Based on the VSEPR model, what is the polarity of CO2
The Correct Answer and Explanation is:
Carbon dioxide (CO2) is a linear molecule, and its polarity can be determined by considering the arrangement of its bonds and the molecular geometry.
According to the Valence Shell Electron Pair Repulsion (VSEPR) model, the carbon atom in CO2 forms two double bonds with two oxygen atoms. The electron pairs around the carbon atom are arranged in a linear geometry, with an angle of 180° between the two bonds. This linear arrangement results in a symmetrical distribution of charge.
While the C=O bonds are polar (because oxygen is more electronegative than carbon), the overall symmetry of the molecule cancels out the individual dipole moments. In other words, the two dipoles are equal in magnitude but opposite in direction. As a result, the molecule does not have a net dipole moment.
Because CO2 has a symmetrical linear structure, it is nonpolar despite having polar bonds. The symmetry ensures that the dipoles in the two C=O bonds cancel each other out, leading to no net polarity. Therefore, the molecule is considered nonpolar.
In summary, although CO2 contains polar bonds, its linear geometry results in a nonpolar molecule because the dipole moments cancel out.
