Talk:Phosphorus trifluoride

message: Overall nice job, but highly technical for the general Wikipedia reader, more so than PCl3 and PBr3.  Some observations:  
:In the introductory paragraph:  
:*"It is highly toxic and it reacts slowly with water."  
:In the "Chemical properties" section:  
:*"Phosphorus trifluoride hydrolyses fairly rapidly in water, and very rapidly under under alkaline conditions, but PF3 is less reactive in this regard than phosphorus trichloride."  
:In the "Precautions" section:  
:*"It also reacts slowly with water to form the highly toxic and corrosive hydrofluoric acid,"
:In the Table:  
:*"Solubility ..... Water:  slow hydrolysis:
:Maybe a bit of a contradiction on the reaction speed here? 
::Well spotted!  I recall the problem when writing this, the different sources used different comparative terms depending on the context, I must have got a bit confused by it all. 
:Also, I went with 2 out of 3 and changed the F-P-F bond angle from 104° to 96.3° in "Physical properties".  See values in picture and table.  
::Thanks, I agree.
:PF3 seems to have a remarkably low boiling point compared to PCl3.  Also. I noticed the (single covalent) bond strength of 119.4 kcal/mole seems rather strong compared with many single covalent bonds in organic compounds.  Bond strengths weren't given for PCl3 or PBr3.  Also, I noticed a dipole moment of 0.8 D was given for PCl3, but no dipole moment was given for PF3 or PBr3.  H Padleckas 17:15, 7 May 2005 (UTC)
replies: text: The reaction of PF3 with water is slow; it is the Chemical properties section which needs copy-editing. I have a slight gripe with the Preparation section: transhalogenation of phosphorus halides is certainly possible, but in this case it is particularly messy. My memory of the preferred preparation is the reaction of phosphorus pentafluoride with elemental phosphorus, but I would rather someone check this before posting it on the article. In general, hydrogen fluoride and calcium fluoride are poor fluorinating agents, and I doubt that they would work well in this case.  Sorry I can't be more precise, but my nearest university libraries are in Lens and Lille so I cannot immediately find sources for this info. Physchim62 19:01, 10 May 2005 (UTC)
replies: text:  As for the dipole moment, it is notably small and so worth a mention if anyone can find a figure for it. Nitrogen trifluoride is even more remarkable from this point of view: the bond dipoles and the dipole due to the lone pair cancel each other out almost exactly. Physchim62 19:09, 10 May 2005 (UTC)

message: Phophorus trifluoride has a bond angle of 107° - where did this come from?  The FPF angle is correct as per Greenwood & Earnshaw, so I am not sure which bond angle is being discussed here.  Clarification would be appreciated.JSR (talk) 15:01, 2 October 2012 (UTC)
thread_title:  Bond angle 

message: In my anatomy textbook it says that PF3 is a required component of the intrinsic mechanism of the initiation of coagulation. -Carl
:Oh, that is platelet factor 3, not the molecule phosphorus trifluoride. We do need to key an eye out for people consulting this article for your topic. --Smokefoot (talk) 14:59, 16 November 2014 (UTC)
thread_title:  Perhaps its role in blood clotting deserves a mention?