GreenJames
Harmless
Posts: 10
Registered: 25-4-2019
Location: United States
Member Is Offline
|
|
Copper(III)
I've been very interested in Copper(III) compounds lately. I already know of the persulfate/periodate method, however I was wondering if there are any
other ways to isolate one of these compounds. These compounds are very interesting to me, and I would like to see more of the chemistry of these
salts.
|
|
|
Bedlasky
International Hazard
Posts: 1219
Registered: 15-4-2019
Location: Period 5, group 6
Member Is Offline
Mood: Volatile
|
|
Hydrated Cu2O3 can be prepared by oxidation of Cu(OH)2 with NaClO or K2S2O8.
|
|
|
josh1037
Harmless
Posts: 3
Registered: 12-11-2019
Member Is Offline
|
|
Copper 3+ compounds are notoriously difficult to work with, given their tendency to degrade. Copper(III) oxide still hasn't been isolated, and that's
one of the most simple copper compounds. These compounds are better in theory and you would have to have an absurdly low temperature to prevent these
compounds from degrading.
|
|
|
12thealchemist
Hazard to Others
Posts: 181
Registered: 1-1-2014
Location: The Isle of Albion
Member Is Offline
Mood: Rare and Earthy
|
|
I've succeeded in making KCuO2 by burning potassium with copper(II) oxide in an oxygen atmosphere, but it was far from pure and degraded
over a period of a few hours due to impurities absorbing atmospheric moisture and accelerating decomposition.
Analysis was optical spectroscopy - a dull blue powder was formed, and it was impossible for it to be any hydrated copper(II) compound due to the
conditions involved. Also, KCuO2 is dark blue.
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
