|WikiProject Chemicals||(Rated Start-class, Mid-importance)|
|WikiProject Occupational Safety and Health|
HEY!!! Everyone smart - this makes no sense and i hate chemistry!!! Delete if this is not funny rip):
- 1 It's Not Easy Being Green
- 2 Wilson's disease
- 3 Use in disposal
- 4 Melting point?
- 5 Copper II oxide - Copper II hydroxide equilibrium
- 6 Protective layer?
- 7 "When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary."
- 8 Deleted battery claim
- 9 External links modified
It's Not Easy Being Green
It is my understanding that copper (II) oxide is green, what with pennies and copper alloys forming a green patina over time. Where was the picture in the description found and why is it black? Note that some Wikipedia pages call copper (II) oxide a green powder. Kyoobur9000 (talk) 16:51, 8 December 2012 (UTC)
The "health effects" section mentions that prolonged exposure to the substance can cause Wilson's disease. When I checked the source , the MSDS described increased copper toxicity in people with Wilson's disease, but did not claim that exposure to copper could cause the disease.
Use in disposal
These equations were under the 'Use in disposal' section with no explanation. If someone can write an explanation, please do so and move these back into the article.--Bfesser (talk) 00:10, 5 February 2008 (UTC)
- C6H5OH + 14CuO → 6CO2 + 3H2O + 14Cu
- C6Cl5OH + 2H2O + 9CuO → 6CO2 + 5HCl + 9Cu
Copper II oxide - Copper II hydroxide equilibrium
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)
"When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary."
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)
Deleted battery claim
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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