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JEE MainChemistryChemical Bonding and Molecular Structure

Consider the following sequence of noble gas compounds: XeF ₂ , XeF ₄ , XeO ₃ , XeO ₄ . Which of the following options provides a sequence of main-group species that have similar Lewis dot structures (isoelectronic and isostructural) to the given noble gas compounds, in the exact same respective order?

Options

  1. ACO ₂ , SF ₄ , SO ₃²⁻ , SO ₄²⁻
  2. BI ₃⁺ , BrF ₄⁺ , BrO ₃⁻ , ClO ₄⁻
  3. CBeCl ₂ , SiF ₄ , SO ₃ , CCl ₄
  4. DI ₃⁻ , ICl ₄⁻ , ClO ₃⁻ , ClO ₄⁻

Correct answer

D. I ₃⁻ , ICl ₄⁻ , ClO ₃⁻ , ClO ₄⁻

Step-by-step solution

Species with the same number of valence electrons and identical skeletal connectivity generally have similar Lewis dot structures. Calculate the total valence electrons for the given noble gas sequence: XeF ₂ : 8 + 2(7) = 22 valence electrons (2 bond pairs, 3 lone pairs, linear). XeF ₄ : 8 + 4(7) = 36 valence electrons (4 bond pairs, 2 lone pairs, square planar). XeO ₃ : 8 + 3(6) = 26 valence electrons (3 bond pairs, 1 lone pair, pyramidal). XeO ₄ : 8 + 4(6) = 32 valence electrons (4 bond pairs, 0 lone pairs, tetra

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