Ostwald ripening

 ( Physical Chemistry ) 

Ostwald ripening is a phenomenon observed in and liquid sols that involves the change of an inhomogeneous structure over time, in that small crystals or sol particles first dissolve and then redeposit onto larger crystals or sol particles.

Dissolution of small crystals or sol particles and the redeposition of the dissolved species on the surfaces of larger crystals or sol particles was first described by Wilhelm Ostwald in 1896.Ostwald, W. (1896). Lehrbuch der Allgemeinen Chemie, vol. 2, part 1. Leipzig, Germany. For systems, Ostwald ripening is also found in water-in-oil , while flocculation is found in oil-in-water emulsions.

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Mechanism This thermodynamics-driven spontaneous process occurs because larger particles are more energetically favored than smaller particles.

Lorenz Ratke (2026). 9783540425632, Springer. . ISBN 9783540425632

This stems from the fact that molecules on the surface of a particle are energetically less stable than the ones in the interior.

Consider a cubic crystal of atoms: all the atoms inside are bonded to 6 neighbours and are quite stable, but atoms on the surface are only bonded to 5 neighbors or fewer, which makes these surface atoms less stable. Large particles are more energetically favorable since, continuing with this example, more atoms are bonded to 6 neighbors and fewer atoms are at the unfavorable surface. As the system tries to lower its overall energy, molecules on the surface of a small particle (energetically unfavorable, with only 3 or 4 or 5 bonded neighbors) will tend to detach from the particle and diffuse into the solution.

Kelvin equation describes the relationship between the radius of curvature and the chemical potential between the surface and the inner volume:

$\backslash Delta\; \backslash mu\; =\; \backslash frac\; \{2\; \backslash sigma\; \backslash nu\_\backslash mathrm\{at\}\}\; \{r\}$

where $\backslash mu$ corresponds to the chemical potential, $\backslash sigma$ to the surface tension, $\backslash nu\_\backslash mathrm\{at\}$ to the molar volume and $r$ to the radius of the particle. The chemical potential of an ideal solution can also be expressed as a function of the solute's concentration if liquid and solid phases are in equilibrium.

$\backslash mu\; =\; k\_\backslash mathrm\{B\}T\backslash log(C\_\backslash mathrm\{eq\})$

where $k\_\backslash mathrm\{B\}$ corresponds to the Boltzmann constant, $T$ to the temperature and $C\_\backslash mathrm\{eq\}$ to the solute concentration in a solution in which the solid and the liquid phase are in equilibrium.

Combining both expressions the following equation is obtained:

$k\_\backslash mathrm\{B\}\; T\; \backslash log\backslash left(\backslash frac\; \{C\_\backslash mathrm\{eq\}\}\; \{C\_\{\backslash infty\}\}\; \backslash right)\; =\; \backslash frac\; \{2\; \backslash sigma\; \backslash nu\_\backslash mathrm\{at\}\}\; \{r\}\; \backslash rightarrow\; C\_\backslash mathrm\{eq\}(r)\; =\; C\_\backslash mathrm\{eq\}(\backslash infty)\; \backslash mathrm\{e\}^\{\backslash frac\; \{2\; \backslash sigma\; \backslash nu\_\backslash mathrm\{at\}\}\; \{r\; k\_\backslash mathrm\{B\}\; T\}\}$

Thus, the equilibrium concentration, $C\_\{eq\}$, is lower around bigger particles than it is around smaller particles.

$C\_\backslash mathrm\{eq\}(r)\; >\; C\_\backslash mathrm\{eq\}\; (R)$

where $r$ and $R$ are the particles radius, and . Inferring from Fick's first law of diffusion, the particles will move from big concentrations, corresponding to areas surrounding small particles, to small concentrations, corresponding to areas surrounding large nanoparticles. Thus, the small particles will tend to shrink while the big particles will grow. As a result, the average size of the nanoparticles in the solution will grow, and the dispersion of sizes will decrease. Therefore, if a solution is left for a long time, in the extreme case of $t\; \backslash rightarrow\; \backslash infty$, its particles would evolve until they would finally form a single huge spherical particle to minimize the total surface area.

The history of research progress in quantitatively modeling Ostwald ripening is long, with many derivations. In 1958, Lifshitz and Slyozov performed a mathematical investigation of Ostwald ripening in the case where diffusion of material is the slowest process. They began by stating how a single particle grows in a solution. This equation describes where the boundary is between small, shrinking particles and large, growing particles. They finally conclude that the average radius of the particles ⟨R⟩, grows as follows:

$\backslash langle\; R\; \backslash rangle\; ^3\; -\; \backslash langle\; R\; \backslash rangle\; \_0\; ^3\; =\; \backslash frac\; \{8\; \backslash gamma\; c\_\{\backslash infty\}v^2D\}\; \{9R\_g\; T\}\; t$

where

average radius of all the particles

particle surface tension or surface energy

solubility of the particle material

molar volume of the particle material

mass diffusivity of the particle material

gas constant

absolute temperature and

time.

