Thank you so much! All of my teachers just threw big molecules at us and told us to draw Lewis Structures without even really teaching us how to do it.
I cannot begin to explain how much you have helped me! I have been struggling with Lewis structures for years now. You have really saved my Chem grade.
I really hope you read this comment because that table you drew in this video just cleared so much confusion and connected all the dots. I am not very good with words but I hope you know this video helped me so much and I have the video paused right now just so I could type up this comment. I almost never comment on videos but you deserve it. Thank you for making the world a better place.
Don't know if you still need an answer but everything you need is a periodic table Learn how to read it and it will be a shortcut to understanding all about bonds and electron configuration For example O is in 16th group so it has 6 valence electrons (electrons in valence shell), but he wants to have 8 (octet rule) So he needs 2 more and he will get them with bonds (aka makes 2 bonds) Every covalent bond is in fact two electrons shared between the atoms so in order to get 2 electrons from the other atom he has to share his own 2 with that atom. When he shares his 2 atoms (out of 6) 4 remain (aka 2 lone pairs)
This video has made many things clear. But how to draw lewis structure for a molecule whose formal charge is not equal to zero? Does every molecule support lewis structure?
the video was really helpful, but in our textbooks its given 1/2 bond pairs are subtracted instead whole bond pairs. could you please clarify once, i would really want to follow your method. thanks
NH4Cl is an ionic compound. It cannot be defined with a lewis structure as a collective molecule. Since NH4 has a positive FORMAL charge and a negative FORMAL charge, you would need to draw lewis structures for individual ions.
The electronegativity decreases going down and left of the periodic table. You do not need to know the exact values for this specific lesson but rather which element is the least electronegative as it would be the central atom (which in this case was carbon).
The table of valence electrons and lone pares you drew in the beginning just solved a 2-year mystery I had with Lewis structures in school. Thank you!
Thank you so much! All of my teachers just threw big molecules at us and told us to draw Lewis Structures without even really teaching us how to do it.
I cannot begin to explain how much you have helped me! I have been struggling with Lewis structures for years now. You have really saved my Chem grade.
I'm so glad I found this, now I won't have to take decades to draw these thank you very much.
I really hope you read this comment because that table you drew in this video just cleared so much confusion and connected all the dots. I am not very good with words but I hope you know this video helped me so much and I have the video paused right now just so I could type up this comment. I almost never comment on videos but you deserve it. Thank you for making the world a better place.
This is very concise, very clear. Thank you so much!
where did you get that table you drew on the top right? I don't see anything like it in my text book. Thanks
Don't know if you still need an answer but everything you need is a periodic table
Learn how to read it and it will be a shortcut to understanding all about bonds and electron configuration
For example O is in 16th group so it has 6 valence electrons (electrons in valence shell), but he wants to have 8 (octet rule)
So he needs 2 more and he will get them with bonds (aka makes 2 bonds)
Every covalent bond is in fact two electrons shared between the atoms so in order to get 2 electrons from the other atom he has to share his own 2 with that atom. When he shares his 2 atoms (out of 6) 4 remain (aka 2 lone pairs)
Well done 👏 awesome stuff. Never seen this approach before with the table. Love it! Thanks
Thank you very very very much! That table is what i wanted!!!!!!
The bond and lone graph is so useful . Thank you
omg thank you so much i literally didnt understand a thing about lewis structures before watching this video.
You are legend,that table is key to all the problems
Thank you so much! This is a really helpful approach!
THIS WAS SO HELPFUL!!
This video has made many things clear. But how to draw lewis structure for a molecule whose formal charge is not equal to zero? Does every molecule support lewis structure?
This is amazing
Hey can you plz make video on structures of h2p2o7, (hpo3)3 h2s2o8 etc
What happens when, say oxygen, only has 1 of its 2 preferred bonds? What happens to the free electron? Thanks!
This was very helpful. Thanks 😃
Group no. after 1,2 will be 13...18. Also I think it is better to write electronic conf. and then count valence electrons
the video was really helpful, but in our textbooks its given 1/2 bond pairs are subtracted instead whole bond pairs. could you please clarify once, i would really want to follow your method.
thanks
In your textbook 1/2bond pair electrons is given not bond pairs
1\2bond pair electrons is equal to bond pair
This video is really useful however I do not know how to do the NH4Cl, help please??
NH4Cl is an ionic compound. It cannot be defined with a lewis structure as a collective molecule. Since NH4 has a positive FORMAL charge and a negative FORMAL charge, you would need to draw lewis structures for individual ions.
2 lone pairs for oxygen or 4 lone pairs for oxygen?
+Aim High 2
2 lone pairs but 4 lone pair electrons
omg literally tysm like wow
actUALLY BLESS
How did he find out th3 electronegativity?
The electronegativity decreases going down and left of the periodic table. You do not need to know the exact values for this specific lesson but rather which element is the least electronegative as it would be the central atom (which in this case was carbon).
This doesn't seem to work for N2O4 (Dinitrogen Tetroxide) and other covalent compounds having charges, anyone knows why?
This is not a universal solution and sometimes doesn't work
Look for another video with "5 steps" of drawing lewis
That method works
Why is it that N2=10?
5 valence electrons (each oxygen) 2 = 10 valence electrons
thx b
pls sub to me
bro is intelligent
los vídeos en español están muy mal explicados, que bueno que se ingles