aging. This confirms the previous studies that have suggested an OA mechanism24,29 in addition to Ostwald ripening, a slow dissolution, and recrystallization process22,50.

The anisotropy of LDH’s surface is most likely responsible for its propensity to undergo OA. While the hydroxide groups at the basal surface of LDH sheets are triply coordinated, the edge hydroxide groups are bi- and mono-coordinated, which are labile and amphoteric51,52. These groups are responsible for the chemisorption of heavy metal ions, such as arsenate and chromate. In suspensions with high pH values (10–11), such as the synthesis conditions used in this study, these edges decrease in charge via dissociation of hydroxyl groups and adsorbed water, decreasing Coulombic repulsion such that aggregation at the edges is kinetically favored.

Adsorbed anionic species may also play a significant role in OA by mediating the acid/base interactions of edge hydroxyl groups. For example, amphoteric polyprotic anions such as carbonate increase the aggregation and crystallization of LDH53,54, presumably by both screening the surface charge of LDH while retaining its amphoteric nature. Conversely, using ligands and/or solvents that inhibit acid/base interactions may inhibit OA and increase the basal/edge interactions. This could be the primary mechanism behind the generation of flower-like morphologies when LDH is synthesized using anions like organic acids55 and organic solvents like acetone56. Further exploring the effects of anionic species and solvent interactions on OA in LDH would be useful in the rational assembly of LDH nanostructures.

The observation of dynamic particle movements, like walking and rotation, also introduces the use of LDH particles to quantitatively study these non-DLVO factors. It may also be possible to explore the formation mechanisms of dense or fractal aggregates, which were also observed (see Supplementary Figures 3 and 4 and Supplementary Discussion-Aggregate Formation). In such studies, it would be important to carefully consider the effects of the electron beam on the local ionic environment, particle charge, and silicon nitride surface.

### Kinetic analysis

The particle size distributions of LDH synthesized at 4.1 × 104 s−1 (A), 8.4 × 105 s−1 (B) and 3.2 × 106 s−1 (C) were measured to determine the effect of shear on nucleation and growth kinetics. The particle areas and calculated hexagonal side length a are compiled in Fig. 6a. From A to B, the median particle area decreases from 43.4 to 39.0 nm2 and the side length distribution narrows from 3.92 ± 1.03 to 3.89 ± 0.94 nm. From B to C, the area distribution becomes multimodal and the side length distribution widens to 3.75 ± 0.97 nm. By deconvoluting the area distribution of C, we find five peaks regularly separated by 11.7 nm2, approximately the area of the smallest particle measured (10.6 nm2). This particle, as seen in Fig. 6b, possesses a side length of 2.14 nm and is composed of only 113 cations.

We speculate that this is the critical nucleus size, above which particles grow via surface addition or aggregation. This explains why LDH nanoparticles as small as 4 and 7.8 nm have been observed in previous studies27,29,57. This critical size is influenced by a range of factors such as the initial supersaturation, temperature, and pH, which are explained by classical nucleation theory. The size may also represent a non-classical, or metastable, configuration at which the surface is sufficiently stabilized by complex local solvent–solute–surface interactions5. This seems likely, as aggregates anneal slowly after attachment, which is seen Supplementary Figure 4, even under the excitation of the electron beam. The structure and evolution of these interactions are still not well known and are a subject of future study.

We interpret these changes in particle size distribution by considering the effects of shear on mixing, kinetics, and thermodynamics. For this analysis, we use the concept of characteristic aggregation timescales based on previously developed kinetic rate theories for the growth and aggregation of Brownian particles, which are described in Methods. At 4.1 × 104 s−1, the mixing time is approximately 4.4–2.1 ms, which is lower, but on the same order as the characteristic growth time 16.6 ms. Therefore, nucleation and surface growth may occur concurrently, producing a more polydisperse population. The characteristic aggregation time for two nuclei, which we approximate as Brownian discs 0.7 nm in thickness and 2 nm in radius is 0.68 s, implying that aggregation is not a dominant growth mechanism.

At 8.4 × 105 s−1, the mixing time decreases to 1.9–0.43 ms, which is faster than the timescale of surface growth, resulting in the effective segregation of nucleation and growth and a more homogeneous size distribution. The calculated characteristic aggregation time is 150 ms, which is an order of magnitude greater than the growth timescale.

At 3.2 × 106 s−1, the mixing time is <1 ms, ensuring segregation of nucleation and growth steps, and the shear rate is significant enough to affect the motion of colloidal particles <10 nm. The Peclet number (Pe) represents the ratio of hydrodynamic forces to Brownian forces, where at Pe<<1 hydrodynamic forces may be neglected. The rotational Peclet number (Per) reflects the effect of hydrodynamic forces on particle rotation, where at Per<<1 particle rotation is random; at higher Per particles may align in the direction of flow (see Methods). For disc-like particles of 4 and 8 nm in diameter, Pe equals 0.07 and 0.46, respectively, and the rotational Peclet number (Per) equals 0.06 and 0.47. This implies that hydrodynamic forces may significantly affect the motion and alignment of particles at this shear rate. The calculated characteristic aggregation time for a nuclei is 77 ms, which is at the same order of the growth timescale. Thus aggregative growth via OA is accelerated and occurs simultaneously with surface growth, resulting in a multimodal particle size distribution. This aggregation time may be even lower due to flow-induced alignment; this effect could be estimated by developing a generalized kinetic model for the OA of highly anisotropic nanoparticles in shear flow, which is outside the scope of this study. Further discussion of how the velocity field affects particles via gradient tensor decomposition and an alternate approach for calculating particle growth rate using the Sherwood number are included in Supplementary Information.

