Final answer:
A molecule with polar bonds will not always be polar; the overall molecular polarity is determined by the symmetry of the molecule and the orientation of the polar bonds, not solely by bond polarity.
Step-by-step explanation:
No, it is not true that a molecule with polar bonds will always be polar. Molecular polarity depends on both bond polarity and the overall shape of the molecule. For instance, if a molecule contains just one polar bond, it's definitely polar as there's nothing to balance out its dipole moment. However, if there are multiple polar bonds, the shape of the molecule dictates whether the bond polarities cancel out.
For molecules with symmetrical shapes, such as linear, trigonal planar, or tetrahedral structures with equal bonds, the polarity of individual bonds can cancel each other out, leading to a nonpolar molecule. On the other hand, asymmetric molecules with polar bonds, like water (H2O), fail to cancel out these individual bond polarities, which results in an overall polar molecule.
Thus, while bond polarity and electronegativity are important, the symmetry of the molecule is crucial in determining the net dipole moment and hence the overall polarity of the molecule.