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In which of the following pairs of molecules/ions, the central atoms have $\mathrm{sp}^2$ hybridisation?
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The correct answer is:
$\mathrm{BF}_3$ and $\mathrm{NO}_2^{-}$
Key Idea For $\mathrm{sp}^2$ hybridisation, there must be $3 \sigma$-bonds or $2 \sigma$-bonds along with a lone pair of electrons.
(i) $\mathrm{NO}_2^{-} \Rightarrow 2 \sigma+1 \mathrm{lp}=3$, ie, $\mathrm{sp}^2$ hybridisation
(ii) $\mathrm{NH}_3 \Rightarrow 3 \sigma+1 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
(iii) $\mathrm{BF}_3 \Rightarrow 3 \sigma+0 \mathrm{lp}=3$, ie, $\mathrm{sp}^2$ hybridisation
(iv) $\mathrm{NH}_2^{-} \Rightarrow 2 \sigma+2 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
(v) $\mathrm{H}_2 \mathrm{O} \Rightarrow 2 \sigma+2 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
Thus, among the given pairs, only $\mathrm{BF}_3$ and $\mathrm{NO}_2^{-}$ have $\mathrm{sp}^2$ hybridisation.
(i) $\mathrm{NO}_2^{-} \Rightarrow 2 \sigma+1 \mathrm{lp}=3$, ie, $\mathrm{sp}^2$ hybridisation
(ii) $\mathrm{NH}_3 \Rightarrow 3 \sigma+1 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
(iii) $\mathrm{BF}_3 \Rightarrow 3 \sigma+0 \mathrm{lp}=3$, ie, $\mathrm{sp}^2$ hybridisation
(iv) $\mathrm{NH}_2^{-} \Rightarrow 2 \sigma+2 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
(v) $\mathrm{H}_2 \mathrm{O} \Rightarrow 2 \sigma+2 \mathrm{lp}=4$, ie, $\mathrm{sp}^3$ hybridisation
Thus, among the given pairs, only $\mathrm{BF}_3$ and $\mathrm{NO}_2^{-}$ have $\mathrm{sp}^2$ hybridisation.
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