Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to `10^(-18)` esu cm.
Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc.
Q. Which of the following statement is correct regarding `C_(2)H_(2)F_(2)` molecule?

Options

A. One isomer is polar, one is non-polar
B. Two isomers are polar, one is non-polar
C. Two isomers are planar, one is non-planar
D. Two isomers are only possible and planar

Answer

B

Explanation