Silver oxide (Ag2O) is a chemical compound composed of silver and oxygen. It is commonly used as an oxidizing agent and catalyst in various chemical reactions.
| IUPAC Name | Silver(I) oxide |
| Molecular Formula | Ag2O |
| CAS Number | 11113-88-5 |
| Synonyms | Silver monoxide; Silver(1+) oxide; Dioxosilver; Argentous oxide, disilver;oxygen(2-) |
| InChI | InChI=1S/2Ag.O |
Silver Oxide Properties
Silver Oxide Formula
The formula of silver monoxide is Ag2O. It consists of two silver (Ag) atoms bonded with one oxygen (O) atom. This formula represents the ratio of elements present in the compound.
Silver Oxide Molar Mass
The molar mass of silver monoxide is calculated by adding the atomic masses of its constituent elements. Silver has an atomic mass of 107.87 g/mol, and oxygen has an atomic mass of 16.00 g/mol. Therefore, the molar mass of silver monoxide is approximately 231.87 g/mol.
Silver Oxide Boiling Point
Silver monoxide does not have a distinct boiling point as it decomposes before reaching its boiling point. Upon heating, it undergoes a chemical reaction and breaks down into silver metal and oxygen gas.
Silver Oxide Melting Point
Silver monoxide has a melting point of around 280 °C (536 °F). At this temperature, solid silver monoxide converts into a liquid state. The melting point indicates the temperature at which the solid form transitions into the liquid form.
Silver Oxide Density g/mL
The density of silver monoxide is approximately 7.14 g/mL. This value represents the mass of the compound per unit volume. The high density of silver monoxide is attributed to the heavy atomic mass of silver.
Silver Oxide Molecular Weight
The molecular weight of silver monoxide is calculated by summing the atomic masses of its constituent elements. The molecular weight of Ag2O is approximately 231.87 g/mol. It provides information about the mass of one mole of the compound.
Silver Oxide Structure
Silver monoxide has a crystal structure. The silver and oxygen atoms are arranged in a lattice-like pattern. The structure consists of Ag^+ cations and O^2- anions held together by ionic bonds.
Silver Oxide Solubility
Silver monoxide is sparingly soluble in water. It dissolves to a limited extent, producing silver hydroxide (AgOH). The solubility of silver monoxide can be enhanced by using acidic or alkaline solutions, which convert it into soluble silver salts.
| Appearance | Black or dark brown solid |
| Specific Gravity | 7.14 g/cm³ |
| Color | Black |
| Odor | Odorless |
| Molar Mass | 231.87 g/mol |
| Density | 7.14 g/cm³ |
| Melting Point | 280 °C (536 °F) |
| Boiling Point | Decomposes |
| Flash Point | Not applicable |
| Water Solubility | Sparingly soluble |
| Solubility | Soluble in acidic or alkaline solutions |
| Vapour Pressure | Not applicable |
| Vapour Density | Not applicable |
| pKa | Not applicable |
| pH | Not applicable |
Silver Oxide Safety and Hazards
When handling silver monoxide, take precautions to ensure safety. Swallowing or inhaling it can be harmful, and it can irritate the skin, eyes, and respiratory system. Ensure adequate ventilation to prevent the accumulation of dust or fumes. Wear protective equipment like gloves and goggles to minimize contact with the compound. Store silver monoxide in a cool, dry place away from flammable materials and incompatible substances. If ingested, inhaled, or in contact with skin, seek immediate medical attention. Follow proper handling and disposal procedures to prevent environmental contamination.
| Hazard Symbols | None |
| Safety Description | Harmful if swallowed or inhaled. |
| UN IDs | Not applicable |
| HS Code | 2841.90.90 |
| Hazard Class | Not classified |
| Packing Group | Not applicable |
| Toxicity | Moderate toxicity |
Silver Oxide Synthesis Methods
There are several methods for synthesizing silver monoxide.
