Cuprate

This oxide cuprate has been the subject of extensive research due to its ability to conduct electricity without resistance at relatively high temperatures.

[2] KCuO2 was discovered first in 1952 by V. K. Wahl and W. Klemm, they synthesized this compound by heating copper(II) oxide and potassium superoxide in an atmosphere of oxygen.

[3] It can also be synthesized by heating potassium superoxide and copper powder:[4] KCuO2 reacts with the air fairly slowly.

[4] Sodium cuprate(III) NaCuO2 can be produced by using hypochlorites or hypobromites to oxidize copper hydroxide under alkaline and low temperature conditions.

[5] Sodium cuprate(III) is reddish-brown, but turns black gradually as it decomposes to copper(II) oxide.

[citation needed] Copper forms many anionic coordination complexes with negatively charged ligands such as cyanide, hydroxide, and halides, as well as alkyls and aryls.

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

[12][13][14][15] Sodium tetrahydroxycuprate(II) (Na2[Cu(OH)4]) is an example of a homoleptic (all ligands being the same) hydroxide complex.

Organic cuprates often have the idealized formulas [CuR2]− and [CuR3]2−, both of which contain copper in an oxidation state of +1, where R is an alkyl or aryl.