Nickel(II) oxide is a chemical compound with the formula NiO. It is a black solid, commonly used as a catalyst and in the production of ceramics and pigments.
| IUPAC Name | Nickel(II) oxide |
| Molecular Formula | NiO |
| CAS Number | 1313-99-1 |
| Synonyms | Nickelous oxide, Nickel monoxide, Ni(II) oxide |
| InChI | InChI=1S/Ni.O |
Nickel(II) Oxide Properties
Nickel(II) Oxide Formula
The chemical formula of nickel monoxide is NiO. It consists of one atom of nickel (Ni) and one atom of oxygen (O), resulting in a simple and straightforward formula.
Nickel(II) Oxide Molar Mass
The molar mass of nickel monoxide can be calculated by summing the atomic masses of its constituent elements. For NiO, the molar mass is approximately 74.69 grams per mole (g/mol).
Nickel(II) Oxide Boiling Point
Nickel monoxide does not have a distinct boiling point as it undergoes decomposition before reaching its boiling point. Upon heating, it decomposes into its constituent elements, nickel and oxygen.
Nickel(II) Oxide Melting Point
The melting point of nickel monoxide is approximately 1984 degrees Celsius (1984 °C). At this temperature, the solid NiO transforms into a liquid state.
Nickel(II) Oxide Density g/mL
The density of nickel monoxide is around 6.67 grams per milliliter (g/mL). This value indicates the amount of mass packed into a given volume, making it a measure of the compactness of the substance.
Nickel(II) Oxide Molecular Weight
The molecular weight of nickel monoxide is calculated by summing the atomic weights of its constituent elements. For NiO, the molecular weight is approximately 74.69 grams per mole (g/mol).
Nickel(II) Oxide Structure
Nickel monoxide possesses a cubic crystal structure. It consists of nickel ions (Ni2+) and oxide ions (O2-) arranged in a regular, repeating pattern. This structure contributes to its characteristic properties and behavior.
Nickel(II) Oxide Solubility
Nickel monoxide is sparingly soluble in water. It exhibits limited solubility, meaning it dissolves only to a small extent in water. However, it can react with acids to form soluble nickel salts, displaying some degree of chemical reactivity.
| Appearance | Black solid |
| Specific Gravity | 6.67 g/mL |
| Color | Black |
| Odor | Odorless |
| Molar Mass | 74.69 g/mol |
| Density | 6.67 g/mL |
| Melting Point | 1984 °C |
| Boiling Point | Decomposes |
| Flash Point | Not applicable |
| Water Solubility | Sparingly soluble |
| Solubility | Soluble in acids, form soluble nickel salts |
| Vapour Pressure | Not available |
| Vapour Density | Not available |
| pKa | Not applicable |
| pH | Neutral |
Please note that some properties, such as flash point, vapour pressure, and pKa, are not applicable or available for nickel monoxide.
Nickel(ii) Oxide Safety and Hazards
Nickel monoxide poses certain safety considerations and hazards. It is important to handle it with care. Direct contact with skin, eyes, or inhalation of its dust or fumes should be avoided. It may cause skin irritation and allergic reactions in some individuals. In case of ingestion or inhalation, immediate medical attention is necessary. nickel monoxide is not considered highly flammable but can contribute to fire if exposed to combustible materials. It is important to store and handle it in a well-ventilated area. Proper personal protective equipment, such as gloves and goggles, should be worn when working with nickel monoxide to minimize potential risks.
| Hazard Symbols | None |
| Safety Description | Handle with care. Avoid direct contact and inhalation. Use proper protective equipment. Obtain medical attention if needed. |
| UN IDs | Not applicable |
| HS Code | 2825.70.10 |
| Hazard Class | Not classified |
| Packing Group | Not classified |
| Toxicity | Considered harmful if swallowed or inhaled. May cause skin irritation and allergic reactions. |
Please note that nickel monoxide is not assigned specific hazard symbols, UN IDs, hazard class, or packing group. The provided safety information is based on general knowledge and precautions associated with the handling and use of nickel monoxide. It is essential to refer to specific safety data sheets (SDS) and follow recommended safety practices for accurate and detailed information.
