SILVER OXIDE

SILVER OXIDE
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.

CAS Number:20667-12-3
EC Number:243-957-1

IUPAC names:
alpha-chaconine
disilver oxid
Disilver Oxide
Disilver oxide
disilver oxide
Disilver oxide
Disilveroxid
disilveroxide
disliver oxide
Ezüst-oxid
Silberoxid
Silver (I) oxide
Silver oxide
silver oxide
Silver oxide
Silver oxide (Ag2O)
silver(1+) oxide
Silver(I) oxide

SYNONYMS

Silver(I) oxide;Argentous oxide;Silver oxide (Ag2O);MFCD00003404;Disilver oxide;Silver(1+) oxide;Silberoxyd;silver;hydrate;EINECS 243-957-1;Silver (I) Oxide;Silver oxide (ous);Silver(I) oxide 99+%;DTXSID40893897;Silver(I) oxide, Electrical Grade;Silver(I) oxide, ReagentPlus(R), 99%;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);Silver oxid;Silver oxide;Disilberoxid;ver(I) oxide;disilveroxide;Silver(Ⅰ)Oxide;Oxydisilver(I);ARGENTOUS OXIDE;SILVER(I) OXIDE;silver(1+)oxide;argentous oxide;disilver oxide;silver oxide (Ag2O);silver;hydrate;silver(1+) oxide;silver(I) oxide;Oxoargent ;Oxosilber ;Oxosilver;silver (II) oxide;Silver oxide;Silver peroxide;Silver suboxide;Silver(II) oxide;Silver, oxo- ;[1301-96-8];11113-88-5 [RN];20667-12-3 [RN];215-098-2 [EINECS];InChI=1S/Ag.O;MFCD00044285 [MDL number];SILVER(I,III) OXIDE;Silver(II) oxide (99.9%-Ag);SilverOxide;SİLVER OXİDEDisilberoxid; silver(l) oxide; silver hemioxide; Argentous oxide; Silver oxide (Ag2O); ARGENTOUS OXIDE; SILVER(I) OXIDE; SILVER OXIDE; disilveroxide; silver(1+)oxide; silveroxide(ag2o); triethoxy(chloromethyl)silane; SILVER(I) OXIDE, 99.99+%; SILVER(I) OXIDE, REAGENTPLUS, 99%; SILVER(I) OXIDE, NANOPOWDER, 99.9%; SILVER OXIDE EXTRA PURE; Silver(I) oxide, 99+%; SILVER(I) OXIDE (Ag2O); Silver(I)oxide,99+%(99.99%-Ag); silver(i) oxide, electrical grade; SILVEROXIDE,POWDER,REAGENT; Disilberoxid; SILVER(I) OXIDE: 99.9% (93% AG); Silver oxide; SILVER (I) OXIDE HIGH DENSITY CAS NO:20667-12-3

SİLVER OXIDE

Silver oxide can be prepared by combining aqueous solutions of silver nitrate and an alkali hydroxide. This reaction does not afford appreciable amounts of silver hydroxide due to the favorable energetics for the following reaction:

2 AgOH → Ag2O + H2O (pK = 2.875[10])
With suitably controlled conditions, this reaction can be used to prepare Ag2O powder with properties suitable for several uses including 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. It is soluble in ammonia solution, producing active compound of Tollens' reagent. A slurry of Ag2O is readily attacked by acids:

Ag2O + 2 HX → 2 AgX + H2O
where HX = HF, HCl, HBr, HI, or CF3COOH. It will also react with solutions of alkali chlorides to precipitate silver chloride, leaving a solution of the corresponding alkali hydroxide.

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

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.

Chemical Properties
Silver Oxide (Ag2O) is a heavy, brownish black powder, easily reduced by exposure to light. odorless; metallic taste. Soluble in ammonium hydroxide, potassium cyanide solu- tion, nitric acid, and sodium thiosulfate solution; slightly soluble in water; insoluble in alcohol.
Silver Oxide has been known for several centuries, and it is still widely used in synthetic chemistry, including in novel strategies. It has many applications: it can act as a base – due to the presence of oxide –, as an oxidant – due to its easy reduction to metallic silver –, as an halogen scavenger – due to the precipitation of silver halides –, or as a source of silver ion, particularly useful for organometallics preparation.

