Cuprate

From Wikipedia, the free encyclopedia

Template:Short description Script error: No such module "For".

Template:DMCA Template:DMCA

Cuprates are a class of compounds that contain copper (Cu) atom(s) in an anion. The term 'cuprate' itself originates from 'cuprum', the Latin word for copper. Cuprates appear mainly in three contexts: anionic organocopper species; inorganic, anionic coordination complexes; and complex oxides.[citation needed]

Organic cuprates typically have a Page Module:Chem2/styles.css has no content.[CuR2]− formula, corresponding to a copper(I) oxidation state, where at least one of the R groups can be any organic group. These compounds are frequently used in organic synthesis as weak nucleophiles that preferentially attack π bonds.[citation needed] An example of an organic cuprate is dimethylcuprate(I) anion Page Module:Chem2/styles.css has no content.[Cu(CH3)2]−.

Inorganic cuprate complexes have a wide variety of formulas. An inorganic cuprate example is the tetrachloridocuprate(II) or tetrachlorocuprate(II) (Page Module:Chem2/styles.css has no content.[CuCl4]2−) anion, a copper(II) atom coordinated to four chloride ions.

Cuprate oxide salts are layered materials with general formula Page Module:Chem2/styles.css has no content.XYCumOn, and some are non-stoichiometric. Many of these compounds are known for their superconducting properties.[citation needed]

Oxide cuprates

File:Potassium cuperate.png
Potassium cuprate

Many stable or metastable alkali metal cuprates(III) are known, all salts of the polyanion Page Module:Chem2/styles.css has no content.[CuO−2]n. They are strong oxidants, oxidizing water.[1] They are typically produced through extremely large oxygen activities. Alkali metals larger than sodium produce dark-blue salts,[2][3] but sodium cuprate(III) is red-brown.[1]

One of the simplest oxide-based cuprates is potassium cuprate(III) Page Module:Chem2/styles.css has no content.KCuO2.[2] Even so, Page Module:Chem2/styles.css has no content.KCuO2 is a non-stoichiometric compound, so the more exact formula is Page Module:Chem2/styles.css has no content.KCuOx and x is very close to 2. This causes the formation of defects in the crystal structure, and this leads to the tendency of this compound to be reduced.[3]

One of the most studied inorganic cuprates is Page Module:Chem2/styles.css has no content.YBa2Cu3O7, also known as YBCO. This oxide cuprate has been the subject of extensive research due to its ability to conduct electricity without resistance at relatively high temperatures. It is the parent of a family of cuprate superconductors.[citation needed]

Coordination complexes

Copper forms many anionic coordination complexes with negatively charged ligands such as cyanide, hydroxide, and halides, as well as alkyls and aryls (see § Organic cuprates).

Copper(I)

Cuprates containing copper(I) tend to be colorless, reflecting their d10 configuration. Structures range from linear 2-coordinate, trigonal planar, and tetrahedral molecular geometry. Examples include linear Page Module:Chem2/styles.css has no content.[CuCl2]− and trigonal planar Page Module:Chem2/styles.css has no content.[CuCl3]2−.[4] Cyanide gives analogous complexes but also the trianionic tetracyanocuprate(I), Page Module:Chem2/styles.css has no content.[Cu(CN)4]3−.[5] Dicyanocuprate(I), Page Module:Chem2/styles.css has no content.[Cu(CN)2]−, exists in both molecular or polymeric motifs, depending on the countercation.[6]

Copper(II)

File:CCs2CuF6.svg
Caesium salt of hexafluorocuprate(IV)

Cuprates containing copper(II) include trichlorocuprate(II), Page Module:Chem2/styles.css has no content.[CuCl3]−, which is dimeric, and square-planar tetrachlorocuprate(II), Page Module:Chem2/styles.css has no content.[CuCl4]2−, and pentachlorocuprate(II), Page Module:Chem2/styles.css has no content.[CuCl5]3−.[7][8] 3-Coordinate chlorocuprate(II) complexes are rare.[9]

Tetrachlorocuprate(II) complexes tend to adopt flattened tetrahedral geometry with orange colors.[10][11][12][13]

Sodium tetrahydroxycuprate(II) (Page Module:Chem2/styles.css has no content.Na2[Cu(OH)4]) is an example of a homoleptic (all ligands being the same) hydroxide complex.[14]

Page Module:Chem2/styles.css has no content.Cu(OH)2 + 2 NaOH → Na2[Cu(OH)4]

Copper(III) and copper(IV)

Hexafluorocuprate(III) Page Module:Chem2/styles.css has no content.[CuF6]3− and hexafluorocuprate(IV) Page Module:Chem2/styles.css has no content.[CuF6]2− are rare examples of copper(III) and copper(IV) complexes. They are strong oxidizing agents.

Organic cuprates

File:Lithium-diphenylcuprate-etherate-dimer-from-xtal-2D-skeletal.png
Structure of lithium diphenylcuprate(I) etherate, Page Module:Chem2/styles.css has no content.2Ph2Cu]−Li+·2OEt2.[15]

Script error: No such module "Labelled list hatnote". Cuprates have a role in organic synthesis. They are invariably Cu(I), although Cu(II) or even Cu(III) intermediates are invoked in some chemical reactions. Organic cuprates often have the idealized formulas Page Module:Chem2/styles.css has no content.[CuR2]− and Page Module:Chem2/styles.css has no content.[CuR3]2−, both of which contain copper in an oxidation state of +1, where R is an alkyl or aryl. These reagents find use as nucleophilic alkylating reagents.[16]

See also

References

Page Template:Reflist/styles.css has no content.

