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| [[Image:Phospholipids aqueous solution structures.svg|thumb|250px|right|Cross-section view of the structures that can be formed by phospholipids in aqueous solutions (Note that, unlike this illustration, micelles are usually formed by single-chain lipids, since it is tough to fit two chains into this shape)]]
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| [[Image:Micelle scheme-en.svg|thumb|250px|right|Scheme of a micelle formed by [[phospholipid]]s in an [[aqueous]] solution]]
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| {{Quote box
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| |title = IUPAC definition
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| |quote = '''Micelle''': Particle of colloidal dimensions that exists in equilibrium with the<br/>molecules or ions in solution from which it is formed.
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| ''Note'': Based on definition in ref.<ref>{{cite book|title=Compendium of Chemical Terminology: IUPAC Recommendations|publisher=Blackwell Science|location=Oxford|isbn=0865426848|edition=2nd|editor=Alan D. MacNaught, Andrew R. Wilkinson}}</ref>
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| <ref>{{cite journal|title=Terminology of polymers and polymerization processes in dispersed systems (IUPAC Recommendations 2011)|journal=[[Pure and Applied Chemistry]]|year=2011|volume=83|issue=12|pages=2229–2259|doi=10.1351/PAC-REC-10-06-03|url=http://pac.iupac.org/publications/pac/pdf/2011/pdf/8312x2229.pdf}}</ref>
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| '''Micelle (polymers)''': Organized auto-assembly formed in a liquid and<br/>composed of amphiphilic ''macromolecules'', in general amphiphilic di-<br/>or tri-block copolymers made of solvophilic and solvophobic blocks. | |
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| ''Note 1'': An amphiphilic behavior can be observed for water and an organic<br/>solvent or between two organic solvents. | |
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| ''Note 2'': Polymeric micelles have a much lower critical micellar concentration<br/>(CMC) than soap or surfactant micelles, but are nevertheless at equilibrium<br/>with isolated macromolecules called unimers. Therefore, micelle formation<br/>and stability are concentration-dependent.<ref>{{cite journal|title=Terminology for biorelated polymers and applications (IUPAC Recommendations 2012)|journal=[[Pure and Applied Chemistry]]|year=2012|volume=84|issue=2|pages=377–410|doi=10.1351/PAC-REC-10-12-04|url=http://pac.iupac.org/publications/pac/pdf/2012/pdf/8402x0377.pdf}}</ref> | |
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| A '''micelle''' (pronounced {{IPA|/maɪˈsɛl/}} or {{IPA|/maɪˈsiːl/}}, plural '''micelles''', '''micella''', or '''micellae''') is an aggregate of [[surfactant]] molecules dispersed in a liquid [[colloid]]. A typical micelle in [[aqueous solution]] forms an aggregate with the [[hydrophilic]] "head" regions in contact with surrounding [[solvent]], sequestering the [[hydrophobic]] single-tail regions in the micelle centre. This phase is caused by the [[Lipid bilayer phase behavior|packing behavior]] of single-tail [[lipids]] in a [[lipid bilayer|bilayer]]. The difficulty filling all the volume of the interior of a bilayer, while accommodating the area per head group forced on the molecule by the hydration of the lipid head group, leads to the formation of the micelle. This type of micelle is known as a normal-phase micelle (oil-in-water micelle). Inverse micelles have the head groups at the centre with the tails extending out (water-in-oil micelle). Micelles are approximately spherical in shape. Other [[Polymorphism (biophysics)|phase]]s, including shapes such as ellipsoids, cylinders, and [[bilayer]]s, are also possible. The shape and size of a micelle are a function of the molecular geometry of its surfactant molecules and solution conditions such as surfactant concentration, [[temperature]], [[pH]], and [[ionic strength]]. The process of forming micelles is known as micellisation and forms part of the [[Phase behaviour]] of many lipids according to their [[polymorphism (biophysics)|polymorphism]].
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| ==History==
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| The ability of a soapy solution to act as a [[detergent]] has been recognized for centuries. However, it is only at the beginning of the twentieth century that the constitution of such solutions was scientifically studied. Pioneering work in this area was carried out by [[James William McBain]] at the [[University of Bristol]]. As early as 1913, he postulated the existence of “colloidal ions” to explain the good electrolytic conductivity of [[sodium palmitate]] solutions.<ref>McBain, J.W., Trans. Faraday Soc. 1913, 9, 99</ref> These highly mobile, spontaneously formed clusters came to be called micelles, a term borrowed from biology and popularized by G.S. Hartley in his classic book ''Paraffin Chain Salts: A Study in Micelle Formation''.<ref>Hartley, G.S., Aqueous Solutions of Paraffin Chain Salts, A Study in Micelle Formation, 1936, Hermann et Cie, Paris</ref>
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| ==Solvation==
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| Individual surfactant molecules that are in the system but are not part of a micelle are called "monomers". Lipid micelles represent a molecular assembly, in which the individual components are thermodynamically in equilibrium with monomers of the same species in the surrounding medium. In water, the hydrophilic "heads" of surfactant molecules are always in contact with the solvent, regardless of whether the surfactants exist as monomers or as part of a micelle. However, the lipophilic "tails" of surfactant molecules have less contact with water when they are part of a micelle—this being the basis for the energetic drive for micelle formation. In a micelle, the hydrophobic tails of several surfactant molecules assemble into an oil-like core, the most stable form of which having no contact with water. By contrast, surfactant monomers are surrounded by water molecules that create a "cage" of molecules connected by [[hydrogen bonds]]. This water cage is similar to a [[clathrate hydrate|clathrate]] and has an [[ice]]-like [[crystal]] structure and can be characterized according to the hydrophobic effect. The extent of lipid solubility is determined by the unfavorable entropy contribution due to the ordering of the water structure according to the hydrophobic effect.