Post-synthesis processing steps of centrifugation and rinsing most likely caused these particles to aggregate into the stable 30 nm platelets seen in AFM. Because the population of particles formed at 8.4 × 105 s−1 was more homogeneous, it readily formed ordered assemblies, which crystallized to form the highly anisotropic particles. More polydisperse populations, formed in poorly mixed conditions at 4.1 × 104 s−1 or in aggregation-dominated conditions at 3.2 × 106 s−1, formed more disordered assemblies, creating polycrystalline particles. These polycrystalline particles then clustered in a more disordered fashion, with lower anisotropy. This behavior is attributed to the increase in surface free energy required to form ordered assemblies, slowing the kinetics of crystallization58,59. A schematic of this process is illustrated in Fig. 6c.

## Methods

### Annular microreactor construction

Three quartz tubes were installed in a tube-in-tube configuration to create two annular flow zones (see Fig. 1a). In section A1, air flow through T1 forced Liquid Phase 1 into a thin film at the inner walls of T2. In A2, the thin film of Liquid 1 from A1 is then contacted with a thin film of Liquid Phase 2. In T3, mixing and reaction occur. The smooth surfaces of the quartz tubes increase flow stability and decrease scaling. They are also amenable to in situ analytical techniques, such as laser scattering, spectroscopy, optical microscopy, and X-ray scattering.

Liquids were delivered to the reactor using a KDS Legato Dual Syringe Pump using disposable plastic 50 or 10 mL Terumo syringes. Compressed dried air was passed through a 200 µm filter (Swagelok) and delivered to the reactor using a Sierra SmartTrak C50L Mass Flow controller (20 L min−1 max, 2% accuracy). For low gas flowrates (0.1 mL min−1), a laboratory rotameter was used. The pressure of the Liquid 2 stream was monitored inline to determine when flow had reached a steady state.

Stainless steel tee connectors with 1/4” and 1/16” diameter compression fittings were purchased from Swagelok. Precision quartz capillary round tubes of the following dimensions: 0.30 mm inner diameter (ID) × 0.4 mm outer diameter (OD) × 100 mm L (T1), 0.50 mm ID × 0.7 mm OD × 100 mm L (T2), and 1 mm ID × 1.2 mm OD × 100 mm L and 300 mm L (T3) were purchased from VitroCom (supplied by ArteGlass Japan). Gas tight connections between stainless steel fittings and quartz tubes were made with graphite and Teflon 1/16” compression ferrules. Also, 0.8 mm ID and 0.5 mm ID ferrules were purchased from Restek, and 1/16” PTFE ferrules were purchased from Swagelok. PTFE (0.8 mm ID) tubing from ChemiKalie was used for delivery of liquid solutions to the reactor.

### Fluorescence microscopy

For high-speed microscopic studies, a mount was constructed using a Formlabs 1+3D printer with high temperature resin and a 1 mm quartz glass slide. Channels and tube connections were sealed with rubber silicone sealant and epoxy adhesive. Gas flowrates from 0.4 to 3 L(STP) min−1 and liquid flowrates from 2 to 20 mL min−1 were evaluated, keeping both inlet liquid streams at the same flowrate.

Confocal fluorescence imaging was performed with a Leica TCS SP5 using a scanning Ar laser at 8000 Hz with ×10 objective magnification. The reactor tube was immersed in glycerol and placed above a 200 µm glass coverslip to reduce the effects of refraction from the tube curvature.

To accurately determine the liquid profile, a dilute fluorescein (Sigma Aldrich) solution was used in both liquid streams. Axial cross-section images were taken over the first 7–8 mm of the reactor at a resolution of 0.57 µm pixel−1 and averaged over 64 frames. Owing to the wavy nature of the liquid, the average height was calculated as the distance from the reactor wall to the point at which the intensity was 1/$$\sqrt 2$$ of the maximum intensity, the root mean square of a sine wave.

To determine mixing dynamics, a dilute fluorescein solution was used in the first annular inlet flow and a blank water stream was used in the second. Video over the first several millimeters of the tube was taken without frame averaging. A median filter with a radius of two pixels was applied to reduce image noise.

To determine macromixing time, a dilute fluorescein solution was used in the first annular inlet flow and a blank water stream was used in the second. The liquid profile was determined as previously described. The average intensity at each tube length was then determined. The mixing length was determined as the point at which the intensity was within a standard deviation of its stable average; this was then divided by the average liquid velocity to determine the effective macromixing time.

### Micromixing characterization

To experimentally quantify the mixing efficiency of the reactor at various flow conditions, the Villermaux–Dushman method40,60 was used. This test characterizes micromixing time with a parallel competing reaction system in which the quasi-instantaneous neutralization of boric acid (Eq. 1) by sulfuric acid competes with the reduction of iodate (Eq. 2) to iodine, which forms a triiodide ion (Eq. 3) that can be measured via ultraviolet (UV) spectrometry. In a system with infinitely fast mixing, boric acid will completely neutralize the acid species before iodine may be formed; in a very slowly mixed system, a significant amount of iodine will evolve. By varying reagent concentrations and volumetric fractions, one may tailor the characteristic iodide reaction time to the expected mixing time, with enough sensitivity to detect changes with different flow conditions.

$${\mathrm{H}}_2{\mathrm{BO}}_3^ - + {\mathrm{H}}^ + \leftrightarrow {\mathrm{H}}_3{\mathrm{BO}}_3$$
(1)
$$5{\mathrm{I}}^ - + {\mathrm{IO}}_3^ - + 6{\mathrm{H}}^ + \leftrightarrow 3{\mathrm{I}}_2 + 3{\mathrm{H}}_2{\mathrm{O}}$$
(2)
$${\mathrm{I}}^ - + {\mathrm{I}}_2 \leftrightarrow {\mathrm{I}}_3^ -$$
(3)

By using the incorporation micromixing model39, the characteristic mixing time tm may be determined from the concentration of triiodide. By comparing the measured segregation index to the model, the characteristic micromixing time may be determined with good accuracy in continuous and batch reactors. It should be noted that, because the known kinetics of this reaction are debated, the characteristic reaction times calculated using this method should only be used to rank mixers characterized using the same protocol61,62,63. In this case, the pH of the mixture was carefully controlled to 7.4 so as to ensure the complete dissociation of sulfuric acid, which has been previously noted as a point of concern64. Comparing both the mixing time measured by fluorescence microscopy and mixing time from Villermaux/Dushman test reaction allows for a more universal estimation of the mixing time.

