Resonance Structures, Basic Introduction - How To Draw The Resonance Hybrid, Chemistry

This general chemistry video tutorial provides a basic introduction into resonance structures. It explains how to draw the resonance structures using curved arrow notation and how to draw the resonance hybrid as well with all of the lone pairs, bonds, and partial charges. This video contains 2 examples / practice problems.
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Lewis Dot Structures:
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• How To Draw The Lewis ...
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Octet Rule Exceptions:
• Exceptions To The Octe...
Resonance Structures:
• Resonance Structures, ...
Polar and Nonpolar Molecules:
• Polar and Nonpolar Mol...
Formal Charge Calculations:
• How To Calculate The F...
Lewis Structures - Mega Review:
• Lewis Structures, Intr...
________________________________
Hybridization of Atomic Orbitals:
• Hybridization of Atomi...
Molecular Orbital Theory:
• Molecular Orbital Theo...
Dipole Dipole Forces of Attraction:
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Hydrogen Bonding:
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Unit Cell Chemistry:
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_________________________________
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I was at first trying to relocate certain atoms and ions to other parts of the structure, but realized that that would turn the molecule into another molecule or a molecule that doesn't exist. So better do it the more labor intense way and draw all the resonance forms:)

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my ochem professor makes us not put lone pairs on the resonance hybrid. maybe just a preference thing? patron here. best science videos ever!

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I have found a more developed way to get the number of lone pairs, here’s how it works - First count the number of valence electrons, just like he does but if you have have Hydrogen in the molecule, count its valence electrons as ‘7’. Now that you have the total valence electrons, divide it by 8. Now you will have a quotient and a remainder, the quotient tells you about the number of sigma bonds in the molecule and then divide the remainder by 2 and it will give you the number of lone pairs on the molecule(Just try it once, although it only works on single central atom species). You can even use this to get the HYBRIDIZATION of a molecule. For example take NO2- , here VE(N) = 5, VE(O)=6 and count the electron as 1, so total we get 5 + 2 x 6 + 1 = 18, now divide by 8 we get 2 as quotient and 2 as remainder, that means, there are two sigma bonds and 2/2=1 lone pair on the central atom, And the fun part is if you add 2(sigma bonds) and 1(lone pair) you get three which states that it is a sp2 hybridized molecule. ( 2= sp , 3=sp2, 4=sp3 and so on) good tryy ittt. Thank you for reading and do try it with a hydrogen species as well, just remember to count its valence as 7. And channel owner sir please pin it as well so others can be helped as well😷👍

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How do you know where to place the charges on the structure? I know you said oxygen always has a - charge if it has 1 bond and 3 lone pairs, but does that rule apply to other elements? thanks!

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Please make a vedio of showing how to draw resonance structure for NO2+( nitronium ion) I'm so confused With it.

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When you break the first N-O double bond, are you not supposed to evenly distribute the two electrons from that bond between N and O, in which case the oxygen ends up having 2 lone pairs and one unpaired electron instead of the 3 lone pairs on the diagram??

[@MrYahya0101]

btw could a more general Lone Pair formula be: (#total electrons - (#valence electrons if outer energy level is filled)*(#noncentral atoms))/2 ? Note I wrote #total electrons, not #valence electrons as you named it because formal charge should be added to valence electrons to give total electrons.

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can someone explain like what is the overall goal in resonance structures like how do we know which e- is going to which atom

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what is the difference between resonance structure and lewis structure? I really need to know in order to survive on my midterm test🙏🏻

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Is it a must to add the lone pairs in the resonance hybrid?

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Sir I have a doubt , is resonating always have coordinate covalent bond?

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