Title : What Is A Network Solid
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What Is A Network Solid
everything we've been dealingwith so far has just been with the individual atoms,but atoms bond. or another way of saying itis, they stick together. because if atoms didn't sticktogether, then we'd all be essentially just a collectionof atoms and this video
What Is A Network Solid, wouldn't be being produced. so atoms stick together andthey form molecules. you take a bunch ofatoms together and they'll stick together.
and they'll form molecules. and then obviously moleculesstart building up and you get other structures. and if we started talking aboutorganic chemistry, you'd have a bunch of atoms, a lot ofcarbons and hydrogens and other things, fittingtogether and they'd be forming proteins. and then proteins would fittogether to form organic structures.
and you fit enough of thosetogether, and you'll eventually get someone recordinga youtube video. so this is whereit all starts. atoms bond. or they stick together. and the purpose of this videois to think about the different types of waysthat an atom can stick to another atom. so the first, and kind of themost powerful way-- or i think
of it as the most powerful way--is if you take an atom that really wants to give anelectron, and then you have another atom that really wantsto take an electron. right? and we've talked aboutthis before. an atom that wants to give anelectron wants to give it because it's trying to get intoa stable configuration in its outer shell. everyone wants to looklike a noble gas.
they're all envious of the noblegases, because the noble gases have eight electronsin their outer shell. so who wants to give? well if you look at the periodtable, the people who want to give really badly-- and we'vetalked about this a good bit-- are the alkali metals. these guys just really wantto offload an electron. and there are other peoplewho want to give them. but let's take theextreme example.
so these guys really wantto offload an electron. and who wants to takean electron? well, the halogens. we've talked about it. these guys love takingelectrons. they're not the only ones. but they have a very highelectronegativity. they really want totake electrons. so if you put these aroundeach other, what happens?
let's say, sodiumand chlorine. and let's say we wanted toflavor some of our food. so you have some sodium andyou have some chlorine. so sodium-- let me draw itsvalence shell-- sodium's valence shell looks like this. it's got one electron sittingthere that it would really just like to get rid of. and then chlorinelooks like this. it has seven valenceelectrons.
one, two, three, four,five, six, seven. so what happens is thisguy wants to escape. this little blue electron righthere really wants to escape the sodiumand essentially move into the chlorine. and obviously, it's notlike a one-for-one. you'd have billions andtrillions of these atoms rolling around, and theseelectrons jump off, then they go to one, then theyjump to another.
but for the sake of ourpurposes, let's say we just have these two atoms. and whatyou have is that that electron jumps off. and then if that electronjumps off, what happens to sodium? well then the sodiumhas no electrons in its valence shell. although it does. now its valence shell is onelower, but we can say it's
lost that one electronthat was out there. and now its atomic configurationwill look a lot like neon. sodium, you lose an electron,now it looks a lot like neon, at least its electronconfiguration. but now it has one fewerelectrons than protons. so now, it has a positivecharge. it was neutral back here. now it's positive.
and now, what does achlorine look like? and i'm kind of mixing upnotations, but that's really just to give you the idea. so chlorine before hadseven electrons. that electron had jumpedonto the chlorine. so now it's happy. it looks a lot like argon now. it has a completely filledvalence shell. and what's the charge now?
well in has one more. now it will have 18 electronsinstead of 17. so what is its charge now? it has 17 protons,18 electrons. it has a negative one charge. so i'll just put a negativeup there. it has a negative charge nowbecause it got that electron from sodium. so now these guys are bothhappy from an electron
configuration point of view. they both have these stablevalence shells. but they're attracted toeach other, right? coulomb forces. positive is attracted tonegative, negative is attracted to positive. and it can be very strong, thiselectrostatic force, so they stick to each other. and so this forceof attraction,
this is an ionic bond. so they essentiallywill form nacl. they're not sharing electrons. this guy wanted the electrons sobadly, and this guy wanted to give them away so badly, hejust handed the electron over. but then he says, oh, by theway, now that i handed you the electron, you're negative,i'm positive. i want to stick to you. and then we formed tablesalt and we're ready
to season our food. now that's the situation whereone guy really wants to offload an electron, one guyreally wants to take it. what happens in the situationwhere they're both not as extreme in their views inwhether or not they want to give or take electrons? so let's think of a fewother examples. the best example iselemental oxygen. let's see, elemental oxygen.
so this right hereis an ionic bond. not to jump back and forth,but i'm not sure if i just mentioned that. why is it calledan ionic bond? because we formed ions. when we donated the electronfrom sodium to chlorine, we formed an ion. the sodium, this became acation, because it's positive. and this became an anion,because it's negative.
and then they stuckto each other, so fair enough. now what happens, like i wasjust starting to say, if we have two elements that aren'tthat different in how much they want electrons. their electronegativityis very similar. and the best exampleof that is we had two of the same element. so let's say i had oxygen.
