Silver carbonate

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Silver carbonate
Ag2CO3-bas.png
Silver carbonate.jpg
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 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.

Contents

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]+) 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]

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

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

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

Solubility equilibrium is a type of dynamic equilibrium that exists when a chemical compound in the solid state is in chemical equilibrium with a solution of that compound. The solid may dissolve unchanged, with dissociation, or with chemical reaction with another constituent of the solution, such as acid or alkali. Each solubility equilibrium is characterized by a temperature-dependent solubility product which functions like an equilibrium constant. Solubility equilibria are important in pharmaceutical, environmental and many other scenarios.

<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">Sodium percarbonate</span> Chemical compound

Sodium percarbonate, or sodium carbonate peroxide is a chemical substance with formula Na
2H
3CO
6. It is an adduct of sodium carbonate and hydrogen peroxide whose formula is more properly written as 2 Na
2CO
3 · 3 H
2O
2. It is a colorless, crystalline, hygroscopic and water-soluble solid. It is sometimes abbreviated as SPC. It contains 32.5% by weight of hydrogen peroxide.

<span class="mw-page-title-main">Silver chloride</span> Chemical compound with the formula AgCl

Silver chloride is a chemical compound with the chemical formula AgCl. This white crystalline solid is well known for its low solubility in water and its sensitivity to light. Upon illumination or heating, silver chloride converts to silver, which is signaled by grey to black or purplish coloration in some samples. AgCl occurs naturally as a mineral chlorargyrite.

<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.

In organometallic chemistry, acetylide refers to chemical compounds with the chemical formulas MC≡CH and MC≡CM, where M is a metal. The term is used loosely and can refer to substituted acetylides having the general structure RC≡CM. Acetylides are reagents in organic synthesis. The calcium acetylide commonly called calcium carbide is a major compound of commerce.

<span class="mw-page-title-main">Tollens' reagent</span> Chemical reagent used to distinguish between aldehydes and ketones

Tollens' reagent is a chemical reagent used to distinguish between aldehydes and ketones along with some alpha-hydroxy ketones which can tautomerize into aldehydes. The reagent consists of a solution of silver nitrate, ammonium hydroxide and some sodium hydroxide. It was named after its discoverer, the German chemist Bernhard Tollens. A positive test with Tollens' reagent is indicated by the precipitation of elemental silver, often producing a characteristic "silver mirror" on the inner surface of the reaction vessel.

<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">Potassium fluoride</span> Ionic compound (KF)

Potassium fluoride is the chemical compound with the formula KF. After hydrogen fluoride, KF is the primary source of the fluoride ion for applications in manufacturing and in chemistry. It is an alkali halide salt and occurs naturally as the rare mineral carobbiite. Solutions of KF will etch glass due to the formation of soluble fluorosilicates, although HF is more effective.

<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.

<span class="mw-page-title-main">Phosphorus pentasulfide</span> Chemical compound

Phosphorus pentasulfide is the inorganic compound with the formula P2S5 (empirical) or P4S10 (molecular). This yellow solid is the one of two phosphorus sulfides of commercial value. Samples often appear greenish-gray due to impurities. It is soluble in carbon disulfide but reacts with many other solvents such as alcohols, DMSO, and DMF.

<span class="mw-page-title-main">Sodium dichromate</span> Inorganic compound

Sodium dichromate is the inorganic compound with the formula Na2Cr2O7. However, the salt is usually handled as its dihydrate Na2Cr2O7·2H2O. Virtually all chromium ore is processed via conversion to sodium dichromate and virtually all compounds and materials based on chromium are prepared from this salt. In terms of reactivity and appearance, sodium dichromate and potassium dichromate are very similar. The sodium salt is, however, around twenty times more soluble in water than the potassium salt (49 g/L at 0 °C) and its equivalent weight is also lower, which is often desirable.

<span class="mw-page-title-main">Triflic acid</span> Chemical compound

Triflic acid, the short name for trifluoromethanesulfonic acid, TFMS, TFSA, HOTf or TfOH, is a sulfonic acid with the chemical formula CF3SO3H. It is one of the strongest known acids. Triflic acid is mainly used in research as a catalyst for esterification. It is a hygroscopic, colorless, slightly viscous liquid and is soluble in polar solvents.

<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">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.

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">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.

In organic chemistry, methylenation is a chemical reaction that inserts a methylene group into a chemical compound:

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 .; Collective Volume, 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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