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SILVER OXIDE ( GÜMÜŞ OKSİT)

SILVER OXIDE (GÜMÜŞ OKSİT)
SYNONYMS
Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; SILVER OXIDE; silver oxide; silver oksit; silver oksid; silver oxide; gümüş silver; silver first grade; silver I oxide; gümüş 1 oksit; gümüş 1 oksid; Gümüş(I) Oksit (Silver oxide); Silver(I) oxide; gümüş 1 oksit; gümüş oxid; gümüş oksid; gümüş oksit; gümüş OKSİT; Argentous oxide; gümüş oksit; gümüş; gümüş okside; okside gümüş; oksitlenmiş gümüş; gümüş; altıngümüş; gumus; gumuskolye; OKSİDE GÜMÜŞ; OKSİTLİ GÜMÜŞ; GÜMÜŞ RAW MATERİAL; silver raw material; gümüş suyu; gümüşokside; gümüş oksid; gümüş oksit; gümüş nitrat; nitrate silver; silver nitrate; silver nitrate; silver oxide; gumus kolye; gumus oksıde; oksıde gümüş; gümüş suyu; gümüşlü su; GÜMÜŞ OKSİT; OKSİT GÜMÜŞ; OKİSDE GÜMÜŞ; GÜMÜŞ OKSİT; GÜMÜŞ OKSİD; GÜMÜŞ OKXID; GÜMÜŞ SUYU; OKSİTLEYİCİ GÜMÜŞ; GUMUS MADEN; GÜMÜS OXIDE; GUMUS OKSID; GÜMÜŞ OKSİT; OKSİTLİ GÜMÜŞ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞ BİLEŞİĞİ; GÜMÜŞLÜ BİLEŞİK; SİLVER GÜMÜŞ; GÜMÜŞ Silver oxide (Ag2O); oxide; Silver(1+) oxide; EINECS 243-957-1; MFCD00003404; Silberoxyd; Silver (I) Oxide; Silver oxide (ous); Silver(I) oxide 99+%; DTXSID40893897; Silver(I) oxide, Electrical Grade; Silver(I) oxide, ReagentPlus(R), 99%; LS-145404; FT-0689128; EC243-957-1; silver(I) oxide, SAJ first grade, >=98.0%; Silver(I) oxide, >=99.99% trace metals basis; Silver(I) oxide, SAJ special grade, >=99.0%; Silver(I) oxide, purum p.a., >=99.0% (AT); Silver oxide; 
For the mixed oxide, see silver(I,III) oxide.
Silver oxide
Silver(I) oxide structure in unit cell
Silver(I) oxide powder
Names
IUPAC name
Silver(I) oxide
Other names
Silver rust, Argentous oxide, Silver monoxide
Identifiers
CAS Number
20667-12-3 ☑
3D model (JSmol)
Interactive image
ChemSpider 
7970393 ☒
ECHA InfoCard 100.039.946
EC Number 
243-957-1
MeSH silver+oxide
PubChem CID
9794626
RTECS number 
VW4900000
CompTox Dashboard (EPA)
DTXSID40893897 Edit this at Wikidata
InChI[show]
SMILES[show]
Properties
Chemical formula
Ag2O

 

Silver(I,III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒ verify (what is ☑☒ ?)
Infobox references
Silver(I) 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.

 

 

Silver(I) oxide produced by reacting lithium hydroxide with a very dilute silver nitrate solution
Silver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide.[7][8] This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:[9]
References

 

 

COMPOUND SUMMARY
Silver(I) oxide
PubChem CID: 88641
Structure: 
Silver(I) oxide_small.png
Find Similar Structures
Chemical Safety: 
Oxidizer Corrosive Irritant Environmental Hazard

 

 

Laboratory Chemical Safety Summary (LCSS) Datasheet
Molecular Formula: Ag2O or Ag2H2O
Synonyms: 
Silver(I) oxide

 

Argentous oxide

Silver oxide (Ag2O)

Disilver oxide

Silver(1+) oxide

 

More...
Molecular Weight: 
233.752 g/mol

 

 

Component Compounds: 
CID 23954 (Silver)

 

CID 962 (Water)

 

Dates: 
Modify:
2020-02-26

 

 

Create:
2005-08-08

 

 

1Structures HelpNew Window
1.12D Structure HelpNew Window
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Chemical Structure Depiction
Silver(I) oxide.png
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PubChem
1.23D Status HelpNew Window
Conformer generation is disallowed since MMFF94s unsupported element, mixture or salt

