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3) Draw Lewis dot structures (showing @l bonding and lone electron pairs) of the reactant semicarbazide and product thiatriazole_ What molecule is most likely to be...

Question

3) Draw Lewis dot structures (showing @l bonding and lone electron pairs) of the reactant semicarbazide and product thiatriazole_ What molecule is most likely to be liberated when the thiatriazole undergoes decomposition? Use the dot structure of the thiatriazole to explain why this IS sO showing specifically which bonds are broken in the decomposition Why isn"t the same molecule released by the semicarbazide (at least at that temperature)? Use the dot structure of the semicarbazide t0 expl

3) Draw Lewis dot structures (showing @l bonding and lone electron pairs) of the reactant semicarbazide and product thiatriazole_ What molecule is most likely to be liberated when the thiatriazole undergoes decomposition? Use the dot structure of the thiatriazole to explain why this IS sO showing specifically which bonds are broken in the decomposition Why isn"t the same molecule released by the semicarbazide (at least at that temperature)? Use the dot structure of the semicarbazide t0 explain your answer: [



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Explain why triphenylene resembles benzene in that it does not undergo addition reactions with Br$_2$, but phenanthrene reacts with Br$_2$ to yield the addition product drawn. (Hint: Draw resonance structures for both triphenylene and phenanthrene, and use them to determine how delocalized each $\pi$ bond is.)

He wants us to draw the structures for another three and people have three. So for eight here, let's say it's an L F three. It is going to have a Louis structure of nitrogen with our flooring is on the periphery. And this is gonna have a charge while all surgeons get me in the bottom while in peel F three solicit. That's beat people F three. Um, we have a phosphorous double wanted to an oxygen with our Florian's on the periphery. So the difference between the two is the presence of this double bond here and the Ionic bonds between nitrogen oxygen in this particular case.

He would be drug The levee Sick Tractor Off the reaction Ignition website soldier state Less carbon dioxide. You see a state. You can be your product M g C or tree. So the visit picture of destruction is N g o global bond or MG having through the groans and dividend shin and oxygen having six electrons in the violence here. Plus, we have carbon dioxide, double bond level boned for here. This this double bones wouldn't shift here. And this Feel a take on good Benidorm. So the products formed like mad nation less too. And behave Gurban level Montel Her bendable burned all and year oxygen in here Oxygen tu minus can behave. Then they get you judge militia here like this? No, we identified the Navy's Is it in Navy space? This is ladies base and this is ladies Navies Isett Because ladies base gonna be a rough electron in lady sees it except pair of electrons

Hi. Are you ready to draw some Lewis structures and then use those Lewis structures to help us identify the Lewis acid and the Lewis base? In a reaction, Let's get started. I want to start off with boric acid. So drawing the Louis structure for boric acid. Boron has three valence electrons. Each oxygen brings in six, and each hydrogen will bring in one giving us a Louis structure that looks like this for the boric acid. The boric acid is reacting with water and according to the balanced equation, there actually to water molecules. So I want to draw the Louis structure. For each of those, there's one water and our second water, right. If we recall the octet rule tells us that elements, most elements, they're definitely exceptions. But most elements would like to have eight valence electrons. That is the definition of the octet rule. So when we look at Boron right now, boron on Lee has six valence electrons. When these substances react, the bond in one of our water molecules is going to break between the oxygen and the hydrogen, giving us an H plus and an O. H minus. This h minus that lone pair of electrons from where the bond broke are going to be donated and attached to the boron in this empty position. Since the O. H is donating a lone pair of electrons, it is known as the Louis Space Louis basis. Donate electrons, so just be identified as our base. The boric acid, on the other hand, is accepting the lone pair of electrons, so it is known as the Lewis acid. So we have a bond breaking in the water between the hydroxide and the hydrogen ion, and that is being bonded to the bar. Um, so then you might ask, what happens to this other hydrogen, this proton, this long proton? That's by itself. It, in turn, is going to attach to the lone pair on the other water molecule. When it does this, we can see that the water is still acting as a lone pair donor, so the water is still acting as the Lewis base, so each of these water molecules acted as a Lewis base, donating alone pair of electrons. The bore the boric acid, acted as lewis acid and the H plus ion. It was also a lone pair, except er so it acted as an acid. Let's see what the end result of this is. So on our product side swing, hammer, boron. But now our boron is going to have a full octet as it's gonna be surrounded by four oxygen's that are then attached to correspondingly four hydrogen. Okay, alright. And our other product is going to be and this is going to have a negative charge back up a second year that's gonna have a negative charge or other product is gonna be a hydro me. Um, I on or h 30 plus. All right, So there's your Lewis structures and how you use those Lewis structures to identify your Lewis acid and your Lewis base. Thanks for watching. I hope you found this helpful. Have a great day.

