Fluorine (extra interview footage)

[SepherStar]

That guy looks like Austin Powers...and he;s just as cool.

[plasticraincoat1]

Id love to see some Fluorine be fed some Potassium metal and some yellow Phosphorus - now that would be two very exciting reactions :)

PLEASE............

[punishedexistence]

The Prof is the Chuck Norris of Chem, and the Fluorine expert is the Steven Segall of F Chemistry. F as in Fluorine of course! Very well done and informative, as I am ever fascinated by this evil yet very necessary element.

[Badgerinthenight]

Leicester yay! :D

[LizzyAston]

i always thought that fluorine was the most reactive element. could someone correct me? cos all of its reacted and its impossible to find the gas as unreacted!

[Phosphon]

@LizzyAston flourine is indeed the most reactive element, but that doesn´t mean you couldn´t find it unreacted...

[TheFounderUtopia]

Why doesn't the Flourine react with the Nickle container? I don't recall Nickle being one of the elements that the Prof said it doesn't react with.

[KlaxonCow]

@TheFounderUtopia It was explained briefly in the main video.

Basically, the fluorine does react with the nickel the first time that it's introduced into the container. But in reacting with the nickel, it forms a stable protective layer on the surface of the container, which won't thereafter react with any more fluorine.

That is, to put it crudely, you let it react until it's "all reacted out" and can't react anymore - then it becomes a useful container, as it'll no longer react with it.

[TheFounderUtopia]

@KlaxonCow

I see, thanks for explaining! :)

[DistendedPerinium]

@KlaxonCow An easier way to think of it is that it is like a patina of rust that protects the rest of the metal from reacting, except in this case it is nickel being protected from fluorine instead of iron from oxygen.

[nfguler]

@TheFounderUtopia It reacts but nickel is more resistant than other elements

[Geomanb]

Organic fluorine compounds can be very dangerous, too - Dioxine e.g.

[mewrox99]

@Geomanb

Or have no toxicity like Perfluorodecalin

[myst32YT]

Well Done!!!

[nsub1]

This extra footage is golden. As someone who got a BA in Chemistry in undergrad (but left for less harrowing pastures), it's really interesting for me to see some of the more technical aspects of the lab work. I get to relive and recall the practicalities as well as learn about the more technical scientific concerns at work!

[tybo09]

For some reason, my computer skips or something and I can't understand what he's saying at the same part of the video every time I've seen it (even when I re-load it).

What sort of sorbent is in the sorbent trap to keep the fluorine out of the vacuum pumps?

[ib9rt]

@tybo09 I believe he says soda lime.

[blinking801]

Man that is really an interesting element!

[wowggscrub]

chloroflourocarbons CFC

[odysseus9672]

If fluorine is so reactive, how do they even make elemental fluorine?

[KilgothMirna]

@odysseus9672 It is usually gained in the form of Calcium fluoride and then reacted with sulphuric acid to get HF (hydrofluoric acid). This is then electrochemically seperated into elemental Hydrogen and Fluorine.

There are better ways to get HF, but the electrochemic (?) part can not be avoided.

[hkparker]

@odysseus9672 Electrolysis. We can reverse reactions by applying current. There is only one chemical way to synthesize it but it is not practical: 2 K2MnF6 + 4 SbF5 = 4 KSbF6 + 2 MnF3 + F2. It is produced by electrolysis of saturated potassium fluoride solution.

[L00NGB00W]

I love your videos. =)

One reaction I've always wanted to see would be the combination of Fluorine and Francium. F+Fr -> FFr To make Francium Fluoride.

The ultimate chemical reaction... XD

Unless you could get your hands on some Ununennium....

What do you say? =)

[T1carus]

btw, switch off your pc monitors, they waste alot of energy when just running a screensaver

[DuskY1991]

And how do they know that the carbon-fluorine bonds give those interesting properties to drugs?

[sciencoking]

Why is the bond between fluorine atoms so weak? Shouldn't they have a much lower energy even with a nonpolar covalent bond?

[KilgothMirna]

@sciencoking The problem is that both atoms strongly pull the electron to themselves. That leads to the electrons being located close to the nuclei. Now chemical bonds can be imagined as electron density BETWEEN nuclei. So, since there is hardly any electron density in between, the bond is very very weak.

That is one way to explain it. I guess quantum mechanics may give a more accurate explanation, but that would probably be going too far.

[sciencoking]

Thanks a lot =) (did it post twice, it's not working again grr)