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Why does this exist?
Its synthesis and use is fairly uncommon given its horrific combination of properties. However, it is still used as an cleaner in the semiconductor industry, and is a very effective fluorinating agent in the synthesis of various other (usually dangerous) chemicals. — Preceding unsigned comment added by 72.241.149.143 ( talk) 22:46, 13 November 2016 (UTC)
My english is too bad to edit the article, but I would to signal that there are many errors. My opinion is that the article should be deleted.
Errors include:
Svante 02:19, 21 May 2005 (UTC)
The best I can find so far is [1], which may just be taken from here for all we know.-- Nick Y. 18:09, 25 January 2007 (UTC)
I have found an apparently contradictory reference Zeitschrift für anorganische und allgemeine Chemie, Volume 190, Issue 1 , Pages 270 - 276, DOI:10.1002/zaac.19301900127, [2]. The title translates as "about a new chlorine Flouride-ClF3". I have seen this referenced elsewhere on the web as being the invention.-- Nick Y. 18:43, 25 January 2007 (UTC)
Quoted from Banks, A. A.; Rudge, A. J. “Liquid density of chlorine trifluoride” Journal of the Chemical Society (1950), 191-3 (these were collaborators with Emelius, the master of UK fluorine chem. at the time). The first sentence of their paper: “The preparation of chlorine trifluoride was first described by Ruff and Krug (Z. anorg. Chem., 1930, 190, 270) , since when only nine communications (Schmitz and Schumacher, Z. Naturforsch., 1947, 2a, 362, 363; Domange and Neudorffer, Compt. rend., 1948, 226, 920; Schäfer and Wicke, Z. Elektrochem., 1948, 52, 205; Booth and Pinkston, Chem. Reviews, 1947, 41, 421; B.I.O.S. Final Report No. 1595; C.I.O.S. Report So. XXII-17) dealing with this compound have appeared in the literature.” So it looks like it was Ruff and Krug.-- Smokefoot 18:50, 25 January 2007 (UTC)
I agree. I think we should remove the claim. It could be later reintroduced with appropriate references.
"It was first prepared in 1912 by the electrolysis of molten NaCl/HF, but is now generally made by reacting fluorine gas with 3% aqueous sodium hypochlorite solution:
4F2 + 2NaOCl → 2ClF3 + 2NaF + O2"
-- 128.115.27.10 21:40, 25 January 2007 (UTC)
NFPA 704 safety square | |
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will also go into the table!-- Stone 12:29, 26 January 2007 (UTC)
Bond angle 120° this looks strange for me and also strange compared with the drawing.-- Stone 12:35, 26 January 2007 (UTC)
The article says, "Pure ClF3 is stable to 180° in glass vessels (...)". 180° using which unit?
Gaesadair ( talk) 05:39, 22 March 2008 (UTC)
A friend of mine is curious (as am I, to be honest), are there any 'interesting' reactions to common or weapons-grade radioactive materials? --– Xoid 03:06, 8 March 2010 (UTC)
On the Fluorine page, it stated that Chlorine Trifluoride: 'which as a freely reacting oxidant gives the strongest oxidants' Is there a standard reduction potential for it? —Preceding unsigned comment added by 119.224.31.129 ( talk) 09:14, 11 May 2011 (UTC)
I'm in no doubt that ordinary fire-fighting methods are near-useless. I tagged this sentence as dubious because it's unclear if any fire-extinguishing agent will work on a chlorine trifluoride fire. Two legs of the fire triangle are pretty much untouchable in a ClF3 fire; the stuff is its own oxidizer and so it doesn't need air (making atmosphere-displacement agents useless), and it oxidizes things you wouldn't normally consider fuel (which thus normally make good candidates for fire suppression, such as foams and water). The only thing you can try to control is heat, by supercooling the reactants until they no longer react. I don't know how cold it'd have to get, but I'd bet a nickel on a tanker truck of LN2 not being enough.
Discuss. Liko81 ( talk) 20:33, 17 September 2012 (UTC)
I have just rolled back all the recent edits from user:1YlGC6dsynvm. There are just too many dubious edits in there and I do not have the time or energy to go through them with a fine-tooth comb to pick out what is good and what is bad. Best wishes to anyone wanting to take that task on. Spinning Spark 17:18, 2 March 2013 (UTC)
The current version says ClF3 reacts with Teflon®.
I'd BBIU but it's not clear what to put in its place. Air Products says to use Teflon only with gaseous ClF3, and John Clark's book "Ignition!" says there's mechanical erosion, so they're not truly compatible.
It is of course chemically impossible for a fluorinating agent to fluorinate something that's already completely fluorinated, but it's conceivable that it breaks the carbon-carbon bonds, but in that case there should be a citation. 50.46.146.86 ( talk) 00:21, 19 April 2013 (UTC)
Found this hidden text in the article: "Doesn't ClF3 react with water to produce OF2 + HF + HCl?"
Not in the usual case of water being in excess. The primary reactions would be these:
4ClF3 + 6H2O -> 2Cl2 + 12HF + 3O2
ClF3 + 2H2O -> HCl + 3HF + O2
You might get some of the chlorine oxyacids (HClOx) as well if there were enough water to absorb the heat without boiling. H2O2 would probably show up in small amounts as well. It's a combustion reaction, so it'll inevitably produce a mixture of products.
OF2 could only be produced if ClF3 were in excess, since excess water hydrolyses it to O2 + 2HF. I'm not sure if you'd get much of it even then. Magic9mushroom ( talk) 00:18, 28 January 2015 (UTC)
I have reverted this edit which removed the claim that ClF3 is stable below 180 C in quartz vessels. I am seeing a lot of sources describing ClF3 being introduced into quartz chambers in order either to etch a silicon substrate or else to clean silicon carbide from the walls of the chamber with little or no damage to the quartz [4] [5] [6]. In the Journal of the Chemical Society I found this snippet In filling the cell with chlorine trifluoride a sufficient quantity was distilled in vacuum from a quartz storage vessel which explicitly confirms storage in quartz. In Regulatory Chemicals Handbook it states ClF3 attacks quartz if traces of moisture are present, which implies that that pure quartz with no other materials present will not be attacked. Spinning Spark 09:20, 28 January 2015 (UTC)
JimW Your reference is sort of screwed up. You may wish to correct it. JSR ( talk) 19:12, 11 April 2017 (UTC)
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As dangerous as this stuff is, does this compound react with N2? Or noble gases? DASL51984 ( Speak to me!) 22:17, 9 November 2017 (UTC)
Noble gases except xenon.And some metal fluorides. 小小小硝酸 ( talk) 16:59, 1 December 2018 (UTC)
Recently I came across a paper from the mid 1950's (which I lost the link to, unfortunately) where a company called Union Carbide and Carbon Corporation ran an experiment where they tried to determine the heat of reaction of ClF
3 with excess water. And the result?
If my calculations are correct, this means the reaction of 1 kg of ClF
3 with excess water releases about 3.66 megajoules of energy, or about 876.15 grams of TNT.
DASL51984 (
Speak to me!)
16:46, 18 February 2022 (UTC)