 

 

PubChem
2Names and Identifiers HelpNew Window
2.1Computed Descriptors HelpNew Window
2.1.1IUPAC Name HelpNew Window
silver;hydrate

 

 

Computed by LexiChem 2.6.6 (PubChem release 2019.06.18)
PubChem
2.1.2InChI HelpNew Window
InChI=1S/2Ag.H2O/h;;1H2

 

 

Computed by InChI 1.0.5 (PubChem release 2019.06.18)
PubChem
2.1.3InChI Key HelpNew Window
VFWRGKJLLYDFBY-UHFFFAOYSA-N

 

 

Computed by InChI 1.0.5 (PubChem release 2019.06.18)
PubChem
2.1.4Canonical SMILES HelpNew Window
O.[Ag].[Ag]

 

 

Computed by OEChem 2.1.5 (PubChem release 2019.06.18)
PubChem
2.2Molecular Formula HelpNew Window
Ag2O

 

 

Wikipedia
Ag2H2O

 

 

Computed by PubChem 2.1 (PubChem release 2019.06.18)
PubChem
2.3Other Identifiers HelpNew Window
2.3.1CAS HelpNew Window
20667-12-3
disilver oxide
silver oxide
Silver(I) oxide
Argentous oxide
Silver oxide (Ag2O)Disilver oxide
Silver(1+) oxide
EINECS 243-957-1
MFCD00003404
Silberoxyd
Silver (I) Oxide
Silver oxide (ous)
Silver(I) oxide 99+%
DTXSID40893897
Silver(I) oxide, Electrical Grade
Silver(I) oxide, ReagentPlus(R), 99%
LS-145404
FT-0689128
EC 243-957-1
Silver(I) oxide, SAJ first grade, >=98.0%
Silver(I) oxide, >=99.99% trace metals basis
Silver(I) oxide, SAJ special grade, >=99.0%
Silver(I) oxide, purum p.a., >=99.0% (AT)

 

 


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4.3Related Compounds HelpNew Window
Mixtures, Components, and Neutralized Forms 2 Records
Similar Compounds 8 Records
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abcr GmbH
PubChem SID: 316389157
Purchasable Chemical: AB101522
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PubChem SID: 329752249
Purchasable Chemical: 221163_SIGALD
Parchem
PubChem SID: 354741468
Purchasable Chemical: 39728
Oakwood Products
PubChem SID: 124391994
Purchasable Chemical: 044724
Finetech Industry Limited
PubChem SID: 164779347
Purchasable Chemical: FT-0689128
VWR, Part of Avantor
PubChem SID: 402327302
Purchasable Chemical: BT219735-10G
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PubChem SID: 374041090
Purchasable Chemical: QB-3344
Glentham Life Sciences Ltd.
PubChem SID: 310280017
Purchasable Chemical: GK1310
3B Scientific (Wuhan) Corp
PubChem SID: 375088015
Purchasable Chemical: 3B4-1532
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6Pharmacology and Biochemistry HelpNew Window
6.1MeSH Pharmacological Classification HelpNew Window
Anti-Infective Agents
Substances that prevent infectious agents or organisms from spreading or kill infectious agents in order to prevent the spread of infection. (See all compounds classified as Anti-Infective Agents.)

 

 


7.3General Manufacturing Information HelpNew Window
Industry Processing Sectors
Organic fiber manufacturing

 

 

About Silver(I) Oxide
Oxide IonSilver(I) Oxide is a highly insoluble thermally stable Silver source suitable for glass, optic and ceramic applications. Silver oxide is a photosensetive fine black powder that decomposes High Purity (99.999%) Silver Oxide (Ag2O)Powderabove 280 °. Oxide compounds are not conductive to electricity. However, certain perovskite structured oxides are electronically conductive finding application in the cathode of solid oxide fuel cells and oxygen generation systems. They are compounds containing at least one oxygen anion and one metallic cation. They are typically insoluble in aqueous solutions (water) and extremely stable making them useful in ceramic structures as simple as producing clay bowls to advanced electronics and in light weight structural components in aerospace and electrochemical applications such as fuel cells in which they exhibit ionic conductivity. Metal oxide compounds are basicanhydrides and can therefore react with acids and with strong reducing agents in redox reactions. Silver Oxide is also available in pellets, pieces, powder, sputtering targets, tablets, and nanopowder (from American Elements' nanoscale production facilities). Silver Oxide is generally immediately available in most volumes. High purity, submicron and nanopowder forms may be considered.Additional technical, research and safety (MSDS) information is available.

