Is there something that can oxidise Fluorine?

[verode]

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

[Cap'n Refsmmat]

Chuck Norris can oxidize fluorine.

[Mr Skeptic]

I bet an electrode can oxidize fluorine.

[insane_alien]

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]

The OP was in 2005 and may have lost interest by now.

[verode]

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]

and you still haven't gave an example of oxidised fluorine.

[verode]

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 HIO4

because 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 HIO4

because 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

[verode]

try with FSO2-O-O-SO2F

you can get Br+3 with it

[ayushmaanseth]

• 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]

 

• 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]

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