月: 2023年1月

What Is Zinc Chloride?

Zinc chloride is a compound of zinc and chlorine with the chemical formula ZnCl2. Zinc chloride exists in anhydrous form as well as several hydrates, which form at temperatures below 28 degrees Celsius.

It is a white crystalline powder that is deliquescent and has a very high affinity for water. It is extremely soluble in water and is also soluble in ethanol, acetone, and ether.

Zinc chloride is obtained by reacting metallic zinc with hydrochloric acid. In the recycling process for obtaining purified zinc chloride and high-purity zinc from electric furnace dust, zinc chloride is produced by allowing chlorine gas to act on crude zinc oxide.

Uses of Zinc Chloride

Zinc chloride is used in the zinc plating process. Among the bath types used for zinc plating, zinc chloride baths can be used to plate materials that are difficult to plate with zinc (castings, high carbon steel).

Zinc chloride has a so-called astringent effect that constricts blood vessels, mucous membranes, and skin tissue. Therefore, in the medical field, low concentrations of zinc chloride solutions are used to treat nasopharyngitis and nasopharyngitis. It is also used in mouth rinses and toothpastes because of its ability to prevent bad breath.

Other uses include wood preservative, material for dry cell batteries, and flux for soldering.

What Is Lithium Chloride?

Lithium chloride, denoted as LiCl, is an ionic compound composed of lithium and chlorine. Known for its chloride ion generation in solution, lithium ions act as Lewis acids. This compound is highly relevant in various industrial applications due to its unique properties.

Uses of Lithium Chloride

Lithium chloride serves multiple purposes:

1. Raw Material for Lithium Metal

It is crucial in producing lithium metal through the electrolysis of a molten mixture of lithium chloride and potassium chloride at 450°C.

2. Additives for Coupling Reactions

In organic synthesis, lithium chloride accelerates the Migita-Kosugi-Stille coupling reaction, enhancing the formation of carbon-carbon bonds.

3. Miscellaneous Uses

Its applications extend to acting as an auxiliary agent for aluminum soldering, a dehumidifying agent in air conditioning, and a flame retardant in fireworks due to its red flame coloration.

Properties of Lithium Chloride

Lithium chloride is a colorless crystal with a molecular weight of 42.39 and CAS number 7447-41-8. It melts at 614°C and boils at 1357°C, showing notable hygroscopicity and solubility in water and polar organic solvents. Its aqueous solutions are neutral to slightly alkaline.

Types of Lithium Chloride

Unlike other alkali metal chlorides, lithium chloride forms various hydrates, including monohydrate, trihydrate, and pentahydrate.

Other Information About Lithium Chloride

1. Production

Lithium chloride is produced by reacting lithium carbonate or hydroxide with hydrochloric acid, requiring corrosion-resistant equipment due to its corrosive nature.

2. Handling and Storage

Handling precautions include avoiding contact with strong oxidizers and wearing protective gear due to its corrosiveness and potential toxicity. In case of fire, various extinguishing mediums can be used. It should be kept in a cool, dark place in a sealed container.

What Is Manganese Chloride?

Manganese chloride is a chemical compound combining manganese and chlorine, predominantly known as manganese(II) chloride or manganese dichloride. With a chemical formula of MnCl₂, it is vital to handle this compound carefully due to the risk of manganese poisoning from prolonged exposure to its powder or vapor.

Uses of Manganese Chloride

Manganese(II) chloride has diverse applications across various industries. It is utilized in dyeing, pigment production for ceramics, and pharmaceuticals, and as a catalyst in chloride synthesis. Other notable uses include paint desiccants, accelerators in chemical fertilizers, desiccants in printing inks, components in dry cell batteries, fluxes for light alloys, glass, zeolites, and as a contrast agent for MRI in medicine.

Properties of Manganese Chloride

This compound forms a pale red crystal, slightly soluble in ethanol and water. Its aqueous solution is mildly acidic, producing a pale red tetrahydrate MnCl₂・4H₂O under specific conditions. Manganese chloride is crucial in synthesizing various manganese compounds, acting as a weak Lewis acid.

