A detergent is a surfactant or a mixture of surfactants with cleansing properties when in dilute solutions.[1] There are a large variety of detergents, but the most commonly found are alkylbenzene sulfonates: a family of soap-like compounds that are more soluble in hard water, because the polar sulfonate (of detergents) is less likely than the polar carboxylate (of soap) to bind to calcium and other ions found in hard water.

Detergents

EtymologyEdit

The word detergent is derived from the Latin adjective detergens, from the verb detergere, meaning to wipe or polish off. In domestic contexts, the term detergent by itself refers specifically to synthetic cleaning compounds such as laundry detergent or dish detergent, as opposed to hand soap or other types of cleaning agents distinct from soap, even though soap is also a detergent in the true sense.[2]

Structure and propertiesEdit

Detergents are a group of compounds with an amphiphilic structure, where each molecule has a hydrophilic (polar) head and a long hydrophobic (non-polar) tail. The hydrophobic portion of these molecules may be straight- or branched-chain hydrocarbons, or it may have a steroid structure. The hydrophilic portion is more varied, they may be ionic or non-ionic, and can range from a simple or a relatively elaborate structure.[3] Detergents are surfactants since they can decrease the surface tension of water. Their dual nature facilitates the mixture of hydrophobic compounds (like oil and grease) with water. Because air is not hydrophilic, detergents are also foaming agents to varying degrees.

Detergent molecules aggregate to form micelles, which makes them soluble in water. The hydrophobic group of the detergent is the main driving force of micelle formation, its aggregation forms the hydrophobic core of the micelles. The micelle can remove grease, protein or soiling particles. The concentration at which micelles start to form is the critical micelle concentration (CMC), and the temperature at which the micelles further aggregate to separate the solution into two phases is the cloud point when the solution becomes cloudy and detergency is optimal.[3]

Detergency is the ability to remove unwanted substances termed 'soils' from a substrate (e.g clothing).[4] Detergents work better in an alkaline pH. The properties of detergents are dependent on the molecular structure of the monomer. The ability to foam may be determined by the head group, for example anionic surfactants are high-foaming, while nonionic surfactants may be non-foaming or low-foaming.[5]

Chemical classifications of detergentsEdit

Detergents are classified into four broad groupings, depending on the electrical charge of the surfactants.[6]

Anionic detergentsEdit

Typical anionic detergents are alkylbenzene sulfonates. The alkylbenzene portion of these anions is lipophilic and the sulfonate is hydrophilic. Two varieties have been popularized, those with branched alkyl groups and those with linear alkyl groups. The former were largely phased out in economically advanced societies because they are poorly biodegradable.[7]

Anionic detergents are the most common form of detergents, and an estimated 6 billion kilograms of anionic detergents are produced annually for the domestic markets.

Bile acids, such as deoxycholic acid (DOC), are anionic detergents produced by the liver to aid in digestion and absorption of fats and oils.

 
Three kinds of anionic detergents: a branched sodium dodecylbenzenesulfonate, linear sodium dodecylbenzenesulfonate, and a soap.

Cationic detergentsEdit

Cationic detergents are similar to anionic ones, but quaternary ammonium replaces the hydrophilic anionic sulfonate group. The ammonium sulfate center is positively charged.[7] Cationic surfactants generally have poor detergency.

Non-ionic detergentsEdit

Non-ionic detergents are characterized by their uncharged, hydrophilic headgroups. Typical non-ionic detergents are based on polyoxyethylene or a glycoside. Common examples of the former include Tween, Triton, and the Brij series. These materials are also known as ethoxylates or PEGylates and their metabolites, nonylphenol. Glycosides have a sugar as their uncharged hydrophilic headgroup. Examples include octyl thioglucoside and maltosides. HEGA and MEGA series detergents are similar, possessing a sugar alcohol as headgroup.

