Talk:Copper(II) oxide

Is the melting point correct? I thougth it was 1026 dergrees celsius. —Preceding unsigned comment added by 130.238.56.104 (talk) 13:35, 19 May 2009 (UTC)

Personally not sure. Although I have seen a source that claims the point to actually be higher at 1446°C! ^[1] DeadFire999 (talk) 13:28, 14 May 2015 (UTC)

I have a question about the equilibrium condition that exists between copper II hydroxide and copper II oxide. Here is the reaction: Cu(OH)₂ + heat ←→ CuO + H₂O When heat is added, it drives the equilibrium to the right, forming more copper II oxide. When it is exposed to excessive moisture, it absorbs water to form copper II hydroxide again. But why does copper II hydroxide turn into copper II oxide when it is moist? I think that that would contradict Le Chatalier's principle. Just a question. --Cheminterest (talk) 20:22, 16 March 2010 (UTC)

You can think about it like this. When heated Cu(OH) dries out to CuO, although due to its reactivity to moisture continues back to Cu(OH) when left in the presence of moisture. Remember though the collision theory can effect outcomes of either reaction. (I know this question was old, but maybe it will help others in the future?!) DeadFire999 (talk) 13:23, 14 May 2015 (UTC)

Is copper(ii) oxide protective to the copper from further damage? Qwertyxp2000 (talk) 05:59, 19 August 2014 (UTC)

Yes, Qwerty2000, the oxidized layer will act to protect the layers of copper under the oxide layer. You can see the process with the Statue of Liberty. ^[1] DeadFire999 (talk) 18:49, 19 May 2015 (UTC)

What in the world is the basis for this claim? Copper(II)oxide thermite is called Cadweld. It has been used for decades with no more danger of explosion than iron bearing thermite mixtures. I have shot many charges of Cadweld and have some pictures that clearly are not explosions. Please reevaluate the source material on this "explosive". — Preceding unsigned comment added by 2602:301:7705:75E0:B91F:2C05:D00E:545 (talk) 10:15, 27 December 2015 (UTC)

I deleted the sentence describing the use of CuO in Li batteries. 1) There was no reference provided. 2) CuO is not a typical cathode material for any Li-based battery. 3) The sentence seemed to imply Li metal was used as the anode, which is definitely wrong. — Preceding unsigned comment added by Chris Barile (talk • contribs) 04:57, 11 February 2016 (UTC)

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Paramelaconite is a natural Cu(I) Cu(II) oxide - it is not equal to Cu(II) oxide. Only tenorite fits to CuO.Eudialytos (talk) 18:28, 21 October 2017 (UTC)

Removed. --Vsmith (talk) 18:48, 21 October 2017 (UTC)

Hello, currently the article states:

   >The work function of bulk CuO is 5.3eV[4]

   >Copper(II) oxide is a p-type semiconductor, with a narrow band gap of 1.2 eV.

These seemingly contradictory statements can be both true if the second sentence is referring to some kind of special form of CuO (e.g. a thin film?). Since the second sentence is unsourced, I suggest removing it unless a source backing up this claim is found, and the sentence amended to reflect the particular type of CuO in question.

64.106.125.231 (talk) 07:07, 23 October 2019 (UTC)

I personally have observed azure blue solutions from the rapid addition of Cu salts or freshly precipitated Cu(OH)2 to conc. alkali, but no color at all is produced when dry CuO is added. Partially decomposed Cu(OH)2 separates into a cuprate(II) solution and CuO. There is a line describing the reaction of CuO with alkali. It seems doubtful but I do not know the specifics of what causes the decomposition of [Cu(OH)₄]^2- so I have not removed it. Altreon (talk) 14:13, 23 April 2026 (UTC)