Question

(a) Draw the best Lewis structure(s) for the nitrite ion, NO2-. (b) With what allotrope of oxygen is it isoelectronic? (c) What would you predict for the lengths of the bonds in NO2- relative to N¬O single bonds and double bonds?

Answer 1

(a)
`NO_(2)^(-)` ion has two resonance structures.

(b)
`O_(3)` molecule is isoelectronic.

(c) Due to resonance N-O bond is having double bond character.

Step-by-step explanation:

(a)

The Lewis structure of
`NO_(2)^(-)` is as follows.

(In attachment)

(b)

Isoelectronic means both species having same number of electrons .

`NO_(2)^(-)` is isoelectronic with
`O_(3)` .

Both these molecules having 24 electrons and 18 valence electrons.

Hence,
`O_(3)` molecule isoelectronic with
`NO_(2)^(-)`.

(c)

The bond length of N-O single bond is more than the N-O double bond.

Due to the resonance structure of
`NO_(2)^(-)` N-O bond has double bond character.