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Everything we've been dealing with so far has just been with

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the individual atoms, but atoms bond.

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Or another way of saying it is, they stick together.

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Because if atoms didn't stick together, then we'd all be

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essentially just a collection of atoms and this video

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wouldn't be being produced.

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So atoms stick together and they form molecules.

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You take a bunch of atoms together and

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they'll stick together.

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And they'll form molecules.

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And then obviously molecules start building up and you get

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other structures.

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And if we started talking about organic chemistry, you'd

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have a bunch of atoms, a lot of carbons and hydrogens and

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other things, fitting together and

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they'd be forming proteins.

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And then proteins would fit together to form organic

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structures.

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And you fit enough of those together, and you'll

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eventually get someone recording a YouTube video.

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So this is where it all starts.

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Atoms bond.

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Or they stick together.

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And the purpose of this video is to think about the

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different types of ways that an atom can

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stick to another atom.

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So the first, and kind of the most powerful way-- or I think

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of it as the most powerful way-- is if you take an atom

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that really wants to give an electron, and then you have

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another atom that really wants to take an electron.

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Right?

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And we've talked about this before.

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An atom that wants to give an electron wants to give it

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because it's trying to get into a stable configuration in

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its outer shell.

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Everyone wants to look like a noble gas.

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They're all envious of the noble gases, because the noble

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gases have eight electrons in their outer shell.

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So who wants to give?

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Well if you look at the period table, the people who want to

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give really badly-- and we've talked about this a good bit--

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are the alkali metals.

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These guys just really want to offload an electron.

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And there are other people who want to give them.

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But let's take the extreme example.

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So these guys really want to offload an electron.

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And who wants to take an electron?

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Well, the halogens.

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We've talked about it.

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These guys love taking electrons.

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They're not the only ones.

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But they have a very high electronegativity.

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They really want to take electrons.

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So if you put these around each other, what happens?

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Let's say, sodium and chlorine.

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And let's say we wanted to flavor some of our food.

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So you have some sodium and you have some chlorine.

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So sodium-- let me draw its valence shell-- sodium's

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valence shell looks like this.

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It's got one electron sitting there that it would really

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just like to get rid of.

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And then chlorine looks like this.

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It has seven valence electrons.

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One, two, three, four, five, six, seven.

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So what happens is this guy wants to escape.

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This little blue electron right here really wants to

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escape the sodium and essentially

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move into the chlorine.

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And obviously, it's not like a one-for-one.

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You'd have billions and trillions of these atoms

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rolling around, and these electrons jump off, then they

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go to one, then they jump to another.

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But for the sake of our purposes, let's say we just

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have these two atoms. And what you have is that that

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electron jumps off.

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And then if that electron jumps off,

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what happens to sodium?

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Well then the sodium has no electrons

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in its valence shell.

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Although it does.

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Now its valence shell is one lower, but we can say it's

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lost that one electron that was out there.

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And now its atomic configuration will

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look a lot like neon.

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Right?

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Sodium, you lose an electron, now it looks a lot like neon,

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at least its electron configuration.

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But now it has one fewer electrons than protons.

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So now, it has a positive charge.

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It was neutral back here.

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Right?

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Now it's positive.

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And now, what does a chlorine look like?

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And I'm kind of mixing up notations, but that's really

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just to give you the idea.

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So chlorine before had seven electrons.

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One, two, three, four, five, six, seven.

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That electron had jumped onto the chlorine.

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So now it's happy.

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It looks a lot like argon now.

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It has a completely filled valence shell.

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And what's the charge now?

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Well in has one more.

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Now it will have 18 electrons instead of 17.

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Right?

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So what is its charge now?

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It has 17 protons, 18 electrons.

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It has a negative one charge.

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So I'll just put a negative up there.

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It has a negative charge now because it got that electron

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from sodium.

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So now these guys are both happy from an electron

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configuration point of view.

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They both have these stable valence shells.

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But they're attracted to each other, right?

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Coulomb forces.

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Positive is attracted to negative, negative is

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attracted to positive.

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And it can be very strong, this electrostatic force, so

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they stick to each other.

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And so this force of attraction,

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this is an ionic bond.

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So they essentially will form NaCl.

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They're not sharing electrons.

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This guy wanted the electrons so badly, and this guy wanted

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to give them away so badly, he just handed the electron over.

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But then he says, oh, by the way, now that I handed you the

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electron, you're negative, I'm positive.

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I want to stick to you.

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And then we formed table salt and we're ready

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to season our food.

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Now that's the situation where one guy really wants to

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offload an electron, one guy really wants to take it.

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What happens in the situation where they're both not as

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extreme in their views in whether or not they want to

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give or take electrons?

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So let's think of a few other examples.

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The best example is elemental oxygen.

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Right?

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Let's see, elemental oxygen.

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So this right here is an ionic bond.

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Not to jump back and forth, but I'm not sure if I just

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mentioned that.

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Why is it called an ionic bond?

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Because we formed ions.

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When we donated the electron from sodium to chlorine, we

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formed an ion.

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The sodium, this became a cation, because it's positive.

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And this became an anion, because it's negative.

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And then they stuck to each other, so

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this is an ionic bond.

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Fair enough.

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Now what happens, like I was just starting to say, if we

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have two elements that aren't that different in how much

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they want electrons.

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Their electronegativity is very similar.

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And the best example of that is we had

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two of the same element.

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So let's say I had oxygen.

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Let's have one oxygen there.

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Let's look at the periodic table to make sure that we're

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not-- oxygen has six valence electrons, right?