Amphoteric detergentsEdit

Amphoteric or zwitterionic detergents have zwitterions within a particular pH range, and possess a net zero charge arising from the presence of equal numbers of +1 and −1 charged chemical groups. Examples include CHAPS.

HistoryEdit

Soap is known to be have been used as a surfactant for washing clothes since the Sumerian time in 2,500 B.C.[8] In ancient Egypt, soda was used as a wash additive. In the 19th century, synthetic surfactants began to be created, for example from olive oil.[9] Sodium silicate (water glass) was used in soap-making in the United States in the 1860s,[10] and in 1876, Henkel sold a sodium silicate-based product that can be used with soap and marketed as a "universal detergent" (Universalwaschmittel) in Germany. Soda was then mixed with sodium silicate to produce Germany's first brand name detergent Bleichsoda.[11] In 1907 Henkel also added a bleaching agent sodium perborate to launch the first 'self-acting' laundry detergent Persil to eliminate the laborious rubbing of laundry by hand.[12]

During the First World War, there was a shortage of oils and fats needed to make soap. In order find alternatives for soap, synthetic detergents were made in Germany by chemists using raw material derived from coal tar.[13][14][9] These early products, however, did not provide sufficient detergency. In 1928, effective detergent was made through the sulfation of fatty alcohol, but large-scale production was not feasible until low-cost fatty alcohols become available in the early 1930s.[15] The synthetic detergent created was more effective and less likely to form scum than soap in hard water, and can also eliminate acid and alkaline reactions and decompose dirt. Commercial detergent products with fatty alcohol sulphates began to be sold, initially in 1932 in Germany by Henkel.[15] In the United States, detergents were sold in 1933 by Procter & Gamble (Dreft) primarily in areas with hard water.[14] However, sales in the US grew slowly until the introduction of 'built' detergents with the addition of effective phosphate builder developed in the early 1940s.[14] The builder improves the performance of the surfactants by softening the water through the chelation of calcium and magnesium ions, helping to maintain an alkaline pH, as well as dispersing and keeping the soiling particles in solution.[16] The development of the petrochemical industry after the Second World War also yielded material for the production of a range of synthetic surfactants, and alkylbenzene sulfonates became the most important detergent surfactants used.[17] By the 1950s, laundry detergents had become widespread, and largely replaced soap for cleaning clothes in developed countries.[15]

Over the years, many types of detergents have been developed for a variety of purposes, for example, low-sudsing detergents for use in front-loading washing machines, heavy-duty detergents effective in removing grease and dirt, all-purpose detergents and specialty detergents.[14][18] They become incorporated in various products outside of laundry use, for example in dishwasher detergents, shampoo, toothpaste, industrial cleaners, and in lubricants and fuels to reduce or prevent the formation of sludge or deposits.[19] The formulation of detergent products may include bleach, fragrances, dyes and other additives. The use of phosphates in detergent, however, led to concerns over nutrient pollution and demand for changes to the formulation of the detergents,[20] and concerns over surfactants like branched alkylbenzene sulfonate (tetrapropylenebenzene sulfonate) that lingers in the environment led to the use of surfactants that are more biodegradable of such as linear alkylbenzene sulfonate.[15][17] Developments over the years have included the use of enzymes, substitutes for phosphates such as zeolite A and NTA, TAED as bleach activator, sugar-based surfactants which are biodegradable and milder to skin, and other green friendly products, as well as changes to the form of delivery such as tablets, gels and pods.[21][22]

Major applications of detergentsEdit

Household cleaningEdit

One of the largest applications of detergents is for household and shop cleaning including dish washing and washing laundry. These detergents are commonly available as powders or concentrated solutions, and the formulations of these detergents are often complex mixtures of a variety of chemicals aside from surfactants, reflecting the diverse demands of the application and the highly competitive consumer market. These detergents may contain the following components:[21]

  • foam regulators
  • builders
  • bleach
  • bleach activators
  • enzymes
  • dyes
  • fragrances
  • other additives

