Are #"CCl"_4# or #"CBr"_4# polar?

1 Answer
Apr 22, 2017

Answer:

The bond is, the molecule is not................

Explanation:

We could represent the polarity of an individual #C-Cl# bond as #""^(delta+)C-Cl^(delta-)# in that chlorine is more electronegative than carbon, and charge separation, i.e. polarity occurs. And thus the #C-Cl# bond is POLAR. But molecular polarity is the result of the VECTOR sum of the individual bond dipoles. And thus when we sum geometrically in a vector fashion, the RESULTANT bond dipole is ZERO.............And thus #"CCl"_4# and #"CBr"_4# are NON-POLAR molecules, whereas #"HCCl"_3# and #"CH"_2"Cl"_2# are POLAR........

Do you appreciate this distinction?