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Question
Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs.
Options
\[\ce{[NF3 and BF3]}\]
\[\ce{[BF^{–}4 and NH^{+}4]}\]
\[\ce{[BCl3 and BrCl3]}\]
\[\ce{[NH3 and NO^{-}3]}\]
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Solution
\[\ce{[BF^{–}4 and NH^{+}4]}\]
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.
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