A semi-empirical model of annular flow in microtubes35 was used to predict the pressure drop, liquid film thickness, shear, and velocity after the transient mixing region. According to the Re number, the flowrates used are in the laminar regime. With the predicted pressure drop and velocity, the characteristic mixing time could then be estimated using the relationship between the rate of energy dissipation and micromixing time for high shear flows where vortex engulfment is the dominant mixing mechanism. This relationship is given in Eq. 436, which applies for low Schmidt (Sc) numbers «4000 (for water at ambient conditions $${\mathrm{Sc}} = \frac{\nu }{{\rho D}} = 406$$) where τE is the characteristic engulfment time (s), ν is the kinematic viscosity (m2 s−1), ρ is the density (kg m−3), D is the diffusion coefficient (m2 s−1), in this calculation the self-diffusion coefficient of water65, and ε is the rate of energy dissipation (m2 s−3).

$$\tau _{\mathrm{E}} = 17\sqrt {\frac{v}{\varepsilon }}$$
(4)

Potassium iodide, potassium iodate, boric acid, sodium hydroxide, and sulfuric acid were purchased from HCS Scientific. A buffered solution (solution B) of 0.25 M H3BO4, 0.125 M NaOH, 0.005 M KI, and 0.001 M KIO3 and an acidic solution (solution A) of 0.05625 M H2SO4 were prepared in DI water at approximately 21 °C.

Solutions A and B were delivered to the reactor at equal flowrates with compressed dried air to provide total liquid flowrates (QL) from 0.4 to 20 mL min−1 and total gas flowrates (QG) from 0.1 to 3 L min−1. The length of the mixing zone A2 was kept at 50 mm. Product was collected in a vial and then subjected to UV-visible (Uv-Vis) light absorption analysis with an Agilent Cary 60 at 353 nm, diluting if necessary to get values between 0.1 and 0.3. UV-Vis absorption was used to determine the concentration of triiodide (I3), which was then used to calculate the concentration of I2.The product pH was approximately 7.65, which is in the optimal zone for this reaction to determine mixing efficiency66. Between each experiment, the reactor was flushed with water to avoid cross-contamination.

### LDH synthesis

Hydrotalcite was synthesized via the co-precipitation method, in which Mg and Al salts are combined with NaOH and Na2CO321. At high supersaturation, precipitation is rapid, ensuring complete conversion within the short timescale used27.

Magnesium nitrate hexahydrate, aluminum nitrate nonahydrate, sodium hydroxide, and sodium bicarbonate were purchased from HCS Scientific. A metal ion solution (solution A) of Mg2+ and Al3+ and a basic solution (solution B) of NaOH and Na2CO3 were prepared in DI water at approximately 21 °C. The molar ratio of Mg2+: Al3+ was fixed at 3:1. A mixture with a supersaturation of 3 × 104 corresponds to a solution A concentration of 0.112 M Mg2+ and 0.0372 M Al3+, with a solution B concentration of 0.291 M NaOH and 0.0186 M Na2CO323. Synthesized product suspensions had pH values of approximately 10.65, in which the formation of hydrotalcite is favorable.

While gas flowed through T1, solutions A and B were pumped through T2 and T3, respectively, at equal flowrates. The total liquid flowrate QL was varied from 0.4 to 20 mL min−1 and the gas flowrate QG from 0.1 to 3 L min−1. For TEM, AFM, and XRD analysis, the collected suspension was centrifuged immediately after synthesis in a Hanil 514 R Centrifuge at 6000 RPM for 3 min. The collected solids were rinsed three times with DI water to purge unreacted ions. An aliquot was then diluted in ethanol 100× for TEM, XRD, and AFM sampling.

### Transmission electron microscopy

The ethanol suspensions were ultrasonicated in an Elma Ultrasonic S100h bath for 1 min to disperse large agglomerates, dropped onto Formvar or holey carbon 200 mesh copper TEM grids or SiO-coated copper TEM grids purchased from InLab Supplies, and dried at room temperature. It was found that SiO was a better substrate for stabilizing and dispersing LDH particles during HRTEM imaging. Sonication was limited to 1 min because extended sonication up to 30 min resulted in morphological changes that were observed in AFM, seen in Supplementary Figure 5. High-resolution images were taken with a JEOL 2100F field-emission TEM (FETEM) at 200 kV. Samples were imaged for brief time periods under low current density to prevent radiation-induced restructuring. Representative images of radiation-induced damage can be seen in Supplementary Figure 6.

### Liquid transmission electron microscopy

All liquid TEM work was started within an hour after synthesis. Post-synthesized sample was diluted 10× in DI water approximately after synthesis and imaged using a Protochips Poseidon holder fitted with an E-chips liquid cell. The cell consists of two silicon chips, coated with a 50-nm-thick silicon nitride membrane, with windows of approximately 500 × 50 µm2. The spacer between the two chips, composed of 150-nm-thick SU-8, was deposited in a modified flow configuration.

