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I'd have thought that fluorine, like oxygen, is a strong oxidizer (fluorine being even stronger), and so fluorides, like oxides (e.g. rust) would be extremely s
by FooBarBizBazz 3y ago
I'd have thought that fluorine, like oxygen, is a strong oxidizer (fluorine being even stronger), and so fluorides, like oxides (e.g. rust) would be extremely stable, among the most stable compounds possible. Unless I'm forgetting the other side: Maybe the other half of the compound is not a strong enough reducer? It's a hydrocarbon though, it burns well in oxygen...
That said, even oxides do break down when heated. Like, that's what smelting is...
Hm...
- Retric 3y agoCarbon Florine bonds are some of the strongest you will find. Carbon tetrafluoride CF4 is almost as safe as nitrogen at room temperature. Tetrafluoroethylene C2F4 is actually explosive on the other hand because of it’s carbon carbon bond, the stuff is happy to spit out the carbon and get CF4. https://en.wikipedia.org/wiki/Tetrafluoroethylene https://en.wikipedia.org/wiki/Tetrafluoroethylene
- __alexs 3y agoCarbon tetrafluoride and Carbon tetrachloride are the two "carbon tets" you never want to mix up.
- marcosdumay 3y ago> Maybe the other half of the compound is not a strong enough reducer? It's about as strong as most of the molecules on your body. But I don't think that fluoride moving around is the problem. Looks like the problem is exactly the stability, and some long foreign molecules installing themselves in your body.