verode Posted November 7, 2008 Posted November 7, 2008 I know nobody may oxyder fluorine but MnF4=MnF3+ 1/2 F2 is the only chenical way to get fluorine thanks the SbF5 You don't need fluor always BrF3 and IF5 are a easy way to make fluorine componds fluorine is very dangerous
insane_alien Posted November 8, 2008 Posted November 8, 2008 yes it is possible to do it with an electrode but the OP wants to know if there is a substance that can oxidise it without the need to apply electrical stimulation.
John Cuthber Posted November 8, 2008 Posted November 8, 2008 The OP was in 2005 and may have lost interest by now.
verode Posted November 8, 2008 Posted November 8, 2008 and in not a single one of those is fluorine oxidised. yes the MnF4 becames MnF3 + elemental fluorine it's not the same Cl+5 with fluorine as with oxygen Cl2O5 for example The fluorine only make single bonds and the oxygen makes pi bonds the reactivity of fluorines are very bigger than the the same oxidation state of oxygen examples BrF5 and bromates PtO3 or PtF6
insane_alien Posted November 8, 2008 Posted November 8, 2008 and you still haven't gave an example of oxidised fluorine.
verode Posted November 8, 2008 Posted November 8, 2008 yes the MnF4 becames MnF3 + elemental fluorine it's not the same Cl+5 with fluorine as with oxygen Cl2O5 for example The fluorine only make single bonds and the oxygen makes pi bonds the reactivity of fluorines are very bigger than the the same oxidation state of oxygen examples BrF5 and bromates PtO3 or PtF6 You may note the diference of HClO4 and HIO4 because the low EN of iodine the more stables speccies are H3IO5 or H5IO6 but only you get HClO4 or HBrO4 You may note the diference of HClO4 and HIO4because the low EN of iodine the more stables speccies are H3IO5 or H5IO6 but only you get HClO4 or HBrO4 you may see the HNO3 stable but HPo3 but only H3Po4 is stable EN N 3,1 eN P 2,1 No, there are other stronger oxidizing agents, such as PtF6, which is capable of oxydizing oxygen. Another really strong oxidizer is sodium perxenate, Na4XeO6.8H2O. But indeed, ozone is a very strong oxidizer, similar in strength as peroxodisulfate (redox potential just over 2 volts). @budullewraagh: Permanganyl fluoride is not MnO4F, but MnO3F, with a direct Mn-F bond and Mn in its +7 oxidation state. I recently discovered that I actually made some of this stuff in one of my home experiments, it is a green volatile compound. Just google on permanganyl fluoride and you'll see a few links, where the formula MnO3F is given to this compound. I think that MnO4F does not exist. You can see this green stuff in the following link: http://woelen.scheikunde.net/science/chem/exps/KMnO4+NaF+H2SO4/index.html When I did the experiment I did not know it, but some literature study has shown me that the green compound is MnO3F. what about S2O8F2 like peperoxodisulfate but the metal or H is fluorine it's a very strong oxydant more than ozone You may note the diference of HClO4 and HIO4because the low EN of iodine the more stables speccies are H3IO5 or H5IO6 but only you get HClO4 or HBrO4 you may see the HNO3 stable but HPo3 but only H3Po4 is stable EN N 3,1 eN P 2,1 what about S2O8F2 like peperoxodisulfate but the metal or H is fluorine it's a very strong oxydant more than ozone if you think +5 is one oxidation state this is nothing KrF2 stable powerfull oxydant but KrF+ with the same oxydation state is even more powefull maybe the more powerfull oxydant it's not the same the EN of C in CI3 than in CF3 radicals
ayushmaanseth Posted April 6, 2015 Posted April 6, 2015 (edited) Exceptions are always there in Chemistry. There is an example of Perxenate i.e Xeo3 or Xeo6 4- which is also known as Xenon hexoxide or Xenon trioxide. This is an extremely powerful oxidising agent. XeO6 4- +2F- + 6H+ ------> XeO3 + F2 + 3H2O Here, Fluorine ion is OXIDISED to fluorine atom (neutral gaseous atom) Concluding, it isn't right to say in a general language that Nothing can oxidise fluorine, as exceptions are always there.....in each field of this world . Thumbs Up. Ayushmaan Seth Edited April 6, 2015 by ayushmaanseth
John Cuthber Posted April 7, 2015 Posted April 7, 2015 Exceptions are always there in Chemistry. There is an example of Perxenate i.e Xeo3 or Xeo6 4- which is also known as Xenon hexoxide or Xenon trioxide. This is an extremely powerful oxidising agent. XeO6 4- +2F- + 6H+ ------> XeO3 + F2 + 3H2O Here, Fluorine ion is OXIDISED to fluorine atom (neutral gaseous atom) Concluding, it isn't right to say in a general language that Nothing can oxidise fluorine, as exceptions are always there.....in each field of this world . Thumbs Up. Ayushmaan Seth No. fluoride ions are oxidised to fluorine. That's unusual chemistry, but perfectly possible. but it is not the same as oxidising fluorine- (which chemistry can't do, but an electric arc can).
graficjane Posted August 23, 2016 Posted August 23, 2016 (edited) No but the next best thing is an antidote to fluorine. Boron protects all the metals in the human body. Fluorine Loves attaching to Boron because of its structure and boron will then pass out of the body. It works fabulous. You will want to take it with a calcium magnesium combo to help all your nervous system out. Edited August 23, 2016 by graficjane
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