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Alcohols (Alcohol homologous series (Naming alcohols: (Suffix: -ol
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Alcohols
Classifying alcohols
Primary/ Secondary/ Tertiary: number hydrogen atoms and alkyl groups attached carbon atom that contains OH functional group
Primary alcohols:
E.g. methanol/ ethanol
-OH group attached carbon atom attached 2 hydrogen atoms/ 1 alkyl group
Secondary alcohols:
E.g. propan-2-ol/ pentan-3-ol
-OH group attached carbon atom attached 1 hydrogen atom/ 2 alkyl groups
Tertiary alcohols:
E.g. 2-methylpropan-2-ol/ 2-methylbutan-2-ol
-OH group attached carbon atom attached NO hydrogen atoms/ 3 alkyl groups
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Physical properties
Volatility and boiling points: Alcohols have lower volatility than alkanes because:
Liquid: hydrogen bonds hold alcohol molecules together
(must be broken change into gas) more energy required overcome hydrogen bonds than london forces
Water solubility:
Alcohols more water soluble than alkanes because: alkanes are non-polar cannot form hydrogen bonds in H2O
Methanol/ ethanol: soluble in water- hydrogen bonds form between polar O-H group alcohol and H20 molecules
Solubility decreases = carbon atoms increase (influence OH group decreases)
Alkanes: non-polar bonds because electronegativity of hydrogen and carbon are very similar = NON-POLAR (intermolecular forces: LONDON FORCES)
Alcohols: polar O-H bond because difference electronegativity oxygen and hydrogen atoms = POLAR (intermolecular forces: london forces and HYDROGEN BONDS between polar O-H groups
Reactions of alcohols
Combustion of alcohols
React with O2 produce: CO2/ H2O Exothermic reaction: release energy as heat
Carbon atoms increase quantity released per mole increases
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