 

 

Silver Oxide Nanoparticle Dispersion
Silver Oxide Nanoparticles / Nanopowder
Silver Oxide Pellets
Silver Oxide Rotatable Sputtering Target
Disilver Oxide
Silver Oxide Sputtering Target
Silver Oxide Tablets
Silver Oxide Shot
Silver Oxide Pieces

 

 

See more Silver products. Silver (atomic symbol: Ag, atomic number: 47) is a Block D, Group 11, Period 5 element with an atomic weight of 107.8682. Silver Bohr ModelThe number of electrons in each of Silver's shells is 2, 8, 18, 18, 1 and its electron configuration is [Kr]4d10 5s1. The silver atom has a radius of 144 pm and a Van der Waals radius of 203 pm. Silver was first discovered by Early Man prior to 5000 BC. In its elemental form, silver has a brilliant white metallic luster. Elemental SilverIt is a little harder than gold and is very ductile and malleable, being exceeded only by gold and perhaps palladium. Pure silver has the highest electrical and thermal conductivity of all metals and possesses the lowest contact resistance. It is stable in pure air and water, but tarnishes when exposed to ozone, hydrogen sulfide, or air containing sulfur. It is found in copper, copper-nickel, lead, and lead-zinc ores, among others. Silver was named after the Anglo-Saxon word "seolfor" or "siolfur," meaning 'silver'.
Graphene Oxide/Silver Nanoparticle Coating Produced by Electrophoretic Deposition Improved the Mechanical and Tribological Properties of NiTi Alloy for Biomedical Applications.

 

A visible-light-driven photoelectrochemical molecularly imprinted sensor based on titanium dioxide nanotube arrays loaded with silver iodide nanoparticles for the sensitive detection of benzoyl peroxide.

Methanol Synthesis Using CO₂ and H₂ on Nano Silver-Ceria Zirconia Catalysts: Influence of Preparation Method.

The synergistic enhancement of silver nanocubes and graphene oxide on surface plasmon-coupled emission.

Preparation of silver-loaded titanium dioxide hedgehog-like architecture composed of hundreds of nanorods and its fast response to xylene.

Low diffuse reflection of silver nanowire/ruthenium oxide nanosheet hybrid films for high-performance transparent flexible electrodes.

Plasmonic silvered nanostructures on macroporous silicon decorated with graphene oxide for SERS-spectroscopy.

Zinc oxide/silver bimetallic nanoencapsulated in PVP/PCL nanofibres for improved antibacterial activity.

Photocatalytic mineralization and degradation kinetics of sulphamethoxazole and reactive red 194 over silver-zirconium co-doped titanium dioxide: Reaction mechanisms and phytotoxicity assessment.

Silver-choline chloride modified graphene oxide: Novel nano-bioelectrochemical sensor for celecoxib detection and CCD-RSM model.

 

Silver Oxides
Silver oxide is used as the base in special cases of Suzuki-Miyaura cross-couplings as, for example, in reactions with n-alkylboronic acids ((62)229 and (63)230), including MeB(OH)231,232 -which have been considered as substrates of low nucleophilicity, giving low yields of cross-coupling products under standard conditions.

 

 

Batteries
Balasubramanian Viswanathan, in Energy Sources, 2017

 

 

Silver Oxide-Zinc Battery
A silver oxide battery was introduced in 1902 by Junger, who used a cadmium anode. Andre perfected this battery in 1943 using zinc. The cell representation is:

 

 

Zn|KOH|silver oxide, C, and the cell reaction is Ag2O + 2Zn → 2ZnO +2Ag
The cell is made of gray spongy zinc plates and silver oxide as a cathode material. Cellophane or wetted polypropylene is employed as a separator material. High concentrations of KOH are used as an electrolyte for heavy duty and NaOH is used for long reliability. Additions of Ag2O and MnO2 to the cathode mix result in flat discharge conditions. The battery delivers 1.3-1.5 V during discharge. The battery is costly and is used in ballistic missiles and in the button form in digital watches.