A Tecnai F20 FETEM was used at 200 kV in bright-field mode at an electron dose under 500 e nm−2 s−1. Higher electron doses were used to induce bubble formation. Video was taken at 25 fps at 4k × 4k resolution using a Gatan OneView camera. Sample was imaged under static conditions as well as in flow, under 200 µL h−1 flowrates of DI water. Particle sizes and positions were measured in imageJ.

### Atomic force microscopy

The ethanol suspensions were sonicated for 1 min, dropped onto 1 mm quartz slides, and dried at room temperature. Height and phase maps were taken with a Bruker Dimension ICON AFM with a silicon SPM probe (MikroMasch NSC15) while tapping in air. Maps were flattened using a first- or second-order fit for each line scan and analyzed using Bruker Nanoscope Analysis.

The heights and diameters of at least 100 individual particles were measured for each sample to construct a reasonable particle size distribution. Particle diameter was approximated by treating the area of the particle as the area of a circle. Height was taken to be the difference of the maximum measured height and the surrounding height.

### X-ray diffraction

The ethanol suspensions were deposited onto a non-reflective silicon wafer (100) and dried at ambient temperature. The powder XRD pattern was collected with a Brucker D8 Advance Powder Diffractometer using Cu Kα radiation (λ = 1.5418 Å) at 40 kV from a 2θ of 3–70° with a scanning resolution of 0.02° s−1. Crystallite size of the 110 peak was determined using the Scherrer equation67.

### Peclet number calculation

For a Brownian particle, Pe is given by Eq. 5, where ηm is the medium’s viscosity (Pas), RH is the hydrodynamic radius (m), kB is Boltzmann’s constant (m2 kg s−2 K−1), T is temperature (K), and $$D_{{\mathrm{B}}_0}$$ is the Brownian self-diffusion coefficient (m2 s−1).

$${\mathrm{Pe}} = \frac{{6{\mathrm{\pi }}\eta _{\mathrm{m}}R_{\mathrm{H}}^3\dot \gamma }}{{k_{\mathrm{B}}T}} = \frac{{R_{\mathrm{H}}^2\dot \gamma }}{{D_{{\mathrm{B}}0}}}$$
(5)

The hydrodynamic radius of a disc RH, disc is given by Eqs. 6 and 7, where Hdisc is the disk thickness, Rdisc is the disc radius, and α is the aspect ratio (which is not to be confused with the definition of aspect ratio used in AFM particle analysis)68.

$$\alpha = \frac{{H_{{\mathrm{disc}}}}}{{2R_{{\mathrm{disc}}}}}$$
(6)
$$R_{{\mathrm{H}},{\mathrm{disc}}} = \frac{{3R_{{\mathrm{disc}}}}}{2}\left[ {\sqrt {1 + \alpha ^2} + \frac{1}{\alpha }\ln \left( {\alpha + \sqrt {1 + \alpha ^2} } \right) - \alpha } \right]^{ - 1}$$
(7)

For discs 2 and 4 nm in radius with a thickness of 0.7 nm, Pe equals 0.07 and 0.46, respectively, at a shear rate of 3.16 × 106 s−1. The rotational Peclet number is given by Eq. 8, where Dr is the rotational diffusivity about the cylindrical axis69.

$${\mathrm{Pe}}_{\mathrm{r}} = \frac{{\dot \gamma }}{{D_r}} = \dot \gamma \left( {\frac{{3k_{\mathrm{B}}T}}{{32\eta _{\mathrm{m}}R_{{\mathrm{disc}}}^3}}} \right)^{ - 1}$$
(8)

For disks 2 and 4 nm in radius, Per equals 0.06 and 0.47, respectively, at a shear rate of 3.16 × 106 s−1.

### Characteristic growth time calculation

The surface growth reaction is seen in Eq. 9, in which the addition of a cation A to particle Bi results in a larger particle, Bi+1, where i represents the size. At high supersaturations, this is assumed to be irreversible.

$$A + B_i \to B_{i + 1}$$
(9)

The rate of growth rg, i+1 is the given by Eq. 10, where $$K_i^{\mathrm{g}}$$ is the rate coefficient for a particle of size i (mol-1 m3 s1), [A] is the concentration of cations (mol m−3), and [Bi] is the concentration of Bi particles (mol m−3). An alternate calculation of the growth rate is given in Supplementary Discussion - Calculation of Growth Rate using the Sherwood number.

$$r_{{\mathrm{g}},i + 1} = K_i^{\mathrm{g}}\left[ A \right][B_i]$$
(10)

The characteristic growth timescale of a particle of the critical nucleus size n (Rdisc = 2 nm, Hdisc = 0.7 nm) is then given as τg,n, seen in Eq. 11, where [A]0 and [Bn]0 are the initial concentrations of cations and particles of the critical nucleus size, Bn. The initial concentration of cations is $$\left[ A \right]_0 = 0.75 \cdot 10^{ - 4}\,{\mathrm{mol}}\,{\mathrm{m}}^{ - 3}$$ and the initial concentration of nuclei is $$\left[ {B_n} \right]_0 = 2.0 \cdot 10^{ - 7}{\mathrm{mol}}\,{\mathrm{m}}^{ - 3}$$, which is approximated from the average particle number concentration.

$$\tau _{{\mathrm{g}},n} = \left( {K_n^{\mathrm{g}}\sqrt {\left[ A \right]_0\left[ {B_n} \right]_0} } \right)^{ - 1}$$
(11)

At the micro-scale, the characteristic growth time is assumed to be diffusion-limited at high supersaturation. The rate coefficient is then determined by the rate of collision of the two species. This is given in Eq. 12, where RH, A and RH,Bn are the hydrodynamic radii of monomer A and nucleus Bn (m), DA and DBn are their respective diffusivities (m2 s−1), and NA is Avogadro’s constant (mol−1).