Structure of Manganese Chloride

The anhydrous form of manganese chloride showcases a hexagonal cadmium chloride-type crystal structure and exhibits paramagnetism. Both dihydrate and tetrahydrate forms of manganese chloride are also recognized.

Other Information on Manganese Chloride

1. Manganese(II) Chloride Synthesis

Naturally occurring in places like Vesuvius, manganese(II) chloride can be synthesized through reactions involving chlorine and manganese or by reducing manganese(IV) oxide with hydrochloric acid, a process historically used in chlorine production.

2. Reaction of Manganese(II) Chloride

Reactions with organic compound ligands can form trivalent manganese complexes through air oxidation. Manganese(II) chloride is notably used in synthesizing organomanganese compounds like manganocene under anhydrous conditions.

3. Characteristics of Manganese(III) Chloride

Manganese(III) chloride, a black powder, can be synthesized by reacting manganese acetate with hydrogen chloride at low temperatures. It is thermally unstable and forms a brown chloro complex solution when reacted with chlorine in a concentrated hydrochloric acid solution of manganese(II) chloride.

What Is Magnesium Chloride?

Magnesium chloride, with the formula MgCl₂・6H₂O, is an inorganic compound derived from the reaction of magnesium hydroxide and hydrochloric acid. Commonly referred to as “salt mag,” it is a major component of bittern—a solution left after sodium chloride is extracted from seawater.

This compound is produced both as a byproduct of salt production and in the manufacture of titanium tetrachloride from titanium metal, resulting in both hexahydrate (MgCl₂・6H₂O) and anhydrous (MgCl₂) forms.

Uses of Magnesium Chloride

Magnesium chloride is versatile, used as a coagulant in tofu production and civil engineering as an anti-icing agent, wood preservative, fire-resistant material, and as a base for magnesia cement. In healthcare, it serves as a laxative, dialysis fluid, and infusion solution. The anhydrous form is crucial for producing magnesium metal, acting as a desiccant and exothermic agent, and as a catalyst precursor.

Properties of Magnesium Chloride

Magnesium chloride exists primarily in hexahydrate and anhydrous forms, with the hexahydrate being a highly soluble white crystal and the anhydrous form being known for its exothermic dissolution in water.

1. MgCl₂・6H₂O

This hexahydrate form is a white crystal with a solubility of 160 g/100ml in water and can hydrolyze at high temperatures to form magnesium hydroxide chloride and magnesia.

2. MgCl₂

The anhydrous form is also a white crystal, with a solubility of 54 g/100 ml in water, and exhibits significant exothermicity upon dissolution.

Other Information on Magnesium Chloride

How Magnesium Chloride Is Produced

Magnesium chloride is primarily extracted from bittern. The production process involves removing bromide and sulfate from bittern, then concentrating the solution to precipitate and separate potassium chloride and magnesium chloride crystals.

Anhydrous magnesium chloride can be produced by dehydrating the hexahydrate form, using methods like heating in hydrochloric acid gas or adding ammonium chloride. Additionally, magnesium chloride is a byproduct of titanium smelting in the Kroll process, where titanium tetrachloride is reduced with magnesium, yielding magnesium chloride as a byproduct.

What Is Benzoyl Chloride?

Benzoyl chloride, a colorless liquid with a pungent odor, is a simple aromatic acid halide derived from benzoic acid. It has a molar mass of 140.6 g/mol, with melting and boiling points of -1°C and 197°C, respectively. Its CAS number is 98-88-4.

This compound can be produced through the chlorination of benzoic acid using phosphorus pentachloride, thionyl chloride, or phosgene. Another method involves the partial hydrolysis of trichloromethylbenzene.

Properties of Benzoyl Chloride

Benzoyl chloride reacts with water to form benzoic acid and hydrogen chloride, necessitating careful storage to prevent exposure to moisture. It is toxic and can irritate the skin, eyes, and mucous membranes. Decomposition produces corrosive and highly toxic gases like hydrogen chloride and sulfur dioxide. Proper ventilation and explosion-proof equipment are essential due to the risk of forming explosive mixtures above 72°C.

