Question

\[\ce{CO}\] is isoelectronic with

(i) \[\ce{NO+}\]

(ii) \[\ce{N2}\]

(iii) \[\ce{Sncl2}\]

(iv) \[\ce{NO^{-}2}\]

Answer 1

(i) \[\ce{NO+}\]

(ii) \[\ce{N2}\]

Explanation:

The species having the same number of electrons are known as isoelectronic species. 

The number of electrons in \[\ce{CO}\] species is 14;8 electrons from oxygen atom and 6 electrons from carbon atom.

The number of electrons in \[\ce{NO+}\] is 14;8 electrons from oxygen atom, 7 electrons from nitrogen atom and 1 electron will be subtracted due to the positive charge on the species.

The number of electrons in \[\ce{N2}\] is 14;7 from each nitrogen atom.

The number of electrons in \[\ce{SnCl2}\] is 84;50 from the tin atom and 17 from each chlorine atom.

The number of electrons in \[\ce{NO^{-}2}\] is 24;7 from nitrogen atom, 8 from each oxygen atom and 1 from the negative charge on the species.

Hence \[\ce{NO+}\] and \[\ce{N2}\] are the isoelectronic species of \[\ce{CO}\].