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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 :

Options

  1. AStatement I is false but Statement II is true
  2. BBoth Statement I and Statement II are false
  3. CStatement I is true but Statement II is false
  4. DBoth Statement I and Statement II are true

Correct answer

C. Statement I is true but Statement II is false

Step-by-step solution

Statement I: The bond dissociation enthalpy of halogens follows the order Cl₂ > Br₂ > F₂ > I₂ . The bond energy of F₂ is lower than Cl₂ and Br₂ 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, SnCl₄ > SnCl₂ and PbCl₄ > PbCl₂ are correct. However, for Uranium

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