Dipole Moment, Molecular Polarity & Percent Ionic Character

This organic chemistry video tutorial provides a basic introduction into dipole moment and molecular polarity. It also explains how to calculate the percent ionic character of a bond.
Organic Chemistry - Basic Introduction: • Organic Chemistry - Ba...
Bond Strength and Bond Length:
• Bond Strength and Bond...
Orbital Overlap and Bond Length:
• Hybridization, Orbital...
Steric Number and Hybridization:
• Steric Number, Hybridi...
Intermolecular Forces & Hydrogen Bonds:
• Intermolecular Forces ...
_______________________________
Resonance Structures:
• Resonance Structures
Bond Order and Resonance:
• Bond Order and Resonan...
Curve Arrow Notation:
• Curve Arrow Notation -...
The Major Resonance Contributor:
• Major Resonance Contri...
pKa, Ka, & Acid Strength:
• pKa, Ka, and Acid Stre...
Acids and Bases - Basic Intro:
• Acids and Bases - Basi...
_______________________________
Stability of Negative Charges:
• Stability of Negative ...
pKa Values of Acids:
• pKa Values of Acids - ...
Resonance Stabilization - Conjugate Bases:
• Acids and Bases - Elec...
Organic Chemistry PDF Worksheets:
www.video-tutor.net/orgo-chem...
Organic Chemistry Exam 1 Playlist:
bit.ly/3kJnNXU
Full-Length Videos and Worksheets:
/ collections

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Organic Chemistry PDF Worksheets: www.video-tutor.net/orgo-chem.html
Full-Length Exams and Worksheets: www.patreon.com/MathScienceTutor/collections
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[@herteltm]

Nicely done. I have one comment regarding the direction of the dipole moment: please keep in mind that electric dipole moments always point from negative to positive charges, i.e. in the opposite direction from that shown in the video.
In fact you did use the correct definition at 2:15 where dipole moment \mu is defined as "charge times separation distance". If you use vectorial notation for dipole moment \mu and displacement r instead, this will naturally give you the correct result, i.e. dipole moments pointing toward the positive charges.
Also, this is not an issue of chemists using a different definition for dipole moments than physicists. Although it seems that the majority of chemists is not aware of this misconception (see reference below). But who is to blame them? This has been passed on over generations and you will find dipole moments pointing the wrong direction even in standard chemistry textbooks and ... on the web of course.
The arrow notation which you used, with the cross at one end and the arrow-head at the other was apparently introduced by Linus Pauling. It was originally intended to signify the direction of transfer of negative charge, i.e. the directions in which electrons are moved. Either he himself or others later then erroneously associated this cross-arrow notation with the dipole moment itself.
If you are sceptical - as you should be - look up dipole moment in the online Gold Book of the IUPAC (International Union of Pure and Applied Chemistry), always a good place to resolve disputes on the definition of chemical terms.
Hovick and Poler actually also wrote a nice article about this very issue in J. Chem. Educ. 82 (2005) p889, "Misconceptions in Sign Conventions: Flipping the Electric Dipole Moment". For some reason TH-cam didn't let me post a doi link to their article so you will have to look it up if you want to dig further.
I hope this helps. Keep up the good work.

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[@FettyHuang]

At 7:18, i thought that this molecule would have a weaker dipole moment because dipole moment is the separation of positive and negative charges. For the nonpolar molecule, if the charges are facing the opposite direction, doesn't that mean a higher separation (a.k.a. greater dipole moment)?

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[@ionion642]

sorry for the dumb question..but can I say that the larger the dipole moment of a molecule, the easier it is to form non-covalent bond to other molecules (ionic bond, hydrogen bond, Van der Waals)? I am new to this concept so I'm just trying to understand the significance of dipole moment

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[@code6233]

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[@nonsame8495]

Hey.. if the difference in electronegativity in the compound is 0.5 and that was nonpolar.. then why was the other compound also 0.5 and was polar?

