No, the presence of a polar bond in a molecule does not necessarily make it a polar molecule. Whether a molecule is polar or nonpolar depends on the overall shape and arrangement of the atoms in the molecule.
For example, in carbon dioxide (CO2), the carbon-oxygen bonds are polar due to the difference in electronegativity between carbon and oxygen. However, the molecule itself is linear and symmetrical, with the two oxygen atoms on opposite sides of the carbon atom. As a result, the dipole moments of the individual bonds cancel each other out, making CO2 a nonpolar molecule.
Similarly, the absence of polar bonds in a molecule does not necessarily make it a nonpolar molecule. Again, the overall shape and arrangement of the atoms can determine whether a molecule is polar or nonpolar.
For example, in methane (CH4), all of the carbon-hydrogen bonds are nonpolar, but the molecule itself is tetrahedral in shape, with the four hydrogen atoms arranged symmetrically around the central carbon atom. As a result, the dipole moments of the individual bonds cancel each other out, making CH4 a nonpolar molecule.
In summary, the polarity of a molecule depends on the overall shape and arrangement of the atoms, not just the polarity of individual bonds.