Drawing the Lewis Structure for COF2
Transcript: This is the COF2 Lewis structure. On the periodic table, Carbon, in group 4 or 14, has 4 valence electrons. Oxygen, in group 6, also called 16; 6 valence electrons. For Fluorine, we have 7, but we have those two Fluorines there, for a total of 24 valence electrons. Carbon is the least electronegative so we put that in the center. Let's put the Oxygen up here, and then two Fluorines on the outside. Put two electrons between atoms to form a chemical bond and then around the outside. So we've used 2, 4, 6, 8, 10, and 24.
So at this point, we've used all 24 valence electrons. The Oxygen has 8 valence electrons, as does this Fluorine and the other Fluorine over here. However, in the center, Carbon only has 6 valence electrons so its octet is not filled. Let's take two valence electrons from the Oxygen and we'll put them in the center right here and share them with the Carbon. So by forming that double bond, Oxygen still has 8 valence electrons, but Carbon has 8 valence electrons. Our Fluorines also still have 8. So we've used the 24 valence electrons and filled the octets on each of the atoms in the COF2 Lewis structure.
Note that I shared the valence electrons from Oxygen with the Carbon to form the double bond, and not Fluorine. That's because Oxygen is less electronegative, and it's going to be more likely to share its valence electrons than something like Fluorine, which is very electronegative.
That's the COF2 Lewis structure. This is Dr. B., and thanks for watching.