Silver oxide

Silver oxide
	; Unit cell
	; Crystal packing
Names
	IUPAC name Silver(I) oxide
	Other names Silver rust, Argentous oxide, Silver monoxide
Identifiers
CAS Number	20667-12-3 ;
3D model (JSmol)	Interactive image;
ChemSpider	7970393 ;
ECHA InfoCard	100.039.946
EC Number	243-957-1;
MeSH	silver+oxide
PubChem CID	9794626;
RTECS number	VW4900000;
UNII	897WUN6G6T ;
CompTox Dashboard (EPA)	DTXSID40893897 ;
	InChI InChI=1S/2Ag.O/q2+1;-2 Key: NDVLTYZPCACLMA-UHFFFAOYSA-N ; InChI=1S/2Ag.O/q2+1;-2 Key: NDVLTYZPCACLMA-UHFFFAOYSA-N;
	SMILES [O-2].[Ag+].[Ag+];
Properties
Chemical formula	Ag2O
Molar mass	231.735 g·mol−1
Appearance	Black/ brown cubic crystals
Odor	Odorless
Density	7.14 g/cm3
Melting point	300 °C (572 °F; 573 K) decomposes from ≥200 °C
Solubility in water	0.013 g/L (20 °C); 0.025 g/L (25 °C); 0.053 g/L (80 °C)
Solubility product (Ksp) of AgOH	1.52·10−8 (20 °C)
Solubility	Soluble in acid, alkali; Insoluble in ethanol
Acidity (pKa)	12.1 (estimated)
Magnetic susceptibility (χ)	−134.0·10−6 cm3/mol
Structure
Crystal structure	Cubic
Space group	Pn3m, 224
Thermochemistry
Heat capacity (C)	65.9 J/mol·K
Std molar; entropy (S⦵298)	122 J/mol·K
Std enthalpy of; formation (ΔfH⦵298)	−31 kJ/mol
Gibbs free energy (ΔfG⦵)	−11.3 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H272, H315, H319, H335
Precautionary statements	P220, P261, P305+P351+P338
NFPA 704 (fire diamond)	2 0 1
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	2.82 g/kg (rats, oral)
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). verify (what is ?) Infobox references

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.

Preparation

Silver(I) oxide produced by reacting lithium hydroxide with a very dilute silver nitrate solution

Silver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide.^[8]^[9] This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:^[10]

{\ce {2 AgOH -> Ag2O + H2O}}

(pK = 2.875^[11])

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.^[12]

Structure and properties

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.^[13] It is soluble in ammonia solution, producing active compound of Tollens' reagent. A slurry of Ag₂O is readily attacked by acids:

{\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.^[13]^[14]

Despite the photosensitivity of many silver compounds, silver oxide is not photosensitive,^[15] although it readily decomposes at temperatures above 280 °C.^[16]

Applications

This oxide is used in silver-oxide batteries.^[17] In organic chemistry, silver oxide is used as a mild oxidizing agent.^[18] For example, it oxidizes aldehydes to carboxylic acids.^[19]

References

^ ^a ^b ^c "Silver Oxide MSDS". SaltLakeMetals.com. Salt Lake Metals. Retrieved 2014-06-08.
^ ^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.
^ ^a ^b Perry, Dale L. (1995). Handbook of Inorganic Compounds (illustrated ed.). CRC Press. p. 354. ISBN 0849386713.
^ 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.
^ ^a ^b "Silver oxide".
^ ^a ^b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
^ ^a ^b ^c Sigma-Aldrich Co., Silver(I) oxide. Retrieved on 2014-06-07.
^ O. Glemser and H. Sauer "Silver Oxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1037.
^ Janssen, D. E.; Wilson, C. V. (1963). "4-Iodoveratrole". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 4, p. 547.
^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
^ Biedermann, George; Sillén, Lars Gunnar (1960). "Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag₂O". Acta Chemica Scandinavica. 13: 717–725. doi:10.3891/acta.chem.scand.14-0717.
^ US 20050050990A1, Harigae, Kenichi & Shoji, Yoshiyuki, "Fine-grain silver oxide powder", published 2005-03-10
^ ^a ^b Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry (2nd Ed.). New York:Interscience. p. 1042.
^ General Chemistry by Linus Pauling, 1970 Dover ed. p703-704
^ Herley, P. J.; Prout, E. G. (1960-04-01). "The Thermal Decomposition of Silver Oxide". Journal of the American Chemical Society. 82 (7): 1540–1543. doi:10.1021/ja01492a006. ISSN 0002-7863.
^ Merck Index of Chemicals and Drugs Archived 2009-02-01 at the Wayback Machine, 14th ed. monograph 8521
^ "Duracell PROCELL: The Chemistries: Silver Oxide". 2009-12-20. Archived from the original on 2009-12-20. Retrieved 2024-05-12.
^ 裴, 坚 (2017). 基础有机化学 [Basic Organic Chemistry] (in Chinese) (4th ed.). p. 1064.
^ Chakraborty, Debashis; Gowda, Ravikumar R.; Malik, Payal (2009). "Silver nitrate-catalyzed oxidation of aldehydes to carboxylic acids by H2O2". Tetrahedron Letters. 50 (47): 6553–6556. doi:10.1016/j.tetlet.2009.09.044.