 

 

Volume 7
E. Negishi, in Comprehensive Organometallic Chemistry, 1982

 

 

45.7.4.3 Alkyl Coupling Reactions and Other Radical Reactions of Organoboranes
Alkyldihydroxyboranes react with ammoniacal silver oxide to give alkyl dimers.158 Trialkylboranes react with alkaline silver nitrate either in water or in methanol to undergo similar alkyl coupling reactions159 (equation 117). The alkyl coupling is intermolecular in nature, and an unsymmetrical alkyl dimer (R1R2) may be obtained either from two trialkylboranes (R31B and R32B) or from mixed trialkylboranes (R1R2BX). The use of a large excess of an organoborane containing the less expensive of the two alkyl groups is advantageous in maximizing the yield of a mixed alkyl dimer based on the more expensive alkyl group.159b Although the precise mechanism of the reaction is not clear, the observed results are consistent with a radical mechanism involving organosilver intermediates which decompose via alkyl radicals.

 

 

12.3 Silver Oxide
The oxidation of carbohydrates by silver oxide at 50 °C (in water or potassium hydroxide) and the use of alkaline silver solutions for the detection of spots on paper chromatograms have been summarized in Ref. 1 (p. 1149). That review also describes common uses of the Fétizon reagent (silver carbonate suspended on Celite)193 for oxidizing different types of sugar derivatives. Silver(II) picolinate has been employed as an oxidant for isolated hydroxyl groups;194 with this reagent, 2,3:5,6-di-O-isopropylidene-d-mannofuranose was converted into the corresponding 1,4-lactone, and methyl 6-deoxy-2,3-O-isopropylidene-l-mannofuranoside into the l-lyxo-hexofuransid-5-ulose derivative.

 

 

Batteries
Balasubramanian Viswanathan, in Energy Sources, 2017

 

 

Silver Oxide-Zinc Battery
A silver oxide battery was introduced in 1902 by Junger, who used a cadmium anode. Andre perfected this battery in 1943 using zinc. The cell representation is:

 

 

Zn|KOH|silver oxide, C, and the cell reaction is Ag2O + 2Zn → 2ZnO +2Ag
The cell is made of gray spongy zinc plates and silver oxide as a cathode material. Cellophane or wetted polypropylene is employed as a separator material. High concentrations of KOH are used as an electrolyte for heavy duty and NaOH is used for long reliability. Additions of Ag2O and MnO2 to the cathode mix result in flat discharge conditions. The battery delivers 1.3-1.5 V during discharge. The battery is costly and is used in ballistic missiles and in the button form in digital watches.

 

 

Volume 7
E. Negishi, in Comprehensive Organometallic Chemistry, 1982

 

 

45.7.4.3 Alkyl Coupling Reactions and Other Radical Reactions of Organoboranes
Alkyldihydroxyboranes react with ammoniacal silver oxide to give alkyl dimers.158 Trialkylboranes react with alkaline silver nitrate either in water or in methanol to undergo similar alkyl coupling reactions159 (equation 117). The alkyl coupling is intermolecular in nature, and an unsymmetrical alkyl dimer (R1R2) may be obtained either from two trialkylboranes (R31B and R32B) or from mixed trialkylboranes (R1R2BX). The use of a large excess of an organoborane containing the less expensive of the two alkyl groups is advantageous in maximizing the yield of a mixed alkyl dimer based on the more expensive alkyl group.159b Although the precise mechanism of the reaction is not clear, the observed results are consistent with a radical mechanism involving organosilver intermediates which decompose via alkyl radicals. If the reaction is carried out in CCl4, alkyl chlorides are formed as by-products.159

 

 

(117)
Treatment of boracyclanes, readily obtainable via cyclic hydroboration of dienes, with alkaline silver nitrate produces cycloalkanes.160 Common rings may be obtained in good yields. Even some small and medium rings have been obtained in fair to good yields (equations 118 and 119). Anodic oxidation of trialkylboranes also gives good yields of alkyl dimers.161 Electrolysis of trialkylboranes in acetonitrile162 (equation 120) and nitromethane163 (equation 121) gives homologated nitriles and nitro compounds, respectively.

 

 

(118)
(119)
(120)
(121)
T2
In Bretherick's Handbook of Reactive Chemical Hazards (Eighth Edition), 2017

 

 

TOLLENS' REAGENT
Thu Jun 23 08 16 25 2005

 

 

This mixture of ammoniacal silver oxide and sodium hydroxide solution is potentially dangerous, because if kept for a few hours it deposits an explosive precipitate. This danger was described by Tollens in 1882 but is not generally known now. Prepare the reagent just before use, in the tube to be used for the test, and discard immediately after use, NOT into a container for silver residues [1]. Several earlier references to hazards of storing the reagent before or after use are discussed [2]. On one occasion a violent explosion of the reagent occurred 1 h after preparation and before a precipitate had formed [3], and on another, an empty but unrinsed test tube exploded when picked up [4]. Attempts to recover silver from a batch of the reagent of indeterminate age (!) caused explosions [5]. One hundred and twenty years on, pre-prepared Tollens reagent is still causing explosions [6][7].
See SILVERING SOLUTIONS

