Theo Nash
Chlorine is a highly reactive non-metal that readily forms compounds when reacting with metals. When chlorine and aluminum react with ethyl alcohol, they form chloroform, chloral, and CCl4.
| Characteristics | Values |
|---|---|
| Reaction | Chlorine reacts with ethyl alcohol |
| Products | Chloroform, chloral, CCl |
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What You'll Learn
Chlorine and ethyl alcohol form chloroform, chloral, and CCl
When chlorine reacts with ethyl alcohol, or ethanol, several products can be formed, including ethyl chloride, chloroform, and tetrachloride. This reaction involves a substitution reaction where the hydroxyl group (-OH) is replaced by a chlorine atom.
Chloroform, or trichloromethane, is a volatile, colorless, sweet-smelling, dense liquid with a low boiling point and low global warming potential. It was once used as an inhalational anesthetic in the 19th and 20th centuries. Chloroform can be formed through various processes, including the reaction of chlorine with ethanol, the action of chlorine bleach on ethanol, and the reaction of chlorinated lime with ethanol.
Chloral is another product that can be formed when chlorine reacts with ethyl alcohol. Chloral has been studied by various investigators, including Moldenhawer, a German pharmacist who produced chloral in 1830 by mixing chlorinated lime with ethanol. Justus von Liebig further studied chloral through alkaline cleavage.
The reaction between chlorine and ethyl alcohol can also lead to the formation of CCl, which is believed to be a by-product of water chlorination. This reaction can result in a range of disinfection by-products, which may be present in municipal tap water and swimming pools.
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Aluminium chloride is manufactured at high temperatures
Aluminium chloride (AlCl3) is manufactured on a large scale through the exothermic reaction of aluminium metal with chlorine or hydrogen chloride. This reaction typically occurs at high temperatures, ranging from 650°C to 750°C. At these elevated temperatures, the aluminium metal combines with chlorine to form aluminium chloride.
AlCl3 exhibits different structural forms depending on its state—solid, liquid, or gas. In its solid-state, AlCl3 possesses a sheet-like layered structure characterised by cubic close-packed chloride ions. The aluminium centres within this framework showcase an octahedral coordination geometry. As the temperature rises and AlCl3 enters its melted state, it undergoes a structural transformation. In this state, it exists as the dimer Al2Cl6, featuring tetracoordinate aluminium. The melt produced during this phase conducts electricity poorly, a trait that sets it apart from more ionic halides like sodium chloride.
The synthesis of aluminium chloride can also occur through a single displacement reaction between copper(II) chloride and aluminium. Additionally, hydrated aluminium trichloride, another form of aluminium chloride, can be prepared by dissolving aluminium oxides in hydrochloric acid. This process involves the dissolution of metallic aluminium in hydrochloric acid, releasing hydrogen gas and generating a significant amount of heat.
Aluminium chloride is a versatile compound with a wide range of applications in organic chemistry. It is commonly used in the preparation of anthraquinone, which finds utility in the dyestuffs industry. It also plays a role in the Fischer-Hafner synthesis, where it combines with aluminium in the presence of an arene to synthesise bis(arene) metal complexes. Furthermore, aluminium chloride serves as a catalyst in various reactions, such as the Friedel-Crafts reaction, facilitating the alkylation and acylation of arenes.
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Aluminium chloride reacts with ethanol to form a product that stabilises polyvinyl chloride
Aluminium chloride, also known as aluminium trichloride, is an inorganic compound with the formula AlCl3. It is a colourless crystal and is commercially important due to its low melting and boiling point. It is often used in the production of aluminium and in other areas of the chemical industry. For instance, it is used to induce a variety of hydrocarbon couplings and rearrangements.
Aluminium chloride is also used in organic chemistry, including in the alkylation and acylation of arenes. However, a common problem with the Friedel-Crafts reaction is that the aluminium chloride catalyst is sometimes required in full stoichiometric quantities, leading to the generation of large amounts of corrosive waste. This has led to the displacement of aluminium chloride by zeolites in some applications.
