symboom - 4-1-2012 at 10:02
so if silver peroxide exists
http://www.youtube.com/watch?v=1_a81M9p2so
>>could copper peroxide be produces this way?
and yes copper can be in a higher oxidation state
potassium bis-orthoperiodato dihydroxo cuprate(III)
Zinc peroxide can be prepared by reacting ZnO or zinc acetate with hydrogen peroxide. has anyone tried this
and the zinc peroxide what are its properties i should percipitate right.
the reaction of zinc acetate and hydrogen peroxide
forming acetyl peroxide hydrate "peracetic acid" reacting with the zinc ion to form zinc peroxide. this is what i think happens
>>has anyone done this experiment?
Adas - 4-1-2012 at 10:42
This seems very unlikely to me, but I don't say it's impossible. Why don't give it a try?
AndersHoveland - 4-1-2012 at 22:45
Some metal oxides that are referred to as "peroxide" are not actually peroxides, but rather contain the metal atom in a higher oxidation state. In the
example of silver "peroxide", there is not any oxygen-oxygen bond. Rather, half the silver atoms are in a +3 oxidation state.
Copper can form insoluble peroxides, but only if there is not an excess of ammonia or ammonium salts present. Copper can also form +3 oxidation states
in aqueous solution under certain conditions, but only in the form of a complex.
Nickel "peroxide", NiO2, also apparently exists. It can react with 2-aminopyrazine to form 1,2,3-triazine. I suspect it is actually nickel in the +4
oxidation state.
Persulfates are a powerful oxidizing regents that can oxidize many soluble metal ions to insoluble higher oxides.
The chemistry of metal peroxides is very interesting and surprisingly complex, but unfortunately I am feeling tired now...
[Edited on 5-1-2012 by AndersHoveland]
symboom - 5-1-2012 at 11:28
oh i see your right
It can be prepared by the slow addition of a silver(I) salt to a persulfate solution e.g. AgNO3 to a Na2S2O8 solution.[1] It adopts an unusual
structure, being a mixed-valence compound.[2]
http://en.wikipedia.org/wiki/Silver%28I,III%29_oxide
hmm i wander about the zinc peroxide then if only some form it
[Edited on 5-1-2012 by symboom]
AndersHoveland - 5-1-2012 at 12:39
Zinc peroxide appears to be a real peroxide. Typically, real peroxides are formed using hydrogen peroxide, while higher oxidation states
(pseudo-"peroxides") are formed using persulfate.
Confusingly, barium peroxide was formerly (and more misleadingly) referred to as "barium dioxide".
With a molecular compositions of Ag2O2 and NiO2, you can see why this compounds were initially mistaken for peroxides by early researchers.
You may be wondering about metals in higher oxidation states. Both AgF3 and NiF4 have been prepared, but involve very obscure regents, and are
difficult to prepare in more than very small quantities. Both these compounds can not be directly prepared by reaction of the metal with
fluorine. Silver trifluoride, for example, is apparently a slightly stronger oxidizer than elemental fluorine. http://pubs.acs.org/doi/abs/10.1021/ja00011a021
[Edited on 5-1-2012 by AndersHoveland]
AJKOER - 7-1-2012 at 09:11
Zinc peroxide can be prepared by reacting Zinc sulfate and ammonia solution with 30% H2O2 at 80 to 95 C. Described as not hygroscopic or soluble in
organic solvents.
http://books.google.com/books?id=iTKsAobEo9MC&pg=PA367&a...
Also, per its MSDS, ZnO2 is highly reactive with moisture and decomposes in water (forms H2O2).
http://www.sciencelab.com/msds.php?msdsId=9925490