Silver carbonate

Silver carbonate
Names
	IUPAC name Silver(I) carbonate, Silver carbonate
Identifiers
CAS Number	534-16-7 ;
3D model (JSmol)	Interactive image;
ChemSpider	83768 ;
ECHA InfoCard	100.007.811
EC Number	208-590-3;
MeSH	silver+carbonate
PubChem CID	92796;
UNII	V9WU3IKN4Q ;
CompTox Dashboard (EPA)	DTXSID9042384 ;
	InChI InChI=1S/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2+1/p-2 Key: KQTXIZHBFFWWFW-UHFFFAOYSA-L ; InChI=1/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2+1/p-2 Key: KQTXIZHBFFWWFW-NUQVWONBAD;
	SMILES [Ag]OC(=O)O[Ag];
Properties
Chemical formula	Ag2CO3
Appearance	Pale yellow crystals
Odor	Odorless
Density	6.077 g/cm3
Melting point	218 °C (424 °F; 491 K) ; decomposes from 120 °C
Solubility in water	0.031 g/L (15 °C); 0.032 g/L (25 °C); 0.5 g/L (100 °C)
Solubility product (Ksp)	8.46·10−12
Solubility	Insoluble in alcohol, liquid ammonia, acetates, acetone
Magnetic susceptibility (χ)	−8.09·10−5 cm3/mol
Structure
Crystal structure	Monoclinic, mP12 (295 K); Trigonal, hP36 (β-form, 453 K); Hexagonal, hP18 (α-form, 476 K)
Space group	P21/m, No. 11 (295 K); P31c, No. 159 (β-form, 453 K); P62m, No. 189 (α-form, 476 K)
Point group	2/m (295 K); 3m (β-form, 453 K); 6m2 (α-form, 476 K)
Lattice constant	a = 4.8521(2) Å, b = 9.5489(4) Å, c = 3.2536(1) Å (295 K) α = 90°, β = 91.9713(3)°, γ = 90°
Thermochemistry
Heat capacity (C)	112.3 J/mol·K
Std molar; entropy (S⦵298)	167.4 J/mol·K
Std enthalpy of; formation (ΔfH⦵298)	−505.8 kJ/mol
Gibbs free energy (ΔfG⦵)	−436.8 kJ/mol
Hazards
	Occupational safety and health (OHS/OSH):
Inhalation hazards	Irritant
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H315, H319, H335
Precautionary statements	P261, P305+P351+P338
NFPA 704 (fire diamond)	0 0 0
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	3.73 g/kg (mice, oral)
	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 carbonate is the chemical compound with the formula Ag₂CO₃. Silver carbonate is yellow but typical samples are grayish due to the presence of elemental silver. It is poorly soluble in water, like most transition metal carbonates.

Preparation

Silver carbonate can be easily prepared by combining aqueous solutions of sodium carbonate with a deficiency of silver nitrate.^[8] Freshly prepared silver carbonate is colourless, but the solid quickly turns yellow.^[9] It reacts with ammonia to give the explosive silver fulminate. With hydrofluoric acid, it gives silver fluoride.

Uses

The principal use of silver carbonate is for the production of silver powder for use in microelectronics. It is reduced with formaldehyde, producing silver free of alkali metals:^[9]

Ag₂CO₃ + CH₂O → 2 Ag + 2 CO₂ + H₂

Silver carbonate is used as a reagent in organic synthesis such as the Koenigs-Knorr reaction. In the Fétizon oxidation, silver carbonate on celite acts as an oxidising agent to form lactones from diols. It is also employed to convert alkyl bromides into alcohols.^[8]

References

^ ^a ^b ^c ^d ^e ^f ^g ^h Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 605.
^ Comey, Arthur Messinger; Hahn, Dorothy A. (1921-02). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203. {{cite book}}: Check date values in: |date= (help)
^ ^a ^b Anatolievich, Kiper Ruslan. "silver nitrate". http://chemister.ru. Retrieved 2014-07-21. {{cite web}}: External link in |website= (help)
^ ^a ^b ^c ^d Norby, P.; Dinnebier, R.; Fitch, A.N. (2002). "Decomposition of Silver Carbonate; the Crystal Structure of Two High-Temperature Modifications of Ag₂CO₃". Inorganic Chemistry. 41 (14). doi:10.1021/ic0111177.
^ ^a ^b ^c Sigma-Aldrich Co., Silver carbonate. Retrieved on 2014-05-06.
^ ^a ^b "Silver Carbonate MSDS". http://www.saltlakemetals.com. Salt Lake City, Utah: Salt Lake Metals. Retrieved 2014-06-08. {{cite web}}: External link in |website= (help)
^ ^a ^b McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 3, p. 434.
^ ^a ^b Andreas Brumby et al. "Silver, Silver Compounds, and Silver Alloys" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2008. doi:10.1002/14356007.a24_107.pub2

External links

[crc-1] ^ ^a ^b ^c ^d ^e ^f ^g ^h Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.

[sioc-2] Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 605.

[doc00-3] Comey, Arthur Messinger; Hahn, Dorothy A. (1921-02). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203. {{cite book}}: Check date values in: |date= (help)

[chemister-4] Anatolievich, Kiper Ruslan. "silver nitrate". http://chemister.ru. Retrieved 2014-07-21. {{cite web}}: External link in |website= (help)

[rsc-5] Norby, P.; Dinnebier, R.; Fitch, A.N. (2002). "Decomposition of Silver Carbonate; the Crystal Structure of Two High-Temperature Modifications of Ag₂CO₃". Inorganic Chemistry. 41 (14). doi:10.1021/ic0111177.

[sigma-6] Sigma-Aldrich Co., Silver carbonate. Retrieved on 2014-05-06.

[slm-7] "Silver Carbonate MSDS". http://www.saltlakemetals.com. Salt Lake City, Utah: Salt Lake Metals. Retrieved 2014-06-08. {{cite web}}: External link in |website= (help)

[OS-8] McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 3, p. 434.

[Ull-9] Andreas Brumby et al. "Silver, Silver Compounds, and Silver Alloys" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2008. doi:10.1002/14356007.a24_107.pub2

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