Note that the quantity is different from , and that the statement that ⟨R⟩ goes as relies on being zero; but because nucleation is a separate process from growth, this places outside the bounds of validity of the equation. In contexts where the actual value of is irrelevant, an approach that respects the meanings of all terms is to take the time derivative of the equation to eliminate and . Another such approach is to change the to with the initial time having a positive value.

Also contained in the Lifshitz and Slyozov derivation is an equation for the size distribution function of particles. For convenience, the radius of particles is divided by the average radius to form a new variable, ρ = .

Three years after that Lifshitz and Slyozov published their findings (in Russian, 1958), Carl Wagner performed his own mathematical investigation of Ostwald ripening, examining both systems where diffusion was slow and also where attachment and detachment at the particle surface was slow. Although his calculations and approach were different, Wagner came to the same conclusions as Lifshitz and Slyozov for slow-diffusion systems. This duplicate derivation went unnoticed for years because the two scientific papers were published on opposite sides of the Iron Curtain in 1961. It was not until 1975 that Kahlweit addressed the fact that the theories were identical and combined them into the Lifshitz-Slyozov-Wagner or LSW theory of Ostwald ripening. Many experiments and simulations have shown LSW theory to be robust and accurate. Even some systems that undergo spinodal decomposition have been shown to quantitatively obey LSW theory after initial stages of growth.

Wagner derived that when attachment and detachment of molecules is slower than diffusion, then the growth rate becomes

$\backslash langle\; R\; \backslash rangle\; ^2\; =\; \backslash frac\; \{64\; \backslash gamma\; c\_\{\backslash infty\}\; v^2\; k\_s\}\; \{81\; R\_g\; T\}\; t$

where is the reaction rate constant of attachment with units of length per time. Since the average radius is usually something that can be measured in experiments, it is fairly easy to tell if a system is obeying the slow-diffusion equation or the slow-attachment equation. If the experimental data obeys neither equation, then it is likely that another mechanism is taking place and Ostwald ripening is not occurring.

Although LSW theory and Ostwald ripening were intended for solids ripening in a fluid, Ostwald ripening is also observed in liquid-liquid systems, for example, in an oil-in-water emulsion polymerization. In this case, Ostwald ripening causes the diffusion of (i.e. individual molecules or atoms) from smaller droplets to larger droplets due to greater solubility of the single monomer molecules in the larger monomer droplets. The rate of this diffusion process is linked to the solubility of the monomer in the continuous (water) phase of the emulsion. This can lead to the destabilization of emulsions (for example, by creaming and sedimentation).

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Controlled Ostwald Ripening Inhibition of sulfathiazole crystal growth by polyvinylpyrrolidone. The polymer forms a noncondensed netlike film over the sulfathiazole crystal, allowing the crystal to grow out only through the openings of the net. The growth is thus controlled by the pore size of the polymer network at the crystal surface. The smaller the pore size, the higher is the supersaturation of the solution required for the crystals to grow.

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Specific examples One example of Ostwald ripening is the re-crystallization of water within ice cream which gives old ice cream a gritty, crunchy texture. Larger ice crystals grow at the expense of smaller ones within the ice cream, creating a coarser texture.

Chris Clark (2026). 9780854046294, Royal Society of Chemistry. . ISBN 9780854046294

Another gastronomical example is the ouzo effect, where the droplets in the cloudy microemulsion grow by Ostwald ripening.

In geology, it is the textural coarsening, aging or growth of phenocrysts and crystals in solid rock which is below the solidus temperature. It is often ascribed as a process in the formation of orthoclase , as an alternative to the physical processes governing crystal growth from nucleation and growth rate Thermochemistry limitations.

In aqueous solution chemistry and precipitates ageing, the term refers to the growth of larger crystals from those of smaller size which have a higher solubility than the larger ones. In the process, many small crystals formed initially ( nuclei) slowly disappear, except for a few that grow larger, at the expense of the small crystals ( crystal growth). The smaller crystals act as fuel for the growth of bigger crystals. Limiting Ostwald ripening is fundamental in modern technology for the solution synthesis of . Ostwald ripening is also the key process in the digestion and aging of precipitates, an important step in gravimetric analysis. The digested precipitate is generally purer, and easier to wash and filter.

Ostwald ripening can also occur in emulsion systems, with molecules diffusing from small droplets to large ones through the continuous phase. When a miniemulsion is desired, an extremely hydrophobic compound is added to stop this process from taking place.

Diffusional growth of larger drops in liquid water in the atmosphere at the expense of smaller drops is also characterized as Ostwald ripening.

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See also

• Aggregation
• Chemical crystallography before X-rays
• Coalescence (chemistry)
• Coalescence (physics)
• Critical radius
• Nucleation
• Crystal growth
• Disappearing polymorph
• Digestion and ageing of precipitates
• Kirkendall effect
• Rock microstructure
• Ostwald's rule
• Viedma ripening

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Further reading

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External links

• Ostwald Ripening a 3D Kinetic Monte Carlo simulation

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