In which of the following pairs, the two species are iso-structural?
In which of the following pairs, the two species are iso-structural?
$\mathrm{SO}_3^{2-}$ and $\mathrm{NO}_3^{-}$
$\mathrm{BF}_3$ and $\mathrm{NF}_3$
$\mathrm{BrO}_3^{-}$and $\mathrm{XeO}_3$
$\mathrm{SF}_4$ and $\mathrm{XeF}_4$
Solution
Hybridisation of $\mathrm{Br}$ is $\mathrm{BrO}_3^{-}$
Total valence elctrons $=7+3 \times 6=25$
Charge $=-1$
Total $=25+1=26$ $=\frac{26}{8}=3(\mathrm{Q})+2(\mathrm{R})=5$
hybridization $=d s p^3$
hybridization of $\mathrm{Xe}$ in $\mathrm{XeO}_3$
Total valence electrons $=8+3 \times 6=26=\frac{26}{8}=3(Q)+2(R)=5$
Hybridization $=d s p^3$
The structure $\mathrm{BrO}_3^{-}$and $\mathrm{XeO}_3$ is trigonal pyramidal.
Caution
Molecular structure of $\mathrm{NO}_3^{-}, \mathrm{NH}_3, \mathrm{NF}_3=$ trigonal pyramidal
Molecular structure of $\mathrm{SO}_3^{2-}=$
Trigonal Planar
Molecular structure of $\mathrm{SF}_4=$ Seesaw
Molecular structure of $\mathrm{XeF}_4=$ Square Planar