$$K_n^{\mathrm{g}} = 4\pi \left( {R_{{\mathrm{H}},A} + R_{{\mathrm{H}},B_n}} \right)\left( {D_A + D_{B_n}} \right)N_{\mathrm{A}}$$
(12)

We assume that $$R_{{\mathrm{H}},A} + R_{{\mathrm{H}},B_n} \cong R_{{\mathrm{H}},B_n} = 1.8 \cdot 10^{ - 9}{\mathrm{m}}$$ and $$D_A = 1.020 \cdot 10^{ - 9}{\mathrm{m}}^2{\mathrm{s}}^{ - 1}$$70. DBn is calculated from the Einstein relation in Eq. 13.

$$D_{B_n} = \frac{{k_{\mathrm{B}}T}}{{6{\mathrm{\pi }}\eta _{\mathrm{m}}R_{{\mathrm{H}},B_n}}} = 1.364\cdot 10^{ - 10}{\mathrm{m}}^2{\mathrm{s}}^{ - 1}$$
(13)

Inserting the calculated diffusion coefficient into Eq. 12 yields $$K_n^{\mathrm{g}} = 1.55 \cdot 10^7{\mathrm{m}}^3{\mathrm{s}}^{ - 1}{\mathrm{mol}}^{ - 1}$$. Inserting $$K_n^{\mathrm{g}}$$ and the known concentrations into Eq. 11 yields $$\tau _{\mathrm{g}} = 16.6 \cdot 10^{ - 3}{\mathrm{s}}$$.

### Characteristic aggregation time calculation

For two Brownian particles, the binary collision rate coefficient $$K_{ij}^{\mathrm{A}}$$ is given by Eq. 14, where Wij, the stability coefficient for two particles of the same size, is equal to 1 at carbonate concentrations above 1 mmol53, and RH,i and RH,j are the hydrodynamic diameters of the two particles of sizes i and j, respectively.

$$K_{ij}^{\mathrm{A}} = \frac{{2k_{\mathrm{B}}T}}{{3\eta _{\mathrm{m}}W_{ij}}}\left( {R_{{\mathrm{H}},i} + R_{{\mathrm{H}},j}} \right)\left( {\frac{1}{{R_{{\mathrm{H}},i}}} + \frac{1}{{R_{{\mathrm{H}},j}}}} \right)$$
(14)

The characteristic aggregation time for two particles of size i in the absence of hydrodynamic forces is expressed by Eq. 15. For a binary collision between Brownian discs with a hydrodynamic radius of 2 nm, $$\tau _{nn}^{\mathrm{A}}$$ = 0.68 s.

$$\tau _{ii}^{\mathrm{A}} = \left( {K_{ii}^{\mathrm{A}}\left[ {B_n} \right]_0N_{\mathrm{A}}} \right)^{ - 1} = \frac{{3\eta _{\mathrm{m}}W_{11}}}{{8k_{\mathrm{B}}T\left[ {B_n} \right]_0N_{\mathrm{A}}}}$$
(15)

The scaling of the characteristic aggregation time for a binary encounter between two particles of the same size i with a fixed potential ($$\tau _{ii}^{{\mathrm{A}},{\mathrm{Pe}}}$$) is given by Eq. 1649.

$$\tau _{ii}^{{\mathrm{A}},{\mathrm{Pe}}}\sim \left( {\frac{{\eta _{\mathrm{m}}\dot \gamma R_{{\mathrm{H}},i}^3}}{{k_{\mathrm{B}}T}}} \right)^{ - \frac{1}{2}}{\mathrm{e}}^{\frac{{ - 2\eta _{\mathrm{m}}\dot \gamma R_{\mathrm{H}}^3}}{{k_{\mathrm{B}}T}}} = \left( {\frac{{{\mathrm{Pe}}}}{{6{\mathrm{\pi }}}}} \right)^{ - \frac{1}{2}}{\mathrm{e}}^{ - {\mathrm{Pe}}/3{\mathrm{\pi }}}$$
(16)

For a binary collision between discs of size n, we assume that as Pe→0 the characteristic aggregation time is given by Eq. 15, such that $$\tau _{nn}^{{\mathrm{A}},{\mathrm{Pe}}}\left( {\dot \gamma = 4.1 \cdot 10^4{\mathrm{s}}^{ - 1},{\mathrm{Pe}} = 9.5 \cdot 10^{ - 4}} \right) = 0.68\,{\mathrm{s}}$$. Therefore, $$\tau _{nn}^{{\mathrm{A}},{\mathrm{Pe}}}\left( {\dot \gamma = 8.4 \cdot 10^5\,{\mathrm{s}}^{ - 1},{\mathrm{Pe}} = 1.9 \cdot 10^{ - 2}} \right) = 0.15\,{\mathrm{s}}$$ and $$\tau _{nn}^{{\mathrm{A}},{\mathrm{Pe}}}\left( {\dot \gamma = 3.2 \cdot 10^6\,{\mathrm{s}}^{ - 1},{\mathrm{Pe}} = 7.4 \cdot 10^{ - 2}} \right) = 77\,{\mathrm{ms}}$$.

## Data availability

Source data for plots and other findings are available from the corresponding author on request.

## References

1. 1.

Deng, D. H. et al. Catalysis with two-dimensional materials and their heterostructures. Nat. Nanotechnol. 11, 218–230 (2016).

2. 2.

Pomerantseva, E. & Gogotsi, Y. Two-dimensional heterostructures for energy storage. Nat. Energy 2, 17089 (2017).

3. 3.

Xue, Y. H. et al. Opening two-dimensional materials for energy conversion and storage: a concept. Adv. Energy Mat. 7, 1602684 (2017).

4. 4.

