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NEET CHEMISTRYMedium

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).
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