Halogenoalkanes are compounds in which a halogen atom has replaced at least one of the hydrogen atoms in an alkane chain. They have the general formula: $C_{n}H_{2n+1}X$, where $X$ is a halogen atom.
Their name is based on the length of the longest alkane chain with any halogen groups and positions indicated. If there are more than one halogen atom then they are listed alphabetically.
Halogenoalkanes contain a polar carbon-halogen bond. This polarity arises from the different electronegativity of the carbon and halogen atoms.
The electronegativity of the halogen decreases down the group, resulting in a decrease in polarity of the carbon-hydrogen bond from fluorine to iodine.
The electron deficient carbon atom in halogenoalkanes attracts nucleophiles. This allows halogenoalkanes to react with nucleophiles in substitution reactions.
When halogenoalkanes react with an aqueous solution of hot hydroxide ions, a nucleophilic substitution reaction occurs which gives an alcohol. This reaction is called hydrolysis.
$$CH_{2}ClCH_{3} + NaOH \rightarrow CH_{2}OHCH_{3} + Cl^{-}$$
In nucleophilic substitution, an atom or group of atoms is replaced by a nucleophile (an electron pair donor). During hydrolysis, the halogen atom is replaced by the hydroxide ion:
The hydroxide ion has a lone pair of electrons. These are attracted and donated to the electron-deficient carbon atom in the halogenoalkane. This is known as nucleophilic attack.
The donation of the electron pair leads to the formation of a new covalent bond between the oxygen atom of the hydroxide ion and the carbon atom.
The carbon-halogen bond breaks by heterolytic fission. Both of the bonded electrons move to the halogen, forming a halide ion.
This mechanism for nucleophilic substitution of 1-iodopropane is shown below:
The rates of hydrolysis for different halogenalkanes can be determined using the following experiment:
The aqueous silver nitrate, $AgNO_{3(aq)}$ reacts with any halide ions present, forming a precipitate.
The rate of hydrolysis can be calculated by doing: $$ rate\,of \,hydrolysis = \frac {1}{time} $$
The carbon-iodine bond is the weakest of the halogenoalkanes, therefore this more readily reacts and is broken the most easily. The bond enthalpy decreases down the group.
Many of halogen containing polymers can be produced such as PTFE from the polymerisation of tetrafluorethene and poly(vinyl chloride).
Chlorofluorocarbons are halogenoalkanes containing only carbon, fluorine and chlorine atoms. Developed by Thomas Midgley in 1929, they were popular as refrigerants and propellants due to their non-toxic, unreactive and non-flammable properties.
The stability of CFCs arises from the strength of the carbon-halogen bonds, however this produces a problem.
As an alternative, hydrofluorocarbons have now been developed. Despite the non-flammable and non-toxic properties,they still deplete the ozone layer so are widely considered as a short term replacement.