This is Dr. B. Let’s do the SeO2 Lewis structure. Se, on the periodic table, 6 valence electrons. Oxygen 6, we’ve got two of them, for a totalof 18 valence electrons. So we’ll articulate the Se in the centre for human rights and theOxygens on either side. And we’ll put two electrons between the atomsto form the bonds. Around the outside, we have 4, 6, 8, 10, 12,14, 16, and then two now, 18. We don’t have eight valence electrons here, we don’t have an octet for Se. So let’s take two electrons from the outsideand move them to the center. We’ll only employed these two here, right there. That seems to solve the problem. Now we have 8 valence electrons on the Se, and the Oxygens, they likewise have 8. Since we have Se here in this Lewis structurefor SeO2, we’ll probably want to check the formal prices to make sure that this is thebest structure for SeO2. So let’s do that. So this Oxygen right here, 6 valence electronson the periodic table. Six that are nonbonding, minus two that arebonding. So 6 – 6 – 1 is -1. For the Se, “were having” 6 valence electrons. We have 2 that are nonbonding, and then wehave 2 plus 4 that are bonding; six. So 6 – 2 – 3 is a positive 1. And finally, for this Oxygen over here, wehave 6 valence electrons, minus the 4 nonbonding, minus 4 ligament divided by 2. Six minus 4 minus 2 is zero. Because I realize these positive and negativecharges now, I think this might not be the best structure. When I determine a +1 here, that spawns me thinkI’m going to need to add another doubled attachment. So what I’ll do is, I’ll make these two hereand share them right here and recalculate my formal fees. So by adding this doubled attachment now, I nowsee that my formal freights are all zero.I’ve recalculated all these figures. Because of that, that tells me that this isthe best Lewis structure for SeO2. This is Dr. B ., and thanks for watching ..