Resonance Structures

This organic chemistry video tutorial provides a basic introduction into drawing resonance structures. It explains how to identify the major resonance contributor as well as the minor resonance contributor based on stability. Here are a few key concepts to keep in mind: Negative charges are stabilized by electronegative atoms. Neutral resonance structures are more stable than those with separation of charges. Tertiary carbocations are more stable than secondary and primary carbocations due to the inductive effect and hyperconjugation. Positive charges on carbon atoms are not stable due to the octet rule.
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i hate resonance its been watching hours of videos and i still dont get it

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[@LeylaGonzalezz]

how can you determine if it's primary, secondary, or tertiary?

[@chase1064]

A Carbon that is bonded to a single Carbon is primary. A Carbon that is bonded to two Carbons is secondary, and a carbon bonded to three is tertiary.

[@frohan007]

@@chase1064 specifically the carbon with the + charge i think

[@parultidkae4924]

it is depended on number of Carbon atoms it's surrounded by, if it is surrounded by 1-C atom, then it's primary, if it's surrounded by 2-C atoms then it's secondary and if it's surrounded by 3-C atoms then it's tertiary. thankyou have a beautiful day

[@noname6284]

What do you mean by common and uncommon resonance structures?

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How about the distance formula

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Due to breaking of aromaticity, the “primary” cationic structure is the major resonance contributor for the benzylic cation

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Hi, please I want to know if there is a formula for calculating how many resonance structures there could be in a given organic compound?

[@susantparida8369]

I'm sorry but there isn't.

[@angelic8580]

İsn't third one 3° carbin in 5.56 example?

[@4xking]

Why isn’t the bottom left at 6:05 tertiary?

[@TheThorRs]

2:47 why is the positive charge there? isn't there 4 bonds at that corner so the formal charge is 0? I'm assuming hydrogen is there

[@BrianErwin]

9:19 it's because 2s2 is closer to the nucleus than 2p2, and the more s-character, the more stable.. bigger atoms have more s-character

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hi, i know i'm late, but i really hope you see this. 'bigger atoms have more s-character'- is that because sulphur has 3s subshell while oxygen doesn't?

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Thank you

[@georgiconlon3811]

@9:37 oxygen is more electron neg than sulfur, so wouldn't the major contributor be the structure where the neg charge is on the oxygen, not sulfur...?

[@anikethpai9442]

Electronegativity is the tendency to attract shared pair of electrons to itself. Oxygen is an acceptor, not a contributor.

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Sulphur has larges size

[@winterflower4530]

I did a little more research behind this cuz I was thinking the same thing- it turns out that even though oxygen is more electronegative than sulfur, sulfur is much larger due to periodic trends. This large size allows it to spread out the negative charge better making it more STABLE. I think the key is to think which atom is more stable with the negative charge, not which atom is more likely to have the negative charge. In other words, when comparing elements in the SAME COLUMN (like O and S) look at its ability to stabilize the charge rather than just electronegativity - the greater the size of the atom, the more stable it will be with the charge. On the other hand, when looking at elements in the SAME ROW (ex. C vs O) you can just use your electronegativity trends cuz elements in the same row are roughly the same size- hope this helped :)

[@sumitraturi7791]

@@winterflower4530 yes

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[@specialrat1311]

Wait whats the difference between the primary, secondary, and tertiary?

[@reeddaley6617]

why couldn't the middle carbon gain a lone pair as part of resonance on the first molecule?

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9:35 can it be explained as fajan'd rule?

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[@cherissadover912]

How do you determine which is primary, secondary, or tertiary?

[@johannes7935]

i don't understand it either. Hope someone can help ^^

[@sanafakih3541]

count the number of substituents hung on the carbocation. 1 carbocations are bounded to one carbon, secondary to 2 and tertiary to 3

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[@hikarisan422]

Is it possible for an element in a resonance structure/form to have missing electrons but the rest of the elements have complete octets? I'm really really confused right now.

[@samuel34676]

I believe the carbon can be short

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Good

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Hope it went well, mine is tomorrow

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[@user-sk2du2gn3f]

i really don't understand 1°,2°,3°allelic carbocation😕

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[@justsomenightowl7220]

4:28 why doesn't the carbocation have a lone pair? i thought if there is not enough bonds, you would have a lone pair instead.

[@paysonkeown2960]

If it had a lone pair, it would have a negative formal charge.

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Blue colour is not brightly visible on screen

[@cja12345]

for 6:06 I got 4 resonance structures instead of 3, what did I do wrong😭

[@fmgtruefriend1335]

Identical structure

[@amycool64]

I don’t understand how the positive charges are jumping

[@joharahk4849]

The positive charges are jumping because as shown in the first example, the pi bond is becoming a single bond, basically “losing” a bond, giving it a positive charge since they’re essentially opposite (when a bond is lost it’s positive, when a bond is gained it’s negative). Hope i explained that accurately I'm learning too :)

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I don't understand the last exampleeeeeeeeee

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I've added more content to it. The full version was 31 minutes but now it's over an hour.

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