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, Properties of alcohols
General formula of alcohols- CnH₂n+1OH
Alcohols have a polar O-H bond because of the difference in
electronegativity of the O & H atoms. So the molecules are polar.
Alcohols have both very weak London forces and strong hydrogen
bonding present between the molecules.
The hydrogen bonds between the alcohol molecules must be broken to
change the state from liquid to gas. This requires more energy than
overcoming the weak London forces in alkanes therefore alcohols have a
lower volatility & higher B.P/ M.P than alkanes (with the same number of
C atoms). As chain length increases the B.P increases as there are more
surface area contacts and so stronger induced dipole-dipole
intermolecular forces.
Alcohols are able to dissolve in water easily due to hydrogen bonds
forming between the polar O-H group of the alcohol & the water
molecule. Alkanes are non polar so cannot form H bonds with water, & so
alcohols are more water soluble than alkanes.
As the hydrocarbon chain of the alcohol
increases in size, the solubility of the alcohol
decreases since the aliphatic chain cannot
form H bonds and this becomes the larger
part of the molecule.
, Classifying alcohols
Primary alcohol
functional group attached to a
carbon atom with no more than
one alkyl group. (exception
being methanol which has 3 H
and no alkyl group)
Secondary alcohol
functional group attached to a
carbon atom with two alkyl
groups.
Tertiary alcohol
functional group attached to a
carbon atom with three alkyl
groups.
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