Which of the following pairs shows the highes | vedclass

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(D) $1$. Among halogens,the bond dissociation enthalpy order is $Cl_{2} > Br_{2} > F_{2} > I_{2}$. Thus,$Cl_{2}$ has the highest bond dissociation ent

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$Cl_{2}, HI$

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(D) $1$. Among halogens,the bond dissociation enthalpy order is $Cl_{2} > Br_{2} > F_{2} > I_{2}$. Thus,$Cl_{2}$ has the highest bond dissociation enthalpy. $2$. Among hydrogen halides,the bond dissociation enthalpy decreases down the group due to an increase in bond length: $HF > HCl > HBr > HI$. Thus,$HI$ has the lowest bond dissociation enthalpy. $3$. Therefore,the correct pair is $(Cl_{2}, HI)$.

Which of the following pairs shows the highest bond dissociation enthalpy among halogens and the lowest bond dissociation enthalpy among hydrogen halides?

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