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All right, guys.
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We're doing question number 90 of chapter 9 in chemistry, central science.
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So we have this chart right here, where we have our molecules, electron domain geometry, the hybridization of our central atom, and whether or not are our molecules in dipole.
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So it wants to fill the blank space in the following chart.
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If the molecule comes blank, find an example that fills the conditions of the rest of the row.
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So let's start with co2.
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I'm going to draw the structure of co2.
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I'm going to draw the structure of our molecules over here so we can better understand it.
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So this is our co.
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That's the lewis structure.
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So you have two electron domains here and here.
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And then you have no electron domains, our central item.
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So our electron, so since we have two electron domains, our electron domain geometry is linear.
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And since we're only forming two bonds, we're going to have sp hybridization.
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And generally you can know what hybridization is based on the number of bonds you're forming.
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If you're forming two, then it's sp.
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If you're forming three, it's sp2, and you're forming four, it's sp3.
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That's generally how you can do it.
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And we can see from our dipole moments, we have a dipole moment here and a dipole moment here.
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So the two dipolements cancel out.
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So there is no dipole moment, or rather no net dipole moment.
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So we have a dipole moment.
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We have sp3 hybridization.
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If that's true, then our electron domain geometry is going to be tetrahedral.
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And example of that would be an h3.
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So this would be our nh3 structure.
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Since it's surrounded by four electron domains, it's tetrahedral, tectahedral electron domain geometry, and also it has an sp3 hybridization because it's surrounded by those four electron domains.
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Now, no net dipole moment, it's still going to, and still sp3 hybridization, so it's going to be tetrahedral, but instead of a polar one molecule, we're going to get non -polar.
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So we get ch4.
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So ch4.
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Or there's, you have four electron domains surrounding it, so it has tetrahedral geometry for its electron domains.
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And no lone pairs.
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That means that on central atom, all the bonds are equivalent.
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So that means this is a non -polar atom, non -polar molecule.
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Now, for trigonal planer, we can choose any kind of trigon player dipole moments.
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That means we're going to choose a trigonal plane.
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And so that means we're going to choose a molecule with it looks like ammonia but has no lone pairs on the centrum so in this case we're choosing bh3 since there are three electron domains you have sp2 hybridization so for sf4 so let's draw our our sf4 i'll draw it over here so there are four fluorings and six bit and there's one sulfur so that's going to create 20 valence electrons from the flooring and then and 34 six valence electrons from your sulfur which creates 34 in total so let's see how many electrons we have so far one two three four five six seven one two three four six seven eight nine ten eleven twelve thirteen fourteen fifteen sixteen so that's thirty two that means we have one lone pair here.
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So that means our electron domain geometry is going to be trigonal by pure middle.
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I'm going to put this part down slightly.
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Triginal by pure middle.
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We have us...