Dispersion (chemistry)

This article is about dispersion in chemistry. For other forms of dispersion, see Dispersion (disambiguation).

A dispersion is a system in which particles are dispersed in a continuous phase of a different composition (or state). See also emulsion. A dispersion is classified in a number of different ways, including how large the particles are in relation to the particles of the continuous phase, whether or not precipitation occurs, and the presence of Brownian motion.

IUPAC definition

Material comprising more than one phase where at least one
of the phases consists of finely divided phase domains, often in the
colloidal size range, dispersed throughout a continuous phase.[1]

Note 1: Modification of definition in ref.[2]

There are three main types of dispersions:

Types of dispersions

Dissolved or dispersed phase Continuous medium Solution: Homogeneous mixture: Dissolved phase < 1 nanometer Colloid: Dispersed phase between 1 nanometer and 1 micrometer Coarse dispersion (Suspension): Heterogeneous mixture: Dispersed phase > 1 micrometer
Gas Gas Gas mixture: air (oxygen and other gases in nitrogen) None None none of them
Liquid Gas None Aerosol: fog, mist, vapor, hair sprays Aerosol
Solid Gas None Solid aerosol: smoke, cloud, air particulates Solid aerosol: dust
Gas Liquid Solution: oxygen in water Foam: whipped cream, shaving cream Foam
Liquid Liquid Solution: alcoholic beverages Emulsion: miniemulsion, microemulsion Emulsion: milk, mayonnaise, hand cream
Solid Liquid Solution: sugar in water Sol: pigmented ink, blood Suspension: mud (soil, clay or silt particles are suspended in water), chalk powder suspended in water
Gas Solid Solution: hydrogen in metals Solid foam: aerogel, styrofoam, pumice Foam: dry sponge
Liquid Solid Solution: amalgam (mercury in gold), hexane in paraffin wax Gel: agar, gelatin, silicagel, opal Wet sponge
Solid Solid Solution: alloys, plasticizers in plastics Solid sol: cranberry glass Gravel, granite

Structure and Properties of Dispersions

It is still common belief that dispersions do not display any structure; i.e., the particles (or in case of emulsions: droplets) dispersed in the liquid or solid matrix (the "dispersion medium") are assumed to be statistically distributed. Therefore, for dispersions, usually percolation theory is assumed to appropriately describe their properties.

However, percolation theory can be applied only if the system it should describe is in or close to thermodynamic equilibrium. There are only very few studies about the structure of dispersions (emulsions), although they are plentiful in type and in use all over the world in innumerable applications (see below).

In the following, only such dispersions with a dispersed phase diameter of less than 1 µm will be discussed. To understand the formation and properties of such dispersions (incl emulsions), it must be considered that the dispersed phase exhibits a "surface", which is covered ("wet") by a different "surface" that, hence, are forming an interface (chemistry). Both surfaces have to be created (which requires a huge amount of energy), and the interfacial tension (difference of surface tension) is not compensating the energy input, if at all.

A review article describes various attempts to describe dispersions/emulsions. Dispersion is a process by which (in the case of solids' becoming dispersed in a liquid) agglomerated particles are separated from each other and a new interface, between an inner surface of the liquid dispersion medium and the surface of the particles to be dispersed, is generated. Dispersion is a much more complicated (and less-understood) process than most people believe.

The above-cited review article also displays experimental evidence to support the fact that dispersions have a structure very much different from any kind of statistical distribution (which would be characteristics for a system in thermodynamic equilibrium), but in contrast very much showing structures similar to self-organisation, which can be described by non-equilibrium thermodynamics. This is the reason why some liquid dispersions turn to become gels or even solid at a concentration of a dispersed phase above a certain critical concentration (which is dependent on particle size and interfacial tension). Also, the sudden appearance of conductivity in a system of a dispersed conductive phase in an insulating matrix has been explained. The above-cited review article also introduces into some first complete non-equilibrium thermodynamics theory of dispersions (http://www2.organic-nanometal.de/Research/wisslit/nonequ2.html).

References

  1. ↑ "Terminology of polymers and polymerization processes in dispersed systems (IUPAC Recommendations 2011)" (PDF). Pure and Applied Chemistry. 83 (12): 2229–2259. 2011. doi:10.1351/PAC-REC-10-06-03.
  2. ↑ Richard G. Jones; Edward S. Wilks; W. Val Metanomski; Jaroslav Kahovec; Michael Hess; Robert Stepto; Tatsuki Kitayama, eds. (2009). Compendium of Polymer Terminology and Nomenclature (IUPAC Recommendations 2008) (2nd ed.). RSC Publ. p. 464. ISBN 978-0-85404-491-7.
  1. ^ Handbook of Nanostructured Materials and Nanotechnology; Nalwa, H.S., Ed.; Academic Press: New York, NY, USA, 2000; Volume 5, pp. 501-575
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