 

 

OXIDATIVE REACTIONS AND DEGRADATIONS OF SUGARS AND POLYSACCHARIDES*
Oscar Varela, in Advances in Carbohydrate Chemistry and Biochemistry, 2003

 

 

12.3 Silver Oxide
The oxidation of carbohydrates by silver oxide at 50 °C (in water or potassium hydroxide) and the use of alkaline silver solutions for the detection of spots on paper chromatograms have been summarized in Ref. 1 (p. 1149). That review also describes common uses of the Fétizon reagent (silver carbonate suspended on Celite)193 for oxidizing different types of sugar derivatives. Silver(II) picolinate has been employed as an oxidant for isolated hydroxyl groups;194 with this reagent, 2,3:5,6-di-O-isopropylidene-d-mannofuranose was converted into the corresponding 1,4-lactone, and methyl 6-deoxy-2,3-O-isopropylidene-l-mannofuranoside into the l-lyxo-hexofuransid-5-ulose derivative.

 

 

S2
In Bretherick's Handbook of Reactive Chemical Hazards (Eighth Edition), 2017

 

 

SILVERING SOLUTIONS
Tue Jul 21 11 11 17 1998

 

 

Brashear's silvering solution (alkaline ammoniacal silver oxide containing glucose) or residues therefrom should not be kept for more than 2 hours after preparation, since an explosive precipitate forms on standing [1]. The danger of explosion may be avoided by working with dilute silver solutions (0.35M) in the Brashear process, when formation of Ag(NH3)2OH (and explosive AgNH2 and Ag3N therefrom) is minimized. The use of Rochelle salt, rather than caustic alkali, and shielding of solutions from direct sunlight, are also recommended safeguards [2][3]. Addition of sodium gluconate or tartrate to ammoniacal silver salt-base mixtures inhibits the formation of fulminating silver. 4.7.2 Complexes with some main group and f-elements
Silver derivatives of dialkyl H-phosphonates have been prepared by several methods from silver acetate or silver oxide (1). IR spectroscopic studies of these compounds [411,412] indicate a phosphite-type structure (RO)2P-OAg. Its assignment is based on the disappearance of the absorption bands corresponding to the P-H and P=O stretches in the IR spectra of these derivatives.

 

Silver(I) 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.

 

Preparation
Silver(I) oxide produced by reacting lithium hydroxide with a very dilute silver nitrate solution
Silver(I) oxide produced by reacting lithium hydroxide with a very dilute silver nitrate solution
Silver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide.[7][8] This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:[9]

 

 

2 AgOH → Ag2O + H2O (pK = 2.875[10])
US patent 20050050990 describes the preparation of Ag2O with properties suitable for use as a fine grained conductive paste filler.

 

 

Structure and properties
Ag2O features linear, two-coordinate Ag centers linked by tetrahedral oxides. It is isostructural with Cu2O. It "dissolves" in solvents that degrade it. It is slightly soluble in water due to the formation of the ion Ag(OH)2- and possibly related hydrolysis products.[11] It dissolves in ammonia solution to give soluble derivatives.[citation needed] A slurry of Ag2O is readily attacked by acids:

 

 

Ag2O + 2 HX → 2 AgX + H2O
where HX = HF, HCl, HBr, or HI, HO2CCF3. It will also react with solutions of alkali chlorides to precipitate silver chloride, leaving a solution of the corresponding alkali hydroxide.[11][12]

 

Like many silver compounds, silver oxide is photosensitive. It also decomposes at temperatures above 280 °C.[13]

 

Applications
This oxide is used in silver-oxide batteries. In organic chemistry, silver oxide is used as a mild oxidizing agent. For example, it oxidizes aldehydes to carboxylic acids. Such reactions often work best when the silver oxide is prepared in situ from silver nitrate and alkali hydroxide.

 

Silver oxide

 

Names
IUPAC name
Silver(I) oxide
Other names
Silver rust, Argentous oxide, Silver monoxide
Identifiers 
Silver(I,III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

 

 

Silver Oxide Formation
Let's discuss two ways to create silver oxide. One method happens naturally when elemental silver is in the presence of the oxygen in air. This has to happen at temperatures less than 195° C:

 

4Ag (s) + O2 (g) → 2Ag2 O (s)

The (s) represents solid, and the (g) represents gas.

