Question

Which of the following is isoelectronic and isostructural with $C{O}_2$?

• A. $N{O}_2$
• B. ${N{O}_3}^{-}$
• C. ${N{O}_2}^{-}$
• D. $N_{2}O$

Answer 1

The correct option is D $N_{2}O$

$\to$ Isoelectronic species have the same number of electrons and ISO-structural species have the same type of hybridization at the central atom.

${CO}_2$ = No. of electrons= $6+8\left(2\right)$

$=6+16=22$ electrons

Hybridization of C in ${CO}_2$ $=sp$

a) ${NO}_2$
No. of electrons$=7+8\left(2\right)=7+16=23$ electrons

Hybridization of N in ${NO}_2$ $=sp$

b)${NO}_3^{-}$

No.of electrons$=7+8\left(3\right)+1$

$=31$ electrons

Hybridization=${sp}^2$

c) ${NO}_2^{-}$

No.of electrons$=7+8\left(2\right)+1$

$=24$ electrons

Hybridization$=sp$

d)$N_{2}O$

No. of electrons$=7\left(2\right)+8$

$=22$ electrons

Hybridization$=sp$

Hence $N_{2}O$ is iso electronic and iso structural with ${CO}_2$