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Leya [2.2K]
3 years ago
8

(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?

Chemistry
1 answer:
maria [59]3 years ago
3 0

Answer:

(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.

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.

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6                            s, p, d                        18      (2+6+10)

7                             s, p                            8        (2+6)

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