Nickel(II) chloride, known as NiCl2, is a chemical compound with a greenish-yellow color. It is commonly used in electroplating, catalysts, and as a precursor in the synthesis of other nickel compounds.
| IUPAC name | Nickel(II) chloride |
| Molecular formula | NiCl2 |
| CAS number | 7718-54-9 |
| Synonyms | Nickelous chloride, Nickel dichloride, Dichloronickel, Nickel chloride |
| InChI | InChI=1S/2ClH.Ni/h2*1H;/q;;+2/p-2 |
Nickel Chloride Properties
Nickel Chloride Formula
The formula of nickel dichloride is NiCl2. It indicates that each molecule of nickel dichloride consists of one nickel atom bonded to two chlorine atoms. This chemical formula provides important information about the composition and ratio of the elements present in the compound.
Nickel Chloride Molar Mass
The molar mass of nickel dichloride, calculated by adding the atomic masses of its constituent elements, is approximately 129.6 grams per mole. This value is useful in determining the amount of nickel dichloride present in a given sample and for various stoichiometric calculations.
Nickel Chloride Boiling Point
Nickel dichloride has a boiling point of around 1,007 degrees Celsius (1,845 degrees Fahrenheit). At this temperature, the compound undergoes a phase transition from its liquid state to a gaseous state. The boiling point is an important physical property that helps in understanding the behavior of nickel dichloride when heated.
Nickel Chloride Melting Point
The melting point of nickel dichloride is approximately 1002 degrees Celsius (1836 degrees Fahrenheit). This is the temperature at which the solid form of nickel dichloride transitions into a liquid state. The melting point is significant for applications involving the handling and processing of nickel dichloride.
Nickel Chloride Density g/mL
The density of nickel dichloride is around 3.55 grams per milliliter. Density is a measure of the mass per unit volume of a substance, and it provides information about the compactness of the material. The density of nickel dichloride helps determine its behavior in various applications and in different physical states.
Nickel Chloride Molecular Weight
The molecular weight of nickel dichloride is approximately 129.6 grams per mole. It is calculated by summing the atomic masses of nickel and chlorine in the compound. The molecular weight is essential in understanding the relationships between mass, moles, and the number of particles in chemical reactions.
Nickel Chloride Structure
Nickel dichloride adopts a crystal lattice structure in its solid form. It consists of nickel cations (Ni2+) and chloride anions (Cl-) arranged in an alternating pattern. This arrangement forms a three-dimensional network, contributing to the stability and physical properties of nickel dichloride.
Nickel Chloride Solubility
Nickel dichloride exhibits moderate solubility in water. It can dissolve to form a greenish-yellow solution. The solubility of nickel dichloride is influenced by factors such as temperature and the presence of other substances. Understanding its solubility is important in various industrial processes and chemical applications involving nickel dichloride.
| Appearance | Greenish-yellow solid |
| Specific Gravity | 3.55 g/mL |
| Color | Greenish-yellow |
| Odor | Odorless |
| Molar Mass | 129.6 g/mol |
| Density | 3.55 g/mL |
| Melting Point | 1002 °C (1836 °F) |
| Boiling Point | 1007 °C (1845 °F) |
| Flash Point | Not applicable |
| Water Solubility | Moderate |
| Solubility | Soluble in organic solvents (ethanol, acetone) and acids |
| Vapour Pressure | Not available |
| Vapour Density | Not available |
| pKa | Not available |
| pH | Acidic (around 4) |
Nickel Chloride Safety and Hazards
Nickel dichloride poses certain safety hazards that should be taken into consideration. It is important to handle this compound with care to avoid potential risks. Nickel dichloride can cause skin irritation and sensitization, so protective gloves and clothing should be worn when handling it. Inhalation of nickel dichloride dust or vapors should be avoided as it may lead to respiratory irritation. Ingestion of nickel dichloride can be harmful and should be prevented. Additionally, nickel dichloride is toxic to aquatic life and may cause environmental damage if released into water bodies. Proper storage, handling, and disposal procedures should be followed to minimize the risks associated with nickel dichloride.
| Hazard Symbols | Corrosive, Harmful, Environmental Hazard |
| Safety Description | – Wear protective gloves and clothing – Avoid inhalation of dust or vapors – Prevent ingestion – Store, handle, and dispose of properly |
| Un IDs | UN3288 |
| HS Code | 2827.39.80 |
| Hazard Class | 8 (Corrosive) |
| Packing Group | III |
| Toxicity | Harmful if swallowed, causes skin and eye irritation |
Nickel Chloride Synthesis Methods
There are several methods for synthesizing nickel dichloride, each with its own advantages and applications.
One common method involves the reaction between nickel metal or nickel oxide with hydrochloric acid. In this process, one adds nickel metal or nickel oxide to a suitable container and stirs while slowly adding hydrochloric acid. The reaction between the nickel and acid produces nickel dichloride along with the release of hydrogen gas.
Another synthesis method involves the reaction between nickel carbonate and hydrochloric acid. The hydrochloric acid dissolves nickel carbonate, and the heated solution undergoes a reaction to form nickel dichloride and release carbon dioxide gas.
