Given below are two statements: Statement I : The correct order in terms of bond dissociation enthalpy is Cl _ 2 > Br _ 2 > F _ 2 > I _ 2 . Statement II : The correct trend in the covalent character of the metal halides is [ SnCl _ 4 > SnCl _ 2 ], [ PbCl _ 4 > PbCl _ 2 ] and [ UF _ 4 > UF _ 6 ]. In the light of the above statements, choose the correct answer from the options given below :
C. Statement I is true but Statement II is false
Statement I: The bond dissociation enthalpy of halogens follows the order Cl_2 > Br_2 > F_2 > I_2. The bond energy of F_2 is lower than Cl_2 and Br_2 due to the high inter-electronic repulsion between the lone pairs on the small fluorine atoms. Thus, Statement I is true. Statement II: According to Fajan's rules, for a given metal, the compound with the metal in a higher oxidation state has more covalent character due to higher polarizing power. Therefore, SnCl_4 > SnCl_2 and PbCl_4 > PbCl_2 are correct. However, for Uranium halides, UF_6 has a higher oxidation state (+6) than UF_4 (+4), so UF_6 is more covalent than UF_4. The statement claims UF_4 > UF_6, which is incorrect. Thus, Statement II is false.
Related: Chemistry — Chemical Bonding and Molecular Structure · All PYQ Banks