Question

Which of the following is not aromatic in nature?
A.
B.
C.
D.

Answer 1

Four structural criteria must be satisfied for a compound to be aromatic. The compound must be cyclic, conjugated, planar, and satisfies Huckel’s rule. Electrons in the p orbital are called $\pi$ electrons. Also we can confirm whether an atom is ${{s}}{{{p}}^2}$ hybridized by checking whether the atom has bonded to three atoms and it has no lone pairs.

Complete step by step answer:
Aromatic compounds have a distinctive odor. For a compound to be aromatic, it should be cyclic, planar with resonance bonds, not contain ${{s}}{{{p}}^3}$ hybridized carbon atom and satisfies Huckel’s rule.
When the compound has a ring of atoms, it is called a cyclic compound. It is said to be planar if all the atoms are in the same plane.
Huckel’s rule states that the aromatic compounds contain $\left( {4{{n}} + 2} \right)\pi$ electrons, where ${{n}}$ is any integer.
A.
This compound has two $\pi$ electrons. It is planar, cyclic and obeys Huckel’s rule of aromaticity.
$\left( {4{{n}} + 2} \right) = 2 \\\ 4{{n}} = 0 \\\ {{n}} = 0 \\\$
B.
This compound has six $\pi$ electrons, thereby obeys Huckel’s rule where ${{n}} = 1$ and it is cyclic, planar and conjugated.
C.
It has six $\pi$ electrons since the negative charge is considered as electrons. Thus it obeys Huckel’s rule. It is also cyclic, planar and conjugated.
D. It has eight $\pi$ electrons, which satisfy $4{{n}}\pi$ rule of anti aromaticity, where ${{n}} = 2$. Thus it is not aromatic, but anti aromatic.

So, the correct answer is Option D.

Note: Based on Huckel’s molecular orbital theory, when all the bonding orbitals are filled with electrons, it is said to be stable. In aromatic compounds, two electrons are filled in the lower energy orbital and four electrons are filled in the following energy level.