Silver oxide Property

Melting point:

300°C (dec.)

Density 

7,143 g/cm³

storage temp. 

Store below +15°C.

solubility 

insoluble in ethanol; soluble in acid solutions, alkaline solutions

form 

Powder/Solid

color 

Dark-brown

Specific Gravity

7.22

Water Solubility 

slightly soluble

Sensitive 

Light Sensitive

Crystal Structure

Cu2O type

crystal system

Cube

Merck 

14,8521

Space group

Pn3m

Lattice constant

a/nm	b/nm	c/nm	α/o	β/o	γ/o	V/nm3
0.4721	0.4721	0.4721	90	90	90	0.1052

Stability:

Stable. Oxidiser. Incompatible with most common metals, ammonia, magnesium, many organic materials.

InChIKey

KHJDQHIZCZTCAE-UHFFFAOYSA-N

CAS DataBase Reference

20667-12-3(CAS DataBase Reference)

EPA Substance Registry System

Silver(I) oxide (20667-12-3)

Safety

Hazard Codes 

O,Xi,C,N

Risk Statements 

36/37/38-8-34-50/53-41

Safety Statements 

17-26-36-45-36/37/39-61-60-39

RIDADR 

UN 1479 5.1/PG 2

WGK Germany 

2

RTECS 

VW4900000

F 

8

TSCA 

Yes

HazardClass 

5.1

PackingGroup 

II

HS Code 

28432900

Toxicity

LD50 orally in rats: 2.82 g/kg (Smyth)

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Danger

Hazard statements

H271May cause fire or explosion; strong oxidiser

H318Causes serious eye damage

H410Very toxic to aquatic life with long lasting effects

Precautionary statements

P210Keep away from heat/sparks/open flames/hot surfaces. — No smoking.

P220Keep/Store away from clothing/…/combustible materials.

P273Avoid release to the environment.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P283Wear fire/flame resistant/retardant clothing.

P305+P351+P338IF IN EYES: Rinse cautiously with water for several minutes. Remove contact lenses, if present and easy to do. Continuerinsing.

Silver oxide Chemical Properties,Usage,Production

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).

Uses

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.

Uses

Silver(I) oxide may be used in the synthesis of following:

• (RS)-malic acid
• 1,2-(o)-benzoquinone
• polysubstituted cyclic ethers

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.

Flammability and Explosibility

Non flammable

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.

Purification Methods

Leach the oxide with hot water in a Soxhlet apparatus for several hours to remove any entrained electrolytes. [Glemser & Sauer in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol II p 1037 1965.]