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This is Dr. B. Let's do the Lewis structure for H2Se. On the periodic table, Hydrogen
is in group 1, so it has one valence electron, but we have two of them, so we're going to
multiply it by 2; plus Se is in group 6 or 16, it has 6 valence electrons. We have a
total of 8 valence electrons that we're going to work with here. So we know that Hydrogen
always goes on the outside of a Lewis structure, so we can put the Se right in the center,
and let's just put the Hydrogens on either side of that. OK, so we have that. Let's make
some chemical bonds. We have 8 valence electrons so we'll put two right here. So we've formed
chemical bonds between the Hydrogen and the Se. Also note, Hydrogen only needs two valence
electrons to have a full outer shell, so Hydrogen actually has its octet satisfied right now.
We have four more. Let's put them right here. And that means that Se has 8. So it's good.
Its outer shell is full, as well. So that's the Lewis structure for H2Se. Pretty simple.
This is Dr. B., and thanks for watching.