How do you account for the formation of ethane during chlorination of methane?

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During the chlorination of methane, which is typically carried out in the presence of ultraviolet (UV) light or under high temperatures, ethane is formed as one of the products along with other chlorinated compounds.

The mechanism involves a series of radical reactions. Initially, a chlorine radical (⋅Cl⋅Cl) is generated from the dissociation of molecular chlorine (Cl2Cl2) under UV light or high temperatures:

Cl2→2⋅ClCl2→2⋅Cl

Then, methane (CH4CH4) undergoes homolytic cleavage in the presence of a chlorine radical to form a methyl radical (⋅CH3⋅CH3) and a hydrogen chloride molecule (HClHCl):

CH4+⋅Cl→⋅CH3+HClCH4+⋅Cl→⋅CH3+HCl

The methyl radical (⋅CH3⋅CH3) further reacts with another molecule of methane, leading to the formation of ethane (C2H6C2H6):

⋅CH3+CH4→C2H6⋅CH3+CH4→C2H6

Overall, the chlorination of methane results in the formation of ethane along with other chlorinated products. Understanding this mechanism helps us comprehend the organic synthesis involved in such reactions, which is crucial for mastering organic chemistry concepts.

As an UrbanPro tutor, I would guide my students through such mechanisms, ensuring they grasp not only the concepts but also the application of these reactions in practical scenarios. This approach fosters a deeper understanding of the subject matter, enabling students to excel in their academic endeavors.