# Question 457ca

Jun 9, 2016

#### Explanation:

The methyl fluoride $C {H}_{3} F$ is a polar molecule. The polarity is due to the difference in the electronegativity between fluorine and carbon.

Fluorine, which i the most electronegative element will pull the electron density of carbon toward it, creating a partial negative charge on fluorine and a partial positive charge on carbon as is represented below:

color(blue)(""^(+delta)C-F^(delta-))#

This polar bond will have a net dipole moment that will not cancel out, since the $\textcolor{red}{C - H}$ bonds are considered to be non polar and thus, the molecule will have a net dipole moment and will be polar.

For such a molecule, the possible intermolecular interactions are:

1. London Dispersion Force (LDF).
2. Dipole - Dipole Interactions (DD).

Note, that, in this case DD is stronger than LDF and therefore, the main intermolecular interactions is the dipole-dipole (DD).