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
Molar mass	275.75 g/mol
Appearance	Pale yellow crystals
Odor	Odorless
Density	6.077 g/cm3[1]
Melting point	218 °C (424 °F; 491 K) ; decomposes from 120 °C[1][2]
Solubility in water	0.031 g/L (15 °C); 0.032 g/L (25 °C); 0.5 g/L (100 °C)[3]
Solubility product (Ksp)	8.46·10−12[1]
Solubility	Insoluble in alcohol, liquid ammonia, acetates, acetone[4]
Magnetic susceptibility (χ)	−80.9·10−6 cm3/mol[1]
Structure
Crystal structure	Monoclinic, mP12 (295 K); Trigonal, hP36 (β-form, 453 K); Hexagonal, hP18 (α-form, 476 K)[5]
Space group	P21/m, No. 11 (295 K); P31c, No. 159 (β-form, 453 K); P62m, No. 189 (α-form, 476 K)[5]
Point group	2/m (295 K); 3m (β-form, 453 K); 6m2 (α-form, 476 K)[5]
Lattice constant	a = 4.8521(2) Å, b = 9.5489(4) Å, c = 3.2536(1) Å (295 K)[5] α = 90°, β = 91.9713(3)°, γ = 90°
Thermochemistry
Heat capacity (C)	112.3 J/mol·K[1]
Std molar; entropy (So298)	167.4 J/mol·K[1]
Std enthalpy of; formation (ΔfH⦵298)	−505.8 kJ/mol[1]
Gibbs free energy (ΔfG˚)	−436.8 kJ/mol[1][2]
Hazards
GHS pictograms	[6]
GHS Signal word	Warning
GHS hazard statements	H315, H319, H335[6]
GHS precautionary statements	P261, P305+351+338[6]
Inhalation hazard	Irritant
NFPA 704 (fire diamond)	[7] 0 0 0
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	3.73 g/kg (mice, oral)[7]
	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 and reactions

Silver carbonate can be prepared by combining aqueous solutions of sodium carbonate with a deficiency of silver nitrate.[8]

2 AgNO₃(aq) + Na₂CO₃(aq) → Ag₂CO₃(s) + 2 NaNO₃(aq)

Freshly prepared silver carbonate is colourless, but the solid quickly turns yellow.[9]

Silver carbonate reacts with ammonia to give the explosive fulminating silver. With hydrofluoric acid, it gives silver fluoride. The thermal conversion of silver carbonate to silver metal proceeds via formation of silver oxide:[10]

Ag₂CO₃ → Ag₂O + CO₂

2 Ag₂O → 4 Ag + O₂

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]

2 Ag₂CO₃ + CH₂O → 2 Ag + 3 CO₂ + H₂O

Silver carbonate is used as a reagent in organic synthesis such as the Koenigs-Knorr reaction. In the Fétizon oxidation, silver carbonate on celite serves as an oxidising agent to form lactones from diols. It is also employed to convert alkyl bromides into alcohols.[8] As a base, it has been used in the Wittig reaction.[11] and in C-H bond activation.[12]

gollark: If they are to be consumed at any point, then they were retroactively unsentient, obviously*.

gollark: This is only for purposes.

gollark: Krasimir Angelov is, legally, my alt.

gollark: ++choose lemon cryoapioform

gollark: ++choose helloboi palaiologos gollark/heav

References

Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
Anatolievich, Kiper Ruslan. "silver nitrate". http://chemister.ru. Retrieved 2014-07-21. External link in |website= (help)
Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. p. 605.
Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203.
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-Aldrich Co., Silver carbonate. Retrieved on 2014-05-06.
"Silver Carbonate MSDS". http://www.saltlakemetals.com. Salt Lake City, Utah: Salt Lake Metals. Retrieved 2014-06-08. External link in |website= (help)
McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses.; Collective Volume, 3, p. 434
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
Koga, Nobuyoshi; Shuto Yamada; Tomoyasu Kimura (2013). "Thermal Decomposition of Silver Carbonate: Phenomenology and Physicogeometrical Kinetics". The Journal of Physical Chemistry C. 117: 326–336. doi:10.1021/jp309655s.
Jedinak, Lukas et al. “Use of Silver Carbonate in the Wittig Reaction.” The Journal of Organic Chemistry 78.23 (2013): 12224–12228.
J. Org. Chem., 2018, 83 (16), pp 9312–9321 DOI: 10.1021/acs.joc.8b01284. .

External links

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[crc-1] Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.

[chemister-2] Anatolievich, Kiper Ruslan. "silver nitrate". http://chemister.ru. Retrieved 2014-07-21. External link in |website= (help)

[sioc-3] Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. p. 605.

[doc00-4] Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203.

[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. External link in |website= (help)

[OS-8] McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses.; Collective Volume, 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

[10] Koga, Nobuyoshi; Shuto Yamada; Tomoyasu Kimura (2013). "Thermal Decomposition of Silver Carbonate: Phenomenology and Physicogeometrical Kinetics". The Journal of Physical Chemistry C. 117: 326–336. doi:10.1021/jp309655s.

[11] Jedinak, Lukas et al. “Use of Silver Carbonate in the Wittig Reaction.” The Journal of Organic Chemistry 78.23 (2013): 12224–12228.

[12] J. Org. Chem., 2018, 83 (16), pp 9312–9321 DOI: 10.1021/acs.joc.8b01284. .