Drawing the Lewis Structure for BeCl2
Transcript: Hi, this is Dr. B. Let's do the Lewis structure for Beryllium Chloride. On the periodic table Beryllium is in group 2, it has 2 valence electrons; Chlorine--group 7--7, but we have 2 of those Chlorines. We multiply that by 2 and add this, we get 16 total valence electrons. Let's draw it. We'll put the least electronegative, Beryllium, at the center, and on either side we'll put a Chlorine. And we have 16 valence electrons. Put 2 between the atoms to form the bonds, and then around the outside atoms, 6, 8, 10, 12, 14, 16.
We've used up all the valence electrons and let's see if we have octets. This is good on this Chlorine, and over here we're fine. We have 8 on both. But the Beryllium in the center only has 4. I know that Beryllium is kind of an exception. It doesn't necessarily need 8 valence electrons.
So I'm not sure if this is the right structure. The way to check is to use formal charges. So we have an equation here to calculate the formal charge for each of the atoms. So let's start with this Chlorine right here. Chlorine's in grou 7, so it has 7 valence elecrons. Nonbonding, these ones right here, there are 6 of those. And bonding, there are 2 of those, but we're going to divide that by 2. Seven minus 6 minus 1 is 0. The formal charge on Chlorine is 0, and since both Chlorines are the same, that's going to be 0, too.
OK, let's check out the Beryllium right here. So Beryllium is in group 2, 2 valence electrons. Nonbonding: well, all of the valence electrons for Beryllium are involved in bonds, so that's 0. Minus bonding, these right here dvided by 2. Two minus 0 minus 2 is 0, so the formal charge on Beryllium is also 0.
When the formal charges are all 0, then I'm comfortable that this is really going to be the best structure. This is Dr. B., and thanks for watching.