Silver (I, III) oxide

Crystal structure
	__ Ag + / 3 + __ O 2−
General
Surname	Silver (I, III) oxide
other names	Silver peroxide; Silver (II) oxide;
Ratio formula	AgO
Brief description	dark gray odorless solid
External identifiers / databases
EC number	215-098-2
ECHA InfoCard	100,013,726
PubChem	92152
ChemSpider	83197
Wikidata	Q2380600
properties
Molar mass	123.87 g mol −1
Physical state	firmly
density	7.44 g cm −3
Melting point	> 100 ° C (decomposition)
solubility	reacts with water
safety instructions
H and P phrases	H: 272-314
	P: 221-210-303 + 361 + 353-305 + 351 + 338-405-501
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Silver (I, III) oxide is an inorganic chemical compound of silver from the group of oxides .

Extraction and presentation

Silver (I, III) oxide can be obtained by persulfate oxidation of silver (I) oxide in an alkaline medium ( e.g. sodium hydroxide or potassium hydroxide ) at 90 ° C.

${\ displaystyle {\ ce {4 AgNO3 + 2 K2S2O8 + 8 NaOH ->}}}$ ${\ displaystyle {\ ce {4 AgO + K2SO4 + 3 Na2SO4 + 2 NaNO3 + 2 KNO3 + 4 H2O}}}$

Other representations are the reaction of a mixture of the solutions of silver nitrate and potassium permanganate with potassium hydroxide, the action of ozone-containing oxygen at 240 ° C on metallic silver in the presence of a catalyst , the reaction of sodium hypochlorite with silver (I) oxide or through hydrolysis or thermal Decomposition of Ag ₇ NO ₁₁ , which is obtained by anodic oxidation of silver nitrate solutions, can be shown.

properties

Silver (I, III) oxide is a diamagnetic, light-sensitive, dark gray and odorless solid that reacts with water. It has a strong oxidizing effect, is soluble in nitric acid and decomposes when exposed to sulfuric acid , releasing oxygen. It has a monoclinic crystal structure with the space group P 2 ₁ / c (space group no. 14) and the lattice parameters a = 585.2 pm, b = 347.8 pm, c = 549.5 pm and β = 107.5 ° as well as two formula units per unit cell . As a dry solid, the oxide is temperature-stable up to 100 ° C, above which it begins to decompose. Template: room group / 14

Although the compound is also formally called silver (II) oxide or silver peroxide, previous evidence shows that it is silver (I, III) oxide. Some of the seemingly conflicting data reported for AgO may be due to a lack of accurate understanding of the oxidation state of silver in AgO.

use

Silver (I, III) oxide is used in organic chemistry to convert benzyl halides directly into dibenzyl ether . It also serves as a surface catalyst in the epoxidation of alkenes . Silver is present in charged silver-zinc and other accumulators as silver (I, III) oxide. With silver oxide zinc button cells , silver (I) oxide or silver (I, III) oxide is pressed directly into the cells during manufacture.

Individual evidence

↑ ^a ^b ^c ^d ^e ^f ^g ^h data sheet silver (II) oxide, 99.9% (metals basis), Ag 86.6% min at AlfaAesar, accessed on August 3, 2013 ( PDF )(JavaScript required) .
^ ^A ^b Dale L. Perry: Handbook of Inorganic Compounds, Second Edition . Taylor & Francis US, 2011, ISBN 1-4398-1461-9 , pp. 369 ( limited preview in Google Book search).
^ ^A ^b ^c N. Hammer, Jacob Kleinberg: Silver (II) oxide . In: JC Bailar, Jr. (Ed.): Inorganic Syntheses . tape 4 . McGraw-Hill, Inc., 1953, ISBN 0-88275-165-4 , pp. 12 f . (English).
↑ Georg Brauer (Ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 998.
^ Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists . Springer DE, 1997, ISBN 3-540-60035-3 , pp. 288 f . ( limited preview in Google Book search).
↑ TP Dirkse: Silver (II) oxide , Department of Chemistry, Calvin College Grand Rapids; Uchigan 49506, USA, April 1984
↑ Data sheet Silver oxide, predominantly silver (II) oxide at Sigma-Aldrich , accessed on August 3, 2013 ( PDF ).
↑ Helmut Schaefer: VDI-Lexikon Energietechnik . Springer-Verlag, 2013, ISBN 978-3-642-95748-2 , pp. 42 ( limited preview in Google Book search).
↑ Lucien F. Trueb, Paul Rüetschi: Batteries and accumulators Mobile energy sources for today and tomorrow . Springer-Verlag, 2013, ISBN 978-3-642-58741-2 , pp. 49 ( limited preview in Google Book search).

[Alfa-1] ↑ ^a ^b ^c ^d ^e ^f ^g ^h data sheet silver (II) oxide, 99.9% (metals basis), Ag 86.6% min at AlfaAesar, accessed on August 3, 2013 ( PDF )(JavaScript required) .

[Dale_L._Perry-2] A ^b Dale L. Perry: Handbook of Inorganic Compounds, Second Edition . Taylor & Francis US, 2011, ISBN 1-4398-1461-9 , pp. 369 ( limited preview in Google Book search).

[IS4-3] A ^b ^c N. Hammer, Jacob Kleinberg: Silver (II) oxide . In: JC Bailar, Jr. (Ed.): Inorganic Syntheses . tape 4 . McGraw-Hill, Inc., 1953, ISBN 0-88275-165-4 , pp. 12 f . (English).

[brauer-4] Georg Brauer (Ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 998.

[Jean_D'Ans,_Ellen_Lax-5] Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists . Springer DE, 1997, ISBN 3-540-60035-3 , pp. 288 f . ( limited preview in Google Book search).

[T._P._Dirkse-6] TP Dirkse: Silver (II) oxide , Department of Chemistry, Calvin College Grand Rapids; Uchigan 49506, USA, April 1984

[Sigma-7] Data sheet Silver oxide, predominantly silver (II) oxide at Sigma-Aldrich , accessed on August 3, 2013 ( PDF ).

[Helmut_Schaefer-8] Helmut Schaefer: VDI-Lexikon Energietechnik . Springer-Verlag, 2013, ISBN 978-3-642-95748-2 , pp. 42 ( limited preview in Google Book search).

[Lucien_F._Trueb,_Paul_Rüetschi-9] Lucien F. Trueb, Paul Rüetschi: Batteries and accumulators Mobile energy sources for today and tomorrow . Springer-Verlag, 2013, ISBN 978-3-642-58741-2 , pp. 49 ( limited preview in Google Book search).