Resonance Structures - By The Organic Chemistry Tutor
Transcript
00:00 | in this lesson , we're going to talk about resonant | |
00:02 | structures . How can we draw the resonance structure for | |
00:10 | this ? A lilic , carbo , catomine . The | |
00:16 | first thing you should do is you should start the | |
00:20 | arrow from the double bond and it's going to flow | |
00:22 | towards the positive charge . Electrons will flow from a | |
00:26 | region of high negative charge towards the region of low | |
00:31 | negative charge or from negative to positive . And so | |
00:35 | the arrow , it's always going to go from the | |
00:38 | nuclear filic region of the molecule to the electra filic | |
00:41 | region of the molecule or ion in this case . | |
00:48 | So the resident structure for this , a little cat | |
00:50 | iron looks like this . The double bond is going | |
00:54 | to move to the right side and it's going to | |
00:57 | trade places with the positive charge . Since this carmen | |
01:01 | lost pi electrons , it now has a positive charge | |
01:07 | . This carbon lost a pie bon but regained it | |
01:10 | on the right side . So it doesn't have the | |
01:12 | positive charge now , which of these structures is the | |
01:18 | major resonance contributor ? Is it the one on the | |
01:21 | left or the one on the right ? Both of | |
01:25 | these are primary , a little carbon credits . So | |
01:29 | they're equally stable . So there is no major or | |
01:32 | minor residents contributor . In this example , the residents | |
01:37 | hybrid is actually a blend of these two resonance structures | |
01:42 | . So the pie bon is shared among the three | |
01:45 | carbon atoms and so is the positive charge . It's | |
01:50 | actually shared between These two carbon atoms . So they | |
01:57 | both carry a partial positive charge or you could say | |
02:00 | half Of a positive charge if he divided by two | |
02:11 | . Yeah , go ahead and try this problem . | |
02:18 | Yeah , draws many residents structures as you can and | |
02:22 | identify which one is the major residents contributor or which | |
02:27 | resident structure is the most stable . So the pie | |
02:32 | bon is going to move towards the carbon catomine and | |
02:36 | a positive charge is going to jump to places , | |
02:40 | or two carbon atoms towards the pipe on . So | |
02:44 | the positive charge will not be here . And so | |
02:49 | that's one resident structure that we can draw and we | |
02:52 | can draw another one . Mhm . So the plus | |
03:02 | charge is going to jump two carbons to the left | |
03:05 | . So it's that one that carbon . So in | |
03:09 | our first example we have a primary carbon canteen or | |
03:12 | a little caramel candy . And in the second example | |
03:15 | it's tertiary And in the 3rd 1 it's secondary . | |
03:20 | So therefore This one is the major residents contributor because | |
03:26 | a tertiary , a little carbon canteen is more stable | |
03:29 | than a primary or secondary . A little Karpel Captain | |
03:35 | . So recall that tertiary carbon headlines are more stable | |
03:38 | than secondary ones , which are more stable than primary | |
03:41 | ones . So if we compare , let's say , | |
03:47 | a tertiary carbon canteen with a primary caramel candy . | |
03:53 | It's important to understand that the method groups our electron | |
03:58 | donating groups relative to hydrogen . As a result , | |
04:03 | they can donate electron density to the carbon headline by | |
04:08 | means or through the sigma bond , which is known | |
04:11 | as the inductive effect or through the overlap of atomic | |
04:14 | orbit does , which is known as hyper congregation . | |
04:19 | And so a carbon headline with more method groups or | |
04:23 | more carbon atoms attached to it . It's going to | |
04:25 | be more stable Than one that has less . Now | |
04:31 | , let's move on to our next example . In | |
04:38 | this example , we have a Benz Ilic carbo Katie | |
04:42 | . It drives many resonance structures as possible and identify | |
04:45 | which structure is the major resonance contributor . So we | |
04:51 | can move the double bond towards the positive charge And | |
04:56 | just like before the positive charge is going to jump | |
04:58 | two carbons towards that to move on . And so | |
05:06 | we have this resident structure and then we can move | |
05:11 | this double bond here , Given us our 3rd resident | |
05:25 | structure , and then we can move this double bond | |
05:28 | and that location . So this is a primary carbon | |
05:42 | canteen or technically Ben's Ilic carbon copy . This one | |
05:47 | is secondary , this is secondary , and this is | |
05:50 | secondary . So this one is going to be the | |
05:53 | minor resonance contributor because it's the least stable . Now | |
05:58 | these are equally stable , so they form part of | |
06:03 | the major resonance contributor . Now , going back to | |
06:12 | the last problem , there's one more resonant structure that | |
06:15 | we can draw out of the common ones . There's | |
06:19 | a lot of uncommon resonant structures that we can draw | |
06:21 | . So just keep that amount . I prefer to | |
06:23 | focus on the common ones . So we could take | |
06:26 | this double bond , move it to the plus charge | |
06:30 | and we'll get this answer . It's similar to the | |
06:37 | original answer , but notice that the double bonds in | |
