Silver oxide (I, III)

Silver oxide
Silver oxide
Are common
Systematic ; name	Silver oxide (I, III)
Traditional names	silver monoxide
Chem. formula	Ag + Ag 3+ O 2
Rat formula	Ag 2 O 2
Physical properties
condition	solid
Molar mass	123.87 g / mol
Density	7.483 g / cm³
Thermal properties
T. decomp.	100 ° C
Enthalpy of Education	−24.7 kJ / mol
Chemical properties
Solubility in water	insoluble ( 0.0027 g / 100 g H 2 O)
Classification
Reg. CAS number
PubChem
Reg. EINECS number
Smiles
Inchi
ChemSpider

Silver (I, III) oxide ( silver (III) silver oxide (I) , silver monoxide, silver dioxide ) - Ag ⁺ Ag ³⁺ O ₂ or Ag ₂ O ₂ , an inorganic binary compound of oxygen and silver exhibiting a mixed valence of positional type: +1 and +3. The compound is often mistakenly credited with the AgO formula, but it does not reflect the true nature of the bond in the substance. Another mistake is the name silver peroxide - the O – O bond is absent in this compound.

Used for the manufacture of silver-zinc alkaline current sources and as an oxidizing agent in organic synthesis.

Content

Physical Properties

Dark gray or black crystalline substance, insoluble in water. Forms crystals of monoclinic syngony , space group P 2 ₁ / c , cell parameters a = 0.58517 (3) nm , b = 0.34674 (2) nm , c = 0.54838 (3) nm , β = 107.663 (3 ) ° , Z = 2 ^[2] ^[3] . Semiconductor . It has diamagnetic properties; magnetic susceptibility –19.6 × 10 ⁻⁶ cm ³ / mol ^[1] . It has two phases: α -Ag ₂ O ₂ and β -Ag ₂ O ₂ .

Preparation and chemical properties

Obtained from silver or silver oxide (I) by the action of a strong oxidizing agent: potassium peroxodisulfate or ozone ; from silver by anodic oxidation in dilute sulfuric acid ^[4] .

Strong oxidizing agent. When heated (~ 100 ° C) decomposes with the release of oxygen. In the presence of inorganic acids, hexane , diethyl ether, and other flammable organic compounds are capable of igniting ^[4] .

It is soluble in alkalis, as well as nitric and perchloric acids :

{\mathsf {2Ag_{2}O_{2}+4HNO_{3}=4AgNO_{3}+2H_{2}O+O_{2}}}

{\ displaystyle {\ mathsf {2Ag_ {2} O_ {2} + 4HNO_ {3} = 4AgNO_ {3} + 2H_ {2} O + O_ {2}}}}

Application

Used as an oxidizing agent in a silver-zinc battery .

Notes

↑ ¹ ² CRC Handbook of Chemistry and Physics / DR Lide (Ed.). - 90th edition. - CRC Press; Taylor and Francis, 2009 .-- 2828 p. - ISBN 1420090844 .
↑ Brese NE , O'Keeffe M. , Ramakrishna BL , Von Dreele RB Low temperature structures of CuO and AgO and their relationships to those of MgO and PdO // Journal of Solid State Chemistry. - 1990. - November ( t. 89 , No. 1 ). - S. 184-190 . - ISSN 0022-4596 . - DOI : 10.1016 / 0022-4596 (90) 90310-T .
↑ Jean D'Ans, Ellen Lax. Taschenbuch für Chemiker und Physiker. Springer DE 1997. P. 288f.
↑ ¹ ² Silver oxide // Chemical Encyclopedic Dictionary / Knunyants I. L. (Ch. Ed.). - M .: Soviet Encyclopedia, 1983.- S. 522.- 792 p. - 100,000 copies.

[crc-1] ¹ ² CRC Handbook of Chemistry and Physics / DR Lide (Ed.). - 90th edition. - CRC Press; Taylor and Francis, 2009 .-- 2828 p. - ISBN 1420090844 .

[2] Brese NE , O'Keeffe M. , Ramakrishna BL , Von Dreele RB Low temperature structures of CuO and AgO and their relationships to those of MgO and PdO // Journal of Solid State Chemistry. - 1990. - November ( t. 89 , No. 1 ). - S. 184-190 . - ISSN 0022-4596 . - DOI : 10.1016 / 0022-4596 (90) 90310-T .

[lax97-3] Jean D'Ans, Ellen Lax. Taschenbuch für Chemiker und Physiker. Springer DE 1997. P. 288f.

[ХЭС-4] ¹ ² Silver oxide // Chemical Encyclopedic Dictionary / Knunyants I. L. (Ch. Ed.). - M .: Soviet Encyclopedia, 1983.- S. 522.- 792 p. - 100,000 copies.