Copper +3 oxidation state

[Anders Hoveland]

http://woelen.homesc...uIII/index.html

 

 

Copper(II) salts can be oxidized to Copper(III) complexes, with the help of a hypochlorite or persulfate oxidizer, sodium hydroxide, and sodium periodate.

 

The complex [Cu(H3IO6)2]-2 is oxidized to [Cu(H3IO6)2(OH)2]-3, which has a very deep brown-red color

The composition of these complexes can more simply be thought of as:

 

IO4[-],Cu[+2], IO4[-],(2)OH[-],(2)H2O and

 

IO4[-],Cu[+3],IO4[-],(4)OH[-],(2)H2O

 

 

Actually, Cu(OH)2 is soluble in concentrated solutions of NaOH showing that copper(II) oxide is actually slightly amphoteric.

 

 

 

CsCuCl3, although copper is still in its normal +2 oxidation state, is a bright reddish-orange colored compound

http://woelen.homesc...uCl3/index.html

Edited October 12, 2011 by Anders Hoveland