00:01
To determine whether or not these molecules are polar, we need to draw the lewis structure.
00:06
Silicon has four valence electrons.
00:09
Fluorine has seven, and there are four of them, for a total of 32 valence electrons.
00:15
If we bond each fluorine to silicone, we would have used up two times four, eight of the 32 valence electrons, leaving us 24 valence electrons.
00:27
If we add three lone pairs to each fluorine, we would have used up the remaining 24 valence electrons.
00:35
Silicone has an octet and the fluorines have an octet, and we've used up all our valence electrons.
00:41
We have four electron groups surrounding silicone, which results in a tetrahedral structure.
00:47
A tetrahedral structure, when all bonds are equal, allows for bond polarity cancellation, where the molecule itself is non -polar.
00:58
The next one is hbr.
01:00
This is just a single bonded molecule...