Free Radical Mechanism – From Intuition to Precision
Imagine you have a long chain of paperclips linked together. Now imagine someone snips one link in the middle. That single cut doesn't just break the chain — it creates two new ends, each hungry to grab onto something. That's the core idea of a free radical mechanism: a reaction that proceeds through species with an unpaired electron — a "hungry" atom or molecule that desperately wants to pair up.
The Intuition: Why Radicals Are Special
Most chemical bonds involve paired electrons — two electrons spinning in opposite directions, like a stable couple. A free radical is the chemical equivalent of a lone wolf: it has one unpaired electron, making it highly reactive. It will do almost anything to find a partner — steal an electron from a neighbour, donate its own, or break another bond to create more radicals.
This creates a chain reaction. One radical reacts, produces another radical, which reacts again, and so on — like a row of dominoes falling one after another. That's why free radical mechanisms are often called chain reactions.
The Precise Statement
A free radical mechanism is a stepwise reaction pathway involving species with unpaired electrons (free radicals). It proceeds through three distinct phases:
Initiation – A stable molecule is broken to produce two free radicals. This usually requires energy — heat (thermolysis) or light (photolysis).
Propagation – Radicals react with stable molecules to produce new radicals. This step repeats many times, forming the chain.
Termination – Two radicals combine to form a stable product, ending the chain.
General pattern:
Initiation: A−Bhν or ΔA⋅+B⋅
Propagation: A⋅+C−D→A−C+D⋅
Termination: A⋅+D⋅→A−D
A Concrete Example: Chlorination of Methane
This is the classic textbook example, and it appears in almost every Indian board exam (Class 11/12, JEE, NEET).
Overall reaction:
CH4+Cl2hνCH3Cl+HCl
Step-by-step mechanism:
Initiation – Chlorine molecule absorbs UV light and splits:
Cl2hν2Cl⋅
Propagation – Two steps that repeat:
Chlorine radical attacks methane:
Cl⋅+CH4→HCl+CH3⋅
Methyl radical attacks another chlorine molecule:
CH3⋅+Cl2→CH3Cl+Cl⋅
Notice: the Cl⋅ consumed in step 1 is regenerated in step 2. This is the chain — one radical keeps producing another.
Termination – Any two radicals meet:
Cl⋅+Cl⋅→Cl2
CH3⋅+CH3⋅→C2H6
CH3⋅+Cl⋅→CH3Cl
Watch out
A common mistake: students think termination only happens when the same radicals combine. In reality, any two radicals can terminate — including cross-combination (like CH3⋅+Cl⋅). Also, termination steps are rare because radical concentrations are very low.
Key Characteristics to Remember
Free radicals are neutral — they have no charge, only an unpaired electron. Don't confuse them with ions.
They are highly reactive — lifetimes are typically microseconds or less. …
UV light splits Cl2 into radicals; the radicals abstract H from methane and react with Cl2 in a repeating chain; two radicals finally combine to terminate. …
Initiation. UV light homolyses the weak Cl–Cl bond into two chlorine radicals: Cl2hν2Cl∙. Propagation (repeats, keeping the chain going). Step 1: a chlorine radical abstracts a hydrogen from methane, Cl∙+CH4→CH3∙+HCl. Step 2: the methyl radical reacts with another chlorine molecule, CH3∙+Cl2→CH3Cl+Cl∙, regenerating a chlorine radical that re-enters step 1. Termination. The chain stops when two radicals combine without generating a new one, e.g. Cl∙+Cl∙→Cl2, or CH3∙+Cl∙→CH3Cl, or $\text{ …
Same / Similar Concept — real previous-year questions on the same or a closely similar concept, not this exact question.
CBSE 2023Set annual1 mark
Q.Which of the following radical is more stable? (CH3)3C-radical, CH3CHCH3-radical, CH3CH2-radical
›Reveal solutionSolution
Alkyl substitution stabilizes a free radical, so (CH3)3C-radical (tertiary) is more stable than CH3CHCH3-radical (secondary), which is more stable than CH3CH2-radical (primary).
A free radical is an electron-deficient (odd-electron) species. Its stability is governed mainly by two effects of the alkyl groups attached to the radical carbon:
Inductive (+I) effect: Alkyl groups are electron-releasing relative to hydrogen, so more alkyl groups around the radical centre push electron density towards it, partially compensating for the electron deficiency.
Hyperconjugation: Adjacent C-H sigma bonds can donate electron density into the singly-occupied p orbital on the radical carbon. A tertiary radical has more adjacent C-H bonds (9, from three methyl groups) available for hyperconjugation than a secondary radical (6) or a primary radical (3), so more hyperconjugative structures stabilize it.
Q.Match the Column-A item 'Homolysis' with the correct entry from Column B:
(a) Anion
(b) Free radical
(c) Cation
(d) 7
(e) delta-G = 0
(f) g cm^-3
›Reveal solutionSolution
In homolysis, a covalent bond breaks symmetrically so that each atom retains one electron of the shared pair, generating two free radicals — matching Column B entry (b).
A covalent bond A-B can break in two ways:
Homolytic fission (homolysis): the bond breaks symmetrically, and each fragment takes one electron from the shared pair, giving two neutral species each with an unpaired electron — these are called free radicals (A. and B.). This typically requires energy input such as heat or UV light and is common in reactions like the halogenation of alkanes. …