Photochemical halogenation of alkanes

Halogens react with alkanes in special light-induced reactions called photochemical reactions.

For the reaction to occur:

• Ultraviolet (UV) light must be present.
• This UV light provides the activation energy to start the reaction.

The overall reaction is a substitution, where a hydrogen atom in the alkane molecule is replaced by a halogen atom like chlorine or bromine.

Free radical substitution mechanism

Photochemical halogenation of alkanes follows a three-step free radical substitution mechanism:

1. Initiation - UV light produces reactive radicals.
2. Propagation - Radicals react in a chain reaction.
3. Termination - Radicals join to form stable molecules.

Methane reacts vigorously with chlorine gas in the presence of UV light, as represented by the equation:

CH₄ + Cl₂ ➔ CH₃Cl + HCl

The three-stage mechanism for this reaction is detailed below.

Stage 1 - Initiation

• UV light breaks the Cl-Cl bond in chlorine via homolytic fission to give two chlorine radicals (Cl•): Cl₂ ➔ 2Cl•

• The unpaired electron makes Cl• highly reactive.

Stage 2 - Propagation

• The chlorine radical attacks a methane molecule in a substitution reaction: Cl• + CH₄ ➔ CH₃• + HCl

• The methyl radical (CH₃•) attacks another chlorine molecule: CH₃• + Cl₂ ➔ CH₃Cl + Cl•

• This propagation cycle continues until reagents are used up.

Stage 3 - Termination

• Two radicals join to form a stable covalent bond: Cl• + CH₃• ➔ CH₃Cl

• Other combinations like 2CH₃• ➔ C₂H₆ or 2Cl• ➔ Cl₂ are also possible.

The end products of the termination step depend on which reagent is in excess:

• Excess chlorine - Further substitution on products like chloromethane occurs, producing a mixture of products such as CH₃Cl, CH₂Cl₂, CHCl₃, and CCl₄.
• Excess methane - Predominantly single substitution occurs to form chloromethane.