Uses
Silver oxide is used for polishing and coloring glass yellow. Also, it is used in purifying drinking water; as a catalyst; and as a germicide and parasiticide.
Silver oxide has been used as a base and halide abstracting agent in the synthesis of areneruthenium metallacyclic complexes of dianionic chelating ligands.
Silver oxide is a potentially valuable regenerative CO2 sorbent for space applications because it is a nontoxic solid that reacts with atmospheric CO2 at room temperature to form nontoxic solid silver carbonate.

Preparation
Silver Oxide is prepared by the reaction of aqueous silver nitrate and hydroxide salts.
Ag2O is poorly soluble in all common solvents including water. It is however readily soluble in ammonia, leading the Tollens'reagent which possesses a historical importance in the development of organic chemistry. This also illustrates the fact that (as for other metal-based reagents), properties of Ag2O may depend on the formation of complexes in the reaction medium.
Other commercially important silver chemicals include silver oxide which is used in batteries and silver cyanide which is used in electroplating.

Reactions
Mediates monoprotection of symmetrical diols with alkyl halides in good to excellent yield.
Silver(I) oxide may be used to mediate the following processes:
Selective monoalkylation of symmetric diols in the presence of alkyl halide.
Palladium catalyzed cross-coupling of aryl- and alkenylsilanols with organic halides.
Palladium-catalyzed reaction of aryl and alkenyl halides with terminal alkynes to form arylated or alkenylated alkynes, respectively.

Chemical Properties
Silver(I) oxide, Ag2O, is made by action of oxygen under pressure on silver at 300 °C, or by precipitation of a silver salt with carbonate-free alkali metal hydroxide; it is covalent, each silver atom (in solid Ag2O) having two collinear bonds and each oxygen atom four tetrahedral ones; two such interpenetrating lattices constitute the structure.

Physical properties
Brownish-black cubic crystals; density 7.14 g/cm3 at 16°C; begins to decompose around 200°C, decomposition becoming rapid at 250 to 300°C; insoluble in water and ethanol; soluble in acids and alkalis; sparingly soluble in solutions of caustic alkalis; insoluble in alcohol.

Uses
As catalyst; in the purification of drinking water; in the glass industry (polishing, coloring glass yellow).

Preparation
Silver(I) oxide is precipitated by mixing solutions of silver nitrate and caustic soda: 2AgNO3 + 2NaOH → Ag2O + 2NaNO3 + H2O.

General Description
Odorless brown-black solid. Sinks in water.

Reactivity Profile
Hydrogen sulfide is rapidly oxidized and may ignite in contact with Silver oxide [Bretherick 1979 p. 977]; Mixtures of metal sulfides, gold(III) sulfide, antimony sulfide or mercury (II) sulfide, phosphorus, sulfur, selenium, and selenium disulfide ignite on grinding with the oxide. Ammonia or hydrazine slowly react with Silver oxide forming silver nitride or in the presence of alcohol, silver fulminate may also be produced [Bretherick 1979 p. 203]. Oxidation of magnesium is explosive when warmed with Silver oxide.

Hazard
Fire and explosion risk in contact with organic materials or ammonia.

Health Hazard
Contact with eyes causes mild irritation. If continued for a long period, ingestion or inhalation of silver compounds can cause permanent discoloration of the skin (argyria).

Fire Hazard
Behavior in Fire: Decomposes into metallic silver and oxygen. If large quantities are involved, the oxygen might increase the intensity of the fire.

Safety Profile
A poison by intraperitoneal route. Moderately toxic by ingestion. Flammable by chemical reaction; an oxidizing agent. Explodes in contact with ammonia. Incompatible with CuO, (NH3 + ethanol), (hydrazine + ethanol), CO, HzS, Mg, auric sulfide, Sb sulfide, Hg sulfide, nitroalkanes, Se, S, P, K, Na, NaK, seleninyl chloride. See also SILVER COMPOUNDS.

