Polar and Nonpolar Molecules

[@TheOrganicChemistryTutor]

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[@bonganemathebula7556]

Another way of looking at it: Symmetrical = Nonpolar Asymmetrical = Polar

[@scoutst3r]

but h2o is symmetrical and polar

[@jacque.line_ng]

@@scoutst3r H2O isn't symmetrical though? It has a bent structure. edit: I get what you mean now

[@scoutst3r]

@Kiệt Khuê Lâm yeah I forgot to delete that

[@scoutst3r]

@@jacque.line_ng yeah it's kinda consuming

[@nathangunderson398]

Linear = nonpolar Non-linear = polar

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[@georgesadler7830]

Professor Organic Chemistry Tutor, this is a solid introduction into Polar and Nonpolar Molecules in AP/General Chemistry. Analyzing the geometry and the electronegativity values is an excellent way to learn if a molecule is Polar or Nonpolar in Modern Chemistry.This is an error free video/lecture on KZbin TV with the Organic Chemistry Tutor.

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[@ChefSporty]

Bro this was the best intro to polar and non polar. My teacher just likes to talk for real she don’t be teaching but youtube helps so much. I liked the chart that showed how to know if it’s polar and non polar cause now it’s so easy

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I am a bit confused with Carbon tetrafluoride...How are dipole moments cancel out when you draw it's 3d model.....

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What do you do if there are three elements? (like CH3Cl)

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[@Edenival.v0x]

one imp. note: the structure/geometry of the molecule depends upon the the hybridisation of the molecule and accordingly, the positioning of the elements is done, and a proper dipole moment can be drawn thank u very much ❤

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[@alonraigorodetsky1803]

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[@baharosman1416]

C(n)H(n) ALWAYS is nonpolar Golden rule

[@RutherfordBcrazy]

That doesn't explain anything well done

[@magikal_oz9872]

@@RutherfordBcrazy if a bond only has C and H atoms it is always nonpolar

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your explanations were SO clear! thank you so much

[@allieh2141]

How do we know if the molecule is supposed to be drawn in a bent or linear shape?

[@katrina2023]

check out VSEPR theory / molecular geometry.

[@LordOfTitans04]

If the central atom has a lone pair of electrons like in SO2, it causes the electrons to cause a repulsion effect b/w them as they are like charges and thus, they try to stay as far as the can from each other, causing the the compound to bend. As for CO2, notice that it has no lone pair of electrons on carbon and thus it exists in a linear form. Please do reply if you got it.

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[@blenmulugeta4687]

In the sulfur di oxide you drew 4 bonds then you made the valence electrons of sulfur 10. But there had to be 2 bonds with the one oxygen and 1 with the other. With a coordinate covalent bond. But that was help ful thank you.

[@shalinishastry]

how do you atomatically know if somethings is bent or linear, I know bent has lone pairs but i dont get why linear doesn't

[@jxzxf]

A molecule has linear geometry if it has 1 bond, and has a bent geometry if it has 2 bonding regions and 1 or 2 lone pairs.

[@jxzxf]

2 Bond, 0 Lone Pair = Linear 1 Bond, 3 Lone Pair = Linear 1 Bond, 2 Lone Pair = Linear 1 Bond, 1 Lone Pair = Linear 1 Bond, 0 Lone Pair = Linear 2 Bond, 1 Lone Pair = Bent 2 Bond, 2 Lone Pair = Bent 2 Bond, 3 Lone Pair = T-Shaped (Not Bent) ^I would just memorize this as well as the trigonal planar and tetrahedral for the regents/SAT

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[@lucy.2087]

Thank you so much for this! It has really helped me understand the differences between polar and non-polar molecules and how to identify them.

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[@McmatYangorata]

Am confused about the Lewis structure, symmetrical and asymmetrical. Like for CO2 is symmetrical and SO2 isn't, whyy?

[@arnavgupta3055]

Lone pairs distort the shapes

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shit vid dawg get your electronegativity up on gang. all my homies are nonpolar and wont snitch behind yo back 🔥🔥🔥

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[@azizmaatoug8535]

There is a mistake, the electric dipole moment vector is directed along the line from negative charge toward positive charge + the lewis diagram of so2 is false

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[@anikagupta5820]

Sir, I have a doubt. In 00:50 , in the first diagram it had positive and negative charges in its extreme ends, so why is it not polar ???

[@Romeotje]

they cancel each other out

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Hi, i might be ignorant here, but how do you know the Lewis structure of different molecules? Great video btw!!

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[@jon091201]

Hey so I noticed your SO2 lewis structure didn't seem to match mine. When doing the Lewis structure I had 2 bonds from the sulfur to the oxygen leaving the oxygen with 2 lone pairs and one bond to the other oxygen leaving it with 6 lone pairs. and of course leaving the 2 lone pairs above the sulfur. So I'm curious as how ours differ? How or Why is your sulfur double bonded to both the oxygens?

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