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

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1. **Definition:** Iso-structural species have the same shape and hybridisation of the central atom.
2. **Analyze Option D ($BrO_3^-$ and $XeO_3$):**
   - **$BrO_3^-$ (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 ($sp^3$ hybridisation).
   - **$XeO_3$ (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** ($sp^3$ hybridisation).
   - **Result:** Both are trigonal pyramidal with 1 lone pair. They are iso-structural.
3. **Analyze other options:**
   - $SF_4$ (See-saw) vs $XeF_4$ (Square Planar).
   - $SO_3^{2-}$ (Pyramidal) vs $NO_3^-$ (Trigonal Planar).
   - $BF_3$ (Trigonal Planar) vs $NF_3$ (Pyramidal).

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