Answer
The molecules BF3, CF4, CO2, PF5, and SF6 are all nonpolar, even though they all contain polar bonds, due to the overall symmetry of the molecules.
Work Step by Step
- In these molecules, the central atoms (B, C, P, and S) are bonded to highly electronegative fluorine (F) or oxygen (O) atoms, creating polar bonds.
- However, the overall molecular geometry of these compounds is such that the individual bond dipole moments cancel out, resulting in a net zero dipole moment and a nonpolar molecule.
- For example, in BF3, the three B-F bonds are polar, but the 120-degree bond angles result in a trigonal planar geometry where the bond dipole moments cancel out, making the molecule nonpolar.
- Similarly, in the other molecules, the specific molecular geometries (tetrahedral for CF4 and PF5, linear for CO2, and octahedral for SF6) lead to the cancellation of the individual bond dipole moments, resulting in a nonpolar overall structure.
