# If a molecule has both polar and ionic bonds in it, is it polar or nonpolar overall?

To be more specific, lets take a look at the Lewis Structure of two such examples:

The first one is SiCl${_3}$F. The red arrow represents an ionic bond while the blue is a polar covalent bond.

Now, the polar bonds on the Cl atoms that are separated horizontally cross out. Looking vertically, however, the ionic bond is stronger than the polar bond, so does that mean the molecule over-all is a polar molecule? I say this because my textbook says it is a tetrahedral polar.

The next one is SiF${_2}$Cl${_2}$. Same here; the ionic bonds and polar bonds should cancel out and the molecule would be a non-polar molecule overall, but my textbook says it is a polar molecule for some reason.

• There's no ionic bond in here. Difference in standard electronegativities is not enough to tell, even misleading here. – Mithoron Dec 5 '16 at 1:14
• Beyond what @Mithoron said, remember that these molecules won't be planar -- they're tetrahedral. So, e.g., the 'horizontal' $\ce{Si\!-\!Cl}$ bonds don't cancel each other out -- they'll still have a residual contribution to the overall polarity of the molecule. – hBy2Py Dec 5 '16 at 1:38