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Aww thank you, so glad I could help!

OUCH! It's vital that you get ahead as much as possible and go in each day caught up (and reading ahead) so that you can optimize every moment of your class time.

Thanks for the recommendation. I post free videos as I have time and am always looking for suggestions.

You are so welcome!

You can find what I have so far on my free syllabus guide: leah4sci.com/syllabus

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I'm so happy to be a help for you during such a tough time. Sending hugs.

Happy to throw you a line!

You're welcome, glad you love them!

Wow, thanks so much! Glad I can help

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Awesome, thank you! I'm so glad I was able to help you refresh what you had learned!

You are so very welcome and yes, I'm happy to be here with you on your journey. Check out more of my free resources here: leah4sci.com/syllabus

Thank you so very much, I appreciate it!

I'm sorry to hear this topic had you in tears, but I'm glad I was able to help clear things up for you!

Thanks, glad you liked it!

Good question! First, the lone pair electrons are more free to move and attack than electrons that are tied into a pi bond. Second, if the pi bond were to attack, we would be left with either an oxygen or carbon atom that does not follow the octet rule. Oxygen and carbon are both too small to be exceptions to the octet rule.

@@Leah4sci I agree with point 1. But when you say, 'if the pi bond were to attack, we would be left with either an oxygen or carbon atom that does not follow the octet rule,' do you mean that if the pi bond attacks, it could either create a carbocation or a CH-O+ (I'm not sure how to pronounce a positively charged oxygen)? I don't think these two cases violate the octet rule because they result in oxygen and carbon having empty orbitals, and there are many reaction mechanisms where carbocations are formed, such as in SN1 reactions. However, I've never seen a positively charged oxygen because the C=O bond is more polarized towards oxygen, so only oxygen forms bonds with pi electrons with electrophiles like H+. Yesterday, I asked my teacher why he wrote that the pi bond attacks H+. His answer was, "when you become proficient in reaction mechanisms, you can omit some steps in the mechanism. If you want to write that the lone pair on oxygen attacks H+ and then the pi electrons become the lone pair on oxygen, that's also correct."

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I think you've spotted the error in this video! Nice job. :) Notice the error is mentioned in the title of the video as well as the description. My note is as follows: Note: The molecule at 3:00 is named incorrectly and should be numbered in the opposite direction. The correct name for this structure would be 6-methyl-2-heptyne.

Thank you, but you keep it ;)

For real

Glad you liked it!

I'm having a hard time finding the audio error that you mention. At 8:46, I say that we have the pi bond between carbon 1 and 2. If I mention it otherwise for that example at any point in the video, please disregard. :)

The sp2 carbon atom on the screen at 10:00 is labeled correctly. It has 3 bonds around it (1 double bond and 2 single bonds) and 0 lone pairs. That makes it an sp2 hybridized carbon. For an in depth look at sp3, sp2 and sp hybridization, make sure to view my tutorial on my website at Leah4sci.com/Hybrid

No, secbutyl and isobutyl are two different substituents. You can see them drawn separately on the screen around 7:00. Each group has a different branching pattern, and therefore should be named differently. For more Naming practice and resources, make sure to see my Naming tutorial series and cheat sheet at Leah4sci.com/Naming

Great question. Doing so recreates what we see in Resonance Structure #1, where we have a negatively charged oxygen with alternating pi bonds throughout the ring. The pi bonds will simply be shifted one space over from where they started originally. Most professors will consider this the same molecule as #1. But drawing it does not necessarily make you wrong either!

Glad it was helpful!

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Yes, and sulfur is an exception to the octet rule in this case. It is a large enough atom (with available d orbitals) that it can hold up to 12 electrons around it.

Yes! That method works fine too. Use what works for you!

So happy that I was able to help you!

Thank you!

Thank you!

So happy to help fill the gap and it's great that overall you have a good professor.

Hope your class is going well

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Br is an electronegative atom, when the pi bond attacks, the carbon no longer holding the pi bond is now left deficient and therefor positive. The electronegative Br is attracted to it and therefor attacks

@@Leah4sci Thank you..

Thanks!

So glad I could help!

So glad to help!