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NEET CHEMISTRYChemical Bonding and Molecular StructureMedium

Question

In which of the following pairs, the two species are iso-structural?

A

SF₄ and XeF₄

B

SO₃²⁻ and NO₃⁻

C

BF₃ and NF₃

D

BrO₃⁻ and XeO₃

Step-by-Step Solution

  1. Definition: Iso-structural species have the same shape and hybridisation of the central atom.
  2. Analyze Option D (BrO3−BrO_3^- and XeO3XeO_3):
  • BrO3−BrO_3^- (Bromate ion): Central atom Br has 7 valence electrons. The negative charge adds 1 electron (Total = 8). It forms bonds with 3 Oxygen atoms. To minimize repulsion, it forms a Trigonal Pyramidal shape with 1 lone pair (sp3sp^3 hybridisation).
  • XeO3XeO_3 (Xenon trioxide): Central atom Xe has 8 valence electrons. It forms double bonds with 3 Oxygen atoms (using 6 electrons). 2 electrons remain as 1 lone pair. The geometry is Trigonal Pyramidal (sp3sp^3 hybridisation).
  • Result: Both are trigonal pyramidal with 1 lone pair. They are iso-structural.
  1. Analyze other options:
  • SF4SF_4 (See-saw) vs XeF4XeF_4 (Square Planar).
  • SO32−SO_3^{2-} (Pyramidal) vs NO3−NO_3^- (Trigonal Planar).
  • BF3BF_3 (Trigonal Planar) vs NF3NF_3 (Pyramidal).

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Chemical Bonding and Molecular Structure. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

CHEMISTRYChemical Bonding and Molecular Structurefollowingspeciesisostructural

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