Hydrocarbons Classification and Types

Definition and Classification

• Hydrocarbons are organic compounds consisting of only hydrogen and carbon atoms.
• Classified into two main categories:
  • Saturated hydrocarbons (alkanes): single bonds between carbon atoms
  • Unsaturated hydrocarbons (alkenes and alkynes): one or more multiple bonds between carbon atoms

Types of Hydrocarbons

• Alkanes (saturated):
  • Methane (CH4)
  • Ethane (C2H6)
  • Propane (C3H8)
  • Butane (C4H10)
  • Pentane (C5H12)
• Alkenes (unsaturated):
  • Ethene (C2H4)
  • Propene (C3H6)
  • Butene (C4H8)
• Alkynes (unsaturated):
  • Ethyne (C2H2)
  • Propyne (C3H4)

Physical Properties

• Boiling point and melting point increase with increasing molecular weight
• Density increases with increasing molecular weight
• Solubility in water decreases with increasing molecular weight
• Hydrocarbons are generally non-polar and insoluble in water

Chemical Properties

• Combustion: hydrocarbons react with oxygen to produce carbon dioxide and water
• Halogenation: hydrocarbons react with halogens to form halogenated compounds
• Isomerization: hydrocarbons can undergo isomerization reactions to form structural isomers
• Cracking: hydrocarbons can undergo cracking reactions to form smaller molecules

Importance and Uses

• Energy sources: fossil fuels (petroleum, natural gas, coal) are primarily composed of hydrocarbons
• Industrial applications: used as solvents, lubricants, and fuels
• Biological importance: hydrocarbons are found in biological systems, such as fatty acids and cholesterol

Definition and Classification

• Hydrocarbons are organic compounds composed of only hydrogen and carbon atoms.
• Classified into two main categories: saturated hydrocarbons (alkanes) and unsaturated hydrocarbons (alkenes and alkynes).

Types of Hydrocarbons

• Alkanes (saturated): methane (CH4), ethane (C2H6), propane (C3H8), butane (C4H10), and pentane (C5H12).
• Alkenes (unsaturated): ethene (C2H4), propene (C3H6), and butene (C4H8).
• Alkynes (unsaturated): ethyne (C2H2) and propyne (C3H4).

Physical Properties

• Boiling point and melting point increase with increasing molecular weight.
• Density increases with increasing molecular weight.
• Solubility in water decreases with increasing molecular weight.
• Hydrocarbons are generally non-polar and insoluble in water.

Chemical Properties

• Combustion: hydrocarbons react with oxygen to produce carbon dioxide and water.
• Halogenation: hydrocarbons react with halogens to form halogenated compounds.
• Isomerization: hydrocarbons can undergo isomerization reactions to form structural isomers.
• Cracking: hydrocarbons can undergo cracking reactions to form smaller molecules.

Importance and Uses

• Energy sources: fossil fuels (petroleum, natural gas, coal) are primarily composed of hydrocarbons.
• Industrial applications: used as solvents, lubricants, and fuels.
• Biological importance: hydrocarbons are found in biological systems, such as fatty acids and cholesterol.

Learn about the definition and classification of hydrocarbons, including saturated and unsaturated hydrocarbons, alkanes, and alkenes.