Fuel additivesEdit

Both carburetors and fuel injector components of internal combustion engines benefit from detergents in the fuels to prevent fouling. Concentrations are about 300 ppm. Typical detergents are long-chain amines and amides such as polyisobuteneamine and polyisobuteneamide/succinimide.[23]

Biological reagentEdit

Reagent grade detergents are employed for the isolation and purification of integral membrane proteins found in biological cells.[24] Solubilization of cell membrane bilayers requires a detergent that can enter the inner membrane monolayer.[25] Advancements in the purity and sophistication of detergents have facilitated structural and biophysical characterization of important membrane proteins such as ion channels also the disrupt membrane by binding lipopolysaccharide,[26] transporters, signaling receptors, and photosystem II.[27]

See alsoEdit

ReferencesEdit

  1. ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version:  (2006–) "detergent". doi:10.1351/goldbook.D01643
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  4. ^ Arno Cahn, ed. (2003). 5th World Conference on Detergents. p. 154. ISBN 9781893997400 – via Google Books.
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  11. ^ Ward, James; Löhr (2020). The Perfection of the Paper Clip. Atria Books. p. 190. ISBN 9781476799872.
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  14. ^ a b c d David O. Whitten; Bessie Emrick Whitten (1 January 1997). Handbook of American Business History: Extractives, manufacturing, and services. Greenwood Publishing Group. pp. 221–222. ISBN 978-0-313-25199-3 – via Google Books.
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  18. ^ Paul Sosis, Uri Zoller, ed. (2008). Handbook of Detergents, Part F. p. 497. ISBN 9781420014655.
  19. ^ Uri Zoller, ed. (2008). Handbook of Detergents, Part E: Applications. Taylor & Francis. p. 331. ISBN 9781574447576.
  20. ^ David O. Whitten; Bessie Emrick Whitten (1999). Handbook of Detergents, Part A. Taylor & Francis. p. 3. ISBN 9781439833322 – via Google Books.
  21. ^ a b Middelhauve, Birgit (2003). Arno Cahn (ed.). 5th World Conference on Detergents. pp. 64–67. ISBN 9781893997400.
  22. ^ Long, Heather. "Laundry Detergent History". Love to Know.
  23. ^ Werner Dabelstein, Arno Reglitzky, Andrea Schütze, Klaus Reders "Automotive Fuels" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheimdoi:10.1002/14356007.a16_719.pub2
  24. ^ Koley D, Bard AJ (2010). "Triton X-100 concentration effects on membrane permeability of a single HeLa cell by scanning electrochemical microscopy (SECM)". Proceedings of the National Academy of Sciences of the United States of America. 107 (39): 16783–7. Bibcode:2010PNAS..10716783K. doi:10.1073/pnas.1011614107. PMC 2947864. PMID 20837548.
  25. ^ Lichtenberg D, Ahyayauch H, Goñi FM (2013). "The mechanism of detergent solubilization of lipid bilayers". Biophysical Journal. 105 (2): 289–299. Bibcode:2013BpJ...105..289L. doi:10.1016/j.bpj.2013.06.007. PMC 3714928. PMID 23870250.
  26. ^ Doyle, DA; Morais Cabral, J; Pfuetzner, RA; Kuo, A; Gulbis, JM; Cohen, SL; Chait, BT; MacKinnon, R (1998). "The structure of the potassium channel: molecular basis of K+conduction and selectivity". Science. 280 (5360): 69–77. Bibcode:1998Sci...280...69D. doi:10.1126/science.280.5360.69. PMID 9525859.
  27. ^ Umena, Yasufumi; Kawakami, Keisuke; Shen, Jian-Ren; Kamiya, Nobuo (2011). "Crystal structure of oxygen-evolving photosystem II at a resolution of 1.9 A" (PDF). Nature. 473 (7345): 55–60. Bibcode:2011Natur.473...55U. doi:10.1038/nature09913. PMID 21499260. S2CID 205224374.

External linksEdit