In which of the following pairs of molecules/ | vedclass

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(B) For $sp^{2}$ hybridisation,the steric number (sum of $\sigma$-bonds and lone pairs) must be $3$.$(I)$ $NO_{2}^{-}$: Central $N$ atom has $2$ $\sig

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$BF_{3}$ and $NO_{2}^{-}$

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(B) For $sp^{2}$ hybridisation,the steric number (sum of $\sigma$-bonds and lone pairs) must be $3$.$(I)$ $NO_{2}^{-}$: Central $N$ atom has $2$ $\sigma$-bonds and $1$ lone pair,so steric number $= 3$,which corresponds to $sp^{2}$ hybridisation.$(II)$ $NH_{3}$: Central $N$ atom has $3$ $\sigma$-bonds and $1$ lone pair,so steric number $= 4$,which corresponds to $sp^{3}$ hybridisation.$(III)$ $BF_{3}$: Central $B$ atom has $3$ $\sigma$-bonds and $0$ lone pairs,so steric number $= 3$,which corresponds to $sp^{2}$ hybridisation.$(IV)$ $NH_{2}^{-}$: Central $N$ atom has $2$ $\sigma$-bonds and $2$ lone pairs,so steric number $= 4$,which corresponds to $sp^{3}$ hybridisation.$(V)$ $H_{2}O$: Central $O$ atom has $2$ $\sigma$-bonds and $2$ lone pairs,so steric number $= 4$,which corresponds to $sp^{3}$ hybridisation.Thus,the pair $BF_{3}$ and $NO_{2}^{-}$ both exhibit $sp^{2}$ hybridisation.

List-$I$	List-$II$
$(a)$ $SF_6$	$(i)$ $sp^3d^2$
$(b)$ $PCl_5$	(ii) $sp^3d$
$(c)$ $XeF_4$	(iii) $sp^3d^3$
$(d)$ $IF_7$	(iv) $sp^3d^2$

In which of the following pairs of molecules/ions,the central atoms have $sp^{2}$ hybridisation?

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In which of the following pairs do both the species have $sp^{3}$ hybridization?

Consider the following species: $BrF_5, XeF_5^-, BF_4^-, ICl_4^-, XeF_4, SF_4, NH_4^+, ClF_3, XeF_2, ICl_2^-$. Number of species having $sp^3d$ hybridized central atom is . . . . . . .

Match the following:
List-$I$ List-$II$
$(a)$ $SF_6$ $(i)$ $sp^3d^2$
$(b)$ $PCl_5$ (ii) $sp^3d$
$(c)$ $XeF_4$ (iii) $sp^3d^3$
$(d)$ $IF_7$ (iv) $sp^3d^2$

The correct answer is:

What is the type of hybridization in $IF_5$?

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