The second way to produce silver oxide is to react silver nitrate with the strong base sodium hydroxide:

2AgNO3 (aq) + 2NaOH (aq) → Ag2 O (s) + 2NaNO3 (aq) + H2 O (l)

The (aq) represents an aqueous solution, and the (l) represents liquid. In this reaction, the silver oxide is a precipitate, or solid.

 

Silver Oxide Decomposition
The beauty of chemistry is that right after creating silver oxide, you can reverse the reaction. In the previous section we saw that silver oxide is created naturally when elemental silver is exposed to oxygen in the air at temperatures less than 195° C. The question is: Does heating silver oxide at temperatures higher than 195° C mean the silver oxide will decompose into elemental silver and oxygen? The answer is yes!

 

2Ag2 O + heat → 4Ag (s) + O2 (g)

This is the exact reverse of the composition reaction.

 

Silver Oxide Formula
Silver oxide is an ionic compound containing two silver ions and one oxygen ion. But, how does it form? Silver typically loses one electron to form a positively charged ion, Ag+1. Oxygen gains two electrons and becomes a negatively charged ion, O-2. These ions stick together like glue because they're oppositely charged. This makes silver oxide an ionic compound. The formula for silver oxide is Ag2 O. The diagram below shows the electron transfer between silver and oxygen. As you can see, one silver atom gives up an electron resulting in a +1 ion. Each oxygen atom requires two electrons to be stable. This is why two silver atoms are required to bond to oxygen.

 

 

Silver Oxide Uses
Would you have ever guessed that one of the components of some concretes is silver oxide? This interesting molecule is also impregnated in fabrics used in surgery because it has properties that resist the growth of microbes. Silver oxide was also used in batteries in the Apollo spacecraft. Currently, it serves another function, allowing humans to live in environments with no exposure to Earth's atmosphere. Let's learn some details about silver oxide.
Silver oxide

 

 

Molecular FormulaAg2O
Average mass231.736 Da
Monoisotopic mass229.805099 Da
ChemSpider ID7970393

 

 

Our Silver Oxide is new and freshly prepared. The powder has been ground and sifted.
Silver Oxide Properties:
CAS Number: 20667-12-3
Synonyms: Ag2O, Silver(I)Oxide, Argentic Oxide, Silver Monoxide
Formula Weight: 231.74 grams/Mole - (Contains 93.10% Silver)
Density: 7.143
Melting Point: 280°C ( 536°F ) - begins to release Oxygen to form Silver Powder.
Shelf Life: Indefinite when stored in it's original bottle, securely capped.
This is a dry, brownish black powder that does absorb Carbon Dioxide from humid air.
It is best to buy it pre-ground and sifted (like ours).
Silver Oxide is not light sensitive. (as far as ordinary room lighting is concerned)
It is very slightly soluble in water. (.0002g / Liter @ 20°C)
Although not very soluble in water, it imparts a distinctly metallic taste to water.
It is soluble in dilute Nitric Acid.
It is reduced by Hydrogen gas at 100°C ( 212°F ), forming Silver Powder and water.
NOTE: All Metal Oxides form their respective Carbonates when exposed to Carbon Dioxide (in 25%+ humidity).

 

 

silver oxide noun
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Definition of silver oxide
: an oxide of silver
especially : the compound Ag2O obtained as a dark-brown amorphous precipitate when an aqueous solution of a silver salt is treated with a caustic alkali, that reacts as a hydroxide if moist, that dissolves in ammonia water, and that oxidizes aldehydes to acids
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History and Etymology for silver oxide
SILVER entry 1

 

 

Learn More about silver oxide
Share silver oxide

 

Silver usually occurs in the Ag(I) oxidation state in its compounds. It does, however, not always act like simple alkali metal ions, which also carry a single positive charge. Congling Yin, Max Planck Institute for Solid State Research, Stuttgart, Germany, and Guilin University of Technology, China, Martin Jansen, Max Planck Institute for Solid State Research, and colleagues have synthesized a new ternary silver oxide, Ag16B4O10.

 


The compound was obtained in crystalline form via a hydrothermal synthesis starting from elemental Ag and H3BO3. Its structure was analyzed using X-ray diffraction, its electric and magnetic properties were tested, and its bonding situation was studied using density functional theory (DFT) calculations.

