Which range of electronegativity indicates a nonpolar covalent bond?

A nonpolar covalent bond occurs when the difference in electronegativity between the two atoms involved is minimal. This small difference allows the electrons to be shared equally between the atoms, resulting in no significant charge separation.

In the case of a nonpolar covalent bond, a difference in electronegativity of 0 to 0.4 typically indicates that the two atoms have similar tendencies to attract electrons. Under such conditions, the electron density is evenly distributed across the bond, which is characteristic of nonpolar bonds.

On the other hand, higher values of electronegativity differences, such as those presented in the other ranges, indicate either polar covalent bonds or ionic character. For example, a difference of 1.7 and greater would lead to ionic bonds, where one atom significantly pulls the electrons away from the other, creating distinct positive and negative charges. Values between 0.5 and 1.7 indicate varying degrees of polar covalent bonding, where there is a partial charge separation but not enough to classify it as ionic.

Thus, the correct choice for indicating a nonpolar covalent bond is indeed the range of 0 to 0.4.