No one to draw. The electron got structures for each of the following molecules indicating any unshared electron pairs. And they also want us to determine how likely each of these will be and acting as a Lewis acid or a Lewis base. Right? So it's going to start with aluminum try bromide. And so, if you were to go through the whole process, you should first start with aluminum in the centre, Brahmins on the outside. And then the bro means we're going tohave three pairs of lone pairs each. And if you were to count up, how many electrons we have here you was he would match with what we've normally have. And now the Brody's really want to keep electrons for themselves. So these probably aren't going to do anything. So we need to focus on this aluminum here. Well, it has the electrons to donate, so it would probably want to accept electrons. And so remember Louis basis donate electrons and lewis acids, except electrons. So in this case, this is wanting to accept electrons, and it makes sense, cause aluminum has a lot of metal properties, So this would be a Lewis assets, since it wants to accept electrons. Now, let's drawl out this amino over here in part beat. So we have a carbon, a carbon and nitrogen. So this carbon here would have 300 years. The next one has to then this metre, gin here as too. And that is also going to have a little pair. Now, the carbons don't seem like they're gonna really want to do anything or the hydrogen. But notice Over here. This nitrogen has this lone pair that it may want to do it. And we know a means our nitrogen is normally pretty basic. So it could be very easy for it asked to donate to this. Or we could just use this to attack something else. So it's more likely that this is going to be a Lewis base. Because remember, all Brossel Lowry acid spaces are going to be the equivalent acid base for Louis. So that b H three over here? Well, this is going to look just like what we have in part a boy. Differences in the center we have boron. And then on the outside we have our hydrogen. No, poor odd here. Does it have any electrons to donate the hydrogen is probably aren't going to do anything. So this seems like it would be very likely to accept electrons to form another bond. So this is going to be a Lewis acid since it is accepting electrons right now over here for Hydrofluoric acid that's going toe look like this here and now if they're just talking purely like no kind of reactions outside of anything, it may be tempting toe. Want to call this a Lewis base. But since this is a Brossel Lowry acid, even though it's a very weak one, we would also call this a lewis acid just because when it donates that hydrogen, it would accept electrons from that bond for next one. So for this sulfur compound that we'd have three hydrogen is coming out from each of our carbons, and then remember, sulphur is in the same column as oxygen, so we're gonna have two lone pairs there now. The hydrogen czart really likely to do anything, especially since the carbons there are really, uh, weak acids or the Hodgins on those carbon is going to be extremely weak. So the only thing that we may actually have is one of these lone pairs on the sulfur, babe, donate to something. So this is going to be a Lewis base. It looks like. And then lastly, or titanium tetrachloride, This is gonna be t i CEO seo seal CEO. And if you were toe, go through and check this would be titanium four, uh, using the oxidation number because the chlorine is going to have toe have negative once it would be negative for So that would be titanium for that's why would have it like this year. And then these quarantines are going toe have three, well impairs each. And so now this falls into the same case as a and see where, especially a because we have these Hey, lights where they really want to keep their electrons because they're Electra negative. And titanium doesn't have any lone pairs surround again. So then that would mean the only thing we could do is have something, attack it and donate electrons to it so that titanium or titanium tetrachloride is going to be a Lewis acid, since it would want to accept ElectroComps


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