 

 


B4O108- is a borate cage anion. This anion is rare, but has a standard bonding situation. It is isolated in the structure of Ag16B4O10, i.e., separated from neighboring anions by octahedrons made up of silver atoms. This has allowed the team to determine the precise structure of this anion for the first time.

 

Most students studying Chemistry would have heard the term oxides where a metal or element reacts with oxygen atoms to form Metal Oxides. Silver Oxide, Ag4O4, is an inorganic compound that is used in silver oxide-zinc alkaline batteries. The preparation of the oxide could be done by adding silver salts slowly into a solution of persulfate for instance AGNO3 to a solution of Na2S2O8.

Once done, it forms a structure that is unusual in nature as it is a compound that has mixed valences. The oxide would decompose once there is an O2 evolution happening in water and forms a solid that has a dark brown appearance. Ag2+ ions with brown appearance are formed when this oxide is dissolved in concentrated nitric acid (HNO3).

 

Structure of Silver Oxide
AgO to be precise is diamagnetic despite the empirical formula showing that silver is in the oxidation state of +2 within the compound. There are two different types of coordination environments as per the studies on X-ray diffraction viz. one with two collinear oxide neighbors and the second with neighbors of four coplanar oxides. The formula for AgO would be Ag2O·Ag2O3 or AgIAgIIIO2.

 

Silver Oxide- Ag4O4

 

How to Prepare
To prepare this oxide, silver powder of 65 grams along with sodium hydroxide of 150 grams in a 1.5-litre aqueous solution is suspended with continuous stirring. The density of the silver powder would be around 1.6 grams per cc (cubic centimeter). The grain size distribution would be around 33 percent under 10 microns to 30 microns, 52 percent under 10 microns, more than 30 microns will be 15%.

 

At 85 degree Celsius the liquid is heated and after reaching this temperature Potassium Peroxidisulfate (K2S2O8) is added in parts of 40 grams each adding up to 200 grams is mixed during intervals of 1 hour at least. At least for 3 hours, the stirring would continue once the final mix of the oxidant is added. Once the product is filtered, it is washed properly so that the alkali substances would be removed from it and it would be reduced into a particle form by drying it at a temperature of around 80 degree Celsius.

 

Applications
Major specialties of the silver oxide thus produced would include low internal discharge, high thermodynamic stability, and the resultant extensive shelf life.
Used in silver oxide batteries.
Used as an oxidizing agent like making carboxylic acid from aldehydes.
To learn more about Silver Oxide and different oxides of different elements, register with Byju's and download our app.
After drying the permeable support is removed and the structure is heated, most suitably in a mufile, at a temperature to convert the oxide to metallic silver. Silver oxide begins to decompose at about 300 C. but the action is more rapid at higher temperatures and presently it is preferred to effect the reduction at about 500 C. The temperature should be below the melting point of silver for if the metallic particles fuse the performance of the electrode will be imparied.

 

The blanks thus produced may be activated at once or later. This is accomplished in the manner known in the art, i.e., by anodic oxidation in an alkaline electrolyte, preferably an aqueous solution of potassium hydroxide.

The finished electrodes are strong and adapted to withstand stresses and shock such as are created in the actuation and operation of missiles.

The invention will be further described in conjunction with a specific example by way of illustration and not by way of limitation.

An 11 cm. Biichner funnel was provided to simulate a sheet mold. The funnel was attached to a filter flask, and a filter paper disk (whatman No. 42, -9 cm.) was placed over the holes in the base of the funnel in the usual manner to prevent .loss of material during processing. The diameter of the final pad was calculated to be approximately 10 square inches.

Four grams of silver oxide (Ag O) were placed in a Waring blender with a small quantity of Water, mixed for several minutes, and poured into the funnel, which was under vacuum. After this initial layer had been deposited, a 40 mesh nickel screen disk was placed thereon. Then 10 grams of silver oxide were mixed in the blender with a small quantity of water and poured into the funnel, again under vacuum. Thereupon, the mat was removed and pressed at 200 pounds pressure on a Williams press to decrease the residual moisture content of the pad. It was then pressed on a Denison press at 6 tons (1%" ram). The pressed structure was dried four hours at 65 C. Thereafter, the filter paper was removed and the structure was placed in a mufiie furnace and held at 500 C. for one hour to reduce the oxide to silver. Visual inspection of the resulting unit showed no surface cracks. It was also found to be sufficiently pliable to bend back somewhat and forth without cracking or flaking. Aanalysis of the structure showed that the distribution of the silver on each side of the grid was essentially uniform. It was also found that the distribution through the grid was uniform.

