Silver carbonate Crystal structure of silver carbonate Sample of microcrystaline silver carbonate Names IUPAC name Silver(I) carbonate
Other namesArgentous carbonate
Identifiers ChemSpider ECHA InfoCard 100.007.811 EC Number MeSH silver+carbonate UNII InChI=1S/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2
Y Key: KQTXIZHBFFWWFW-UHFFFAOYSA-L
Y InChI=1/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2
Key: KQTXIZHBFFWWFW-NUQVWONBAD
Properties Ag2 CO3 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)[ 1] [ 4] 0.031 g/L (15 °C)[ 2] 8.46·10−12 [ 1] Solubility Insoluble inethanol ,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)6 2m, No. 189 (α-form, 476 K)[ 5] 2/m (295 K)6 m2 (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°
Thermochemistry 112.3 J/mol·K[ 1] 167.4 J/mol·K[ 1] −505.8 kJ/mol[ 1] −436.8 kJ/mol[ 1] [ 4] Hazards Occupational safety and health Inhalation hazards
Irritant GHS labelling[ 7] Danger H315, H319, H335 P261, P305+P351+P338 NFPA 704 Lethal dose or concentration (LD, LC):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).
Chemical compound
Silver carbonate is thechemical compound with theformula Ag 2 C O 3 . This salt is yellow but typical samples are grayish due to the presence of elementalsilver . It is poorly soluble in water, like mosttransition metal carbonates .
Preparation and reactions [ edit ] Silver carbonate can be prepared by combining aqueous solutions ofsodium carbonate with a deficiency ofsilver nitrate .[ 8]
2 AgNO3 (aq) + Na2 CO3 (aq) → Ag2 CO3 (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 diamminesilver(I) ([Ag(NH3 )2 ]+ )complex ion . Like other diamminesilver(I) solutions, includingTollen's reagent , there is a possibility that explosiveSilver nitride may precipitate out of the solution. Silver nitride was previously known asfulminating silver but due to confusions withsilver fulminate it has been discontinued by theIUPAC .[ 10]
Withhydrofluoric acid , it givessilver fluoride .
The thermal conversion of silver carbonate to silver metal proceeds via formation of silver oxide:[ 11]
Ag2 CO3 → Ag2 O + CO2 2 Ag2 O → 4 Ag + O2 The principal use of silver carbonate is for the production of silver powder for use in microelectronics. It is reduced withformaldehyde , producing silver free of alkali metals:[ 9]
Ag2 CO3 + CH2 O → 2 Ag + 2 CO2 + H2 Silver carbonate is used as areagent inorganic synthesis .[ 12] Fétizon oxidation , silver carbonate onCelite [ 13] oxidising agent to form:
aldehydes from primary alcohols, ketones from secondary alcohols, keto-alcohols from diols, and ketones from hydroxymethyl compounds. In theKoenigs-Knorr reaction it is used to convert alkyl bromides to the methyl ethers. It is also employed to convertalkyl bromides intoalcohols .[ 8] Wittig reaction .[ 14] [ 15]
^a b c d e f g h Lide, David R., ed. (2009).CRC Handbook of Chemistry and Physics Boca Raton, Florida :CRC Press .ISBN 978-1-4200-9084-0 ^ Seidell, Atherton; Linke, William F. (1919).Solubilities of Inorganic and Organic Compounds New York City : D. Van Nostrand Company. p. 605. ^ Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921).A Dictionary of Chemical Solubilities: Inorganic ^a b Anatolievich, Kiper Ruslan."silver nitrate" .chemister.ru . Retrieved2014-07-21 . ^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 Ag2 CO3 ".Inorganic Chemistry 41 (14):3628– 3637.doi :10.1021/ic0111177 .PMID 12099865 . ^a b "Silver Carbonate MSDS" .saltlakemetals.com .Salt Lake City , Utah: Salt Lake Metals. Retrieved2021-08-05 .^ Sigma-Aldrich Co. ,Silver carbonate . Retrieved on 2021-08-05.^a b McCloskey C. M.; Coleman, G. H. (1955)."β-d-Glucose-2,3,4,6-Tetraacetate" .Organic Syntheses 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 ^ Brumby, Andreas; Braumann, Peter; Zimmermann, Klaus; Brodeck, Francis; Vandevelde, Thierry; Goia, Dan; Renner, Hermann; Schlamp, Gunter; Zimmermann, Klaus; Weise, Wolfgang; Tews, Peter; Dermann, Klaus; Knodler, Alfons; Schroder, Karl-Heinz; Kempf, Bernd; Luschow, Hans; Peter, Cartrin; Schiele, Rainer (2008).Ullmann's Encyclopedia of Industrial Chemistry doi :10.1002/14356007.a24_107.pub2 .ISBN 9783527306732 . Retrieved2020-12-24 . ^ 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 . ^ Ladd, Carolyn L. (2001). "Silver(I) Carbonate".Encyclopedia of Reagents for Organic Synthesis . pp. 1– 10.doi :10.1002/047084289X.rn01865 .ISBN 978-0-470-84289-8 ^ Fétizon, Marcel; Li, Yiming; Jiang, Xuefeng (2017). "Silver(I) Carbonate on Celite".Encyclopedia of Reagents for Organic Synthesis . pp. 1– 19.doi :10.1002/047084289X.rs014.pub2 .ISBN 978-0-470-84289-8 ^ Jedinak, Lukas et al. “Use of Silver Carbonate in the Wittig Reaction.” The Journal of Organic Chemistry 78.23 (2013): 12224–12228https://doi.org/10.1021/jo401972a . ^ J. Org. Chem., 2018, 83 (16), pp 9312–9321https://doi.org/10.1021/acs.joc.8b01284 .
H2 CO3 He Li2 CO3 ,LiHCO3 BeCO3 +BO3 (RO)(R'O)CO +C2 O4 (NH4 )2 CO3 ,NH4 HCO3 ,+NO3 O +F Ne Na2 CO3 ,NaHCO3 ,Na3 H(CO3 )2 MgCO3 ,Mg(HCO3 )2 Al2 (CO3 )3 SiCO4 ,+SiO4 P +SO4 +Cl Ar K2 CO3 ,KHCO3 CaCO3 ,Ca(HCO3 )2 Sc Ti V CrCO3 ,Cr2 (CO3 )3 MnCO3 FeCO3 CoCO3 ,Co2 (CO3 )3 NiCO3 Cu2 CO3 ,CuCO3 ,Cu2 CO3 (OH)2 ZnCO3 Ga Ge As Se Br Kr Rb2 CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh PdCO3 Ag2 CO3 CdCO3 In Sn Sb Te I Xe Cs2 CO3 ,CsHCO3 BaCO3 * Lu2 (CO3 )3 Hf Ta W Re Os Ir Pt Au HgCO3 Tl2 CO3 PbCO3 (BiO)2 CO3 Po(CO3 )2 At Rn Fr RaCO3 ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og * La2 (CO3 )3 Ce2 (CO3 )3 Pr2 (CO3 )3 Nd2 (CO3 )3 Pm Sm2 (CO3 )3 EuCO3 ,Eu2 (CO3 )3 Gd2 (CO3 )3 Tb2 (CO3 )3 Dy2 (CO3 )3 Ho2 (CO3 )3 Er2 (CO3 )3 Tm2 (CO3 )3 Yb2 (CO3 )3 ** Ac Th(CO3 )2 Pa UO2 CO3 Np Pu Am Cm Bk Cf Es Fm Md No
Silver(0,I) Silver(I)
Silver(II) Silver(III) Silver(I,III)
