Overview:
The aromatic nitrogen molecule refers to a nitrogen atom that is a part of an aromatic ring, such as in pyridine or pyrrole. The hybridization of the nitrogen atom determines its shape and bonding characteristics. In the case of an aromatic nitrogen molecule, the nitrogen atom is sp2 hybridized.

Explanation:
To understand why the correct answer is option C, let's break down the concept of hybridization and examine the electronic configuration of nitrogen.

Hybridization:
Hybridization is a concept in chemistry that explains the mixing of atomic orbitals to form new hybrid orbitals. These hybrid orbitals have different shapes and energy levels than the original atomic orbitals. Hybridization occurs when an atom forms bonds with other atoms.

Electronic Configuration of Nitrogen:
The electronic configuration of nitrogen is 1s2 2s2 2p3. Nitrogen has five valence electrons, three of which are in the 2p orbital.

Hybridization of Nitrogen in Aromatic Molecules:
In an aromatic nitrogen molecule, the nitrogen atom is a part of an aromatic ring. The aromatic ring is a planar structure with delocalized π electrons. To accommodate the delocalization of π electrons, the nitrogen atom must have a planar geometry.

The nitrogen atom in an aromatic molecule undergoes sp2 hybridization, where one s orbital and two p orbitals mix to form three sp2 hybrid orbitals. These hybrid orbitals are oriented in a trigonal planar arrangement, with an angle of 120 degrees between them. One of the hybrid orbitals overlaps with a carbon atom in the aromatic ring to form a sigma bond, while the other two hybrid orbitals contain a lone pair of electrons and form a π bond.

Conclusion:
In summary, the correct statement regarding the aromatic nitrogen molecule is that it is sp2 hybridized. The sp2 hybridization allows the nitrogen atom to have a planar geometry and participate in the delocalization of π electrons in the aromatic ring.