Uses of Benzoyl Chloride

Benzoyl chloride is utilized in various applications, including:

1. Organic Chemistry

Its reactive thionyl chloride moiety makes it a versatile reagent in esterification reactions with alcohols and in producing benzoyl derivatives with phenol, amines, and other nucleophiles. It acts as a benzoylating agent, facilitating carbon-carbon and heteroatom bond formation. Moreover, it’s involved in the Kurtius transition for synthesizing amines, including routes to pharmaceuticals like Tamiflu, and is used in Friedel-Crafts reactions.

2. Synthesis of Substances

By reacting with sodium peroxide, benzoyl chloride can be converted into benzoyl peroxide, a radical polymerization initiator and curing agent for unsaturated polyesters. It also serves as a synthetic intermediate for dyes, chemicals, and fragrances, highlighting its importance in the chemical industry.

Other Information on Benzoyl Chloride

Legal Information

Regulated under various laws, benzoyl chloride is categorized as a flammable liquid and a deleterious substance, emphasizing the need for cautious handling and compliance with safety regulations.

What Is Vinyl Chloride?

Vinyl chloride, an organic compound known as chloroethylene or chloroethene, consists of vinyl groups and chlorine. It is regulated under multiple laws due to its potential health risks, including being designated as a “Class 2 Monitoring Chemical Substance” and a “Class 2 Specified Chemical Substance” under various safety and health regulations.

Uses of Vinyl Chloride

Primarily, vinyl chloride is transformed into polyvinyl chloride (PVC), a polymer with widespread applications. PVC pipes, known for their mechanical stability, durability, and flame resistance, are used in various sectors such as construction, automotive, home appliances, and medical equipment. Soft PVC finds application in synthetic leather for furniture and clothing, enhancing its versatility.

Properties of Vinyl Chloride

With a melting point of -154°C and a boiling point of -13°C, vinyl chloride is highly reactive, facilitating easy polymerization under light and catalysts. Notably, it has been identified as a carcinogen linked to hepatic angiosarcoma, leading to regulatory measures limiting its use, despite ongoing production for PVC manufacturing.

Structure of Vinyl Chloride

The molecular structure of vinyl chloride, CH₂=CHCl, allows for addition polymerization to form polyvinyl chloride, denoted as [-CH₂-CHCl-]n, showcasing its fundamental role in PVC production.

Other Information on Vinyl Chloride

1. Vinyl Chloride Synthesis

Synthesized through direct chlorination and oxychlorination, vinyl chloride production involves reacting ethylene with chlorine in the presence of iron (III) chloride catalyst to form 1,2-dichloroethane, which is then decomposed to vinyl chloride. This process minimizes by-products, reducing environmental impact.

2. Synthesis of Polyvinyl Chloride

Polyvinyl chloride (PVC) is produced by polymerizing vinyl chloride monomers, distinguishing PVC from its monomer form and highlighting its importance in various applications.

What Is Barium Chloride?

Barium chloride is an inorganic compound with the formula BaCl₂. It exists as anhydrous, monohydrate, and dihydrate forms, with the dihydrate being the most commonly available. The CAS registration numbers are 10361-37-2 for the anhydrous form and 10326-27-9 for the dihydrate.

Classified by the GHS as acutely toxic when ingested, it is also corrosive to skin, irritating to eyes, and toxic to specific target organs upon both single and repeated exposure.

Uses of Barium Chloride

Barium chloride is utilized in various applications, including as a component in organic pigments, paper fillers, metal heat treatment agents, roentgen contrast media, and phosphors.

1. Raw Material for Barium Salts

Its primary use is as a precursor for other barium salts, such as barium sulfate, which serves as a bulking agent in paint and rubber, and as an X-ray contrast agent. Barium sulfate is produced either by reacting barium sulfide with sodium sulfate or through a coprecipitation reaction with barium chloride and sodium sulfate.

2. Turbidimetric Analysis of Sulfate

Barium chloride plays a crucial role in the turbidimetric analysis of sulfate ions, where it forms insoluble barium sulfate upon reaction with sulfate ions for both qualitative and quantitative analysis.

