The species in which the central atom uses ${s p}^{2}$ - hybrid orbitals in its bonding is

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Solution

The correct option is C

${C H_{3}}^{+}$

C is central atom

ep = $\frac{V + L + A - C}{2}$ = $\frac{4 + 3 - 1}{2}$ = 3

3 $\Rightarrow$ Trigonal Planar $\Rightarrow$ ${s p}^{2}$ hybridization.

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s p^{2}

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The correct order of hybridization of the central atom in the following species $N H_{3}, [P t C l_{4}]^{2 -}$ , $P C l_{5}$ and $B C l_{3}$ is

s p^{2}

C H {_{3}}^{+}

C H {_{3}}^{-}

∙ C H_{3}

C H_{2}

{N_{3}^{-}, N O C l, N_{2} O}

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