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Question
Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?
Options
Br2 > I2 > F2 > Cl2
F2 > Cl2 > Br2 > l2
I2 > Br2 > Cl2 > F2
Cl2 > Br2 > F2 > I2
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Solution
Cl2 > Br2 > F2 > I2
Explanation:
Bond dissociation enthalpy generally decreases down the group due to increasing atomic size. However, F2 is an exception due to strong lone pair repulsions in the small F-F bond, which weakens it. Hence, Cl2 has the highest bond energy among halogens, followed by Br2, then F2, and least in I2.
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