If a covalent bond were to be formed between a nitrogen atom (electronegativity 3.0) and an oxygen atom (electronegativity 3.5), which of the following statements would best describe such a bond?

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The key idea is how strongly each atom pulls on the shared electrons, which determines bond character. A large difference in electronegativity leads to ionic character; a small difference leads to nonpolar covalent; a moderate difference gives polar covalent bonds with partial charges.

Here, nitrogen has 3.0 and oxygen has 3.5, a difference of 0.5. That sits in the range for polar covalent bonds. The more electronegative oxygen pulls the bonding electrons closer, giving oxygen a partial negative charge and nitrogen a partial positive charge. The bond remains covalent because the electrons are still shared rather than fully transferred, so it’s not ionic. It’s not metallic because that involves a sea of delocalized electrons across metal atoms, not a heteronuclear nonmetal bond.