From the foregoing example, it is evident that this process is a rapid and economical way of producing these electrodes. It will be noted that the top layer of the electrode was prepared, or deposited, with an amount of the silver oxide that was about 71 percent of the total. It is of primary consequence that the second slurry contain from 2 /2 to 4 times as much silver oxide as the first slurry.

It will be noted from the foregoing example that the silver oxide slurry was prepared using water as the slurry medium. However, other inert liquids can be used as well, though water normally will be used in view of the economics involved. Similarly, silver peroxide can beused in place of the Ag O in practice of the invention.

In addition to the advantages already stated, electrodes produced in accordance with my invention are further advantageous in that the internal electrical resistance will be less than those produced in which an inert binder is necessary.

The process can be adapted for continuous operation. By using a continuous paper machine, a first layer of oxide can be deposited on a continuous filter paper base. Then the resulting deposit is covered with a grid after which asecond, or top, layer is deposited. In one run, approximately 4 feet of material were processed. It was found that distribution of the oxide across and through the grid was excellent and that the deposit per sq. inch of the material was in the vicinity of 1.3 grams.

It will be appreciated that this invention can be applied to the formation of electrodes other than those of silver oxide, where thermal reduction is practiced to provide the elemental material so that bonding can be achieved by means of pressure. It will also be appreciated that the grid material can be any material that is compatible with the material to be carried by it, and which has sufficient conductive properties for electrode applications. As indicated above, the screen should range from to 60 mesh of wire that is standard for those mesh sizes. The actual quantity of active material applied to any grid is largely dependent on the grid mesh size, because a larger grid can accommodate more material per unit of surface than could a smaller grid.

The silver-grid-silver structures produced in accordance with this invention can be used in primary or secondary cells and batteries, suitably with zinc negative electrodes.

In accordance with the provisions of the patent statutes, I have explained the principle of my invention and have described what I now consider to represent its best embodiment. However, I desire to have it understood that within the scope of the appended claims, the invention may be practiced otherwise than as specifically described.

I claim:

1. In a method of making a silver oxide electrode the steps comprising applying a first slurry of silver oxide to a porous support while applying vacuum thereto to withdraw liquid therefrom and form a substantially uniform layer of silver oxide on said support, applying an electrically conductive screen to the surface of said layer, applying a second silver oxide slurry to the exposed surface of said screen while applying vacuum to said support to withdraw liquid from the thus deposited silver oxide and form a substantially uniform layer of it on said screen, said first slurry containing from about 0.25 to 1.5 grams of silver oxide per square inch of said screen surface area, and said second slurry containing from 2.5 to 4 times as much silver oxide by weight as in said first slurry, applying pressure to the article to reduce its moisture content and compact said layers, and then heating at a temperature below C.

2. A method according to claim 1, said screen being of 30 to 40 mesh size.

3. A method according to claim 2,. said screen being of silver coated nickel.

4. In a method of making a silver oxide electrode the steps comprising applying a first slurry of silver oxide to a porous support while applying vacuum thereto to withdraw liquid therefrom and form a substantially uni:

form layer of silver oxide on said support, applying an.

electrically conductive screen to the surface of said layer, applying a second silver oxide slurry to the exposed surface of said screenwhile applying vacuum to said support to withdraw liquid from the thus deposited silver oxide and form a substantially uniform layer of it on said screen, said first slurry containing from about 0.25 to 1.5 grams of silver oxide per square inch of said screen surface area, and said second slurry containing from 2.5 to 4 times as much silver oxide by weight as in said first slurry, applying pressure to the dried article to reduce its water content and compact said layers, drying the resultant structure at a temperature below 100 C., removing said porous support, and then heating in a muflie to a temperature below the melting point of silver to convert the silver oxide to metallic silver.

5. That method of making a silver oxide electrode comprising the steps of applying a firstslurry of silver oxide to a porous support while applying vacuum thereto to withdraw liquid therefrom and form a substantially uniform layer of silver oxide on said support applying an electrically conductive screen to the surface of said layer, applying a second silver oxide slurry to the exposed surface of said screen while applying vacuum to said support to withdraw liquid from the thus deposited.

of silver to convert the silver oxide to metallic silver,

and anodically oxidizing the silver to silver oxide in an alkaline electrolyte.

6. A method according to claim 5, said screen;being of 30 to 40 mesh size.

 

7. A method according to claim 6, said screenbeing of silver coated nickel.
Gümüş Oksit 100 GR• CAS No: 20667-12-3

 

• Formül: Ag2O

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