Silver oxide

Silver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide.^[7][8] This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:^[9]

${\displaystyle {\ce {2 AgOH -> Ag2O + H2O}}}$ (pK = 2.875^[10])

With suitably controlled conditions, this reaction can be used to prepare Ag₂O powder with properties suitable for several uses including as a fine grained conductive paste filler.^[11]

Ag₂O features linear, two-coordinate Ag centers linked by tetrahedral oxides. It is isostructural with Cu₂O. It "dissolves" in solvents that degrade it. It is slightly soluble in water due to the formation of the ion Ag(OH)−2 and possibly related hydrolysis products.^[12] It is soluble in ammonia solution, producing active compound of Tollens' reagent. A slurry of Ag₂O is readily attacked by acids:

${\displaystyle {\ce {Ag2O + 2 HX -> 2 AgX + H2O}}}$

where HX = HF, HCl, HBr, HI, or CF₃COOH. It will also react with solutions of alkali chlorides to precipitate silver chloride, leaving a solution of the corresponding alkali hydroxide.^[12][13]

Despite the photosensitivity of many silver compounds, silver oxide is not photosensitive,^[14] although it readily decomposes at temperatures above 280 °C.^[15]

This oxide is used in silver-oxide batteries. In organic chemistry, silver oxide is used as a mild oxidizing agent. For example, it oxidizes aldehydes to carboxylic acids. Such reactions often work best when the silver oxide is prepared in situ from silver nitrate and alkali hydroxide.

Wikimedia Commons has media related to Silver(I) oxide.

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