Tan, C. L. et al. Recent advances in ultrathin two-dimensional nanomaterials. Chem. Rev. 117, 6225–6331 (2017).

5. 5.

De Yoreo, J. J. et al. Crystallization by particle attachment in synthetic, biogenic, and geologic environments. Science 349, aaa6760 (2015).

6. 6.

Baldyga, J. Mixing and fluid dynamics effects in particle precipitation processes. KONA Powder Part. J. 33, 127–149 (2016).

7. 7.

Wu, K. J., Bohan, G. M. D. & Torrente-Murciano, L. Synthesis of narrow sized silver nanoparticles in the absence of capping ligands in helical microreactors. React. Chem. Eng. 2, 116–128 (2017).

8. 8.

Mura, F. & Zaccone, A. Effects of shear flow on phase nucleation and crystallization. Phys. Rev. E 93, 042803 (2016).

9. 9.

Richard, D. & Speck, T. The role of shear in crystallization kinetics: from suppression to enhancement. Sci. Rep. 5, 14610 (2015).

10. 10.

Bihannic, I. et al. Orientational order of colloidal disk-shaped particles under shear-flow conditions: a rheological-small-angleX-ray scattering study. J. Phys. Chem. B 114, 16347–16355 (2010).

11. 11.

Kim, J., Peretti, J., Lahlil, K., Boilot, J. P. & Gacoin, T. Optically anisotropic thin films by shear-oriented assembly of colloidal nanorods. Adv. Mater. 25, 3295–3300 (2013).

12. 12.

Zaccone, A. et al. Breakup of dense colloidal aggregates under hydrodynamic stresses. Phys. Rev. E Stat. Nonlin. Soft Matter Phys. 79, 061401 (2009).

13. 13.

Conchuir, B. O., Harshe, Y. M., Lattuada, M. & Zaccone, A. Analytical model of fractal aggregate stability and restructuring in shear flows. Ind. Eng. Chem. Res. 53, 9109–9119 (2014).

14. 14.

Zheng, Y. L. & Chen, Y. H. Preparation of polypropylene/Mg-Al layered double hydroxides nanocomposites through wet pan-milling: formation of a second-staging structure in LDHs intercalates. RSC Adv. 7, 1520–1530 (2017).

15. 15.

Paton, K. R. et al. Scalable production of large quantities of defect-free few-layer graphene by shear exfoliation in liquids. Nat. Mater. 13, 624–630 (2014).

16. 16.

Vermant, J. & Solomon, M. J. Flow-induced structure in colloidal suspensions. J. Phys. Condens. Mat. 17, R187–R216 (2005).

17. 17.

Mountain, R. D., Hatch, H. W. & Shen, V. K. Molecular dynamics simulation of trimer self-assembly under shear. Fluid Phase Equilibr. 440, 87–94 (2017).

18. 18.

Fan, G., Li, F., Evans, D. G. & Duan, X. Catalytic applications of layered double hydroxides: recent advances and perspectives. Chem. Soc. Rev. 43, 7040–7066 (2014).

19. 19.

Rives, V., del Arco, M. & Martin, C. Intercalation of drugs in layered double hydroxides and their controlled release: a review. Appl. Clay Sci. 88-89, 239–269 (2014).

20. 20.

Sahoo, R., Pal, A. & Pal, T. 2D materials for renewable energy storage devices: outlook and challenges. Chem. Commun. 52, 13528–13542 (2016).

21. 21.

Cavani, F., Trifiro, F. & Vaccari, A. Hydrotalcite-type anionic clays: preparation, properties and applications. Catal. Today 11, 173–301 (1991).

22. 22.

Galvao, T. L. P. et al. Control of crystallite and particle size in the synthesis of layered double hydroxides: Macromolecular insights and a complementary modeling tool. J. Colloid Interface Sci. 468, 86–94 (2016).

23. 23.

Sato, T., Fujita, H., Endo, T., Shimada, M. & Tsunashima, A. Synthesis of hydrotalcite-like compounds and their physicochemical properties. React. Solid 5, 219–228 (1988).

24. 24.

Pang, X. J. et al. Growth behavior of water dispersed MgAl layered double hydroxide nanosheets. RSC Adv. 7, 14989–14997 (2017).

25. 25.

Zhang, Y. P., Li, H. P., Du, N., Zhang, R. J. & Hou, W. G. Large-scale aqueous synthesis of layered double hydroxide single-layer nanosheets. Colloid Surf. A 501, 49–54 (2016).

26. 26.

Hu, G., Wang, N., O’Hare, D. & Davis, J. J. Synthesis of magnesium aluminium layered double hydroxides in reverse microemulsions. J. Mater. Chem. 17, 2257–2266 (2007).

27. 27.

Abello, S. & Perez-Ramirez, J. Tuning nanomaterials’ characteristics by a miniaturized in-line dispersion-precipitation method: application to hydrotalcite synthesis. Adv. Mater. 18, 2436–2439 (2006).

28. 28.

Ren, M. Y., Yang, M., Chen, G. W. & Yuan, Q. High-throughput preparation of monodispersed layered double hydroxides via microreaction technology. J. Flow Chem. 4, 164–167 (2014).

29. 29.

Abello, S., Mitchell, S., Santiago, M., Stoica, G. & Perez-Ramirez, J. Perturbing the properties of layered double hydroxides by continuous coprecipitation with short residence time. J. Mater. Chem. 20, 5878–5887 (2010).

30. 30.

Pang, X. J., Sun, M. Y., Ma, X. M. & Hou, W. G. Synthesis of layered double hydroxide nanosheets by coprecipitation using a T-type microchannel reactor. J. Solid State Chem. 210, 111–115 (2014).

31. 31.