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| Micelles composed of ionic surfactants have an electrostatic attraction to the ions that surround them in solution, the latter known as [[counterion]]s. Although the closest counterions partially mask a charged micelle (by up to 90%), the effects of micelle charge affect the structure of the surrounding solvent at appreciable distances from the micelle. Ionic micelles influence many properties of the mixture, including its electrical conductivity. Adding salts to a colloid containing micelles can decrease the strength of electrostatic interactions and lead to the formation of larger ionic micelles.<ref>N.J. Turro and A. Yekta, J. Am. Chem. Soc.100, 5951 (1978)</ref> This is more accurately seen from the point of view of an effective charge in hydration of the system.
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| ==Energy of formation==
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| {{See also|Thermodynamics of Micellization}}
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| Micelles form only when the concentration of surfactant is greater than the [[critical micelle concentration]] (CMC), and the temperature of the system is greater than the critical micelle temperature, or [[Krafft temperature]]. The formation of micelles can be understood using [[thermodynamics]]: Micelles can form [[spontaneous process|spontaneously]] because of a balance between [[entropy]] and [[enthalpy]]. In water, the [[hydrophobic effect]] is the driving force for micelle formation, despite the fact that assembling surfactant molecules together reduces their entropy. At very low concentrations of the lipid, only monomers are present in true solution. As the concentration of the lipid is increased, a point is reached at which the unfavorable entropy considerations, derived from the hydrophobic end of the molecule, become dominant. At this point, the lipid hydrocarbon chains of a portion of the lipids must be sequestered away from the water. Therefore, the lipid starts to form micelles. In broad terms, above the CMC, the entropic penalty of assembling the surfactant molecules is less than the entropic penalty of caging the surfactant monomers with water molecules. Also important are enthalpic considerations, such as the electrostatic interactions that occur between the charged parts of surfactants.
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| {{anchor|Reverse Micelles}}
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| ==Micelle Packing Parameter==
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| The micelle packing parameter equation is utilized to help "predict molecular self-assembly in surfactant solutions":<ref>R. Nagarajan, Molecular Packing Parameter and Surfactant Self-Assembly: The Neglected Role of the Surfactant Tail</ref>
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| <math> \frac{v_o}{a_e*l_o}</math>
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| where <math>v_o</math> is the surfactant tail volume, <math>l_o</math> is the tail length, and <math>a_e</math> is the equilibrium area per molecule at the aggregate surface.
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| ==Inverse/reverse micelles==
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| In a [[non-polar]] solvent, it is the exposure of the hydrophilic head groups to the surrounding solvent that is energetically unfavourable, giving rise to a water-in-oil system. In this case, the hydrophilic groups are sequestered in the micelle core and the hydrophobic groups extend away from the centre. These inverse micelles are proportionally less likely to form on increasing headgroup charge, since hydrophilic sequestration would create highly unfavorable electrostatic interactions.
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| ==Uses==
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| When surfactants are present above the CMC ([[Critical micelle concentration]]), they can act as [[emulsifier]]s that will allow a compound that is normally insoluble (in the solvent being used) to dissolve. This occurs because the insoluble species can be incorporated into the micelle core, which is itself solubilized in the bulk solvent by virtue of the head groups' favorable interactions with solvent species. The most common example of this phenomenon is [[detergent]]s, which clean poorly soluble lipophilic material (such as oils and waxes) that cannot be removed by water alone. Detergents clean also by lowering the [[surface tension]] of water, making it easier to remove material from a surface. The emulsifying property of surfactants is also the basis for [[emulsion polymerization]].
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| Micelle formation is essential for the absorption of fat-soluble vitamins and complicated lipids within the human body. [[Bile acid|Bile salts]] formed in the liver and secreted by the gall bladder allow micelles of fatty acids to form. This allows the absorption of complicated lipids (e.g., lecithin) and lipid-soluble vitamins (A, D, E, and K) within the micelle by the small intestine.
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| Micelles are used for [[targeted drug delivery]].<ref>{{cite journal|last=Chen|first=Xi|coauthors=He, ZP, etc|title=Core-shell-corona Au-micelle composites with a tunable smart hybrid shell|journal=Langmuir|date=05|year=2008|month=08|volume=24|issue=15|pages=8198-8204|doi=10.1021/la800244g}}</ref>
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| ==See also==
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| *[[Liposome]]
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| *[[Vesicle (biology)]]
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| *[[Lipid bilayer]]
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| *[[Surfactant]]
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| *[[Micellar liquid chromatography]]
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| ==Notes==
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| {{reflist}}
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| ==References==
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| * J. M. Seddon, R. H. Templer. ''Polymorphism of Lipid-Water Systems'', from the Handbook of Biological Physics, Vol. 1, ed. R. Lipowsky, and E. Sackmann. (c) 1995, Elsevier Science B.V. ISBN 0-444-81975-4
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| * S.A. Baeurle, J. Kroener, ''Modeling effective interactions of micellar aggregates of ionic surfactants with the Gauss-Core potential'', J. Math. Chem. 36, 409–421 (2004).
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| * McBain, J.W., Trans. Faraday Soc. 1913, 9, 99.
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| * Hartley, G.S., Aqueous Solutions of Paraffin Chain Salts, A Study in Micelle Formation, 1936, Hermann et Cie, Paris.
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| * Makoto Takeo (1999). ''Disperse Systems'', WILEY-VCH, ISBN 3-527-29458-9
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| [[Category:Supramolecular chemistry]]
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| [[Category:Colloidal chemistry]]
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