You would not believe how much of a pain in the arse it is to dissolve such a tiny amount of stuff in a tiny bloody container. This was dissolved in 5ml of diethylether in a 25ml erlenmeyer flask, and stirred. It should have been a gram, but I was in a hurry as there were only 4 balances, and 17 people vying for them, so I was urged to “hurry the hell up”. 0.9870 grams of borneol was weighed out carefully on an analytical balance. I may have used a slight excess of acid due to being distracted. 2 grams of sodium dichromate were dissolved in 8ml distilled water, and slowly ~1.6ml of concentrated sulphuric acid was added. Įxperimental/Cooking (Jesse! We need to cook!):ġ. Spills of such material are a serious hazard. This is a strong oxidizing agent, and also a suspected carcinogen, so it must be In this experiment, we use H 2SO 4/Na 2Cr 2O 7 as our oxidizing agent, to convert Borneol (a secondary alcohol) to Camphor (a ketone). We use an oxidizing agent to perform this. Oxidation occurs when protons (Hydrogen) is stripped away from a compound, often replacing it with oxygen. You can also do things like oxidize an amine to a nitro group (I was never able to confirm this, as back then I did not have a FTIR at my disposal, but I believe it worked, your mileage may vary – some experimental procedures use this route), and the likes. Notably, the conversion of 1* alcohols to aldehydes or acids, and conversion of 2* alcohols to ketones. Oxidation reactions are useful mechanisms for converting one functional group in an organic compound to another. Ended up publishing it on one of the forums and figured it was worth hosting here… I decided to be a bit more “descriptive” to make up for the lack of pictures! I was not going to bother posting this up, as it lacks in pretty pictures, but ah well.
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