  1. ^ a b Page Module:Citation/CS1/styles.css has no content.Magee, J. S.; Wood, R. H. (1965). "Studies of Sodium Cuprate(III) Stability". Canadian Journal of Chemistry. 43 (5): 1234–1237. doi:10.1139/v65-164.
  2. ^ a b Page Module:Citation/CS1/styles.css has no content.G. Brauer, ed. (1963). "Potassium Cuprate (III)". Handbook of Preparative Inorganic Chemistry. Vol. 2 (2nd ed.). NY: Academic Press. p. 1015.
  3. ^ a b Page Module:Citation/CS1/styles.css has no content.Costa, Giorgio A.; Kaiser, Elena (1995). "Structural and thermal properties of the alkaline cuprate KCuO2". Thermochimica Acta. 269–270: 591–598. doi:10.1016/0040-6031(95)02575-8. Retrieved January 20, 2023.
  4. ^ Page Module:Citation/CS1/styles.css has no content.Stricker, Marion; Linder, Thomas; Oelkers, Benjamin; Sundermeyer, Jörg (2010). "Cu(I)/(II) based catalytic ionic liquids, their metallo-laminate solid state structures and catalytic activities in oxidative methanol carbonylation". Green Chemistry. 12 (9): 1589. doi:10.1039/c003948a.
  5. ^ Page Module:Citation/CS1/styles.css has no content.Kroeker, Scott; Wasylishen, Roderick E. (1999). "A multinuclear magnetic resonance study of crystalline tripotassium tetracyanocuprate". Canadian Journal of Chemistry. 77 (11): 1962–1972. doi:10.1139/v99-181.
  6. ^ Page Module:Citation/CS1/styles.css has no content.Bowmaker, Graham A.; Hartl, Hans; Urban, Victoria (2000). "Crystal Structures and Vibrational Spectroscopy of [NBu4][Cu(CN)X] (X = Br, I) and [NBu4][Cu3(CN)4]·CH3CN". Inorganic Chemistry. 39 (20): 4548–4554. doi:10.1021/ic000399s.
  7. ^ Page Module:Citation/CS1/styles.css has no content.Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
  8. ^ Page Module:Citation/CS1/styles.css has no content.Willett, Roger D.; Butcher, Robert E.; Landee, Christopher P.; Twamley, Brendan (2006). "Two Halide Exchange in Copper(II) Halide Dimers: (4,4Template:Prime-Bipyridinium)Cu2Cl6−x BRX". Polyhedron. 25 (10): 2093–2100. doi:10.1016/j.poly.2006.01.005.
  9. ^ Page Module:Citation/CS1/styles.css has no content.Hasselgren, Catrin; Jagner, Susan; Dance, Ian (2002). "Three-Coordinate [CuIIX3]− (X = Cl, Br), Trapped in a Molecular Crystal". Chemistry – A European Journal. 8 (6): 1269–1278. doi:10.1002/1521-3765(20020315)8:6<1269::AID-CHEM1269>3.0.CO;2-9. PMID 11921210.
  10. ^ Page Module:Citation/CS1/styles.css has no content.Mahoui, A.; Lapasset, J.; Moret, J.; Saint Grégoire, P. (1996). "Tetraethylammonium Tetramethylammonium Tetrachlorocuprate(II), [(C2H5)4N][(CH3)4N][CuCl4]". Acta Crystallographica Section C. 52 (11): 2674–2676. doi:10.1107/S0108270196009031.
  11. ^ Page Module:Citation/CS1/styles.css has no content.Guillermo Mínguez Espallargas; Lee Brammer; Jacco van de Streek; Kenneth Shankland; Alastair J. Florence; Harry Adams (2006). "Reversible Extrusion and Uptake of HCl Molecules by Crystalline Solids Involving Coordination Bond Cleavage and Formation". J. Am. Chem. Soc. 128 (30): 9584–9585. doi:10.1021/ja0625733. PMID 16866484.
  12. ^ Page Module:Citation/CS1/styles.css has no content.Kelley, A.; Nalla, S.; Bond, M. R. (2015). "The square-planar to flattened-tetrahedral CuX42− (X = Cl, Br) structural phase transition in 1,2,6-trimethylpyridinium salts". Acta Crystallogr. B. 71 (Pt 1): 48–60. doi:10.1107/S205252061402664X. PMID 25643715.
  13. ^ Page Module:Citation/CS1/styles.css has no content.Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic Chemistry. Academic Press. pp. 1252–1264. ISBN 0-12-352651-5.
  14. ^ Page Module:Citation/CS1/styles.css has no content.Brauer, G., ed. (1963). "Sodium Tetrahydroxocuprate(II)". Handbook of Preparative Inorganic Chemistry. Vol. 1 (2nd ed.). New York, NY: Academic Press. p. 1015.
  15. ^ Page Module:Citation/CS1/styles.css has no content.Lorenzen, Nis Peter; Weiss, Erwin (1990). "Synthesis and Structure of a Dimeric Lithium Diphenylcuprate:[{Li(OEt2)}(CuPh2)]2". Angewandte Chemie International Edition in English. 29 (3): 300. doi:10.1002/anie.199003001.
  16. ^ Page Module:Citation/CS1/styles.css has no content.Louis S. Hegedus (1999). Transition metals in the synthesis of complex organic molecules. University Science Books. pp. 61–65. ISBN 1-891389-04-1.

Lua error in package.lua at line 80: module 'Module:Navbox/configuration' not found.

Retrieved from "https://cosmopedia.co/index.php?title=Cuprate&oldid=624966"