How to Draw Lewis Structures, The Octet Rule and Exceptions | Study Chemistry With Us
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- Опубліковано 24 бер 2020
- I'll cover how to properly draw lewis structures of regular molecules and lewis structures of ions. We will also go over what the octet rule is and all the exceptions that go along with this. Plus we will talk about the valence electrons you will need to memorize for your next chemistry exam.
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💁♀️ HI I'M MELISSA MARIBEL
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Hello MM, ...what happens at the sides of a graphene layer related to bonding?
Thanks ❤
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How's it going? The good points you got going are your stamina and desire to get it done. You have chosen a noble path that will only make you a better person. Keep plugging away. Don't give up trying. Many would give up but I can tell you are made of much stronger fabric. Be productive!!!!
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Never give up! I'm so proud of you, that's some great dedication!
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That is awesome! Congrats 🎉
Damn yall r learning this in college?
Your doing this in college?
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@@KH-ks7si you realize this topic comes back in general chemistry in college. in my first year, I've revisited so many things I've learned in high school in more depth and difficulty. you need to do it again in college just to get prereqs out of the way. you can start doing ochem and other things after you've passed gen chem.
Seriously thank you so much for these videos, I have been basically teaching myself Chem and I have learned more from your videos in one day then the entire month and a half I have been in school! Thank you!
WHAT WHAT WHAT THAT MAKES SO MUCH SENSE NOW THANK YOU SO MUCH!!!!!!!!
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ikr thats why melissa maribel is a total lifesaver
oh this was totally great ! It helps me a lot to understand more about Lewis Structure. Thankyou for this.
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Professor Melissa, thank you so much. Huge huge help. I was struggling understanding the exceptions with B and Be, also about the lone pairs and your student asked the precise question in my head (we already have to respect the total number of valence electrons involved and not go over them). Thanks a million!
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The best video on lewis structures I've seen! thank you!!
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Thank you for this Melissa :D
You’re very welcome 😊
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Thank you so much Clara!
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Thank you so much for this!!
You’re very welcome!
your teaching style is amazing
Wow, I wish utube was around whilst I was at school. Just watched your video and got the hang of how bond's are worked out. One science teacher just threw metal rods at us lol
I did go on to manufacture fireworks, but wish I could have been able to write up what I was actually doing and why I got the beautiful colors.
Cheers, from an Australian pyro
Thank you Melissa for this video, it was very helpful. Please may l request that you make a video on mole concept, it will go a long way. Thank you so much.
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Thank you so much!
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For the CO2 example, why does oxygen begin with 7 valance electrons instead of 6? There are 3 lone pairs but still a bond between an extra valance electron with the carbon. 🤔
I wondered the same thing.
THANK YOU VERY MUCH❤️❤️
love it thank you
Thank you!!
Thank you thank you thank you!!!!
Hi Melissa! First off thank you for all your content - It's helping me a ton in my 8week summer session of college gen chem.
I have a question about the final two structures.
When I drew my structure for ClO4-, I tended to want to draw my Cl atom with double bonds for 3 out of 4 of the Oxygen atoms and a single bond to the 4th Oxygen atom. The single electron hanging around by itself on the outside of Oxygen kind of made sense in my mind because the whole molecule in the end was supposed to be negatively charged. My main focus was making sure that the central Cl atom had 7 electrons attached to it.
I'm not understanding how its okay to leave a central Cl with only 4 electrons when it's supposed to have 7.
I hope that wasn't too confusing of an explanation. Is it like a law of physics no-no to have a single electron hanging out by itself on an exterior element or something?
Thanks for any insight!
Thanks!!
Thank you so much
THANK YOU.
Thank you so much ma'am...
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THANK YOU, GRABE
in 19:47 can we keep, one lone pair to carbon as well as to oxygen and keep one bond pair of hydrogen to oxygen
THANK YOU
MS.Melissa I also a chemistry tuition teacher teaching ISC 11th grade students . Your video on formal charges is excellent and very clear . It helped a lot to handle my students. Thanks a lot . Can i send my doubts. Isit possible for you to clarify. Thank you
Really helpful video! Quick question: for the ClO4- ion, shouldn't there be 3 double bonds between the Cl and O, since that would be the most appropriate in terms of formal charges?
thanks😊
how do you know how many central atoms to use? will there ever be a case where there are more than two atoms in the center? THANK YOU for these videos they are saving me right now!!
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hi melissa do you have the instructional notes where you check things off for these?
I love you thank you
For the lewis structure of IOF5, why is I in the center of the lewis structure, when O is more electronegative than I? O is much closer to F than I on the periodic table. Thank you,
Thank you Melissa for your amazing dedication. Question: why does Oxygen consistently have 3 lone pairs if I t has 6 valence electrons and is bonded to an element?
Same question! Like if all 6 electrons are hanging on the outside, what's keeping it attached to the central - that's what tripped me up at least.
@@mirandabeaudry5337 EXACTLY!!
learned more in 36 mins than a whole year class someone give this mami a mf raise
I have a chem final tomorrow... you saved my grade
Hi, does it matter (in CH3COH) which lone pair electrons are moved to form teh double bond?
thanks