One common approach involves the reaction between a soluble silver salt, such as silver nitrate (AgNO3), and an alkali hydroxide, such as sodium hydroxide (NaOH). The reaction proceeds by mixing aqueous solutions of the silver salt and alkali hydroxide, resulting in the formation of a silver monoxide precipitate. Collect the precipitate and dry it to obtain solid silver monoxide.
Another method involves the thermal decomposition of a silver compound, such as silver nitrate or silver carbonate. Heat the compound to a specific temperature to form silver monoxide as a product. The decomposition process releases nitrogen dioxide gas (NO2) or carbon dioxide gas (CO2) depending on the starting compound used.
Employ electrolysis to synthesize silver monoxide. This method involves passing an electric current through a silver electrode immersed in a suitable electrolyte solution, often containing silver nitrate. Oxidation of the silver electrode occurs, resulting in the formation of silver monoxide on the electrode surface.
It is worth noting that the choice of synthesis method depends on factors such as desired purity, yield, and the specific application of silver monoxide. Follow proper safety precautions during synthesis, including using appropriate protective equipment and adhering to recommended procedures.
Silver Oxide Uses
Silver monoxide has various applications due to its unique properties. Here are some uses of silver monoxide:
- Oxidizing Agent: Organic synthesis reactions commonly employ silver monoxide as an oxidizing agent to convert alcohols into aldehydes or ketones.
- Catalyst: Silver monoxide acts as a catalyst in various chemical reactions, including the oxidation of alkenes and aldehydes, and the reduction of nitro compounds.
- Batteries: Button cell batteries utilize silver monoxide as the cathode material due to its high energy density and stability.
- Antimicrobial Agent: Silver monoxide exhibits antimicrobial properties, making it useful in applications such as wound dressings, medical devices, and water purification systems.
- Conductive Paste: The production of electronics, including printed circuit boards and thick film resistors, employs silver monoxide in conductive pastes.
- Photographic Industry: The photographic industry employs silver monoxide for its light-sensitive properties, particularly in black-and-white photography.
- Pyrotechnics: Pyrotechnic mixtures utilize silver monoxide to produce special effects and colors in fireworks.
- Chemical Reagents: Laboratory settings employ silver monoxide as a chemical reagent for various analytical and synthetic procedures.
- Glass Manufacturing: Specialty glasses, such as mirror coatings, utilize silver monoxide due to its reflective properties.
- Silver Plating: Silver plating applications sometimes use silver monoxide to provide a durable and corrosion-resistant coating.
These diverse applications highlight the versatility and importance of silver monoxide in various industries.
Questions:
Q: Is Ag2O soluble in water?
A: Ag2O is sparingly soluble in water.
Q: How many grams of Ag2O decomposed if 4.58 L of O2 was formed at P=745 mmHg and T=308K?
A: The mass of Ag2O decomposed can be calculated using stoichiometry and the ideal gas law.
Q: Is Ag2O ionic?
A: Yes, Ag2O is an ionic compound.
Q: Why is it called silver oxide and not disilver oxide?
A: The naming convention for binary ionic compounds does not use prefixes like “di-“. Hence, it is called silver oxide.
Q: Which disaccharide cannot react with Ag2O?
A: Ag2O does not react with disaccharides as it is primarily used as an oxidizing agent in organic synthesis.
Q: What is silver oxide?
A: Silver monoxide (Ag2O) is a chemical compound composed of silver and oxygen, often used as an oxidizing agent and catalyst.
Q: Can alkaline and silver oxide be used interchangeably?
A: Alkaline and silver oxide may not be interchangeable as they have different chemical properties and applications.
Q: How many moles of silver would be deposited if 0.632 mole of lead was oxidized to lead(II) nitrate?
A: The stoichiometry of the balanced equation would determine the number of moles of silver deposited.
Q: How long does oxidized silver last?
A: Various factors such as environmental conditions and maintenance determine the longevity of oxidized silver, but proper care can preserve it for extended periods.