Chemistry:Silver carbonate
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| Names | |
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| IUPAC name
Silver(I) carbonate
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| Other names
Argentous carbonate
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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| MeSH | silver+carbonate |
PubChem CID
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| UNII | |
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| Properties | |
| 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][4] |
| 0.031 g/L (15 °C) 0.032 g/L (25 °C) 0.5 g/L (100 °C)[2] | |
Solubility product (Ksp)
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8.46·10−12[1] |
| Solubility | Insoluble in alcohol, liquid ammonia, acetates, acetone[3] |
| −80.9·10−6 cm3/mol[1] | |
| Structure | |
| Monoclinic, mP12 (295 K) Trigonal, hP36 (β-form, 453 K) Hexagonal, hP18 (α-form, 476 K)[5] | |
| P21/m, No. 11 (295 K) P31c, No. 159 (β-form, 453 K) P62m, No. 189 (α-form, 476 K)[5] | |
| 2/m (295 K) 3m (β-form, 453 K) 6m2 (α-form, 476 K)[5] | |
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°
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| Thermochemistry | |
Heat capacity (C)
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112.3 J/mol·K[1] |
Std molar
entropy (S |
167.4 J/mol·K[1] |
Std enthalpy of
formation (ΔfH⦵298) |
−505.8 kJ/mol[1] |
Gibbs free energy (ΔfG˚)
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−436.8 kJ/mol[1][4] |
| Hazards | |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H315, H319, H335 | |
| P261, P305+351+338 | |
| Inhalation hazard | Irritant |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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3.73 g/kg (mice, oral)[6] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Silver carbonate is the chemical compound with the formula Ag2CO3. This salt 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]
- [math]\ce{ 2 AgNO3(aq) + Na2CO3(aq) -> Ag2CO3(s) + 2 NaNO3(aq) }[/math]
Freshly prepared silver carbonate is colourless, but the solid quickly turns yellow.[9]
Silver carbonate reacts with ammonia to give the diamminesilver(I) ([Ag(NH3)2]+) complex ion. Like other diamminesilver(I) solutions, including Tollen's reagent, there is a possibility that explosive Silver nitride may precipitate out of the solution. Silver nitride was previously known as fulminating silver but due to confusions with silver fulminate it has been discontinued by the IUPAC.[10]
With hydrofluoric acid, it gives silver fluoride.
The thermal conversion of silver carbonate to silver metal proceeds via formation of silver oxide:[11]
- [math]\ce{ Ag2CO3 -> Ag2O + CO2 }[/math]
- [math]\ce{ 2 Ag2O ->4 Ag + O2 }[/math]
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]
- [math]\ce{ Ag2CO3 + CH2O -> 2 Ag + 2 CO2 + H2 }[/math]
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 keto alcohols from diols. It is also employed to convert alkyl bromides into alcohols.[8] As a base, it has been used in the Wittig reaction.[12] and in C-H bond activation.[13]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 1.7 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 City: D. Van Nostrand Company. p. 605. https://archive.org/details/solubilitiesino01seidgoog.
- ↑ Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203. https://archive.org/details/in.ernet.dli.2015.163725.
- ↑ 4.0 4.1 Anatolievich, Kiper Ruslan. "silver nitrate". http://chemister.ru/Database/properties-en.php?dbid=1&id=2374. Retrieved 2014-07-21.
- ↑ 5.0 5.1 5.2 5.3 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): 3628–3637. doi:10.1021/ic0111177. PMID 12099865.
- ↑ 6.0 6.1 "Silver Carbonate MSDS". Salt Lake Metals. http://www.saltlakemetals.com/MSDS_Silver_Carbonate.htm. Retrieved 2021-08-05.
- ↑ Sigma-Aldrich Co., Silver carbonate. Retrieved on 2021-08-05.
- ↑ 8.0 8.1 McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=cv3p0434.; Collective Volume, 3, pp. 434
- ↑ 9.0 9.1 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
- ↑ Brumby, Andreas; Braumann, Peter; Zimmermann, Klaus; Brodeck, Francis; Vandevelde, Thierry; Goia, Dan; Renner, Hermann; Schlamp, Gunter et al. (2008). Ullmann's Encyclopedia of Industrial Chemistry. p. 49. doi:10.1002/14356007.a24_107.pub2. ISBN 9783527306732. https://onlinelibrary.wiley.com/doi/10.1002/14356007.a24_107.pub2. Retrieved 2020-12-24.
- ↑ 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 https://doi.org/10.1021/jo401972a.
- ↑ J. Org. Chem., 2018, 83 (16), pp 9312–9321 https://doi.org/10.1021/acs.joc.8b01284.
External links
| H2CO3 | He | ||||||||||||||||
| Li2CO3, LiHCO3 |
BeCO3 | B | C | (NH4)2CO3, NH4HCO3 |
O | F | Ne | ||||||||||
| Na2CO3, NaHCO3, Na3H(CO3)2 |
MgCO3, Mg(HCO3)2 |
Al2(CO3)3 | Si | P | S | Cl | Ar | ||||||||||
| K2CO3, KHCO3 |
CaCO3, Ca(HCO3)2 |
Sc | Ti | V | Cr | MnCO3 | FeCO3 | CoCO3 | NiCO3 | CuCO3 | ZnCO3 | Ga | Ge | As | Se | Br | Kr |
| Rb2CO3 | SrCO3 | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag2CO3 | CdCO3 | In | Sn | Sb | Te | I | Xe |
| Cs2CO3, CsHCO3 |
BaCO3 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl2CO3 | PbCO3 | (BiO)2CO3 | Po | At | Rn | |
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La2(CO3)3 | Ce2(CO3)3 | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | Th | Pa | UO2CO3 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
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