Physical Properties
Gray monoclinic or cubic crystals or powder; diamagnetic; semiconductor; density 7.48 g/cm3; decomposes to its elements above 100°C; insoluble in water (solubility 27 mg/L at 25°C); soluble in alkalis; decomposes in ammonia solution evolving nitrogen; dissolves in dilute acids with decomposition evolving oxygen; forms a brown solution in concentrated nitric acid, and forms intense green coloration in concentrated sulfuric acid.

Uses
Silver oxide is used to make silver oxide-zinc alkali batteries. Also, it is an oxidizing agent.

Preparation
Silver oxide is prepared by reacting silver nitrate with potassium persulfate in the presence of a base.

Chemical Properties
Grey to black powder

Uses
In the manufacture of silver oxide-zinc alkali batteries.

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.

Compound Formula    Ag2O
Molecular Weight    231.74
Appearance            Brown Powder
Melting Point            280° C (536° F)
Boiling Point            N/A
Density                    7220 kg/m-3
Solubility in H2O    N/A
Exact Mass            N/A
Monoisotopic Mass    229.805101 Da
Charge              N/A

Silver(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.

USES
•As a laboratory reagent.
•To remove Carbon Dioxide from aqueous solutions in laboratory reactions.
•In pollution control filters.
•As a precursor to making Silver Powder. ( by heating it above 280°C ( 536°F ) )
•As a component in making Silver Oxide batteries.
•To remove Chlorine from acid plating baths, and to remove dissolved Chlorine from water.
•As an Antibacterial agent for concrete ( 1 Lb Silver Oxide per cubic yard of Concrete (4,050 lbs) ).
•As an Antimicrobial agent in some infection resistant surgical fabric materials.
•As an Antimicrobial agent in some Swimming Pools, Spas and Fountains.
•As a Carbon Dioxide Scrubber :
•Nuclear Submarines use Silver Oxide to scrub Carbon Dioxide from their air.
•The International Space Station uses Silver Oxide to scrub Carbon Dioxide from their air.
•The Space Shuttle uses Silver Oxide to scrub Carbon Dioxide from their air.
 
How Carbon Dioxide Scrubbing Works :
• Silver Oxide absorbs CO2 from air when the humidity is > 25%. (Normal air contains 249ppm CO2)
• While absorbing CO2, Silver Oxide turns into the yellow-greenish Silver Carbonate (Ag2CO3).
• Silver Carbonate can then be ‘recharged’ back to Silver Oxide by heating it.
• Silver Carbonate begins to decompose to Silver Oxide as it approaches 160°C (320°F).
• Above about 210°C ( 410°F ) the Silver Carbonate completely decomposes to Ag2O, Silver Oxide.
• In this way, Silver Oxide can be recycled indefinitely as a Carbon Dioxide scrubber.
• Above about 280°C ( 536°F ) however, Silver Oxide releases Oxygen to form Silver Powder. (not good here)

Mediates monoprotection of symmetrical diols with alkyl halides in good to excellent yield.

Silver(I) oxide may be used to mediate the following processes:
• Selective monoalkylation of symmetric diols in the presence of alkyl halide.
• Palladium catalyzed cross-coupling of aryl- and alkenylsilanols with organic halides.
• Palladium-catalyzed reaction of aryl and alkenyl halides with terminal alkynes to form arylated or alkenylated alkynes, respectively.

Silver(I) oxide reacts with CO2 present in the atmosphere to afford silver carbonate. It is widely used in the preparation of ceramic pigments. It participates in the Arndt-Eistert synthesis.

Applications
Polishing glass, coloring glass yellow, catalyst, purifying drinking water, lab reagent, carbon dioxide scrubber, and chemical sensors. It is used in the preparation of other silver compounds, and silver-oxide batteries. In organic chemistry, silver oxide finds use as an oxidizing agent for aldehyes to produce carboxylic acids.

Physical State: Solid
Appearance: brown-black
Odor: odorless
pH: Not available.
Vapor Pressure: Not available.
Vapor Density: Not available.
Evaporation Rate:Not available.
Viscosity: Not available.
Boiling Point: Not available.
Freezing/Melting Point:392 deg F
Decomposition Temperature:Not available.
Solubility: Negligible in water.
Specific Gravity/Density:7.14
Molecular Formula:Ag2O
Molecular Weight:231.7358

Description
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.

