The bond dissociation energies of F_2, Cl_2, | vedclass

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(D) The bond strength is directly proportional to the bond dissociation energy. Lower bond dissociation energy indicates a weaker bond. Comparing the

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$I_2$

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(D) The bond strength is directly proportional to the bond dissociation energy. Lower bond dissociation energy indicates a weaker bond. Comparing the given values: $F_2 (155 \ kJ \ mol^{-1})$,$Cl_2 (244 \ kJ \ mol^{-1})$,$Br_2 (193 \ kJ \ mol^{-1})$,and $I_2 (151 \ kJ \ mol^{-1})$. Since $I_2$ has the lowest bond dissociation energy of $151 \ kJ \ mol^{-1}$,it has the weakest bond.

The bond dissociation energies of $F_2, Cl_2, Br_2$ and $I_2$ are $155, 244, 193$ and $151 \ kJ \ mol^{-1}$ respectively. Which of these has the weakest bond?

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