Identify the pair in which the geometry of the species is T-shaped and square-pyramidal, respectively,

1. ${\mathrm{ICl}}_2^{-}$ and ${\mathrm{ICl}}_5.$
2. ${\mathrm{IO}}_3^{-}$ and $\mathrm{ }{\mathrm{IO}}_2{\mathrm{F}}_2^{-}.$
3. ${\mathrm{ClF}}_3$ and ${\mathrm{IO}}_4^{-}.$
4. ${\mathrm{XeOF}}_2$ and ${\mathrm{XeOF}}_4.$

Solution

In ${\mathrm{XeOF}}_2$, the central atom has $3$ bond pairs and $2$ lone pairs. Hence, the electrons will enter a trigonal bipyramidal geometry. The $2$ lone pairs will take up equatorial positions giving the molecule a T-shape. $\mathrm{Xe}$ in ${\mathrm{XeOF}}_4$ has $5$ bond pairs and $1$ lone pair. The electrons will take up square bipyramidal geometry, but due to a lone pair, the shape of the molecule will be square pyramidal.

Asked in: JEE Main 2018 (15 Apr)

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