Application
S 0133 (OTTO) Silver oxide, 99.99% Cas 20667-12-3 - used in the preparation of other silver compounds, and silver-oxide batteries. In organic chemistry, silver oxide finds use as an oxidizing agent for aldehyes to produce carboxylic acids.

•It is used in silver oxide batteries.
•It is used in many reactions as a mild oxidizing agent such as in oxidation reactions of converting aldehydes to carboxylic acids. 
•It is used in synthesis of many compounds. It is used in preparation of Tollen's reagent as well.

OVERVIEW
Silver(I) oxide (SILL-ver one OK-side) is an odorless dark brown or black powder with a metallic taste. It is used primarily for polishing glass, the purification of water, and coloring glass.

HOW IT IS MADE
Silver(I) oxide is made by reacting silver nitrate (AgNO3) with sodium or potassium hydroxide (NaOH or KOH). For example:

2AgNO3 + 2NaOH → Ag2O + 2NaNO3 + H2O

The silver(I) oxide settles out as a precipitate that can then be washed and purified.

COMMON USES AND POTENTIAL HAZARDS
Silver(I) oxide finds limited commercial and industrial application. It is used as an ingredient in the manufacture of glass to give a yellowish caste to the glass. It is also a component of mixtures used to polish glass, including the glass used in optical lenses. Silver(I) oxide is also used as a catalyst in certain industrial operations and in some water purification systems.

AQUEOUS
Referring to a solution that consists of some material dissolved in water.

PRECIPITATE
A solid material that settles out of a solution, often as the result of a chemical reaction.
Silver(I) oxide is a skin, eye, and respiratory irritant that may cause coughing, wheezing, shortness of breath, and pulmonary edema (accumulation of fluid in the lungs). It can also cause burning of the eyes and skin. Ingestion can produce burning of the gastrointestinal tract accompanied by nausea, vomiting, and abdominal pain. Long-term exposure to silver(I) oxide can cause argyreia, a bluish-gray discoloration of the skin, eyes, and mucous membranes (the soft tissues lining the breathing and digestive passages).

Uses of Silver Oxide
Silver oxide is a chemical compound. This fine dry powder with a brownish-black color is primarily used in the preparation of other silver compounds. It is a three-dimensional polymer (i.e. chemical compound consisting essentially of repeating structural units) and is not readily soluble in most solvents. Although silver oxide hydrolyzes only slightly in water, it gives the water a distinctive metallic taste. However, silver oxide is soluble in dilute nitric acid and is easily attacked by acids. Like other silver compounds, silver oxide is not light sensitive and decomposes at temperatures above 280 degrees Celsius.

Laboratory Reagent
Silver oxide is used as a reagent in laboratory reactions to form various chemical compounds. It dissolves in ammonium hydroxide solutions to give soluble derivatives. Also, silver oxide reacts with alkali chloride solutions to yield alkali hydroxide. It is often employed in the synthesis of transition metal-carbene complexes (i.e. organometallic compound featuring a divalent organic ligand). For example, silver oxide readily reacts with ligand precursors to form the corresponding complexes.

Carbon Dioxide Scrubber
Silver oxide is very effective in removing (or scrubbing) carbon dioxide from humidified air (humidity greater than 25 percent). This property is extensively used in nuclear submarines, the international space station and space shuttles. Silver oxide reacts with carbon dioxide in the presence of water to generate silver carbonate. It is capable of regenerating all the scrubbed carbon dioxide by prolonged heating, which enables each canister (a perforated metal box that absorbs airborne poisons and irritants) to be recycled about 60 times.

In the Manufacture of Pollution Control Filter
Silver oxide is used in the manufacture of filters for gas sensors. This filter helps increase the efficiency of chlorine dioxide detectors to free the gas stream from hydrogen sulfides without producing any unwanted compounds.

In the Preparation of Silver Powder
Silver oxide acts as a catalyst in the preparation of silver powder. If heated above 280 degrees Celsius, silver oxide is converted into silver powder while releasing oxygen gas as a by-product.

