Silver carbonate

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Silver carbonate
Crystal structure of silver carbonate Ag2CO3-bas.png
Crystal structure of silver carbonate
Sample of microcrystaline silver carbonate Silver carbonate.jpg
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 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 208-590-3
MeSH silver+carbonate
PubChem CID
UNII
  • InChI=1S/CH2O3.2Ag/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2 Yes check.svgY
    Key: KQTXIZHBFFWWFW-UHFFFAOYSA-L Yes check.svgY
  • 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
AppearancePale yellow crystals
Odor Odorless
Density 6.077 g/cm3 [1]
Melting point 218 °C (424 °F; 491 K)
decomposes from 120 °C [1] [2]
0.031 g/L (15 °C)
0.032 g/L (25 °C)
0.5 g/L (100 °C) [3]
8.46·10−12 [1]
Solubility Insoluble in ethanol, liquid ammonia, acetates, acetone [4]
−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°
Thermochemistry
112.3 J/mol·K [1]
Std molar
entropy (S⦵298)
167.4 J/mol·K [1]
−505.8 kJ/mol [1]
−436.8 kJ/mol [1] [2]
Hazards
Occupational safety and health (OHS/OSH):
Inhalation hazards
Irritant
GHS labelling: [6]
GHS-pictogram-acid.svg GHS-pictogram-pollu.svg
Danger
H315, H319, H335
P261, P305+P351+P338
NFPA 704 (fire diamond)
[7]
NFPA 704.svgHealth 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) [7]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Silver carbonate is the chemical compound with the formula Ag 2 C O 3. 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.

Contents

Preparation and reactions

Silver carbonate can be prepared by combining aqueous solutions of sodium carbonate with a deficiency of silver nitrate. [8]

2 AgNO3(aq) + Na2CO3(aq) → Ag2CO3(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, 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]

Ag2CO3 → Ag2O + CO2
2 Ag2O → 4 Ag + O2

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]

Ag2CO3 + CH2O → 2 Ag + 2 CO2 + H2

Organic synthesis

Silver carbonate is used as a reagent in organic synthesis. [12] In the Fétizon oxidation, silver carbonate on Celite [13] serves as an oxidising agent to form:

In the Koenigs-Knorr reaction it is used to convert alkyl bromides to the methyl ethers. It is also employed to convert alkyl bromides into alcohols. [8] As a base, it has been used in the Wittig reaction. [14] and in C-H bond activation. [15]

Related Research Articles

<span class="mw-page-title-main">Silver nitrate</span> Chemical compound

Silver nitrate is an inorganic compound with chemical formula AgNO
3. It is a versatile precursor to many other silver compounds, such as those used in photography. It is far less sensitive to light than the halides. It was once called lunar caustic because silver was called luna by ancient alchemists who associated silver with the moon. In solid silver nitrate, the silver ions are three-coordinated in a trigonal planar arrangement.

<span class="mw-page-title-main">Silver(I) fluoride</span> Chemical compound

Silver(I) fluoride is the inorganic compound with the formula AgF. It is one of the three main fluorides of silver, the others being silver subfluoride and silver(II) fluoride. AgF has relatively few niche applications; it has been employed as a fluorination and desilylation reagent in organic synthesis and in aqueous solution as a topical caries treatment in dentistry.

<span class="mw-page-title-main">Cerium(III) chloride</span> Chemical compound

Cerium(III) chloride (CeCl3), also known as cerous chloride or cerium trichloride, is a compound of cerium and chlorine. It is a white hygroscopic salt; it rapidly absorbs water on exposure to moist air to form a hydrate, which appears to be of variable composition, though the heptahydrate CeCl3·7H2O is known. It is highly soluble in water, and (when anhydrous) it is soluble in ethanol and acetone.

<span class="mw-page-title-main">Sodium borohydride</span> Chemical compound

Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate, is an inorganic compound with the formula NaBH4. It is a white crystalline solid, usually encountered as an aqueous basic solution. Sodium borohydride is a reducing agent that finds application in papermaking and dye industries. It is also used as a reagent in organic synthesis.

<span class="mw-page-title-main">Potassium superoxide</span> Chemical compound

Potassium superoxide is an inorganic compound with the formula KO2. It is a yellow paramagnetic solid that decomposes in moist air. It is a rare example of a stable salt of the superoxide anion. It is used as a CO2 scrubber, H2O dehumidifier, and O2 generator in rebreathers, spacecraft, submarines, and spacesuits.

<span class="mw-page-title-main">Silver oxide</span> Chemical compound

Silver oxide is the chemical compound with the formula Ag2O. It is a fine black or dark brown powder that is used to prepare other silver compounds.

Boron trichloride is the inorganic compound with the formula BCl3. This colorless gas is a reagent in organic synthesis. It is highly reactive towards water.

<span class="mw-page-title-main">Potassium hydride</span> Chemical compound

Potassium hydride, KH, is the inorganic compound of potassium and hydrogen. It is an alkali metal hydride. It is a white solid, although commercial samples appear gray. It is a powerful superbase that is useful in organic synthesis. It is sold commercially as a slurry (~35%) in mineral oil or sometimes paraffin wax to facilitate dispensing.

<span class="mw-page-title-main">Silver acetate</span> Chemical compound with formula AgC₂H₃O₂

Silver acetate is a coordination compound with the empirical formula CH3CO2Ag (or AgC2H3O2). A photosensitive, white, crystalline solid, it is a useful reagent in the laboratory as a source of silver ions lacking an oxidizing anion.

