chapter 14

• Alcohols are less volatile, have higher melting points and greater water solubility than alkanes
• Alcohols have a polar o-h bond due to the difference in electronegativity , making alcohols polar
• Alcohols have weak london forces but also have strong hydrogen bonds
• alcohols are less volatile tha alkanes, because they have hydrogen bonds which require more energy to overcome than alkanes weak London forces
• Alcohols are soluble as hydrogen bonds form between the oh group of the alcohol and the water molecules
• As the hydrocarbon chain increases in size, the influence of the oh group becomes smaller
• Primary alcohols- oh attached to carbon attached to one other carbon

  Secondary alcohol- oh attached to carbon attached to two other carbons

  Tertiary alcohols- oh attached to carbon attached to three other carbons
• In oxidation, dichromate ions are reduced to chromium ions, the colour change is from orange to green
• A primary alcohol can be oxidised with acidified potassium dichromate and is distilled out as it’s formed to produce an aldehyde
• A primary alcohol can be oxidised with acidified potassium dichromate while being heated strongly under reflux to produce a carboxylic acid
• A secondary alcohol can be oxidised heated under reflux with acidified potassium dichromate to form a ketone
• Tertiary alcohols do not undergo oxidation reactions
• Dehydration or elimination of an alcohol-

  The alcohol is heated under reflux in the presence of hot concentrated sulfuric acid to give an Alkene and a water molecule
• An alcohol can react with sulfuric acid and a sodium halide( to form a hydrogen halide) in situ while being heated under reflux to form a haloalkane and a water molecule