Silver carbonate

Silver carbonate

Names
IUPAC name Silver(I) carbonate, Silver carbonate
Identifiers
CAS Number	534-16-7 Y
3D model (Jmol)	Interactive image
ChemSpider	83768 Y
ECHA InfoCard	100.007.811
EC Number	208-590-3
MeSH	silver+carbonate
PubChem	92796
UNII	V9WU3IKN4Q N
InChI 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
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)	−80.9·10−6 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
Specific heat capacity (C)	112.3 J/mol·K
Std molar entropy (So298)	167.4 J/mol·K
Std enthalpy of formation (ΔfHo298)	−505.8 kJ/mol
Gibbs free energy (ΔfG˚)	−436.8 kJ/mol
Hazards
GHS pictograms
GHS signal word	Warning
GHS hazard statements	H315, H319, H335
GHS precautionary statements	P261, P305+351+338
EU classification (DSD)	Xi
R-phrases	R36/37/38
S-phrases	S26, S36
Inhalation hazard	Irritant
NFPA 704	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).
N  (what is YN ?)
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.

Silver carbonate can be easily prepared by combining aqueous solutions of sodium carbonate with a deficiency of silver nitrate. Freshly prepared silver carbonate is colourless, but the solid quickly turns yellow. It reacts with ammonia to give the explosive silver fulminate.

With hydrofluoric acid, it gives silver fluoride.

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:

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.