Aromaticity requires that a species be cyclic, planar, fully conjugated around the ring, and contain a specific number of delocalised pi electrons given by Huckel's rule, namely $(4n+2)$ where $n$ is a non-negative integer. Substituting $n=0,1,2$ gives allowed counts of $2,6,10$ pi electrons, which is why benzene with six pi electrons is the archetypal aromatic compound. The option specifying $4n$ electrons such as $4,8,12$ is wrong because those counts correspond to antiaromatic systems, which are actually destabilized, like cyclobutadiene. The option allowing any even number is incorrect because $4n$ even counts are not aromatic, so evenness alone is insufficient. The claim of exactly eight pi electrons is false since eight equals $4n$ and would be antiaromatic, not aromatic. The rule also requires planarity and continuous overlap, which is why non-planar or non-conjugated rings are not aromatic even with the right electron count. The physical basis of the rule lies in molecular orbital theory: a $(4n+2)$ count exactly fills all the bonding molecular orbitals of the cyclic pi system, giving a closed-shell, low-energy arrangement, whereas a $4n$ count leaves two electrons in non-bonding or partially filled orbitals and is destabilised. This is the NCERT and JEE statement of Huckel's rule applied to cyclic conjugated systems. A plausibility check: benzene's six pi electrons fit $(4n+2)$ with $n=1$, anchoring the rule.