06:39 | the benzene ring have been shifted . Now let's move | |
06:44 | on to our next example , draw the resident structure | |
06:51 | of the benzene molecule . All we can do here | |
06:55 | is simply rotate the pie bahn's and so this is | |
07:05 | the resident structure for benzene . And that's all we | |
07:09 | can do here . Now what about for the car | |
07:18 | box , leyte island . What resonance structure can we | |
07:21 | draw ? Go ahead and try that problem . So | |
07:26 | what we can do is we can take a lump | |
07:28 | here from the negatively charged oxygen , use it to | |
07:32 | create a pie bon and then break this pylon . | |
07:39 | And so that's going to give us this particular structure | |
07:49 | . Now these two structures are identical and so they're | |
07:53 | equally stable . There is no major or minor resonant | |
07:57 | structure in this example . Now let's move on to | |
08:07 | the next example . So let's say if we have | |
08:11 | a sulfur atom instead of an auction item , identify | |
08:17 | the major resonance contributor in this case . So we | |
08:22 | could follow the same pattern in order to draw the | |
08:24 | resident structure . So the question is , is it | |
08:39 | better to put a negative charge on the oxygen atom | |
08:44 | or on the sulfur atom ? Now granted oxygen is | |
08:49 | more electro negative than sulfur . So that fact favors | |
08:53 | oxygen . However , sulfur is bigger than oxygen . | |
09:00 | And let's say if we have a small atom versus | |
09:03 | a larger atom , if we were to make each | |
09:07 | adamant ion by giving it a negative charge , which | |
09:11 | charges more stable a big guy on is more stable | |
09:16 | than a small line , assuming they have the same | |
09:18 | charge , because this has more volume where it can | |
09:23 | stabilize that negative charge . So this negative charges you | |
09:27 | can think of , It has been diluted over a | |
09:29 | larger surface area , this one here , it's more | |
09:33 | concentrated and so larger ions can are more stable than | |
09:39 | small ions . The bigger the atom the better it | |
09:42 | can stabilize a negative charge . So therefore it's better | |
09:46 | to put the negative charge on the sulfur atom and | |
09:48 | then on an oxygen atom . So this is going | |
09:51 | to be the major residents contributor on the left . | |
09:56 | This one here is the minor resonance contributor . Here's | |
10:01 | another example , let's say we have an alcohol but | |
10:07 | adjacent to the O . H . Group , there's | |
10:08 | a positive charge . Draw the resonant structure and identify | |
10:13 | the major business contributor . So we know the electrons | |
10:18 | will flow from a region of high negative charge towards | |
10:21 | the region of low negative charge . So the arrow | |
10:25 | is going to point towards like from the lone pair | |
10:28 | but towards the positive charge . And so we can | |
10:31 | use that lone pair to create a pi bond . | |
10:34 | And so now the oxygen has one lone pair as | |
10:37 | opposed to two because this carbon atom , it gained | |
10:40 | a pie bon , the positive charge on that carbon | |
10:44 | atom has been neutralized . The oxygen lost the lump | |
10:47 | here . So now it has a positive formal charge | |
10:51 | . So is it better to put a positive charge | |
10:55 | on an oxygen atom or on a carbon atom ? | |
11:00 | Now oxygen is more electoral negative than carbon . And | |
11:04 | so as a result it's better to put the positive | |
11:07 | charge on a carbon atom . However , it turns | |
11:10 | out that the structure on the left is the major | |
11:13 | residence contributor and the one on the I mean this | |
11:17 | is the right side , not the left side , | |
11:18 | the one on the left is the minor resident contributor | |
11:23 | . So why is this the major resident contributor ? | |
11:26 | If we have a positive charge on an election negative | |
11:29 | atom , when we know it's better to put a | |
11:31 | positive charge on a more electoral positive atoms like carbon | |
11:37 | . The answer has to do with the arctic rule | |
11:41 | . So if you look at the structure on the | |
11:43 | left , the carbon atom , it doesn't obey the | |
11:46 | oxide rule , it doesn't have eight electrons . It | |
11:49 | has three bonds , no lone pairs , so it | |
11:51 | has six electrons . If we look on the right | |
11:56 | side , this carbon atom has four bonds . So | |
11:59 | it has eight electrons . It satisfies the octet rule | |
12:04 | . The oxygen also satisfies the octet rule . It | |
12:07 | has three bonds that six electrons plus a lump here | |
12:10 | . So it has eight electrons on the left side | |
12:15 | . The oxygen satisfies the octet rule has one bond | |
12:18 | plus the O . H . Bond . That's two | |
12:20 | that's four electrons plus two lone pairs . So it | |
12:23 | has eight . So the reason why this is the | |
12:26 | minor resonance contributor is because carbon does not obey the | |
12:30 | octet rule when it has a positive charge . And | |
12:34 | so that's why you'll see that when dealing with resident | |
12:37 | structures , it's better to put the positive charge on | |
12:40 | the oxygen atom as opposed to the carbon atom , | |
12:44 | to satisfy the octet rule . So electro negativity is | |
12:48 | not a priority in this example . |
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