Aluminium chloride reacts with ethanol at room temperature to form a product or product mixture that can act as a thermal stabiliser for poly(vinyl chloride) (PVC). This stabilisation is revealed by a decrease in the rate of thermal dehydrochlorination at 190 °C and by a reduction in the average length of the resulting polyene sequences.
PVC is an important industrial chemical used to produce polyvinyl chloride. It is a colourless, flammable gas with a sweet odour and is carcinogenic. The reaction of aluminium chloride with ethanol can thus help to stabilise PVC, which has a variety of industrial applications.
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Aluminium chloride is a powerful Lewis acid
Aluminium chloride, also known as AlCl3, is a chemical compound with a variety of industrial applications. It is formed through the reaction of aluminium metal with chlorine or hydrogen chloride at high temperatures. While it is commonly believed that pure AlCl3 is a Lewis acid, this is a misconception. However, anhydrous aluminium chloride, which is not found as a mineral, is a powerful Lewis acid.
Lewis acids are substances that can accept electrons from other molecules, known as Lewis bases. In the context of aluminium chloride, the Lewis acid-base interaction involves the transfer of electrons to the aluminium ion (Al3+), which is coordinated with chlorine ions in the outermost layer. This interaction is responsible for the compound's catalytic properties in various chemical reactions, such as the Friedel-Crafts reaction.
The Friedel-Crafts reaction is a widely used application of aluminium chloride. In this reaction, an acyl chloride or alkyl halide reacts with an aromatic system. Specifically, aluminium chloride facilitates the addition of acyl groups or alkyl groups to the aromatic ring, leading to the formation of various products, including anthraquinone, which is used in the dye industry. However, one challenge associated with the Friedel-Crafts reaction is that aluminium chloride sometimes needs to be used in full stoichiometric quantities due to its strong complexation with the products. This can result in the generation of corrosive waste, leading to the exploration of alternative catalysts, such as zeolites.
Beyond the Friedel-Crafts reaction, aluminium chloride finds diverse applications in organic chemistry. For example, it can catalyse the ene reaction, such as the addition of 3-buten-2-one (methyl vinyl ketone) to carvone. Additionally, aluminium chloride is involved in inducing hydrocarbon couplings and rearrangements, demonstrating its versatility in organic synthesis.
In conclusion, aluminium chloride, specifically anhydrous aluminium chloride, is a powerful Lewis acid due to its ability to coordinate with Lewis bases and facilitate various chemical reactions. Its applications in organic chemistry, particularly in the Friedel-Crafts reaction and related processes, highlight its importance as a catalyst. However, the challenge of corrosive waste has led to the exploration of alternative catalysts with similar properties.
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Aluminium and ethanol form aluminium triethoxide
Aluminium triethoxide, also known as aluminium ethoxide, is a metallo-organic compound with the formula Al(OCH2CH3)3. It is a moisture-sensitive white powder that is slightly soluble in hot dimethyl benzene, chlorobenzene, and other high-boiling-point non-polar solvents.
Aluminium triethoxide is formed when aluminium reacts with ethanol. This reaction occurs at a high temperature of 623 Kelvin and results in the formation of ethyl acetate. The reaction can be represented as follows:
Al + EtOH -> Al(OCH2CH3)3 + ethyl acetate
Aluminium triethoxide has several applications. It is used as a reducing agent for aldehydes and ketones and as a polymerization catalyst. One of its primary applications is in the Sol-Gel Process preparation of high-purity aluminium sesquioxide, a polymerization agent.
The structure of aluminium triethoxide has not been fully established by X-ray crystallography. However, related compounds, such as aluminium isopropoxide, have been studied using techniques like NMR spectroscopy and X-ray crystallography. These studies have revealed that aluminium isopropoxide has a tetrameric structure, with a unique central Al atom arranged in an octahedral geometry and three other Al centres adopting a tetrahedral geometry.
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Frequently asked questions
Chlorine reacting with ethyl alcohol forms chloroform, chloral, and CCl.
Aluminium reacting with ethanol forms aluminium triethoxide, which is both flammable and can cause severe skin burns and eye damage.
Aluminium chloride is an inorganic compound with the formula AlCl3. It is manufactured on a large scale by the exothermic reaction of aluminium metal with chlorine or hydrogen chloride at temperatures between 650 and 750 °C.