Properties of Barium Chloride

1. Basic Information on Barium Chloride (Anhydrous)

The anhydrous form has a molecular weight of 208.23, melts at 961°C, and boils at 1,560°C. It appears as a white solid at room temperature, with a density of 3.9 g/mL, and is highly soluble in water but has low solubility in alcohols.

2. Basic Information on Barium Chloride (Dihydrate)

The dihydrate form, with a molecular weight of 244.26, also melts at 962°C and boils at 1,560°C. It appears as white crystals or powder, becomes anhydrous at 121°C, and is highly soluble in water but virtually insoluble in ethanol.

Types of Barium Chloride

Barium chloride is commercially available in forms suitable for both research and industrial use, predominantly sold as the dihydrate form, with limited availability of anhydrous and monohydrate forms from some suppliers.

1. Reagent Products for Research and Development

For research and development, it is mainly available as dihydrate, with some anhydrous forms, or as a 10 w/v% solution. Available in quantities like 25g, 100g, and 500g, these reagents are designed for easy laboratory handling and can be stored at room temperature.

2. Industrial Chemicals

In the industrial sector, barium chloride is typically sold as dihydrate, though monohydrate forms are also offered by some manufacturers. Sold in larger quantities, such as 25 kg, specific product inquiries should be directed to individual manufacturers.

Other Information on Barium Chloride

1. Synthesis of Barium Chloride

Barium chloride can be synthesized by reacting barium hydroxide or barium carbonate with hydrochloric acid. Industrial production methods often involve melting baryte with calcium chloride or reacting barium sulfide with hydrochloric acid.

2. Regulations on Barium Chloride

Due to its hazardous nature, barium chloride is regulated under various health and safety laws, requiring proper labeling, notification, and risk assessments. It is also classified as a deleterious substance under poison control laws, necessitating careful handling in compliance with regulatory standards.

What Is Nickel Chloride?

Nickel chloride, a chemical compound, is known for its hazardous properties.

Classified by the GHS as acutely toxic, skin and respiratory sensitizer, carcinogenic, and toxic for reproduction, it also poses risks of specific target organ toxicity from single and repeated exposure. Nickel chloride exists in anhydrous, monohydrate, and hexahydrate forms.

As a carcinogen, it is regulated under various laws, which require it to be labeled and notified. It is also designated as a “priority evaluation chemical substance” and a “specified Class I designated chemical substance” under environmental protection laws.

Uses of Nickel Chloride

Nickel chloride is utilized in various industrial processes, such as in ammonia gas absorbents, nickel plating, dyes, and batteries. In complex chemistry, it serves as a precursor for nickel complexes and is used as an additive and reagent in organic synthesis, especially in nickel plating to increase solution solubility and as a source of nickel ions in plating baths.

Its role extends to providing chloride ions, enhancing the corrosive action necessary for nickel dissolution during anodic reactions.

Properties of Nickel Chloride

This compound appears as a pale yellowish-orange mass, crystal, or powder and is hygroscopic. The hexahydrate form, commonly used, is green to yellowish-green and deliquescent, soluble in water and alcohols.

Divalent nickel in nickel chloride has two unpaired electrons, leading to antimagnetic properties in planar four-coordinated nickel complexes.

Structure of Nickel Chloride

Nickel chloride, with the chemical formula NiCl₂, has an anhydrous salt formula weight of 129.59 and a specific gravity of 3.55. The hexahydrate has a formula weight of 237.69 and a specific gravity of 1.92, sharing a crystal structure similar to cadmium chloride. The Ni-Cl bonds exhibit ionic characteristics, with each Ni²⁺ center coordinated to six Cl⁻ ions.

In hexahydrate form, NiCl₂•6H₂O, only four water molecules directly bind to nickel, forming a complex with two additional water molecules weakly associated.

Other Information on Nickel Chloride

1. Nickel Chloride Synthesis Methods

Production involves dissolving metallic nickel, nickel oxide, or nickel carbonate in hydrochloric acid, followed by dehydration under hydrogen chloride gas to obtain the anhydrous form, indicated by a color change from green to yellow.

