by Alkanes
Alkanes, also known as paraffins, are a class of saturated hydrocarbons. This means they consist solely of carbon (C) and hydrogen (H) atoms, with only single bonds between the carbon atoms. The general chemical formula for alkanes is CnH2n+2, where “n” represents the number of carbon atoms in the molecule.
Due to their saturated nature, alkanes are relatively unreactive compared to other hydrocarbons like alkenes (which have double bonds) and alkynes (which have triple bonds). They are typically stable and do not readily undergo chemical reactions.
Alkanes are a significant component of natural gases and petroleum products. They serve as the foundation for various organic compounds, including fuels like gasoline and diesel. The first few alkanes in the series are methane (CH4), ethane (C2H6), propane (C3H8), and butane (C4H10), with their molecular structures following a linear progression.
Alkenes
Alkenes, also known as olefins, are a class of unsaturated hydrocarbons. This means they contain carbon (C) and hydrogen (H) atoms and possess at least one carbon-carbon double bond (C=C) in their chemical structure. The general formula for alkenes is CnH2n, where “n” represents the number of carbon atoms in the molecule.
Because of the presence of double bonds, alkenes are more reactive than alkanes (saturated hydrocarbons with only single bonds). They can undergo various chemical reactions, including addition reactions, where atoms or groups of atoms are added to the carbon atoms involved in the double bond.
Alkenes are important in the chemical industry as they serve as the starting materials for the synthesis of a wide range of compounds, including plastics, solvents, and various industrial chemicals. They are also found in natural sources like plant oils. Examples of alkenes include ethene (C2H4), propene (C3H6), and butene (C4H8).
Alkynes
Alkynes are a class of unsaturated hydrocarbons, similar to alkenes and alkanes. They contain carbon (C) and hydrogen (H) atoms and have at least one carbon-carbon triple bond (C≡C) in their chemical structure. The general formula for alkynes is CnH2n-2, where “n” represents the number of carbon atoms in the molecule.
The presence of triple bonds makes alkynes more reactive than both alkenes (which have double bonds) and alkanes (which have only single bonds). This allows them to undergo a variety of chemical reactions, including addition reactions.
Alkynes are utilized in the chemical industry for the synthesis of a wide range of compounds, including polymers, solvents, and pharmaceuticals. They are also found in natural sources, including certain plants and fungi. Examples of alkynes include ethyne (C2H2) and propyne (C3H4).
Important Differences Between Alkanes, Alkenes and Alkynes
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Basis of Comparison |
Alkanes | Alkenes |
Alkynes |
| Carbon-Carbon Bonds | Single bonds | Double bonds | Triple bonds |
| Chemical Formula | CnH2n+2 | CnH2n | CnH2n-2 |
| Saturation Level | Saturated | Unsaturated | Unsaturated |
| Hybridization | sp3 | sp2 | sp |
| Example | Ethane (C2H6) | Ethene (C2H4) | Ethyne (C2H2) |
| Bond Angle | 109.5 degrees | 120 degrees | 180 degrees |
| Physical State | Usually gaseous | Usually gaseous or liquid | Gaseous or liquid |
| Reactivity | Least reactive | More reactive than alkanes | Most reactive |
| Addition Reactions | Less susceptible | More susceptible | Most susceptible |
| Isomerism | Only chain isomers | Can have geometric isomers | Can have positional and geometric isomers |
| Uses | Fuels, lubricants | Petrochemical feedstock | Welding and cutting gases, specialty chemicals |
Important Similarities Between Alkanes, Alkenes and Alkynes
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Hydrocarbons:
All three are types of hydrocarbons, meaning they are composed solely of hydrogen and carbon atoms.
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Organic Compounds:
They are all organic compounds, meaning they primarily consist of carbon atoms bonded to each other.
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Saturated/Unsaturated:
They can all be either saturated (containing only single bonds) or unsaturated (containing double or triple bonds) depending on the arrangement of their carbon atoms.
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Isomerism:
All three groups can exhibit structural isomerism, where different compounds have the same chemical formula but different structural arrangements.
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Bonding:
They all exhibit covalent bonding, where electrons are shared between atoms to form chemical bonds.
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Combustion:
They can all undergo combustion reactions, reacting with oxygen to release energy.
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Reactivity:
They can participate in various chemical reactions, including addition and substitution reactions.
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