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One, two, three, four, five, six valence electrons.

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Right?

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It's 2s2, 2p4.

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So on the second shell it has six electrons.

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So oxygen has one, two, three, four, five, six.

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And then let's say we have another oxygen.

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It has one, two, three, four, five, six electrons.

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Now both of these oxygen atoms would love

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to have eight electrons.

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They'd be stable.

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They could start pretending like they're a noble gas.

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But clearly, they don't have eight electrons.

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And let's say in this, all they have around each other is

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other oxygen atoms. So what they can do is say, this

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oxygen goes to that oxygen, and says, hey, why don't we

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share some electrons and then we can both pretend that we

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have eight electrons.

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And this guy says, oh, sure enough.

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So we can just bring him over here.

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And I'll just write him in blue.

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Oxygen doesn't necessarily have to change colors.

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I'm joking.

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So I'm just going to draw this guy over on this side just so

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you recognize that this is different than this guy.

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And then they share these electrons.

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So they share these electrons.

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And we could do it by drawing a line here.

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So they're sharing two pairs of electrons.

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So this guy right here, he had six electrons, but he can kind

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of pretend that he has this electron and that electron.

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So he has eight in his valence shell.

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And this guy, he's going to do the same thing.

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He has one, two, three, four, five, six, but he also can

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kind of pretend that these guys are also

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in his valence shell.

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So he's happy.

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And this notion, where you're actually sharing electrons,

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where these electrons are going to go and both electron

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probability distribution clouds of both atoms. This is

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called a covalent bond.

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And this is typical when you're dealing with two

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elements that aren't very different in terms of their

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electronegativity or their desire to attract electrons.

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Now, when we talked about ionization energy, I think, we

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talked about when oxygen and water bond, right?

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And oxygen-- oxygen, we've drawn that-- is six.

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Not oxygen.

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Water.

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Oxygen and hydrogen to form water, and hydrogen looks

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something like this.

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Right?

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You have a hydrogen atom there.

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You have a hydrogen atom there.

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They said, hey, why don't we get together.

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Let's share some atoms. And the hydrogen atoms say, oh,

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OK, let's share some atoms. Let me rewrite this oxygen

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like this, so it becomes clear that we're sharing.

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So if I rewrite this oxygen like this.

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I essentially split up one of these pairs.

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And these hydrogens come along and they share one hydrogen

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there, one hydrogen there.

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This guy can pretend like he has his first shell filled,

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because you can only put two there.

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That's where the eight rule breaks down

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in the first shell.

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This guy can pretend, too.

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And now oxygen can pretend like he's got eight electrons

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in his valence shell.

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And everyone's happy.

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So this is also a covalent bond.

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Another way we could have written this, and I think I

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did this in the last video, I could have

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written it like this.

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Where the implication of this line, each of these lines

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involve two electrons.

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These are equivalent statements.

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But in this situation, oxygen is more

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electronegative than hydrogen.

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It wants to get the electrons more than hydrogen.

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So in this situation, the electrons are going to spend

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more time around oxygen than they will around hydrogen.

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So hydrogen will experience, I guess you could call it, a

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partial positive charge on this side of the molecule,

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while the oxygen side will experience a partial negative.

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I'm going to draw it real small, because

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it's a partial negative.

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This is called a polar covalent bond.

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Because it's still covalent.

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We're sharing electrons.

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But it's polar, because the electrons are getting pulled

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to spend most of their time at one side of the atom.

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And since that is the case, the molecule as a whole, the

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collection of atoms, is going to have polarity.

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One side of the molecule is going to be more negative than

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the other side, which will be more positive because the

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electrons are spending more time on that side.

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Now the last bond we can talk about, and I've touched on

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this a little bit, is the metallic bond.

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I was in a metallic bond in high school, but anyway,

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that's a subject for another video.

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But with metals, you can't really draw the electron

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structure there.

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But what happens with, let's say we have iron, right?

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And you have just a bunch of neutral iron

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atoms sitting around.

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And we established the one commonality of metals, what

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makes something metallic or have metallic characteristics

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is that they have a bunch of electrons in their outer

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orbital that they're very giving.

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They're very happy to share.

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So if you put a bunch of these guys together, what happens is

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they share their electrons.

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So they all become positive.

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They're very communal this way.

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The metallic atoms. And then their electrons kind of just

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form this sea out here.

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But they all share.

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E minus.

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E minus.

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E minus.

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E minus.

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And because their electrons are all on the sea and they've

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kind of gotten this positive charge, they're attracted to

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the sea that they've created.

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They're attracted to their shared electron pool that all

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of the atoms have donated to.

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And this is essentially what allows, well definitely,

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metals to be conductive, because you have this pool of

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electrons that are very easy to move around.

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And also it's what makes them malleable.

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Because even if you have visually--

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it's a little intuitive.

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There's nothing exact here.

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But you can kind of move these.

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You can imagine that this is kind of a big pudding of

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electrons or big glue of electrons.

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And you can move, you can bend the rod or flatten the rod

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without having it break or get brittle.

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While if you're talking about salts that have a very strong

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but rigid bond, if you were to try to bend a bar of salt, the

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bond will just be broken.

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There's no, kind of, squishy electron mush that you can

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kind of bend around and play with.

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Anyway, so those are the three bonds.

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And hopefully that gives you a little intuition.

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And this is super useful, because in the rest of

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chemistry, everything we do will essentially involve some

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combination of these bonds.

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And we'll start talking about what these bonds mean in terms

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of the temperature at which they boil, or the properties

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of the molecules themselves.

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Anyway, see you in the next video.

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