Wang, Q., Tang, S. V. Y., Lester, E. & O’Hare, D. Synthesis of ultrafine layered double hydroxide (LDHs) nanoplates using a continuous-flow hydrothermal reactor. Nanoscale 5, 114–117 (2013).

32. 32.

Patterson, J. P. et al. Observing the growth of metal-organic frameworks by in situ liquid cell transmission electron microscopy. J. Am. Chem. Soc. 137, 7322–7328 (2015).

33. 33.

Park, J. et al. Direct observation of nanoparticle superlattice formation by using liquid cell transmission electron microscopy. ACS Nano 6, 2078–2085 (2012).

34. 34.

Yuk, J. M. et al. High-resolution EM of colloidal nanocrystal growth using graphene liquid cells. Science 336, 61–64 (2012).

35. 35.

Han, Y., Kanno, H., Ahn, Y. J. & Shikazono, N. Measurement of liquid film thickness in micro tube annular flow. Int. J. Multiphas. Flow 73, 264–274 (2015).

36. 36.

Baldyga, J. & Bourne, J. R. Simplification of micromixing calculations. 1. Derivation and application of new model. Chem. Eng. J. 42, 83–92 (1989).

37. 37.

Baldyga, J. & Bourne, J. R. Simplification of micromixing calculations. 2. New applications. Chem. Eng. J. 42, 93–101 (1989).

38. 38.

Baldyga, J. & Jasinska, M. Energetic efficiency of mixing and mass transfer in single phase and two-phase systems. Chem. Process Eng. 38, 79–96 (2017).

39. 39.

Fournier, M. C., Falk, L. & Villermaux, J. A new parallel competing reaction system for assessing micromixing efficiency - determination of micromixing time by a simple mixing model. Chem. Eng. Sci. 51, 5187–5192 (1996).

40. 40.

Fournier, M. C., Falk, L. & Villermaux, J. A new parallel competing reaction system for assessing micromixing efficiency - experimental approach. Chem. Eng. Sci. 51, 5053–5064 (1996).

41. 41.

Towler, G. & Sinnott, R. in Chemical Engineering Design ( Second Edition) Ch. 1 (Butterworth-Heinemann, Oxford; Waltham, MA, 2013).

42. 42.

Towler, G. & Sinnott, R. in Chemical Engineering Design ( Second Edition) Ch. 6 (Butterworth-Heinemann, Oxford; Waltham, MA, 2013).

43. 43.

Maceiczyk, R. M., Lignos, I. G. & deMello, A. J. Online detection and automation methods in microfluidic nanomaterial synthesis. Curr. Opin. Chem. Eng. 8, 29–35 (2015).

44. 44.

Sans, V. et al. Non-equilibrium dynamic control of gold nanoparticle and hyper-branched nanogold assemblies. Chem. Sci. 5, 1153–1157 (2014).

45. 45.

Tathod, A. P. & Gazit, O. M. Fundamental insights into the nucleation and growth of Mg-Al layered double hydroxides nanoparticles at low temperature. Cryst. Growth Des. 16, 6709–6713 (2016).

46. 46.

Grogan, J. M., Schneider, N. M., Ross, F. M. & Bau, H. H. Bubble and pattern formation in liquid induced by an electron beam. Nano Lett. 14, 359–364 (2014).

47. 47.

Lattuada, M. & Morbidelli, M. Effect of repulsive interactions on the rate of doublet formation of colloidal nanoparticles in the presence of convective transport. J. Colloid Interface Sci. 355, 42–53 (2011).

48. 48.

Zaccone, A., Gentili, D., Wu, H. & Morbidelli, M. Shear-induced reaction-limited aggregation kinetics of Brownian particles at arbitrary concentrations. J. Chem. Phys. 132, 134903 (2010).

49. 49.

Zaccone, A., Wu, H., Gentili, D. & Morbidelli, M. Theory of activated-rate processes under shear with application to shear-induced aggregation of colloids. Phys. Rev. E Stat. Nonlin. Soft Matter Phys. 80, 051404 (2009).

50. 50.

Sun, X. & Dey, S. K. Insights into the synthesis of layered double hydroxide (LDH) nanoparticles: Part 2. Formation mechanisms of LDH. J. Colloid Interface Sci. 458, 160–168 (2015).

51. 51.

Jobbagy, M. & Regazzoni, A. E. Complexation at the edges of hydrotalcite: the cases of arsenate and chromate. J. Colloid Interface Sci. 393, 314–318 (2013).

52. 52.

Wang, Y. F. & Gao, H. Z. Compositional and structural control on anion sorption capability of layered double hydroxides (LDHs). J. Colloid Interface Sci. 301, 19–26 (2006).

53. 53.

Pavlovic, M., Huber, R., Adok-Sipiczki, M., Nardin, C. & Szilagyi, I. Ion specific effects on the stability of layered double hydroxide colloids. Soft Matter 12, 4024–4033 (2016).

54. 54.

Sun, X., Neuperger, E. & Dey, S. K. Insights into the synthesis of layered double hydroxide (LDH) nanoparticles: Part 1. Optimization and controlled synthesis of chloride-intercalated LDH. J. Colloid Interface Sci. 459, 264–272 (2015).

55. 55.

Yokoi, T., Tsukada, K., Terasaka, S., Kamitakahara, M. & Matsubara, H. Morphological control of layered double hydroxide through a biomimetic approach using carboxylic and sulfonic acids. J. Asian Ceram. Soc. 3, 230–233 (2015).

56. 56.

Chen, C. P., Yang, M. S., Wang, Q., Buffet, J. C. & O’Hare, D. Synthesis and characterisation of aqueous miscible organic-layered double hydroxides. J. Mater. Chem. A 2, 15102–15110 (2014).

57. 57.

