# Why is a molecule of CO_2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar?

$\text{Because the C=O dipoles are horizontally opposed..........}$
$\text{......and their VECTOR sum gives no resultant dipole.}$
$C {O}_{2}$ is a linear molecule, and the $\angle \text{O"-"C"-"O}$ is ${180}^{\circ}$. Dipoles are vector quantities; they have magnitide and direction. While there is charge separation, i.e. polarity, in an individual $\text{C"="O}$ bond, the resultant vector from the sum of the individual bond dipoles in the ${\text{^(delta-)"O"="C"^(delta+)="O}}^{\delta -}$ molecule is clearly ZERO. The same thing is observed with the ${\text{CCl}}_{4}$ molecule, but not with the ${\text{CHCl}}_{3}$ or ${\text{CH"_2"Cl}}_{2}$ molecule. Capisce?