Lithium chloride (LiCl) is a compound used in batteries and air conditioning systems. It absorbs moisture, making it an effective desiccant.
| IUPAC Name | Lithium chloride |
| Molecular Formula | LiCl |
| CAS Number | 7447-41-8 |
| Synonyms | Lithium monochloride, Lithium(I) chloride |
| InChI | InChI=1S/ClH.Li/h1H; |
Lithium Chloride Properties
Lithium Chloride Formula
The chemical formula of lithium monochloride is LiCl. It consists of one lithium-ion (Li+) and one chloride ion (Cl-). This simple formula represents the composition of lithium monochloride in a precise and compact manner.
Lithium Chloride Molar Mass
Lithium monochloride has a molar mass of approximately 42.39 grams per mole (g/mol). This value is obtained by adding the atomic masses of lithium (6.94 g/mol) and chlorine (35.45 g/mol). Molar mass is crucial in various chemical calculations.
Lithium Chloride Boiling Point
The boiling point of lithium monochloride is relatively high at around 1,382 degrees Celsius (2,520 degrees Fahrenheit). At this temperature, lithium monochloride transforms from a liquid to a gaseous state, making it useful in high-temperature applications.
Lithium Chloride Melting Point
Lithium monochloride has a relatively low melting point of about 614 degrees Celsius (1,137 degrees Fahrenheit). At this temperature, the solid lithium monochloride turns into a liquid, allowing for various applications in industries like metallurgy and pharmaceuticals.
Lithium Chloride Density g/mL
The density of lithium monochloride is approximately 2.07 grams per milliliter (g/mL). This density value is relatively high, making lithium monochloride a dense compound that can be used in various processes, including as a solvent and in nuclear applications.
Lithium Chloride Molecular Weight
The molecular weight of lithium monochloride is approximately 42.39 grams per mole (g/mol). This value is determined by adding the atomic weights of lithium and chlorine in one mole of lithium monochloride.
Lithium Chloride Structure
Lithium monochloride adopts a simple ionic crystal lattice structure. It consists of alternating layers of lithium and chloride ions, held together by strong electrostatic forces of attraction. This arrangement contributes to the compound’s stability and properties.
Lithium Chloride Solubility
Lithium monochloride is highly soluble in water, meaning it can dissolve easily in this solvent. It forms a clear and colorless solution. The solubility of lithium monochloride in water is vital for its applications in various chemical processes and as a desiccant in air conditioning systems.
| Appearance | White solid |
| Specific Gravity | 2.07 g/mL |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 42.39 g/mol |
| Density | 2.07 g/mL |
| Melting Point | 614°C (1,137°F) |
| Boiling Point | 1,382°C (2,520°F) |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble |
| Solubility | Soluble in polar solvents such as ethanol, acetone, pyridine |
| Vapour Pressure | Low |
| Vapour Density | 1.99 (air = 1) |
| pKa | ~ -1 (in water) |
| pH | ~ 7 (aqueous solution) |
Lithium Chloride Safety and Hazards
Lithium monochloride poses some safety and hazard concerns. It can irritate the skin, eyes, and respiratory system upon contact or inhalation. When ingested, it may cause gastrointestinal discomfort. Care should be taken to handle it with protective equipment, including gloves and goggles. Lithium monochloride is not combustible but can release toxic fumes when heated. Avoid direct contact with the substance and ensure proper ventilation when working with it. In case of accidental exposure or ingestion, seek medical attention immediately. Following proper handling procedures and safety protocols is crucial to minimize potential risks and ensure safe usage.
| Hazard Symbols | Irritant |
| Safety Description | Causes skin and eye irritation. Harmful if swallowed or inhaled. Use with adequate ventilation. Wear protective gear. Avoid direct contact. In case of exposure, seek medical attention. |
| UN IDs | UN 2056 |
| HS Code | 2827391000 |
| Hazard Class | 8 (Corrosive substances) |
| Packing Group | III |
| Toxicity | Low toxicity; irritation potential |
The hazard symbol indicates that lithium monochloride can cause skin and eye irritation and presents harmful effects if swallowed or inhaled. It falls under Hazard Class 8, designated for corrosive substances. The toxicity level of lithium monochloride is generally considered low. Proper handling, safety measures, and personal protective equipment should be employed to ensure safe use and avoid any potential health risks.
