Based upon electronegativity differences, which of the following bonds is(are) labeled correctly with respect to indicating a bond dipole?
I.
II.
III.

Question

Based upon electronegativity differences, which of the following bonds is(are) labeled correctly with respect to indicating a bond dipole?
I. 
II. 
III.

Quizplus · Accepted Answer

In order for a bond to have a dipole moment, there must be a difference in electronegativity between the two atoms involved. In choice I, both carbon and hydrogen have similar electronegativity values, so there would be no bond dipole. In choice II, both oxygen atoms have similar electronegativity values, so there would also be no bond dipole. However, in choice III, there is a difference in electronegativity between the carbon and chlorine atoms, indicating a bond dipole.

Based Upon Electronegativity Differences, Which of the Following Bonds Is(are)