The formal charges of N_{(1)},N_{(2)},and O a | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) The formal charge $(FC)$ is calculated as: $FC = (	ext{Total valence electrons}) - (	ext{Non-bonding electrons}) - \frac{1}{2}(	ext{Bonding ele

Vedclass · Accepted Answer

$-1, +1, 0$

Vedclass · Answer

(B) The formal charge $(FC)$ is calculated as: $FC = (	ext{Total valence electrons}) - (	ext{Non-bonding electrons}) - \frac{1}{2}(	ext{Bonding electrons})$.For $N_{(1)}$ (terminal nitrogen with $4$ non-bonding electrons and $2$ bonding electrons from a double bond): $FC = 5 - 4 - \frac{1}{2}(4) = -1$.For $N_{(2)}$ (central nitrogen with $0$ non-bonding electrons and $8$ bonding electrons from two double bonds): $FC = 5 - 0 - \frac{1}{2}(8) = +1$.For $O$ (oxygen with $4$ non-bonding electrons and $4$ bonding electrons from a double bond): $FC = 6 - 4 - \frac{1}{2}(4) = 0$.Thus,the formal charges are $-1, +1, 0$.

The formal charges of $N_{(1)}$,$N_{(2)}$,and $O$ atoms in the structure $N_{(1)} = N_{(2)} = O$ are respectively:

Similar Questions

Which among the following is $NOT$ an odd electron molecule?

Indicate the nature of bonding in $CCl_4$ and $CaH_2$.

Which of the following molecules has an axis of symmetry and a coaxial plane of symmetry?

Born-Haber cycle may be used to calculate:
$I$. $\Delta_{eg}H$
$II$. Mass number
$III$. Electronegativity
$IV$. Lattice energy

Which of the following are isostructural pairs?
$A.$ $SO_{4}^{2-}$ and $CrO_{4}^{2-}$
$B.$ $SiCl_{4}$ and $TiCl_{4}$
$C.$ $NH_{3}$ and $NO_{3}^{-}$
$D.$ $BCl_{3}$ and $BrCl_{3}$

Vedclass Test Series

Exam Paper Generator

Online Exam Module