In the Manufacture of Silver Oxide Batteries
Silver oxide and zinc form the main components of a silver oxide battery (also called silver –zinc battery). While silver oxide acts as the positive electrode (cathode), zinc behaves as the negative electrode (anode). Unlike its competitor counterparts, a silver oxide battery has higher durability, can handle higher current loads, and is free from thermal runaways and inflammability. Such batteries are used in electronic devices as well as U.S. military and Apollo space programs.

Antimicrobial Agent
Silver oxide has enhanced antimicrobial properties and is often used in the manufacture of some infection-resistant surgical fabric materials and fibrous textile articles. It is also used in concrete and in some swimming pools and spas to protect the water from undesired microbes.

Abstract
Silver oxide nanoparticles are wonderful material and having great potential towards biomedical applications. Silver oxide nanoparticle were synthesized via Chemical Aqueous method and characterized by applying manifold available techniques. X-ray diffraction (XRD) was used for analyzing structural property of nanoparticle crystals, the morphology of synthesized nanoparticles was studied by scanning electron microscope (SEM), elemental analysis of the composition was observed by energy dispersive X-ray spectra (EDXS) and the optical properties was analyzed by the Uv–Vis spectrometer. Spectroscopic analysis confirmed the spherical morphology of the nanoparticles with the effect of calcined temperature. Phototoxic and cytotoxic effects of grown particles were examined by conducting various relevant experimental techniques on hepatocellular (HepG2 Cell line) model. The obtained results were verified by applying polynomial fit which confirmed the goodness of fit. Silver oxide NPs has unique bio interaction characteristics and physicochemical properties as anticancer agent. This research will be beneficial particularly for cancer therapeutics.

A silver oxide powder that replaces silver powder as a silver conductive paste filler has a specific surface area measured by the BET method is 1.0-25.0 m2/g, average primary particle diameter is 1-50 nm, and average secondary particle diameter is 1-1000 nm. The silver oxide powder is made by preparing a neutralization medium that is an aqueous solution containing one or both of sodium hydroxide and potassium hydroxide in a total amount of 0.5 mole/L or less, simultaneously adding an aqueous solution containing silver salt in an amount of 6.0 mole/L or less and an aqueous solution of at least one of sodium hydroxide and potassium hydroxide to the liquid medium to conduct a neutralization reaction, thereby obtaining a neutralized precipitate, maintaining the liquid at a pH in the range of 12±1.5 during the reaction, and subjecting the precipitate to filtration, washing, and drying.
Silver(I) oxide (Ag2O) has been known for several centuries, and it is still widely used in synthetic chemistry, including in novel strategies. Ag2O is a black powder that is prepared by the reaction of aqueous silver nitrate and hydroxide salts  This reagent has many applications: it can act as a base – due to the presence of oxide –, as an oxidant – due to its easy reduction to metallic silver –, as an halogen scavenger – due to theprecipitation of silver halides –, or as a source of silveron, particularly useful for organometallics preparation.Ag2O is poorly soluble in all common solvents including.

Silver oxide is an oxide of silver. It is used to prepare other silver compounds, and in the silver oxide battery. Silver is a metallic element with the chemical symbol Ag and atomic number 47. It occurs naturally in its pure, free form, as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite. (5, 6, 8)

Compound Type    
Industrial/Workplace Toxin
Inorganic Compound
Silver Compound
Synthetic Compound

Silver Oxide, Powder, Reagent is a black or brown chemical compound used to prepare silver compounds. In organic synthesis, silver oxide is used as a mild oxidizing agent.

Description
Dark brown or black powder. Silver oxide is used for polishing glass and for coloring glass yellow. It has also been used at excavation sites for the treatment of Bronze disease. However, it is not as effective as Benzotriazole and can leave dark spots on the surface. Silver oxide is used medicinally as a germicide.

It is the process for tinting silver-plated products slightly black and obtaining an antique appearance. If necessary, the coating can be improved by using varnish. Also, the varnish does not have a bad effect on the color.

