The hybridization of atomic orbitals of nitro | vedclass

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(B) To determine the hybridization,we use the formula: $	ext{Hybridization} = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electro

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$sp$,$sp^2$,and $sp^3$ respectively

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(B) To determine the hybridization,we use the formula: $	ext{Hybridization} = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.$1$. For $NO_2^+$: $	ext{Hybridization} = \frac{1}{2} [5 + 0 - 1 + 0] = 2$,which corresponds to $sp$ hybridization.$2$. For $NO_3^-$: $	ext{Hybridization} = \frac{1}{2} [5 + 0 - 0 + 1] = 3$,which corresponds to $sp^2$ hybridization.$3$. For $NH_4^+$: $	ext{Hybridization} = \frac{1}{2} [5 + 4 - 1 + 0] = 4$,which corresponds to $sp^3$ hybridization.Thus,the correct order is $sp$,$sp^2$,and $sp^3$ respectively.

The hybridization of atomic orbitals of nitrogen in $NO_2^+$,$NO_3^-$,and $NH_4^+$ are:

Similar Questions

How many $sp^2$ and $sp$ hybridized carbon atoms are present respectively in the following compound? (The structure is $1,2-didehydrobenzene$ or $benzyne$ derivative,specifically $1,2-didehydrocyclohexadiene$ structure shown in the image).

In which of the following molecules is the $N$ atom not $sp^2$ hybridized?

The compounds with $sp^2$ hybridized central atom among the following are:
$(A)$ $H_2CO_3$
$(B)$ $SiF_4$
$(C)$ $BF_3$
$(D)$ $HClO_2$

Which of the following will be octahedral?

Which one of the following has the regular tetrahedral structure?
(Atomic no. : $B = 5, S = 16, Ni = 28, Xe = 54$)

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