Nickel(ii) Oxide Synthesis Methods
There are several methods for synthesizing nickel monoxide. One common approach is thermal decomposition of nickel compounds, such as nickel carbonate or nickel hydroxide. In this method, heat a specific precursor compound in the absence of oxygen to form nickel monoxide.
Another method involves the oxidation of metallic nickel. Nickel metal can react with oxygen or air at elevated temperatures to produce nickel monoxide. Carry out this process by calcinating or roasting nickel metal in an air or oxygen atmosphere to produce nickel monoxide.
Utilize precipitation reactions to synthesize nickel monoxide by reacting nickel salts, such as nickel chloride or nickel nitrate, with an alkaline solution like sodium hydroxide or ammonium hydroxide. This reaction forms a precipitate of nickel monoxide.
Sol-gel synthesis is another viable method. It involves the hydrolysis and condensation of suitable nickel precursors, such as nickel alkoxides, in a solution. Obtain nickel monoxide by drying and calcining the gel formed during the precipitation reaction.
Employ electrodeposition techniques for nickel monoxide synthesis. By applying an electric current to a nickel electrode immersed in an electrolyte solution, nickel monoxide can be formed on the electrode surface.
When choosing a synthesis method, one should consider factors such as desired purity, scalability, and specific application requirements, as each method offers its own advantages.
Nickel(ii) Oxide Uses
Nickel monoxide finds various uses in different industries due to its unique properties. Here are some of its common applications:
- Catalyst: Nickel monoxide actively catalyzes various chemical reactions, such as hydrogenation and oxidation processes, facilitating the conversion of reactants into desired products.
- Ceramics: In the production of ceramic materials, nickel monoxide actively functions as a coloring agent, actively assisting in achieving specific colors and patterns in ceramic glazes and pigments.
- Batteries: Rechargeable nickel-cadmium (NiCd) and nickel-metal hydride (NiMH) batteries actively utilize nickel monoxide as a positive electrode material, actively enabling the storage and release of electrical energy.
- Gas Sensors: Nickel monoxide actively detects gases such as carbon monoxide (CO) and nitrogen dioxide (NO2) in gas sensing applications when employed in sensors based on it.
- Glass Manufacturing: The glass industry actively utilizes nickel monoxide to impart various colors to glass products, actively contributing to the production of colored glass, including green, brown, and black shades.
- Conductive Coatings: Nickel monoxide actively functions as a component in conductive coatings, which actively render materials like glass or plastics conductive when applied to them.
- Fuel Cells: Nickel monoxide actively functions as a component in solid oxide fuel cells (SOFCs), actively acting as a cathode material and participating in the electrochemical reactions within the fuel cell.
- Catalyst Support: Nickel monoxide actively serves as a support material for other catalysts, actively enhancing their stability and performance.
Nickel monoxide’s diverse range of applications underscores its significance in various industries, highlighting its usefulness and versatility.
Questions:
Q: What is the formula for nickel(II) oxide?
A: The formula for nickel(II) oxide is NiO.
Q: What salt is formed in the reaction of nickel(II) oxide with nitric acid?
A: The reaction of nickel(II) oxide with nitric acid forms nickel(II) nitrate (Ni(NO3)2).
Q: What voltage does nickel(II) oxidize to nickel(III)?
A: Nickel(II) oxidizes to nickel(III) at a voltage of approximately +1.63 V.
Q: What happens when Ni(s) is oxidized to the nickel(II) ion as shown in the image?
A: During oxidation of Ni(s) to the nickel(II) ion, electrons are lost, resulting in the formation of Ni2+ ions.
Q: What masses of nickel(II) oxide and aluminum must be used to produce 13.3 g of nickel?
A: The masses of nickel(II) oxide and aluminum needed to produce 13.3 g of nickel depend on the specific reaction and stoichiometry involved.