The acidic strength of HX (X = F, Cl, Br and I) follows the order: HF > HCl > HBr > HI.
Fluorine exhibits –1 oxidation state whereas other halogens exhibit +1, +3, +5 and +7 oxidation states also.
The enthalpy of dissociation of F2 is smaller than that of Cl2.
Fluorine is stronger oxidising agent than chlorine.
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The Correct Option isA
Solution and Explanation
The acidic strength of the hydrogen halides (HX) increases down the group: \(HF < HCl < HBr < HI\). This trend is due to the decreasing bond strength of the H-X bond as the size of the halogen atom increases. The weaker the bond, the more readily the hydrogen ion (H+) can dissociate, resulting in a stronger acid. Thus, statement (1) is incorrect.
The other statements are correct:
Fluorine is the most electronegative element and only exhibits a -1 oxidation state. Other halogens can exhibit multiple oxidation states (+1, +3, +5, and +7).
The bond dissociation enthalpy of F2 is smaller than that of Cl2 due to the high electron-electron repulsion between the lone pairs in the small fluorine molecule.
Fluorine is a stronger oxidizing agent than chlorine due to its higher electronegativity and smaller size.
