Silver oxide

This article is about silver(I) oxide. For the mixed-valence oxide, see Silver(I,III) oxide.
Silver oxide
Silver(I) oxide structure in unit cell

Silver(I) oxide powder
Names
IUPAC name
Silver(I) oxide
Other names
Silver rust, Argentous oxide, Silver monoxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.039.946 Edit this at Wikidata
EC Number
  • 243-957-1
MeSH silver+oxide
RTECS number
  • VW4900000
UNII
  • InChI=1S/2Ag.O/q2*+1;-2 ☒N
    Key: NDVLTYZPCACLMA-UHFFFAOYSA-N ☒N
  • InChI=1S/2Ag.O/q2*+1;-2
    Key: NDVLTYZPCACLMA-UHFFFAOYSA-N
  • [O-2].[Ag+].[Ag+]
Properties
Ag2O
Molar mass 231.735 g·mol−1
Appearance Black/ brown cubic crystals
Odor Odorless[1]
Density 7.14 g/cm3
Melting point 300 °C (572 °F; 573 K) decomposes from ≥200 °C[3][5]
0.013 g/L (20 °C)
0.025 g/L (25 °C)[2]
0.053 g/L (80 °C)[3]
Solubility product (Ksp) of AgOH
 1.52·10−8 (20 °C)
Solubility Soluble in acid, alkali
Insoluble in ethanol[2]
Acidity (pKa) 12.1 (estimated)[4]
−134.0·10−6 cm3/mol
Structure
Cubic
Pn3m, 224
Thermochemistry
65.9 J/mol·K[2]
122 J/mol·K[6]
−31 kJ/mol[6]
−11.3 kJ/mol[5]
Hazards
GHS labelling:
GHS03: OxidizingGHS07: Exclamation mark[7]
Danger
H272, H315, H319, H335[7]
P220, P261, P305+P351+P338[7]
NFPA 704 (fire diamond)
[1]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
0
1
Lethal dose or concentration (LD, LC):
2.82 g/kg (rats, oral)[1]
Related compounds
Related compounds
 Silver(I,III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Silver oxide is the chemical compound with the formula Ag2O. It is a fine black or dark brown powder that is used to prepare other silver compounds.

  1. ^ a b c "Silver Oxide MSDS". SaltLakeMetals.com. Salt Lake Metals. Retrieved 2014-06-08.
  2. ^ a b c Lide, David R. (1998). Handbook of Chemistry and Physics (81 ed.). Boca Raton, FL: CRC Press. pp. 4–83. ISBN 0-8493-0594-2.
  3. ^ a b Perry, Dale L. (1995). Handbook of Inorganic Compounds (illustrated ed.). CRC Press. p. 354. ISBN 0849386713.
  4. ^ Perrin, D. D., ed. (1982) [1969]. Ionisation Constants of Inorganic Acids and Bases in Aqueous Solution. IUPAC Chemical Data (2nd ed.). Oxford: Pergamon (published 1984). Entry 210. ISBN 0-08-029214-3. LCCN 82-16524.
  5. ^ a b "Silver oxide".
  6. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
  7. ^ a b c Sigma-Aldrich Co., Silver(I) oxide. Retrieved on 2014-06-07.