ACS Chemistry Practice Exam 2025 – The All-in-One Guide to Exam Success!

A bent compound is expected to exhibit the largest dipole moment because of its molecular geometry, which results in an unequal distribution of electron density. In a bent structure, such as water (H₂O), the bond angles are typically less than 180 degrees, causing the bond dipoles to not cancel each other out. Instead, they add up to produce a net dipole moment that points in the direction of the more electronegative atom, leading to a stronger overall dipole.

In contrast, a linear compound can have bond dipoles that point in opposite directions, potentially canceling each other out if the substituents are identical, which minimizes the dipole moment. Similarly, a trigonal planar compound often exhibits symmetry that allows the dipole moments to balance out, resulting in a smaller dipole. A tetrahedral compound, while asymmetrical, may still feature sets of identical bonds that can lead to cancellation.

Thus, it is the bent structure that, by virtue of its geometry, maximizes the net dipole moment compared to the other types of compounds presented.