Introduction:
Carbon monoxide (CO) is a neutral compound, despite being an oxide of a nonmetal. This can be explained by understanding its electronic structure and bonding.

Electronic Structure:
Carbon monoxide consists of a carbon atom bonded to an oxygen atom by a triple bond. The carbon atom provides two electrons, and the oxygen atom provides six electrons. This results in a total of eight valence electrons, fulfilling the octet rule for both carbon and oxygen.

Polarity of the CO Bond:
The CO bond is polar due to the difference in electronegativity between carbon and oxygen. Oxygen is more electronegative, resulting in a partial negative charge on the oxygen atom and a partial positive charge on the carbon atom.

Interaction with Water:
When carbon monoxide dissolves in water, it forms carbonic acid (H2CO3), which is a weak acid. The CO molecule acts as a Lewis acid, accepting a lone pair of electrons from a water molecule to form a coordinate covalent bond. This reaction results in the formation of a hydronium ion (H3O+) and a hydroxide ion (OH-). The overall reaction can be represented as:
CO + H2O -> H3O+ + OH-

Neutral Nature:
The neutral nature of carbon monoxide can be attributed to its ability to act as both an acid and a base. In the reaction with water, it accepts a pair of electrons from water, behaving as an acid. On the other hand, carbon monoxide can also donate a pair of electrons to form a coordinate covalent bond, behaving as a base. This amphoteric nature allows carbon monoxide to maintain neutrality.

Conclusion:
In summary, carbon monoxide is a neutral compound despite being an oxide of a nonmetal because it fulfills the octet rule, possesses a polar bond, and can act as both an acid and a base. Its ability to accept and donate electrons allows it to maintain neutrality.