Which one of the following pairs is isostructural (i.e., having the same shape and hybridization)?

1. ${\text{BF}}_4^{-}$: Central atom B has 3 valence electrons + 1 (from charge) = 4. It forms 4 bonds with F. Hybridization is $s{p}^3$, Shape is Tetrahedral.2. ${\text{NH}}_4^{+}$: Central atom N has 5 valence electrons - 1 (from charge) = 4. It forms 4 bonds with H. Hybridization is $s{p}^3$, Shape is Tetrahedral.Since both have the same hybridization and shape, they are isostructural.Other options:${\text{BCl}}_3$ ($s{p}^2$, trigonal planar) vs ${\text{BaCl}}_2$ (Ionic/linear in gas).${\text{NH}}_3$ ($s{p}^3$, pyramidal) vs ${\text{NO}}_3^{-}$ ($s{p}^2$, trigonal planar).${\text{NF}}_3$ ($s{p}^3$, pyramidal) vs ${\text{BF}}_3$ ($s{p}^2$, trigonal planar).