Silver carbonate

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Silver carbonate
Crystal structure of silver carbonate
Sample of microcrystaline silver carbonate
Names
IUPAC name
Silver(I) carbonate, Silver carbonate
Identifiers
534-16-7 YesY
ChemSpider 83768 YesY
EC Number 208-590-3
Jmol 3D model Interactive image
MeSH silver+carbonate
PubChem 92796
UNII V9WU3IKN4Q N
  • InChI=1S/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 YesY
    Key: KQTXIZHBFFWWFW-UHFFFAOYSA-L YesY
  • InChI=1/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2
    Key: KQTXIZHBFFWWFW-NUQVWONBAD
  • [Ag]OC(=O)O[Ag]
Properties
Ag2CO3
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]
8.46·10−12[1]
Solubility Insoluble in alcohol, liquid ammonia, acetates, acetone[3]
−8.09·10−5 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°
Thermochemistry
112.3 J/mol·K[1]
167.4 J/mol·K[1]
−505.8 kJ/mol[1]
−436.8 kJ/mol[1][4]
Vapor pressure {{{value}}}
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
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.[6] Freshly prepared silver carbonate is colourless, but the solid quickly turns yellow.[7] 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:[7]

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.[6]

References

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External links

Carbonates
H2CO3 He
Li2CO3 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 Uut Fl Uup Lv Uus Uuo
↓
La2(CO3)3 Ce 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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  6. ↑ 6.0 6.1 Lua error in package.lua at line 80: module 'strict' not found.; Lua error in package.lua at line 80: module 'strict' not found.
  7. ↑ 7.0 7.1 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
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