External links

Annealing of Silver Oxide – Demonstration experiment: Instruction and video

[slm-1] "Silver Oxide MSDS". SaltLakeMetals.com. Salt Lake Metals. Retrieved 2014-06-08.

[hand-2] Lide, David R. (1998). Handbook of Chemistry and Physics (81 ed.). Boca Raton, FL: CRC Press. pp. 4–83. ISBN 0-8493-0594-2.

[crc2-3] Perry, Dale L. (1995). Handbook of Inorganic Compounds (illustrated ed.). CRC Press. p. 354. ISBN 0849386713.

[P82db-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.

[chemister-5] "Silver oxide".

[b1-6] Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.

[sigma-7] Sigma-Aldrich Co., Silver(I) oxide. Retrieved on 2014-06-07.

[8] O. Glemser and H. Sauer "Silver Oxide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1037.

[9] Janssen, D. E.; Wilson, C. V. (1963). "4-Iodoveratrole". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 4, p. 547.

[10] Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.

[11] Biedermann, George; Sillén, Lars Gunnar (1960). "Studies on the Hydrolysis of Metal Ions. Part 30. A Critical Survey of the Solubility Equilibria of Ag₂O". Acta Chemica Scandinavica. 13: 717–725. doi:10.3891/acta.chem.scand.14-0717.

[12] US 20050050990A1, Harigae, Kenichi & Shoji, Yoshiyuki, "Fine-grain silver oxide powder", published 2005-03-10

[c_w-13] Cotton, F. Albert; Wilkinson, Geoffrey (1966). Advanced Inorganic Chemistry (2nd Ed.). New York:Interscience. p. 1042.

[pauling-14] General Chemistry by Linus Pauling, 1970 Dover ed. p703-704

[15] Herley, P. J.; Prout, E. G. (1960-04-01). "The Thermal Decomposition of Silver Oxide". Journal of the American Chemical Society. 82 (7): 1540–1543. doi:10.1021/ja01492a006. ISSN 0002-7863.

[merck-16] Merck Index of Chemicals and Drugs Archived 2009-02-01 at the Wayback Machine, 14th ed. monograph 8521

[17] "Duracell PROCELL: The Chemistries: Silver Oxide". 2009-12-20. Archived from the original on 2009-12-20. Retrieved 2024-05-12.

[18] 裴, 坚 (2017). 基础有机化学 [Basic Organic Chemistry] (in Chinese) (4th ed.). p. 1064.

[19] Chakraborty, Debashis; Gowda, Ravikumar R.; Malik, Payal (2009). "Silver nitrate-catalyzed oxidation of aldehydes to carboxylic acids by H2O2". Tetrahedron Letters. 50 (47): 6553–6556. doi:10.1016/j.tetlet.2009.09.044.

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Names
Unit cell
Crystal packing

IUPAC name Silver(I) oxide
Other names Silver rust, Argentous oxide, Silver monoxide
Identifiers
CAS Number	20667-12-3^Y
3D model (JSmol)	Interactive image
ChemSpider	7970393^N
ECHA InfoCard	100.039.946
EC Number	243-957-1
MeSH	silver+oxide
PubChem CID	9794626
RTECS number	VW4900000
UNII	897WUN6G6T^Y
CompTox Dashboard (EPA)	DTXSID40893897
InChI InChI=1S/2Ag.O/q2+1;-2^N Key: NDVLTYZPCACLMA-UHFFFAOYSA-N^N InChI=1S/2Ag.O/q2+1;-2 Key: NDVLTYZPCACLMA-UHFFFAOYSA-N
SMILES [O-2].[Ag+].[Ag+]
Properties
Chemical formula	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]
Solubility in water	0.013 g/L (20 °C) 0.025 g/L (25 °C)^[2] 0.053 g/L (80 °C)^[3]
Solubility product (K_sp) of AgOH	1.52·10⁻⁸ (20 °C)
Solubility	Soluble in acid, alkali Insoluble in ethanol^[2]
Acidity (pK_a)	12.1 (estimated)^[4]
Magnetic susceptibility (χ)	−134.0·10⁻⁶ cm³/mol
Structure
Crystal structure	Cubic
Space group	Pn3m, 224
Thermochemistry
Heat capacity (C)	65.9 J/mol·K^[2]
Std molar entropy (S^⦵₂₉₈)	122 J/mol·K^[6]
Std enthalpy of formation (Δ_fH^⦵₂₉₈)	−31 kJ/mol^[6]
Gibbs free energy (Δ_fG^⦵)	−11.3 kJ/mol^[5]
Hazards
GHS labelling:
Pictograms	^[7]
Signal word	Danger
Hazard statements	H272, H315, H319, H335^[7]
Precautionary statements	P220, P261, P305+P351+P338^[7]
NFPA 704 (fire diamond)	^[1] 2 0 1
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	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). N verify (what is ^YN ?) Infobox references