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Affinity for hydrogen decreases in the group from fluorine to iodine. Which of the halogen acids should have highest bond dissociation enthalpy?
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Verified Answer
The correct answer is:
$\mathrm{HF} \quad$
$\mathrm{HF} \quad$
On moving down the group, size of halogen atom increases hence, the $\mathrm{H}-\mathrm{X}$ bond length increases. As a result, bond dissociation enthalpy decreases.
Hence, the correct order of bond enthalpy is :
$$
\mathrm{H}-\mathrm{F}>\mathrm{H}-\mathrm{Cl}>\mathrm{H}-\mathrm{Br}>\mathrm{H}-\mathrm{I} \text {. }
$$
Hence, the correct order of bond enthalpy is :
$$
\mathrm{H}-\mathrm{F}>\mathrm{H}-\mathrm{Cl}>\mathrm{H}-\mathrm{Br}>\mathrm{H}-\mathrm{I} \text {. }
$$
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