Some Families of Organic Compounds HL

Objectives

• Define tetrahedral carbon
• Explain the term alcohol
• Describe alcohols as a homologous series
• Explain chloroalkanes
• Name chloroalkanes and alcohols, primary and secondary, up to C4
• Discuss chloroalkanes as solvents
• Draw structural formulas for chloroalkanes and alcohols up to C4
• Account for physical properties (state, solubility) of alkanes, chloroalkanes, and alcohols up to C4
• Discuss solubility of methanol and butan-1-ol in cyclohexane and water
• Use of ethanol as a solvent and methanol as a denaturing agent
• Recall fermentation as a source of ethanol
• Discuss fermentation in brewing and distilling industries
• Define planar carbon and carbonyl compound
• Describe aldehydes, ketones, carboxylic acids, and esters as homologous series
• Name and draw structural formulas for aldehydes, ketones, carboxylic acids, and esters up to C4
• Discuss solubility of relevant compounds in cyclohexane and water
• Recall examples and uses of various organic compounds

Key Concepts & Definitions

Tetrahedral Carbons

• Tetrahedral carbon: A carbon with tetrahedral geometry, occurring when bonded to four single bonds.

Chloroalkanes

• Definition: Alkanes where hydrogen atoms are replaced by chlorine atoms.
• Uses: Industrial solvents, e.g., dry cleaning.
• Physical Properties: Weakly polar, not soluble in water, soluble in non-polar solvents.

Alcohols

• Functional Group: -OH, name ends in '-ol'.
• Types:
  • Primary: OH bonded to one other carbon
  • Secondary: OH bonded to two other carbons
  • Tertiary: OH bonded to three other carbons
• Example: Ethanol (C2H5OH)
  • Produced by fermenting glucose
  • Denatured with methanol (methylated spirits)
• Physical Properties: Higher boiling points due to hydrogen bonding, solubility varies with molecule size.

Planar Carbons

• Planar carbon: Carbon with planar geometry, occurring when unsaturated.

Aldehydes

• Functional Group: -CHO, name ends in '-al'.
• Physical Properties: Polar carbonyl group, dipole-dipole intermolecular forces, higher boiling points than alkanes.

Ketones

• Functional Group: -CO-, name ends in '-one'.
• Uses: Propanone in nail polish remover.
• Physical Properties: Dipole-dipole forces, soluble in water.

Carboxylic Acids

• Functional Group: -COOH, name ends in '-oic acid'.
• Used as flavouring agents and preservatives.
• Physical Properties: Hydrogen bonding intermolecular forces, high boiling points.

Esters

• Functional Group: -COOC-, name ends in '-yl -oate'.
• Formation: From alcohol and carboxylic acid, condensation reaction.
• Uses: Flavourings and fragrances.
• Physical Properties: Dipole-dipole intermolecular forces.

Aromatic Compounds

• Structure: Contains a benzene ring.
• Bonding in Benzene: Stable structure with equal bond lengths.
• Examples: Many natural products contain benzene rings.

Important Notes

• Ability to name and draw structural formulas of each type of compound is crucial.
• Recognition of carcinogenic nature of some aromatic compounds like benzene, and non-carcinogenic like aspirin.
• Understanding of aromatic compounds in various applications, including pharmaceuticals and industrial solvents.