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Hi there.
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Lewis dot structures are used to show the valence electrons in each atom and how these valence electrons participate in the formation of the covalent bombs.
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So let's go ahead and start drawing the lewis structures for each of these molecules.
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Our first one is nf3.
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First thing i want to do is look at the periodic table.
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And i see that nitrogen is in group five of the periodic table.
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So nitrogen will have five valence electrons.
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Because group 5a, all of the elements, have five valence electrons.
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Fluorine is in group 7a.
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All of the halogens in group 7a have seven valence electrons.
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So each fluorine will have seven valence electrons.
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So now i can begin drawing my structure.
00:55
I'm going to start off with nitrogen, with its five valence electrons, would look something like that.
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Remember if we have a single element, it belongs in the center when we're doing these lewis structures, unless you're told otherwise.
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All right, so the fluorines then are going to surround this nitrogen and form a covalent bond with the nitrogen in each of these three positions.
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This fluorine will bring in seven dots or seven valence electrons.
01:33
This fluorine will bring in seven valence electrons, and this fluorine will bring in seven valence electrons.
01:44
So what we see is this structure has a single bond to each of the three fluorines, right? and each of the florins would, of course, have its dots around it.
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But the first picture here is the lewis dot structure showing all of the dots.
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The second one is more the structural formula.
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All right, so that would be, your lewis structure.
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All right, letter b, we have hbr.
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We're going to start off the same way with each of these problems.
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H is in group one of the periodic table, so it has one valence electron, and br is a halogen like fluorine.
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It will have seven.
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So we have hydrogen with its one valence electron, and bromine bringing in seven.
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The pair in between the hydrogen and the bromine indicate the shared pair of electrons that form the bond.
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All right, letters c.
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Sbr2...