If isolation of the Nickle oxide hydroxide is feesible then I love the idea of using it. I think the method using the H₂O₂ im attempting is far removed from this process and I will try to figure out and explore the mechanism later on. I tryed to run the experiment again as clean as I could and the results where the same.

This time I added abit of H₂O₂ and EtOH to a test tube and waited to see if the peroxide had any effect over an hour on the EtOH which it did not. As soon as they mixed it formed a cloudy solution which I was not expecting at all. Any theorys as to why EtOH and H₂O₂ form this cloudy mixture?

The undoubtly acidic Ni+Cu chloride solution was dripped via pippett into the solution and right away fine bubbles began being formed. When heated they increased in pace and fineness forming what looked like smoke almost in the liquid. I capped it off with my finger and allowed it to build pressure and attempted to light it. Nothing happened so its not H₂ evolving. The splint test or O₂ also proved negative so the only assumption I could make was that these bubbles are just acetaldahyde forming and exiting the solution.

Im going to run some more test notibly with Ethylene glycol to see if I can perform a reductive amination to EthyleneDiamine from the formed dialdahyde. I also want to test its ability to form acetone from Isopropyl alcohol to test its capabilitys with secondary alcohols.

Since am pretty sure we are discussing different mechanics here when I get all my ducks in a row I will start a new thread on the use of this VERY over the counter oxidizing agent for Primary alcohols. I have a feelin that like the NaOCl process the Oxygen from the H2O2 is being mediated to the substrate thru the Nickle salt in a simular fashion. It appears to work so well so far I can't wait to get yields on it.

[EDIT]

Well this experiment will be delayed a bit since I have just figured out how to purify the nickle from coins and remove all the added copper. Once I recover my pure nicklechloride I will be on th path of reproducng your experimnts and trying some of the H2O2 ones using pure Nickle chlorides as the starting material.

One of the Nickle peroxide patents is what gave me the idea on how to seperate the Ni from the Cu in my mixture using Ammonia hydroxide to precipitate the NiO. Figured Cu will stay as a complex and it did just that so now I have "clean" NiO to work with. The patent I seen also stated using persulfates to form the NiO₂ and to top it all off I see alot of room for this to become an electrochemical oxidation method.

Kind of along the same line of thought. A sulfate salt in the anode cell along with H₂SO₄ can generate persulfate and NiO₂ in the pot was my line of thinking. Some Ni salts should be there as well for good measure I feel.

ah shit, some of the systems i mentioned are not suitable for your substrate because i was searching for aldehyde -> carboxylic acid.

in particular the oxone/DMF method will not work on alcohols.  i also found an iron catalyst + O2 method, and a NaOH/KOH caustic fusion at 185C method but neither were documented to work on alcohols.

here is a reference for some methods which should work (many were mentioned already by Chemchem thx).

http://www.organic-chemistry.org/synthesis/C2O/ketones/oxidationsalcohols.shtm

i see in the other phenylethanol thread you say to drip the phenylethanol in acetone into refluxing h2so4/dichromate.  is an excess of dichromate or h2so4 used?  what is the length of the reaction?  what is the esther you mention having to hydrolyze?

is this esther formed only when oxidizing an alcohol, not when oxidizing an aldehyde?  (or am i confused about what esther you encounter.)