O3 Lewis Structure - Ozone

[@TheOrganicChemistryTutor]

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[@TalkingTacosFood]

Bro saved me in viva Ayo nah man pure respect 💀❤ So those who didn't understood the 8 multiples one Its easy since octet has 8 electrons so we divide the valence electrons by 8 The quotient is basically the no of bonds it forms And remainder divided by 2 gives us lone pairs But remember this only applies for even electron species 💀 Nest those who didn't understood hybridization Its structure is bent because it is AB2L1 And sp2 = 2 bond bairs + 1 lone pair :)))

[@Anod-x4i]

This, this actually makes sence, I cant beleive I am ablw to understand inorganic, thank you so much, this feels so reasonable and something that will help me when i am giving my exam, tqsm, sir, plz keep up the good work, wishing u LOTS of success, Thanx again!

[@antisymmetric237]

You are such a great teacher. Thank you!

[@orion3043]

We can't thank you enough for all your videos.

[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for a short and beautiful explanation of the O3 Lewis Structure in AP/General Chemistry. From different Chemistry books, Resonance forms do not imply different kinds of molecules. There is only one O3 molecule whose structure is believed to lie between those of the two-resonance forms. Resonance can be expected when it is possible to write two or more Lewis structures which are about equally reasonable. In these structures, the nuclei are in the same position. That is, the atoms must be bonded in the same order. They differ only in the distribution of valence electrons between atoms. This is an error free video/lecture on KZbin TV with the Organic Chemistry Tutor.

[@LawrenceNdelemani]

Thank you sir for your videos may God bless you.

[@GrandWiziy101]

Hey quick question, why do we even need resonance structures for those typs of molecules? I get it for molecules like azide where the electron movement create dipols, but here its just kinda obvious. Don't get me wrong i know they can be important but i think its one reason why some people don't think of molecules moving in 3D

[@peybak]

Because the resonance structure here is actually telling you the bonds between the oxygen atoms are in between a single and double bond. It seems redundant but if you only draw one structure, that could mean you only have a single bond and a double bond between the oxygens whereas in reality, the bonds have characteristics of both a single and a double. That's one use of drawing resonances, not to mention contributions to stability and so on.

[@lilaclilac1907]

So helpful! Thank you!

[@AviroMusic]

It helped me a lot! Thank you...

[@nabilahkhan7221]

How does one atom of o share 2e ??

[@maiaallman4635]

Very good explanation.

[@SharonOmouna]

question, how does oxygen have 3 lone pairs with a single bond? with 6 unpaired electrons, does that mean the two electrons used to pair are coming from the other oxygen molecule?

[@mspzabbe]

love your work

[@zinabosman4980]

Why multiples of 8 ? Is this a rule always multiples of 8?

[@notmadewithmematic9577]

octet rule bruv

[@user-yy9wb3fm8v]

Is that for all elements or only oxygen as its atomic no. is 8

[@redalien75]

@@user-yy9wb3fm8vAll period 2 elements

[@tensai_desu7]

0:57, why only 8

[@redalien75]

Octet rule

[@bipeshgurung68]

what about coordinate covalent bond ?

[@haikalsharifudin1707]

Why are u not using lone pair formula that u usually use in this video

[@rohitbashel5347]

Fantastic 🎉

[@shizooka711]

can u explain why oxygen form more than 2 bonds thus it"s p orbital has only 2 unpaired electrons and it has not any d orbital

[@Tanzistr]

Its a dative or a coordinate bond...

[@abcd6095]

Thank you Sir

[@zorotenesin6515]

Thank you

[@newssense9222]

Thankyou so much...

[@ShaheryarRauf]

It’s difficult to understand.

[@oochipchoogi]

I don't think that's his problem. He always starts directly to the main subject. Maybe you don't understand some parts of the video?

[@leagueoflegends4466]

Start from the fundamentals first, maybe you skipped and make it straight to this topic.

[@moonbabeee]

I know it doesn’t make any sense at all.

[@notavailable-ih4zc]

1. add electrons 2. find lone pairs by subtracting multiples of 8 for each octet that can fit even the total electrons 3. each like represents a pair of electrons shares. 1 electron is originally one of the atoms within the bond

[@Uplift-Original]

Yes me too. I have problem, see the third O atom with -1 charge. An O Atom has 6 valence electrons of its own, but it has 7 of its own and 1 is shared. Same with the central O atom, it should have 6 valence electrons of its own but it has 5 valence electrons of its own and 3 are shared.

[@zehaojiang9737]

why the number of central electrons can be calculated like that?

[@TalkingTacosFood]

Bruh because an octet has 8 electrons 😂 So after completing octet the remaining will be counted as stray electrons of if in pairs then lone pairs

[@rowentaylor9784]

What is a lone pair?

[@nihal8874]

You are a great teacher but i can't understand anything because I am watching this video one day before the exam😢😢

[@himanshujangir3852]

Thanks 😊

[@musannabaktiar1795]

you should change your youtube channel name to The best tutor

[@laxmikanthkumsikar1366]

why Ozone does'nt exist in triangular shape?? can you explain?

[@nocap3637]

The angles would be too quick so electrons of each oxygen would be too close to each other

[@christysam3787]

Thank u sir

[@kimanhchung8372]

Thanks

[@anupachemistry8574]

But side oxygen have 6 e then how covalent bond with central atom why coordinate bond

[@santoshubale7220]

Cool man 😎😎

[@laylaa.hassanbiology1264]

Thank you so much.

[@thuwailibailm6251]

1:24

[@thuwailibailm6251]

4:29

[@Mars143ve]

Tq

[@rabiadalkc8136]

Thank you . I turkey

[@sofasobarna1740]

🕳️ 🚧

[@martha8315]

You sound like The Weeknd lmaoo

[@yomanxy]

1st?

[@thehowyoudoinpodcast]

yep

[@Mars143ve]

Tq

[@AmarKumar-ss7uk]

Thank you sir

[@erangasandunikumari1622]

Thank you sir