Talk:Beryllium fluoride

Be2+ ions
I thought that beryllium didn't form any compounds considered ionic? Whoever wrote that all beryllium compounds contain Be2+ ions clearly didn't know what he/she was talking about. Bbi5291 00:16, 24 June 2007 (UTC)

Greatest amount of ionic character?
"It is the beryllium compound with the greatest amount of ionic character (due to the high electronegativity of fluorine), but even so it is not considered ionic by many chemists."

Fluorine isn't the strongest oxidizing agent out there. What if you tried using "stronger" anions like hexafluoroplatinate, hexafluorophosphate, or hexafluoroantimonate (for example in the world's strongest acid)? Wouldn't those compounds have more ionic character than BeF2? Perhaps they might even be "true" ionic compounds as well. Seeing as how PtF6 can oxidize oxygen (0) to oxygen (1/2) and xenon to xenon (II), it certainly has at least a chance of oxidizing Be to Be2+.

I added the word "binary" to emphasize that we are only talking about binary compounds. There are plenty of polyatomic anions that are stronger than Fluoride.

If anyone knows whether BePtF6 or any of the other compounds I mentioned are truly ionic or just covalent/polymeric like BeF2, I'd certainly be interested!

Stonemason89 (talk) 15:35, 26 August 2008 (UTC)

Graphic too misleading to use
The image captioned "Structure of solid BeF2" is wrong in several respects:
 * It shows only an amorphous network, when BeF2 also has a quartz-like crystalline phase.
 * The network is shown as two dimensional, when the solid has three-dimensional bonding.
 * The network shows tri-coordinate Be ions, when they are in reality tetracoordinate.

I have deleted the graphic. Adapting (re-captioning) an image of silica would be an excellent alternative: The literature describes SiO2 as a close structural analogue of BeF2, as already discussed in the article.

I have also removed the statement that "BeF2 is considered to be highly covalent"; surprisingly, it isn't (as discussed in a paper I read a few days ago). Eric Drexler

(talk) 22:52, 28 April 2013 (UTC)

Be-F bond distance
The article states 177 pm, which I could not find in the referenced book, however, according to a German textbook, it is 143 pm for Be-F and 177 pm for Be-Cl. So it seems that the wrong value is included in the article and this should be corrected. Szaszicska (talk) 22:02, 1 August 2014 (UTC)
 * Great detective work! The Be-F distance is shorter for the two-coordinate species than it is for the tetrahedral derivative, following the normal trends.  --Smokefoot (talk) 23:10, 2 August 2014 (UTC)

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