Talk:Tungsten hexafluoride

message: Correction: Tungsten hexafluoride is not the densest known gas, that prize goes to uranium hexafluoride. Physchim62 15:54, 24 May 2005 (UTC)
replies: text: Uranium hexafluoride is a volatile solid; it sublimes at 56.5 ˚C.  So at room temperature, tungsten hexafluoride is still the densest "gas".  The solid UF6 would almost certainly exist in equilibrium with some vapor, so depends on what you consider gas. --71.227.190.111 03:54, 31 July 2006 (UTC)
thread_title: Untitled

message: "The dominant application of tungsten fluoride is in semiconductor industry" well, even if only a minor part of the tungsten carbide is manufactured through the tungsten hexafluoride process this would probably be a more important application at least by volume.  —Preceding unsigned comment added by 150.227.15.253 (talk) 08:30, 27 July 2010 (UTC)
thread_title:  Semiconductor industry 

message: Tungsten hex is a water white colorless liquid.  If it is contaminated with Cr then it is yellow to orangish red depending on how much Cr and which Cr speicies is contaminating it.
It will form HF on contact with water and it will cause damage, not may.  24.229.244.111 17:10, 11 February 2006 (UTC)
thread_title:  Corrections 

message: Tungsten hexafluoride is not a gas at standard conditions. STP for gases is defined as 0° C and 1 atm. The standard boiling point of this compound is listed as 17.1° C. It is a gas at room temperature, but not at standard temperature.
144.162.23.122 (talk) 22:27, 24 September 2013 (UTC)
replies: text: Good point. Maybe, the standard conditions should actually be linked to standard state, in which tungsten hex would be a gas. Hopefully someone can clear this up. Piguy101 (talk) 00:30, 9 April 2014 (UTC)
thread_title: Not a gas?

message: *Well, I guess that the prize for the most dense gas could become legalistic, depending on conditions and the degree to which one wants to discuss transient species and plasmas, but by most normal  perspectives UF6 is probably it.  I dont know if perfluorides are known for the still heavier elements such the congener of W.
*Back to the WF6 report.  It is claimed to be "odorless".  Thus, the rate of hydrolysis must be quite slow, because I would expect it to smell like HF.
*Also, I propose to replace the tentative "may"s in the following quote, fix the awkward which ( implying that water can penetrate...), and remove the claim that WF6 can damage bone (seems silly)
"WF6 may form hydrofluoric acid (HF) on contact with water, which can penetrate the skin and cause damage to the subdermal tissues and bone. Inhalation may cause respiratory tract burns and can be toxic. This compound is a lachrymator which causes tearing and irritation of the eyes. Contact may cause burns to the eyes, skin and mucous membranes."
One question is whether WF6 poses dangers beyond being an in situ source of con HF.
Smokefoot 17:44, 11 February 2006 (UTC)
thread_title: Comments

message: The statements made about its synthesis do not make much sense and seem to be circular. Besides the reference is not very satisfactory because it is a patent about its use rather than its synthesis and only the abstract seems open to scrutiny.
Jcwf (talk) 03:43, 20 November 2008 (UTC)
replies: text: I attempted to address this gap about the prep and gave more general refs.  It is made by direct fluorination.--Smokefoot (talk) 04:55, 20 November 2008 (UTC)
thread_title: Synthesis

message: Substituted at 18:10, 5 June 2016 (UTC)
thread_title: Assessment comment