2. Reaction Using Nickel Chloride

Figure 1. Reaction Using Nickel Chloride

Nickel chloride and its hydrates facilitate various organic synthetic reactions. It acts as a weak Lewis acid in regioisomerization of dienols and, combined with chromium(II) chloride, synthesizes allyl alcohols from vinyl iodide and aldehydes. It is also useful in reductions with lithium aluminum hydride and preparing nickel boride with sodium borohydride.

3. Complexes of Nickel Chloride

Figure 2. Complexes Obtained From Nickel Chloride

Nickel chloride hexahydrate readily exchanges its H₂O molecules with ammonia, amines, phosphines, thioethers, and thiolates, forming various complexes such as the purple octahedral [Ni(NH₃)₆]Cl₂, the orange planar tetrahedral NiCl₂(Ph₂PCH₂CH₂PPh₂), the colorless planar tetrahedral [Ni(CN)₄]^2-, and the blue tetrahedral [NiCl₄]^2-.

4. Reactions Using Nickel Chloride Complexes

Figure 3. Reaction Using Nickel Chloride Complex

NiCl₂-glyme complexes, more soluble than the hexahydrate, find use in various reactions. Nickel(II) acetylacetonate, a precursor to bis(1,5-cyclooctadiene)nickel, can be synthesized from nickel chloride.

What Is Sodium Chloride?

Sodium chloride, the main component of seawater, naturally occurs as rock salt.

Commonly known as salt or dietary salt, sodium chloride was initially used for food or medical purposes. Today, it is mass-produced in factories through seawater refinement using ion exchange membranes, among other processes. In laboratories, sodium chloride can be synthesized by neutralizing hydrochloric acid with sodium hydroxide.

Sodium chloride plays a crucial role in maintaining osmotic pressure in the blood and tissues of animals.

Uses of Sodium Chloride

Sodium chloride serves as a raw material for various sodium compounds and is the primary ingredient in salt, widely used in seasonings. Its antiseptic and sterilizing properties make it essential for preparing salted and preserved foods.

In cosmetics, sodium chloride is used to adjust thickness, stabilize emulsions and suspensions, and as an electrolyte supplement due to its significant physiological roles. It also acts as a solubilizer, buffer, boiler water softener, and anti-freeze agent, lowering the water’s freezing point.

Properties of Sodium Chloride

Sodium chloride dissolves well in water but not in ethanol. It forms an ionic crystal of sodium and chloride ions. In its crystalline form, it is an insulator, but its aqueous solutions conduct electricity.

Odorless and with a distinctive salty taste, pure sodium chloride remains non-deliquescent up to 75% humidity at 20°C (68°F).

It has a density of 2.16 g/cm³, a melting point of 800.4°C, and a boiling point of 1,413°C. Sodium chloride conducts electricity when melted, separating into chloride and sodium ions.

Sodium chloride, NaCl, has a formula weight of 58.44. It is a colorless crystalline solid with a face-centered cubic lattice and octahedral coordination.

Other Information About Sodium Chloride

1. Crystallization of Sodium Chloride

Sodium chloride’s solubility changes little with temperature, yielding only a small amount of crystals upon cooling. Evaporation or the introduction of hydrogen chloride gas is used to concentrate sodium chloride solutions for crystallization.

2. Sodium Chloride as a Resource

Seawater and rock salt are abundant sources of sodium chloride, contributing to the annual global production of 280 million tons. Japan, one of the largest salt importers, imports around 7 million tons yearly, with a self-sufficiency rate of about 11%, relying heavily on imports for industrial salt despite its island geography.

3. Applications of Sodium Chloride

Sodium chloride’s versatility extends to fire extinguishing agents for metallic sodium, magnesium, and potassium fires, enhancing fluidity and moisture resistance when mixed with low melting point cross-linking agents. It is colored light blackish brown for identification.

It is also used in infrared optics as prisms, lenses, and windows, and in rubber manufacturing for neoprene, buna, and white rubber. Additionally, saltwater and sulfuric acid coagulate emulsified latex in rubber production.

Due to its hygroscopic nature, sodium chloride serves as an inexpensive desiccant and regenerates ion exchange resins in water-softening systems. It is a common educational tool in schools for studying solubility changes.

