* Polar Bonds: The bonds between the carbon atom and each oxygen atom are polar. Oxygen is more electronegative than carbon, meaning it pulls the shared electrons closer to itself. This creates a partial negative charge (δ-) on the oxygen atoms and a partial positive charge (δ+) on the carbon atom.

* Linear Geometry: CO₂ has a linear molecular geometry. The two oxygen atoms are positioned on opposite sides of the carbon atom, creating a symmetrical arrangement.

* Zero Dipole Moment: The polarities of the two carbon-oxygen bonds cancel each other out because they are equal in magnitude and opposite in direction. This results in a net dipole moment of zero for the CO₂ molecule.

In essence, although CO₂ has polar bonds, its symmetrical shape ensures that the individual bond dipoles cancel out, leading to an overall nonpolar molecule.