Question

Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs.

Options

• \[\ce{[NF3 and BF3]}\]

• \[\ce{[BF^{–}4 and NH^{+}4]}\]

• \[\ce{[BCl3 and BrCl3]}\]

• \[\ce{[NH3 and NO^{-}3]}\]

Answer 1

\[\ce{[BF^{–}4 and NH^{+}4]}\]

Explanation:

In a molecular structure if a central atom has the same hybridization as the central atom of another molecular species, then the two structures are known as isostructural species.

(i) In \[\ce{NF3}\] the central nitrogen atom is sp³ hybridized and in \[\ce{BF3}\] the central boron atom is sp². So, these two molecules are not isostructural pairs.

(ii) In \[\ce{BF4^{-}4}\]  the central boron atom is sp³ hybridized and in \[\ce{NH^{+}4}\]  the central nitrogen atom is also sp³ hybridized. So, these two molecules are identified as isostructural pairs.

(iii) In \[\ce{BCl3}\] the central boron atom is sp² hybridized and in \[\ce{BrCl3}\] the central bromine atom is sp³d hybridized. So, these two molecules are not isostructural pairs.

(iv) In \[\ce{NH3}\] the central nitrogen atom is sp³ and in \[\ce{NO^{-}3}\] the central nitrogen atom is sp² hybridized. So, these two molecules are not isostructural pairs.