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<p>[QUOTE=&quot;GDJMSP, post: 983694, member: 112&quot;]Did you read the first link I provided ? It pretty much contradicts everything you&#039;re saying.</p><p><br /></p><p><i>&quot;Amorphous AuxOy compounds have been produced under <u>standard temperature and pressure</u> but decomposed to metallic gold.&quot;</i></p><p><i><br /></i></p><p><i>&quot;Of all the metals, gold, chemical symbol Au, has the lowest tendency to react with air to form oxides.&quot;</i></p><p><br /></p><p>So gold oxides do exist and they can occur under completely normal conditions.</p><p><br /></p><p><br /></p><p><i>&quot;Structurally, Au2O3, the most stable Au oxide, exists as a square planar compound, exhibiting distorted octahedral geometry coordination on the Au3+ ion and a tetrahedral coordination on the O2- ion. The distorted geometry occurs as a result of d8 orbital splotting, the Jahn-Teller effect. Additionally, radius ratio rules support a distorted octahedral geometry by predicting an octahedral coordination for Au3+ (r = 0.85 A) and a tetrahedral coordination for O2- (r = 1.32 A). [3,5,7] Despite its observed geometry, Au2O3 and other AuxOy compounds exist in an amorphous state.&quot;</i></p><p><br /></p><p><i>&quot;One hypothesis that could be made for lower pressure / lower temperature reactions is that the positive slope of the near verticle phase boundary for the stability of the Au metal would decrease to the point that the area of stability of the Au metal would be dominant. By regraphing the data on a ln PO2 vs T plot, a linear relationship would probably be seen with the Au metal area of stability located at the pressure and temperature ranges existing in nature.&quot;</i>[/QUOTE]</p><p><br /></p>

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