1. Unsaturation: Ethene is an unsaturated hydrocarbon because of the carbon-carbon double bond. Decane and hexane, on the other hand, are saturated hydrocarbons, meaning they only contain carbon-carbon single bonds. The presence of the double bond in ethene makes it more reactive towards various chemical reactions.
2. Addition Reactions: Ethene readily undergoes addition reactions where other molecules or atoms add across the carbon-carbon double bond. This is a characteristic property of alkenes (compounds containing a carbon-carbon double bond). Decane and hexane, being alkanes, do not have double bonds and thus do not participate in addition reactions.
Some common addition reactions of ethene include:
- Hydrogenation: Ethene reacts with hydrogen gas (H2) in the presence of a catalyst (such as platinum or palladium) to form ethane (C2H6).
- Halogenation: Ethene reacts with halogens (such as chlorine or bromine) to form dihaloalkanes. For example, ethene reacts with chlorine gas (Cl2) to form 1,2-dichloroethane (C2H4Cl2).
- Hydration: Ethene reacts with water (H2O) in the presence of an acid catalyst (such as sulfuric acid) to form ethanol (C2H5OH).
3. Polymerization: Ethene has the ability to undergo polymerization, which is a process where multiple ethene molecules combine to form long chains of repeating units. This process, known as ethylene polymerization, is crucial in the production of various plastics, such as polyethylene (PE) and polyvinyl chloride (PVC). Decane and hexane, being alkanes, do not undergo polymerization reactions.
4. Combustion: Ethene, decane, and hexane all undergo combustion reactions with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). However, due to the presence of the double bond, ethene has a higher energy content compared to decane and hexane. This means that ethene burns with a hotter and more luminous flame.
In summary, the presence of the carbon-carbon double bond in ethene distinguishes its chemical properties from those of decane and hexane. Ethene's reactivity allows it to undergo addition reactions, polymerization, and combustion differently compared to alkanes like decane and hexane. These differences are vital in determining their applications in various industries, including petrochemicals, plastics, and fuel.
