Question

What is the hybridization of nitrogen in each of the following ions and molecules? (a) NO2+

(b) NO2-
(c) N2O
(d) N2O5
(e)N2O3

Answer 1

The hybridization of nitrogen in different ions and molecules

Step-by-step explanation:

The hybridization of nitrogen in each of the following ions and molecules is as follows:

(a) NO2+: In NO2+, nitrogen is sp2 hybridized.

(b) NO2-: In NO2-, nitrogen is sp2 hybridized.

(c) N2O: In N2O, nitrogen is sp hybridized.

(d) N2O5: In N2O5, nitrogen is sp3 hybridized.

(e) N2O3: In N2O3, nitrogen is sp2 hybridized.

Answer 2

The hybridization of nitrogen varies from sp to sp3 depending on the molecular structure and the number of bonded regions and lone pairs: NO2+ has sp, NO2- and N2O (terminal N) as well as N2O3 have sp2, while N2O5 and N2O (central N) have sp3 and sp hybridization, respectively.

Step-by-step explanation:

The hybridization of nitrogen in each of the given ions and molecules can be determined by considering the steric number, which is the sum of the number of atoms bonded to nitrogen and the number of lone pairs on nitrogen.

Here's the hybridization for each:

• NO2+: The nitrogen in NO2+ has two bonding regions and no lone pairs, leading to sp hybridization.
• NO2-: The nitrogen in NO2- has two bonding regions and one lone pair, resulting in sp2 hybridization.
• N2O: For the terminal nitrogen in N2O, there are three bonding regions and no lone pairs, indicating sp2 hybridization; however, the central nitrogen, which is triple-bonded to another nitrogen, would be sp hybridized.
• N2O5: The nitrogen atoms in N2O5 are equivalent, with each nitrogen having four bonding regions and no lone pairs, which means sp3 hybridization.
• N2O3: For N2O3, each nitrogen has three bonding regions and one lone pair, so sp2 hybridization is appropriate for both nitrogen atoms.