Silver carbonate

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Silver carbonate
Crystal structure of silver carbonate
Sample of microcrystaline silver carbonate
Names
IUPAC name
Silver(I) carbonate
Other names
Argentous carbonate
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.007.811 Edit this at Wikidata
EC Number
  • 208-590-3
MeSH silver+carbonate
UNII
  • InChI=1S/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 checkY
    Key: KQTXIZHBFFWWFW-UHFFFAOYSA-L checkY
  • 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
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]
8.46·10−12[1]
Solubility Insoluble in
liquid ammonia, acetates, acetone[3]
−80.9·10−6 cm3/mol[1]
Structure
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]
Std enthalpy of
formation
(ΔfH⦵298)
 −505.8 kJ/mol[1]
−436.8 kJ/mol[1][4]
Hazards
Occupational safety and health (OHS/OSH):
Inhalation hazards
 Irritant
GHS labelling:[7]
GHS05: Corrosive GHS09: Environmental hazard
Danger
H315, H319, H335
P261, P305+P351+P338
NFPA 704 (fire diamond)
[6]
NFPA 704 four-colored diamondHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
0
0
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).
☒N verify (what is checkY☒N ?)

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]

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]+)

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]

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]

Organic synthesis

Silver carbonate is used as a

oxidising agent
to form

aldehydes from primary alcohols
ketones from secondary alcohols
keto-alcohols from diols
ketones from hydroxymethyl compounds

In the

alkyl bromides into alcohols.[8] As a base, it has been used in the Wittig reaction.[14] and in C-H bond activation.[15]

References

  1. ^
    ISBN 978-1-4200-9084-0
    .
  2. ^ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. p. 605.
  3. ^ Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203.
  4. ^ a b Anatolievich, Kiper Ruslan. "silver nitrate". chemister.ru. Retrieved 2014-07-21.
  5. ^
    PMID 12099865
    .
  6. ^ a b "Silver Carbonate MSDS". saltlakemetals.com. Salt Lake City, Utah: Salt Lake Metals. Retrieved 2021-08-05.
  7. ^ Sigma-Aldrich Co., Silver carbonate. Retrieved on 2021-08-05.
  8. ^ 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.
  9. ^
    doi:10.1002/14356007.a24_107.pub2
  10. ISBN 9783527306732
    . Retrieved 2020-12-24.
  11. doi:10.1021/jp309655s
    .
  12. ISBN 978-0-470-84289-8
    .
  13. ISBN 978-0-470-84289-8
    .
  14. ^ 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.
  15. ^ J. Org. Chem., 2018, 83 (16), pp 9312–9321 https://doi.org/10.1021/acs.joc.8b01284.

External links

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