What Is Thionyl Chloride?

Figure 1. Basic Information on Thionyl Chloride

Thionyl chloride is a colorless liquid with a pungent odor and fuming properties.

It is also known as sulfinyl chloride or thionyl chloride. Thionyl chloride, in liquid or vapor form, is toxic because it is harmful to skin and mucous membranes.

Thionyl chloride is classified as a “deleterious substance” under the Poisonous and Deleterious Substances Control Law, and as a “hazardous and noxious substance” and “hazardous and noxious substance requiring notification of name, etc.” under the Industrial Safety and Health Law.

Uses of Thionyl Chloride

Thionyl chloride is used to replace hydroxyl and mercapto groups with chlorine atoms in the organic synthesis of dyes, medicine, and agricultural chemicals. Thionyl chloride can also be used to introduce sulfone groups by reacting with Grignard reagents. Other uses include use as a dehydrating agent to obtain anhydrous metal halides.

Thionyl chloride in liquid form is useful as a cathode active material in thionyl chloride lithium batteries. Thionyl lithium chloride batteries are widely used for backup of memory ICs, power supplies for electronic equipment, and power supplies for electricity, gas, and water meters.

Properties of Thionyl Chloride

Thionyl chloride has a fuming and pungent odor, a melting point of -104.5°C, and a boiling point of 76°C. It begins to decompose when heated above 140°C and decomposes completely only at 500°C. Decomposition of thionyl chloride yields sulfur dioxide (SO₂), disulfur dichloride (S₂Cl₂), and chlorine (Cl₂).

Thionyl chloride mixes with solvents such as benzene and chloroform. It also reacts with water in a vigorous exothermic reaction to form hydrogen chloride (HCl) and sulfur dioxide (SO₂).

Structure of Thionyl Chloride

Figure 2. Detailed Structure of Thionyl Chloride

Thionyl chloride is a sulfurous acid chloride-like compound with the chemical formula SOCl₂, a liquid with a molecular weight of 118.97 and a specific gravity of 1.65 g/cm³. The sulfur-oxygen bond (S-O) is approximately 143 pm and the sulfur-chlorine bond (S-Cl) is approximately 207 pm in length.

The thionyl chloride molecule has a triangular pyramidal shape. ∠O-S-Cl and ∠Cl-S-Cl are 107.4° and 96.5°, respectively.

Other Information on Thionyl Chloride

1. Synthesis of Thionyl Chloride

Thionyl chloride is obtained by distillation of phosphoryl chloride (POCl₃), which is produced by the reaction of phosphorus pentachloride (PCl₅) with sulfur dioxide (SO₂). Thionyl chloride can also be produced by the reaction of sulfur trioxide (SO₃) with sulfur dichloride (SCl₂).

Instead of sulfur trioxide, thionyl chloride can be produced by oxidation with fuming sulfuric acid (Oleum) or chlorosulfonic acid (ClSO₃H). The reaction is easier when a catalyst such as antimony chloride is used.

Thionyl chloride can also be obtained by reacting a mixture of sulfur dioxide (SO₂) and sulfur tetrachloride (SCl₄) using an activated carbon catalyst and distilling the product.

2. Reaction of Thionyl Chloride

Figure 3. Reaction of Thionyl Chloride With Alcohol

Thionyl chloride is often used to chlorinate carboxylic acids and alcohols. Unlike other halogenating agents, the products of the reaction are gases such as HCl and SO₂, and thionyl chloride has a low boiling point, making it easy to remove from the reaction system.

In addition to that, chlorination of alcohols with thionyl chloride does not proceed in the S_N1 or S_N2 reactions as with other chlorinating agents. Therefore, the reaction occurs in a sterically preserved manner without Walden inversion. A four-membered ring transition state has been proposed as the reaction mechanism and is called the S_Ni mechanism.

3. Storage of Thionyl Chloride

It is recommended that thionyl chloride be stored in a cool, dark, well-ventilated place with the container tightly closed and away from moisture and direct sunlight. Hydrolysis occurs when exposed to moisture, and hydrochloric acid is formed when reacting violently.