By J.H. Simons (Eds.)
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Extra resources for Fluorine Chemistry
Many of these species can be called ions and complexes. As the reactions occur in a condensed phase no radicals could be free so that a free radical mechanism is excluded. As we cannot even postulate an acceptable mechanism for the evaporation of liquid hydrogen fluoride, it seems beyond present capabilities to obtain an acceptable mechanism for the chemical reactions of this process. Any postulation may contain a small element of truth for some minor part of the total chemical changes but be completely in error if employed to explain the entire process.
2 6 with A l to form A1F6 ~ The heats of the six successive reations of 4F~ have been measured 3 by Latimer and 0 Jolly* ). F " + A l + -> A1F++ A S F - + A1+++- * A1F + 2 F" + A F -> AlF (aq) 2 3 = 32 \ = 26 = 18 I cal per deg per m o l e 554a Porter and Zeller* ) determined the heats of dissociation of Al2F6(g) 0 lF and LiF • A 3 )( by g mass spectrometric methods. 0 with the products as gases. 08. 15°K. (NH4)sAlF6 was prepared by Haendler, Johnson, and Crocket* ) by reaction of a methanol solution of AlBr 3 and NH4F.
Sc+++ + H F - ScF++ + H + ScF++ + H F = S c F + + H + 2 ScF + + H F = ScF 2 3 q() a+ H + ScF aq) + H F = S c F ~ + H + 3( 4 7 0 1 Yttrium fluoride of low oxygen content was prepared by Smutz, Burnet, Walker, Tischer, and Olsen* ) by heating a yttrium compound such as the oxide in H F vapor at 600°. Its 751 preparation from Y2O3 and 7 3 4 ) and from Y 0 or YC1 N H 4F • H F at 400° by Walker and Olson* 2 3 3 and F2 by Tischer and Burnet* ) gave 1a0 9product containing more oxygen. Carlson, Schmidt, and Spedding* ) prepared the metal 708 from the fluoride by the reaction with calcium or magnesium at 1000°.