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There appear to be some errors in the "Alkali metal - ammonia solutions" section. Some descriptions regarding density of solutions and concentration seem backwards. 134.76.63.1 (talk) 15:06, 10 January 2011 (UTC)Reply
Uh oh, so metals in ammonia still react after a while? -lysdexia 14:58, 12 October 2007 (UTC) —Preceding unsigned comment added by 68.123.4.253 (talk)
Could anyone get a photo of a solution containing solvated electrons to illustrate the blue color of the solution (perhaps Na in NH3)?---- Bfesser (talk) 18:33, 16 November 2007 (UTC)Reply
research.chem.ox.ac.UK
Images may be subject to copyright.
Olthe3rd1 (talk) 01:37, 17 October 2015 (UTC)Reply
One item which is in error is the mention of the blue color independent of what metal cation is used. Different metals give different colors if the ammonia solution is kept in quartz rather tha Pyrex. In Pyrex it is the sodium from the sodium silicate which leads to cation exchange and the common blue color.
The important work of James Dye is totally overlooked.
There is mention of only an Electride being in solution. Actually there are three - the Electride, the Alkide and the Free Electron.
Thus, there is a lot of literature to be read.
But the article, nevertheless, should be rated as very important.
Some sources regarding the solvated electron are pointed out in the next link: [1]--82.137.9.119 (talk) 05:02, 27 June 2013 (UTC)Reply
Other link: JCP--188.27.144.144 (talk) 14:34, 20 February 2014 (UTC)Reply
Although the solvated electron has been described, it seems that this description is limited to a rather qualitative approach. Are there some sources regarding the involvement of the solvated electron concentration in formulas like Nernst equation?--188.26.22.131 (talk) 09:00, 2 August 2013 (UTC)Reply