# How can molecules with polar bonds be nonpolar?

Take ${\text{CCl}}_{4}$...each individual $C - C l$ bond is polar...and we could represent this as... $\stackrel{\text{^+delta)C-stackrel(} {\delta}^{-}}{C} l$.. HOWEVER, molecular polarity is the VECTOR SUM of the individual bond dipoles, and certainly, the geometric sum of the bond dipoles in this highly symmetric, tetrahedral molecule is a BIG FACT ZERO.... And hence ${\text{CCl}}_{4}$ is NON-POLAR, whereas, $C H C {l}_{3}$, $\text{chloroform}$, is polar...given the bond dipoles here would give a resultant upon addition.
For another example, consider $P {F}_{5}$..would the bond dipoles sum to zero?