Silver oxide is a white, shiny, precious metallic element with the symbol Ag (the symbol Ag comes from the Latin word argentum) on the periodic table of the elements. Its atomic number is 47 and its atomic weight is 107.87 grams. It has a melting point of 961.9 ° C, a boiling point of 1950 ° C, and a specific gravity of 10.5 g / cm.

Silver oxide is an inorganic compound with the chemical formula Ag2O. The force that binds its atoms is purely ionic in nature; Therefore, it consists of an ionic solid in which there is a ratio of two cations + electrostatically interacting with an anion O2-.

The oxide anion is caused by the interaction of silver atoms on the O2-surface with oxygen in the environment; just like iron and many other metals. Instead of reddening and splintering a piece of silver or jewelry, it turns black, which is characteristic of silver oxide.
It is an ionic solid. Therefore, there cannot be Ag-O or Ag = O covalent bonds in its structure; because if it were, the properties of this oxide would have changed drastically. At that time Ag ions + I2- live in a ratio of 2: 1 and electrostatic attraction.
If the number of spheres is counted, it will be seen with the naked eye that there are nine silver blue and four red.
Repeating the structural unit of the AgO tetrahedron4 surrounded by four other Ag + all black solid is created (ignoring any voids or irregularities that these crystalline arrangements may have).
Engraving the surface of the silver bowl in the main image results in a solid that is not only black in color but also has brown or brown hues (top picture). Some of the physical and chemical properties currently reported are:

Molecular weight
231.735 g / mol

View
Powdery black-brown solid (note that although it is an ionic solid, it does not have a crystalline appearance). It is odorless and gives a metallic taste when mixed with water.

Density
7.14 g / mL.

Melting point
277-300 ° C Absolutely turns solid silver; that is, the liquid oxide possibly decomposes before it is formed.

Kps
1.52 ∙ 10-8 in water at 20 ° C. Therefore, it is almost insoluble in water.

Resolution
If you look closely at the image of its structure, the Ag spheres2 + I2- do not differ almost in size. This results in that only small molecules can pass through the interior of the crystal lattice, making it insoluble in almost all solvents; except where it reacts such as bases and acids.

Covalent character
Although it has been repeatedly said that silver oxide is an ionic compound, some properties, such as its low melting point, contradict this statement.Of course, considering the covalent character does not destroy what is explained for its structure, since it would be sufficient to add it to the structure of Ag. 2 Or a sphere and rod model showing covalent bonds.Likewise, tetrahedral and square planes will be linked by covalent bonds (or ionic covalent) as well as AgO4AgOAg lines.With that in mind, Ag2Or would actually be a polymer. However, it is recommended to consider it as an ionic solid of covalent character (the nature of the bond remains a challenge today).

Decomposition

At first it was stated that its formation is thermodynamically reversible, so it absorbs heat to return to its metallic state. All this can be expressed in two chemical equations for such reactions:

4Ag (s) + O2 (g) => 2Ag2O (s) + Q

2Ag2O (s) + Q => 4Ag (s) + O2 (g)

Q represents heat in the equation. This explains why the fire that burns the surface of the oxidized silver bowl turns it into a silvery glow.Therefore, it is difficult to assume that it is Ag.2O (l) as it will instantly decompose from heat; Unless the pressure is raised too high to get the brown black liquid in question.

Applications

-Studies investigating new and sophisticated uses of silver oxide continue to this day. Some of its uses are listed below:

-Dissolve in ammonia, ammonium nitrate and water to form Tollens reagent. This reagent is a useful tool in qualitative analysis in organic chemistry laboratories. It allows determination of the presence of aldehydes in the sample by the formation of a "silver mirror" in the test tube as a positive response.

-In combination with metallic zinc, it forms primary zinc-silver oxide batteries. This is perhaps one of the most common and home uses.

-Acts as a scrubber, for example absorbing CO. 2. When heated, it releases trapped gases and can be reused for many times.

-Due to the antimicrobial properties of silver, its oxide is useful in bioanalysis and soil purification studies.

-It is a mild oxidizing agent that can oxidize aldehydes to carboxylic acids. It is also used in the Hofmann reaction (from tertiary amines) and participates in other organic reactions as a reagent or a catalyst.