Lithium Chloride Synthesis Methods
Various methods enable the synthesis of lithium monochloride.
One common approach involves reacting lithium metal with hydrogen chloride gas. During this process, the lithium metal displaces the hydrogen in the hydrogen chloride gas, resulting in the formation of lithium monochloride and the liberation of hydrogen gas. The chemical equation for this synthesis is:
2 Li + 2 HCl → 2 LiCl + H2
Another method is the reaction of lithium carbonate (Li2CO3) with hydrochloric acid (HCl). In this reaction, lithium carbonate reacts with hydrochloric acid to produce lithium monochloride, water, and carbon dioxide gas. The chemical equation for this synthesis is:
Li2CO3 + 2 HCl → 2 LiCl + H2O + CO2
In the synthesis process, one can use lithium hydroxide (LiOH) to produce lithium monochloride. When lithium hydroxide reacts with hydrochloric acid, it yields lithium monochloride and water. The chemical equation for this reaction is:
LiOH + HCl → LiCl + H2O
These methods provide effective ways for producing lithium monochloride for various industrial and research purposes. However, you must exercise caution due to the reactivity of certain reactants involved. Always adhere to appropriate safety precautions throughout the procedure.
Lithium Chloride Uses
Lithium monochloride finds diverse applications across several industries due to its unique properties. Here are some key uses:
- Batteries: Manufacturers use lithium monochloride in the production of lithium-ion batteries, which empower various devices like smartphones, laptops, and electric vehicles. Its efficient ion-conducting ability enhances battery performance.
- Air Conditioning: Air conditioning systems employ lithium monochloride as a desiccant to absorb moisture, thereby reducing humidity and improving cooling efficiency.
- Pharmaceuticals: Certain pharmaceutical preparations and research applications in the field of neuroscience and psychiatry utilize lithium monochloride.
- Metallurgy: It acts as a flux in metallurgical processes, promoting the fusion of metal ores and enhancing the efficiency of refining processes.
- Catalysts: Lithium monochloride serves as a catalyst in certain chemical reactions, facilitating the conversion of reactants to desired products.
- Pyrotechnics: It imparts a vivid red color to fireworks and flares, making it a valuable component in pyrotechnic formulations.
- Heat Treatment: In metal heat treatment processes, practitioners use lithium monochloride as a heat transfer medium for controlling the temperature and enhancing heat distribution.
- Chemical Synthesis: Lithium monochloride participates in various chemical syntheses, including the preparation of other lithium compounds.
With its versatile applications, lithium monochloride continues to play a vital role in modern industries, contributing to technological advancements and enhancing various manufacturing processes.
Questions:
Q: Is lithium chloride soluble in water?
A: Yes, lithium monochloride is highly soluble in water.
Q: What color does lithium chloride burn?
A: Lithium monochloride burns with a bright red color.
Q: Where to buy lithium chloride?
A: Lithium monochloride can be purchased from chemical suppliers or online stores.
Q: A student weighed 0.550 g of lithium chloride, LiCl, to use in a reaction. How many moles is this?
A: The number of moles of lithium monochloride is approximately 0.0097 moles.
Q: Is lithium chloride a solid, liquid, or gas?
A: Lithium monochloride is a solid at room temperature.
Q: Lithium monochloride solid?
A: Yes, lithium monochloride exists as a solid crystal structure.
Q: How many bonds does each atom have in lithium chloride?
A: Lithium forms one bond, and chlorine forms one bond in lithium monochloride.
Q: How to identify lithium chloride?
A: Lithium monochloride can be identified by its white color and its ability to dissolve in water.
Q: Is lithium chloride soluble in water?
A: Yes, lithium monochloride is highly soluble in water.
Q: How to make lithium chloride from an acid and an alkali?
A: Lithium monochloride can be synthesized by reacting lithium hydroxide (alkali) with hydrochloric acid.
Q: Is LiCl ionic or covalent?
A: Lithium monochloride (LiCl) is ionic in nature.
Q: Which has the largest lattice enthalpy radius LiCl or MgCl2?
A: MgCl2 has a larger lattice enthalpy compared to LiCl due to the higher charge of the magnesium ion and its smaller ionic radius.