There is no p orbital surrounding the Boron atom, so the ring does not have a fully conjugated pi system. In addition, there are 8 electrons, which does not follow Huckel's rule (an aromatic system contains 4n+2 electrons). The pi electrons include the lone pair (not shown, but implicit) on the nitrogen atom, which is why the answers with "6 electrons" are not correct.

The correct answer is (8) Annulene. This is because all aromatic compounds must follow Huckel's Rule, which is 4n+2. Note that "n" in Huckel's Rule just refers to any whole number, and 4n+2 should result in the number of pi electrons an aromatic compound should have. For example, 4(0)+2 gives a two-pi-electron aromatic compound.

It is also important to note that Huckel's Rule is just one of three main rules in identifying an aromatic compound. An annulene is a system of conjugated monocyclic hydrocarbons. A compound is considered anti-aromatic if it follows the first two rules for aromaticity (1. Pi bonds are in a cyclic structure and 2. The structure must be planar), but does not follow the third rule, which is Huckel's Rule.

(8) Annulene follows the first two rules, but not Huckel's Rule, and is therefore antiaromatic; no value of a whole number for "n" will result in 8 with the formula 4n+2.

The lone pairs on the two nitrogen atoms reside in sp2 orbitals, meaning they do not participate in resonance. Within the ring, there are three bonds, meaning there are six electrons. Thus, the molecule is aromatic because it is planar and follows Huckel's rule.

For a compound to be considered aromatic, it must be flat, cyclic, and conjugated and it must obey Huckel's rule. Huckel's rule states that an aromatic compound must have pi electrons in the overlapping p orbitals in order to be aromatic (n in this formula represents any integer). Only compounds with 2, 6, 10, 14, . . . pi electrons can be considered aromatic. Compound A has 6 pi electrons, compound B has 4, and compound C has 8. This eliminates answers B and C. Answer D is not cyclic, and therefore cannot be aromatic. The only aromatic compound is answer choice A, which you should recognize as benzene.

There are 14 pi electrons because oxygen must contribute 2 pi electrons to avoid antiaromaticity. The other 12 pi electrons come from the 6 double bonds.

Nitrogen does not contribute any pi electrons, as it is hybridized and it's lone pairs are stored in sp2 orbitals, incapable of pi delocalization. Each nitrogen's p orbital is occupied by the double bond.

A molecule is aromatic when it adheres to 4 main criteria:

1. The molecule must be planar

2. The molecule must be cyclic

3. Every atom in the aromatic ring must have a p orbital

4. The ring must contain pi electrons

The carbon on the left side of this molecule is an sp3 carbon, and therefore lacks an unhybridized p orbital. The molecule is non-aromatic.

When determining whether a molecule is aromatic, it is important to understand that aromatic molecules are the most stable, followed by molecules that are non-aromatic, followed by molecules that are antiaromatic (the least stable). Therefore, if it is possible that a molecule can achieve a greater stability through switching the hybridization of one of its substituent atoms, it will do this.

An aromatic must follow four basic criteria: it must be a ring planar, have a continuous chain of unhybridized p orbitals (a series of sp2-hybridized atoms forming a conjugated system), and have an odd number of delocalized electron pairs in the system. Furan is planar ring (fulfilling criteria and , and its oxygen atom has a choice of being sp3-hybridized or sp2-hybridized. Depending on what hybridization the oxygen atom chooses will determine whether the molecule is aromatic or not.

If the oxygen is sp3-hybridized, the molecule will not have a continuous chain of unhybridized p orbitals, and will not be considered aromatic (it will be non-aromatic). If the oxygen is sp2-hybridized, it will fulfill criterion . Placing one of its lone pairs into the unhybridized p orbital will add two more electrons into the conjugated system, bringing the total number of electrons to (or, it will have pairs of electrons). Because it has an odd number of delocalized electrons it fulfills criterion , and therefore the molecule will be considered aromatic.

Because an aromatic molecule is more stable than a non-aromatic molecule, and by switching the hybridization of the oxygen atom the molecule can achieve aromaticity, a furan molecule will be considered an aromatic molecule.

An aromatic must follow four basic criteria: it must be a ring planar, have a continuous chain of unhybridized p orbitals (a series of sp2-hybridized atoms forming a conjugated system), and have an odd number of delocalized electron pairs in the system. This molecule cannot be considered aromatic because this sp3 carbon cannot switch its hybridization (it has no lone pairs). Therefore, it fails to follow criterion and is not considered an aromatic molecule. It is a non-aromatic molecule.

If oxygen contributes any pi electrons, the molecule will have 12 pi electrons, or 4n pi electrons, and become antiarmoatic. As it is now, the compound is antiaromatic.

Nitrogen cannot give any pi electrons because it's lone pair is in an sp2 orbital. Boron has no pi electrons to give, and only has an empty p orbital.

An aromatic must follow four basic criteria: it must be a ring planar, have a continuous chain of unhybridized p orbitals (a series of sp2-hybridized atoms forming a conjugated system), and have an odd number of delocalized electron pairs in the system. If the molecule fails any of the first three criteria, it is considered non-aromatic, and if it fails the only the fourth criterion (it has an even number of delocalized electron pairs), the molecule is considered antiaromatic. In the case of cyclobutadiene, by virtue of its structure follows criteria and . However, it violates criterion by having two (an even number) of delocalized electron pairs. Although it's possible that a molecule can try to escape from being antiaromatic by contorting its 3D shape so it is not planar, cyclobutadiene is too small to do this effectively. Therefore, cyclobutadiene is considered antiaromatic.