Question

Select, isoelectronic species out of the following:

$CO,$ $N{O}^{+},$ $O_2^{-},$ $C{H}_4,$ $C{N}^{-},$ $NO$

• A. $CO,$ $N{O}^{+},$$C{N}^{-}$
• B. $N{O}^{+},$$C{H}_4,$ $NO$
• C. $O_2^{-},$ $C{H}_4,$ $NO$
• D. $N{O}^{+},$ $O_2^{-},$$C{N}^{-}$

Answer 1

The correct option is A $CO,$ $N{O}^{+},$$C{N}^{-}$

Isoelectronic species are those which contain the same number of electrons. The total number of electrons are obtained by adding $6$ electrons for carbon, $7$ electrons for nitrogen, $1$ electron for hydrogen, $8$ electrons for oxygen, $+1$ for negative charge and $-1$ for positive charge).

$CO$ has $6+8=14$ electrons.

$N{O}^{+}$ has $7+8-1=14$ electrons.

$O_2^{-}$ has $8+8+1=17$ electrons.

$C{H}_4$ has $6+4=10$ electrons.

$C{N}^{-}$ has $6+7+1=14$ electrons.

$NO$ has $7+8=15$ electrons.