Hydrochloric acid undergoes a reaction with dissolved nickel hydroxide when the solution is heated or allowed to stand, resulting in the synthesis of nickel dichloride. The reaction leads to the formation of nickel dichloride and water.
Furthermore, one can prepare nickel dichloride by reacting nickel metal with chlorine gas. This direct reaction between the two elements yields nickel dichloride.
These synthesis methods provide different routes for obtaining nickel dichloride, allowing for flexibility in terms of starting materials and reaction conditions. The choice of method depends on factors such as the desired purity of the final product, availability of starting materials, and specific application requirements.
Nickel Chloride Uses
Nickel dichloride has various applications across different industries due to its unique properties. Here are some of its notable uses:
- Electroplating: Electroplating processes commonly employ nickel dichloride to provide a protective and decorative coating on various surfaces. Nickel dichloride enhances the appearance of metals like steel, brass, and copper while imparting corrosion resistance.
- Catalyst: Nickel dichloride acts as a catalyst in numerous chemical reactions, including hydrogenation and polymerization processes. It facilitates the conversion of reactants into desired products and finds application in the production of pharmaceuticals, plastics, and synthetic fibers.
- Chemical synthesis: Nickel dichloride serves as a precursor in the synthesis of various nickel compounds, such as nickel oxide, nickel sulfide, and nickel cyanide. Industries utilize these compounds in catalysts, pigments, ceramics, and magnetic materials.
- Batteries: Rechargeable batteries, particularly nickel-metal hydride (NiMH) batteries, use nickel dichloride as an electrolyte. It enables the flow of ions between the electrodes during charging and discharging cycles.
- Gas purification: Industries employ nickel dichloride in gas purification processes to remove impurities like hydrogen sulfide and carbon monoxide. It finds application in natural gas refining and petrochemical processing.
- Animal feed supplement: Livestock diets, particularly in poultry and swine, incorporate nickel dichloride as a nutritional supplement. It aids in enzyme activity and contributes to the overall health and growth of animals.
- Laboratory research: Researchers utilize nickel dichloride in various laboratory experiments, including nickel-catalyzed reactions and as a source of nickel ions for chemical analysis.
These diverse applications demonstrate the versatility and significance of nickel dichloride in industries ranging from manufacturing and energy to agriculture and research.
Questions:
Q: What ions are present in an aqueous solution of NiCl2?
A: In an aqueous solution of NiCl2, the ions present are Ni2+ (nickel cation) and Cl- (chloride anion).
Q: Is NiCl2 soluble in water?
A: Yes, NiCl2 is soluble in water, forming a greenish-yellow aqueous solution.
Q: Which metal reacts spontaneously with NiCl2(aq)?
A: Metals such as magnesium (Mg) and zinc (Zn) react spontaneously with NiCl2(aq) to displace nickel and form their respective chlorides.
Q: Is NiCl2 polar or nonpolar?
A: NiCl2 is a polar compound due to the electronegativity difference between nickel and chlorine, resulting in an uneven distribution of charge.
Q: Is NiCl2 aqueous?
A: Yes, NiCl2 can exist in the aqueous state when dissolved in water, forming an aqueous solution.
Q: What is the name of the compound with the formula NiCl2?
A: The compound with the formula NiCl2 is called nickel(II) chloride.
Q: How would you prepare 1.00 L of a 0.50 M solution of NiCl2?
A: To prepare a 0.50 M solution of NiCl2, dissolve 129.6 grams of NiCl2 in water and make up the volume to 1.00 L.
Q: What is the insoluble salt formed between a solution of Na2S and NiCl2?
A: When a solution of Na2S is mixed with NiCl2, insoluble nickel sulfide (NiS) is formed.
Q: Is NiCl2(aq) a solid?
A: No, NiCl2(aq) refers to an aqueous solution of NiCl2, indicating it is in a liquid form.
Q: What makes the crystal nickel(II) chloride green?
A: The green color of crystal nickel(II) chloride is attributed to the presence of the nickel cations (Ni2+) in the crystal lattice.
Q: Is nickel dichloride toxic?
A: Yes, nickel dichloride is toxic and should be handled with caution. It can cause skin irritation, and respiratory issues, and is harmful if ingested.
Q: Does a reaction occur when aqueous solutions of NiCl2 and Na2S are combined?
A: Yes, a reaction occurs when aqueous solutions of NiCl2 and Na2S are combined, resulting in the formation of insoluble nickel sulfide (NiS) and soluble sodium chloride (NaCl).
Q: How many grams of NiCl2 are required to neutralize 75.0 mL of 0.555 M lithium hydroxide?
A: Approximately 18.4 grams of NiCl2 are required to neutralize 75.0 mL of 0.555 M lithium hydroxide in a stoichiometric reaction.
Q: What happens when you mix ammonium carbonate, nickel dichloride, and water?
A: When ammonium carbonate, nickel dichloride, and water are mixed, a reaction occurs resulting in the formation of ammonium chloride, nickel carbonate, and water.