(A) : Boiling point of F₂ < Cl₂ < Br₂ < I₂
(R) : Down the group from F₂ to I₂ London dispersion forces become stronger

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(A) is true but (R) is false

Both (A) and (R) are correct and (R) is the correct explanation of (A)

Both (A) and (R) are false

Both (A) and (R) are correct but (R) is not the correct explanation of (A)

answer is A.

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Detailed Solution

The boiling point of the halogens (F₂, Cl₂, Br₂, I₂) increases down the group because the size of the atoms and the strength of the London dispersion forces increases.
The London dispersion forces are the intermolecular forces that result from the temporary dipoles that form between non-polar molecules.
As we move down the group from F₂ to I₂, the size of the atoms increases and so does the number of electrons.
This results in an increase in polarizability, which in turn leads to stronger London dispersion forces. Therefore, statement R is true.
Since the boiling point of a substance is directly related to the strength of its intermolecular forces, it follows that the boiling point of the halogens increases down the group. Hence, statement A is also true.

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