<span class="mw-page-title-main">Iron(III) nitrate</span> Chemical compound

Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.

<span class="mw-page-title-main">Silver compounds</span> Chemical compounds containing silver

Silver is a relatively unreactive metal, although it can form several compounds. The common oxidation states of silver are (in order of commonness): +1 (the most stable state; for example, silver nitrate, AgNO3); +2 (highly oxidising; for example, silver(II) fluoride, AgF2); and even very rarely +3 (extreme oxidising; for example, potassium tetrafluoroargentate(III), KAgF4). The +3 state requires very strong oxidising agents to attain, such as fluorine or peroxodisulfate, and some silver(III) compounds react with atmospheric moisture and attack glass. Indeed, silver(III) fluoride is usually obtained by reacting silver or silver monofluoride with the strongest known oxidizing agent, krypton difluoride.

<span class="mw-page-title-main">Nickel(II) nitrate</span> Chemical compound

Nickel nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. In the hexahydrate, the nitrate anions are not bonded to nickel. Other hydrates have also been reported: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O.

<span class="mw-page-title-main">Thiophosphoryl chloride</span> Chemical compound

Thiophosphoryl chloride is an inorganic compound with the chemical formula PSCl3. It is a colorless pungent smelling liquid that fumes in air. It is synthesized from phosphorus chloride and used to thiophosphorylate organic compounds, such as to produce insecticides.

<span class="mw-page-title-main">L-selectride</span> Chemical compound

L-selectride is a organoboron compound with the chemical formula Li[(CH3CH2CH )3BH]. A colorless salt, it is usually dispensed as a solution in THF. As a particularly basic and bulky borohydride, it is used for stereoselective reduction of ketones.

<span class="mw-page-title-main">Silver tetrafluoroborate</span> Chemical compound

Silver tetrafluoroborate is an inorganic compound with the chemical formula AgBF4. It is a white solid, although commercial samples often are gray, that dissolves in polar organic solvents as well as water.

<span class="mw-page-title-main">Silver trifluoromethanesulfonate</span> Chemical compound

Silver trifluoromethanesulfonate, or silver triflate is the triflate (CF3SO3−) salt of Ag+. It is a white or colorless solid that is soluble in water and some organic solvents including, benzene. It is a reagent used in the synthesis of organic and inorganic triflates.

<span class="mw-page-title-main">Vanadyl acetylacetonate</span> Chemical compound

Vanadyl acetylacetonate is the chemical compound with the formula VO(acac)2, where acac– is the conjugate base of acetylacetone. It is a blue-green solid that dissolves in polar organic solvents. The coordination complex consists of the vanadyl group, VO2+, bound to two acac– ligands via the two oxygen atoms on each. Like other charge-neutral acetylacetonate complexes, it is not soluble in water.

Fétizon oxidation is the oxidation of primary and secondary alcohols utilizing the compound silver(I) carbonate absorbed onto the surface of celite also known as Fétizon's reagent first employed by Marcel Fétizon in 1968. It is a mild reagent, suitable for both acid and base sensitive compounds. Its great reactivity with lactols makes the Fétizon oxidation a useful method to obtain lactones from a diol. The reaction is inhibited significantly by polar groups within the reaction system as well as steric hindrance of the α-hydrogen of the alcohol.

<span class="mw-page-title-main">1,2-Bis(dicyclohexylphosphino)ethane</span> Chemical compound

Bis(dicyclohexylphosphino)ethane, abbreviated dcpe, is an organophosphorus compound with the formula (C6H11)2PCH2CH2P(C6H11)2. It is a white solid that is soluble in nonpolar organic solvents. The compound is used as a bulky and highly basic diphosphine ligand in coordination chemistry.

<span class="mw-page-title-main">Bis(benzonitrile)palladium dichloride</span> Chemical compound

Bis(benzonitrile)palladium dichloride is the coordination complex with the formula PdCl2(NCC6H5)2. It is the adduct of two benzonitrile (PhCN) ligands with palladium(II) chloride. It is a yellow-brown solid that is soluble in organic solvents. The compound is a reagent and a precatalyst for reactions that require soluble Pd(II). A closely related compound is bis(acetonitrile)palladium dichloride.

References

  1. 1 2 3 4 5 6 7 8 Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN   978-1-4200-9084-0.
  2. 1 2 Anatolievich, Kiper Ruslan. "silver nitrate". chemister.ru. Retrieved 2014-07-21.
  3. ↑ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York City: D. Van Nostrand Company. p. 605.
  4. ↑ Comey, Arthur Messinger; Hahn, Dorothy A. (February 1921). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 203.
  5. 1 2 3 4 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. ↑ Sigma-Aldrich Co., Silver carbonate. Retrieved on 2021-08-05.
  7. 1 2 "Silver Carbonate MSDS". saltlakemetals.com. Salt Lake City, Utah: Salt Lake Metals. Retrieved 2021-08-05.
  8. 1 2 McCloskey C. M.; Coleman, G. H. (1955). "β-d-Glucose-2,3,4,6-Tetraacetate". Organic Syntheses ; Collected Volumes, vol. 3, p. 434.
  9. 1 2 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
  10. ↑ 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. p. 49. doi:10.1002/14356007.a24_107.pub2. ISBN   9783527306732 . Retrieved 2020-12-24.
  11. ↑ 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.
  12. ↑ 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.
  13. ↑ 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.
  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.
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