Some molecules with polar bonds are nonpolar in nature due to their molecular geometry, which leads to the cancellation of the individual bond dipoles. This occurs when the molecule has a symmetrical structure, causing the bond dipoles to be evenly distributed and resulting in a net dipole moment of zero.A polar bond is formed when there is a significant difference in electronegativity between the two atoms involved in the bond. This difference causes an unequal sharing of electrons, leading to a partial positive charge on the less electronegative atom and a partial negative charge on the more electronegative atom. This creates a bond dipole moment.However, if a molecule has a symmetrical structure, the bond dipoles can cancel each other out, making the overall molecule nonpolar. This is because the individual bond dipoles are pointing in opposite directions, and their magnitudes are equal, leading to a net dipole moment of zero.Examples of molecules with polar bonds but nonpolar nature:1. Carbon dioxide CO2 : Carbon dioxide has two polar C=O bonds, but the molecule is linear, with the oxygen atoms symmetrically placed around the central carbon atom. This symmetry causes the bond dipoles to cancel each other out, resulting in a nonpolar molecule.2. Boron trifluoride BF3 : In this molecule, boron is bonded to three fluorine atoms, forming polar B-F bonds. However, the molecule has a trigonal planar geometry, with the fluorine atoms symmetrically distributed around the central boron atom. This arrangement leads to the cancellation of the bond dipoles, making the molecule nonpolar.3. Methane CH4 : Methane has four polar C-H bonds, but its tetrahedral geometry causes the bond dipoles to cancel each other out. The hydrogen atoms are symmetrically arranged around the central carbon atom, resulting in a nonpolar molecule.