let's have one oxygen there. let's look at the periodic tableto make sure that we're not-- oxygen has six valenceelectrons, right? one, two, three, four, five,six valence electrons. it's 2s2, 2p4. so on the second shellit has six electrons. so oxygen has one, two, three,four, five, six. and then let's say wehave another oxygen. it has one, two, three, four,five, six electrons.
now both of these oxygenatoms would love to have eight electrons. they'd be stable. they could start pretendinglike they're a noble gas. but clearly, they don'thave eight electrons. and let's say in this, all theyhave around each other is other oxygen atoms. so whatthey can do is say, this oxygen goes to that oxygen, andsays, hey, why don't we share some electrons and thenwe can both pretend that we
have eight electrons. and this guy says,oh, sure enough. so we can just bringhim over here. and i'll just writehim in blue. oxygen doesn't necessarilyhave to change colors. i'm joking. so i'm just going to draw thisguy over on this side just so you recognize that this isdifferent than this guy. and then they sharethese electrons.
so they share these electrons. and we could do it bydrawing a line here. so they're sharing twopairs of electrons. so this guy right here, he hadsix electrons, but he can kind of pretend that he has thiselectron and that electron. so he has eight in hisvalence shell. and this guy, he's goingto do the same thing. he has one, two, three, four,five, six, but he also can kind of pretend thatthese guys are also
in his valence shell. so he's happy. and this notion, where you'reactually sharing electrons, where these electrons are goingto go and both electron probability distribution cloudsof both atoms. this is called a covalent bond. and this is typical whenyou're dealing with two elements that aren't verydifferent in terms of their electronegativity or theirdesire to attract electrons.
now, when we talked aboutionization energy, i think, we talked about when oxygenand water bond, right? and oxygen-- oxygen, we'vedrawn that-- is six. not oxygen. water. oxygen and hydrogen to formwater, and hydrogen looks something like this. you have a hydrogenatom there. they said, hey, why don'twe get together.
let's share some atoms. and thehydrogen atoms say, oh, ok, let's share some atoms.let me rewrite this oxygen like this, so it becomes clearthat we're sharing. so if i rewrite thisoxygen like this. i essentially split upone of these pairs. and these hydrogens come alongand they share one hydrogen there, one hydrogen there. this guy can pretend like hehas his first shell filled, because you can onlyput two there.
that's where the eightrule breaks down in the first shell. this guy can pretend, too. and now oxygen can pretend likehe's got eight electrons and everyone's happy. so this is also acovalent bond. another way we could havewritten this, and i think i did this in the lastvideo, i could have written it like this.
where the implication of thisline, each of these lines involve two electrons. these are equivalentstatements. but in this situation,oxygen is more electronegative than hydrogen. it wants to get the electronsmore than hydrogen. so in this situation, theelectrons are going to spend more time around oxygen thanthey will around hydrogen. so hydrogen will experience, iguess you could call it, a
partial positive charge on thisside of the molecule, while the oxygen side willexperience a partial negative. i'm going to draw itreal small, because it's a partial negative. this is called a polarcovalent bond. because it's still covalent. we're sharing electrons. but it's polar, because theelectrons are getting pulled to spend most of their timeat one side of the atom.
and since that is the case, themolecule as a whole, the collection of atoms, is goingto have polarity. one side of the molecule isgoing to be more negative than the other side, which will bemore positive because the electrons are spending moretime on that side. now the last bond we can talkabout, and i've touched on this a little bit, isthe metallic bond. i was in a metallic bond inhigh school, but anyway, that's a subject foranother video.
but with metals, you can'treally draw the electron structure there. but what happens with, let'ssay we have iron, right? and you have just a bunchof neutral iron atoms sitting around. and we established the onecommonality of metals, what makes something metallic or havemetallic characteristics is that they have a bunch ofelectrons in their outer orbital that they'revery giving.
they're very happy to share. so if you put a bunch of theseguys together, what happens is they share their electrons. so they all become positive. they're very communalthis way. the metallic atoms. and thentheir electrons kind of just form this sea out here. but they all share. e minus.
and because their electrons areall on the sea and they've kind of gotten this positivecharge, they're attracted to the sea that they've created. they're attracted to theirshared electron pool that all of the atoms have donated to. and this is essentially whatallows, well definitely, metals to be conductive, becauseyou have this pool of electrons that are veryeasy to move around. and also it's what makesthem malleable.
because even if youhave visually-- it's a little intuitive. there's nothing exact here. but you can kindof move these. you can imagine that this iskind of a big pudding of electrons or big glueof electrons. and you can move, you can bendthe rod or flatten the rod without having it breakor get brittle. while if you're talking aboutsalts that have a very strong
but rigid bond, if you were totry to bend a bar of salt, the bond will just be broken. there's no, kind of, squishyelectron mush that you can kind of bend aroundand play with. anyway, so those arethe three bonds. and hopefully that givesyou a little intuition. and this is super useful,because in the rest of chemistry, everything we do willessentially involve some combination of these bonds.
and we'll start talking aboutwhat these bonds mean in terms of the temperature at which theyboil, or the properties of the molecules themselves. anyway, see you inthe next video.
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