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Silver Oxide is used as a laboratory reagent and in the production of batteries. It reacts with a wide variety of compounds to produce soluble silver derivatives. It also absorbs carbon dioxide and acts as a scrubber. Its molecular formula is Ag2O and it is a fine powder that can be black or dark brown in color. It is odourless and has a metallic substance. It is soluble in water, but it decomposes in alkalis and acids. This odourless Silver oxide is an oxidizing agent in the laboratory that is used to make a variety of compounds. It can be dissolved in ammonium hydroxide or in alkali chlorides to form soluble silver derivatives. In the lab, it is a common compound that is employed in the synthesis of Transition Metal-Carbene Complexes (organometallic compounds featuring a divalent organic ligand). It readily reacts with ligand precursors to form the corresponding complexes. Structurally, it is reminiscent of the disilver complexes decorated with amido-diphosphine ligands 2-P(iPr)2-4-MeC6H42N- which bind to the atoms of silver in a nonsymmetrical manner via phosphorus atoms only. The complexes have distorted trigonal and tetrahedral Ag geometries with short Ag-P(O) bonding distances, which are shorter than 3.6 A. The dramatic effect of the phosphide oxide group on the energy of the long-lived excited state allows for boosting the photocatalytic activity in a cycloaddition reaction that has previously not been accomplished for silver(I) complexes. This is an important step in the development of new families of d10 photofunctional complexes and a significant advance in the chemistry of coinage metals.