Which of the following halogens has the highe | vedclass

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(B) The bond dissociation energy of halogens generally decreases down the group due to the increase in atomic size and bond length. However,$F_2$ is a

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$Cl_2$

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(B) The bond dissociation energy of halogens generally decreases down the group due to the increase in atomic size and bond length. However,$F_2$ is an exception because of the very small size of the fluorine atom,which leads to significant inter-electronic repulsion between the lone pairs of the two fluorine atoms. This makes the $F-F$ bond weaker than the $Cl-Cl$ bond. The order of bond dissociation energy is $Cl_2 > Br_2 > F_2 > I_2$. Therefore,$Cl_2$ has the highest bond dissociation energy.

Which of the following halogens has the highest bond dissociation energy?

Similar Questions

Which of the following oxoacids of chlorine is the least oxidizing in nature?

Considering the parameters such as bond dissociation enthalpy,electron gain enthalpy and hydration enthalpy,compare the oxidising power of $F_{2}$ and $Cl_{2}$.

Give two examples to show the anomalous behaviour of fluorine.

On boiling an aqueous solution of $KClO_3$ with iodine,the following product is obtained:

Consider the following reactions :
$(i)$ $F_2 + 2X^{-} \to 2F^{-} + X_2$ $(X = Cl, Br, I)$
$(ii)$ $Cl_2 + 2X^{-} \to 2Cl^{-} + X_2$ $(X = Br, I)$
$(iii)$ $I_2 + 2Br^{-} \to 2I^{-} + Br_2$
Which option has only the correct set of reactions?

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