Tokudome, Y. et al. Layered double hydroxide nanoclusters: aqueous, concentrated, stable, and catalytically active colloids toward green chemistry. ACS Nano 10, 5550–5559 (2016).

58. 58.

Auer, S. & Frenkel, D. Suppression of crystal nucleation in polydisperse colloids due to increase of the surface free energy. Nature 413, 711–713 (2001).

59. 59.

Solomon, M. J. Directions for targeted self-assembly of anisotropic colloids from statistical thermodynamics. Curr. Opin. Colloid Interface Sci. 16, 158–167 (2011).

60. 60.

Guichardon, P., Falk, L. & Villermaux, J. Characterisation of micromixing efficiency by the iodide-iodate reaction system. Part II: Kinetic study. Chem. Eng. Sci. 55, 4245–4253 (2000).

61. 61.

Bourne, J. R. Comments on the iodide/iodate method for characterising micromixing. Chem. Eng. J. 140, 638–641 (2008).

62. 62.

Kolbl, A., Desplantes, V., Grundemann, L. & Scholl, S. Kinetic investigation of the Dushman reaction at concentrations relevant to mixing studies in stirred tank reactors. Chem. Eng. Sci. 93, 47–54 (2013).

63. 63.

Kolbl, A. & Schmidt-Lehr, S. The iodide iodate reaction method: the choice of the acid. Chem. Eng. Sci. 65, 1897–1901 (2010).

64. 64.

Guichardon, P., Ibaseta, N. Revision of the Dushman Reaction Kinetics for an Improved Micromixing Characterization Proceedings of the 24th International Symposium on Chemical Reaction Engineering pp. 65–66 (Minneapolis, MN, 2016).

65. 65.

Tanaka, K. Self-diffusion coefficients of water in pure water and in aqueous-solutions of several electrolytes with O-18 and H-2 as tracers. J. Chem. Soc. Farad. Trans. 1 Phys. Chem. Condens. Phases 74, 1879–1881 (1978).

66. 66.

Guichardon, P. & Falk, L. Characterisation of micromixing efficiency by the iodide-iodate reaction system. Part I: experimental procedure. Chem. Eng. Sci. 55, 4233–4243 (2000).

67. 67.

Patterson, A. L. The Scherrer formula for X-ray particle size determination. Phys. Rev. 56, 978–982 (1939).

68. 68.

Mazer, N. A., Benedek, G. B. & Carey, M. C. Quasi-elasticlight-scattering-studies of aqueous biliary lipid systems - mixed micelle formation in bile-salt lecithin solutions. Biochemistry 19, 601–615 (1980).

69. 69.

Mewis, J. & Wagner, N. J. Colloidal Suspension Rheology (Cambridge University Press, Cambridge, 2012).

70. 70.

Lobo, V. M. M., Ribeiro, A. C. F. & Verissimo, L. M. P. Diffusion-coefficients in aqueous-solutions of magnesium-nitrate at 298-K. Ber. Bunsen Phys. Chem. 98, 205–208 (1994).

## Acknowledgements

We thank Dr. Kamran Yunus for his assistance in high-speed microscopic studies and Dr. Giorgio Divitini and Dr. Caterina Ducati for their assistance in liquid TEM studies. This project is funded by the National Research Foundation (NRF), Prime Minister’s Office, Singapore under its Campus for Research Excellence and Technological Enterprise (CREATE) program as a part of the Cambridge Centre for Advanced Research and Education in Singapore Ltd (CARES). Funding for the liquid TEM holder was provided by the Engineering and Physical Sciences Research Council’s Henry Royce Institute (EP/P024947/1).

## Author information

Authors

### Contributions

N.A.J. conceived, designed and performed the experiments, and wrote the manuscript. A.A.L. and H.C.Z. advised and contributed to the manuscript.

### Corresponding author

Correspondence to Alexei A. Lapkin.

## Ethics declarations

### Competing interests

N.A.J. and A.A.L. filed a patent application for the reactor described (Singapore patent app. no. 10201801303T). H.C.Z. declares no competing interests.

Publisher’s note: Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

## Rights and permissions

Reprints and Permissions

Jose, N.A., Zeng, H.C. & Lapkin, A.A. Hydrodynamic assembly of two-dimensional layered double hydroxide nanostructures. Nat Commun 9, 4913 (2018). https://doi.org/10.1038/s41467-018-07395-4

• Accepted:

• Published:

• ### Engineering Layered Double Hydroxide–Based Photocatalysts Toward Artificial Photosynthesis: State‐of‐the‐Art Progress and Prospects

• Sue‐Faye Ng
• , Michelle Yu Ling Lau
•  & Wee‐Jun Ong

Solar RRL (2021)

• ### Recent progress in energy storage and conversion of flexible symmetric transducers

• Chao Lu
•  & Xi Chen

Journal of Materials Chemistry A (2021)

• ### TEM and EELS characterization of Ni–Fe layered double hydroxide decompositions caused by electron beam irradiation

• Christopher Hobbs
• , Clive Downing
•  & Valeria Nicolosi

npj 2D Materials and Applications (2021)

• ### A Hierarchical-Structured Impeller with Engineered Pd Nanoparticles Catalyzing Suzuki Coupling Reactions for High-Purity Biphenyl

• Xueyan Sun
• , Shaofeng Li
• , Jinzhe Cao
• , Yuchao Wang
• , Wenbo Yang
• , Lijing Zhang
• , Yijin Liu
• , Jieshan Qiu
•  & Shengyang Tao

ACS Applied Materials & Interfaces (2021)

• ### Scalable and precise synthesis of two-dimensional metal organic framework nanosheets in a high shear annular microreactor

• Nicholas A. Jose
• , Hua Chun Zeng
•  & Alexei A. Lapkin

Chemical Engineering Journal (2020)