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[@aadi_001]

*Those who are wondering electronegativity of hydrogen is 2.2*
C- 2.5 slightly more than hydrogen
Cl - 2.5. More than carbon as well as hydrogen

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[@treea1682]

I have a lot of questions,
1. lipid can also have Dipole Moment right?
2. From Q1, does that mean Lipid is momentarily dissolvable in water?
3. Water is polar molecule, why does it not induced non-polar lipid into polar polar lipid and make it dissolvable?
I have done research online, for a couple of days, but as I get deeper, I couldn’t find a proper explanation.
4. Why Soap form a structure called Micelle? What happens if I don’t have oil in water, does Micelle structure still exist?
5. Micelle has a similar structure to phospholipid, how do soap get rid of phospholipid bilayer? but first, how do oleate past through the phospholipids layer, if the layer of phospholipids are densely connected, which means there would be no place for oleate is step in?

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[@robinmc142]

Wait, so you only have to take the electronegativity difference from the first 2 elements in the formula?

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[@argumentative2532]

Anyone know why the magnitude of charge of proton/ electron doesn't get doubled when putting it into the Mionic=QxR equation?
Because i thought we were measuring the gap between their charges, I would have also thought the difference between them would be taken to get the magnitude of charge, as opposed to an average of the two.
How I'm being stupid?

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[@amnalayth1841]

very good

[@ahmedrihanrihan850]

since we add 2 different charges (+)ve and (-)ve should it be (1.6+1.6) * 10^-19 Coulohms

[@tusharmuhammad9204]

how would you calculate the actual molecular dipole moment between C and O if the observed is not given?

[@mawadaalhalash7074]

thanks very much

[@zannysquad8546]

increase electronegativity difference -> more polar
top right is most polar (F is most polar element)

[@ayasamer7731]

So I'm confused now what is the standard of which is bigger
The M.wt or the net dipole moment or what ???
Please I wanna the answer for this question

[@Laughter...504]

Yo. Very huge fan of ur vids. But there is one mistake. The Electronegativity difference of C and O is 1, which gives 19 - 37% of ionic character, but you got 10.4, which is not within the limit for the ionic character

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[@tusharmuhammad9204]

how would you calculate the observed dipole in a scenario where it's not given? i mean, when it's not observed?

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[@patrickshawn3484]

That's helpful

[@Bharathkumar-od9je]

molecular geometry of a molecule decides whether a molecule is a polar or not , which also determines dipole interactions exists or not , even though a molecule is polar or not .
if the dipole moments cancel out , it is a non polar .
if there is net dipole moment , it is a polar .
for ex : CO2 is a polar molecule , but due its linear structure , the dipole moments cancel out , so therefore it is a non polar molecule .
H20 is a polar molecule , also due to its bent shape struture , the dipole moments add up , so net dipole moment exists .
So water is a polar molecule .
Am i right ?

[@71nxy47]

periodic table im using does not have same electronegative values as yours. my Hydrogen is 2.20 and Carbon is 2.55. So there is less diference of 0.5 in

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[@Alexandra-ug5ph]

How do the arrows in CCl4 cancel? I mean I see that the ones going up and down cancel each other, but the ones on the left and right are pointing in completely diffenent places. How possibly do they cancel?

[@TheMultiRaphael]

the thing is that they are being equally atracted by the carbon, so none of them are more polar than the others

[@code6233]

It's a 3d image
One cl at the top
One at the bottom
And other two at opposite sides (one at the back).

[@hanzou1142]

so for the quiz, if the instructor asks us that: Is C2H2Cl2 polar or non-polar, how can I answer it?

[@orehit3980]

Han Zou its polar because the bond between c and h is nonpolar but the bond between h and cl is polar. There is nothing that can cancel out the vector of cl so it overall c2h2cl2 is polar

[@jessicatang185]

@@orehit3980 Hi, what about 5:56?

[@jasmineroman747]

Is non polar always going be 0 for dipole moment

[@FilipMakaroni_xD]

wait, what happened to the exponents that were not the same in the 2nd problem, 10^-29 and 10^-30

[@ertrimgrabanica4231]

can you teel us the program that you use

[@samisiddiqi5411]

Now that's a Dipole Moment

[@theophilusagada7282]

how did u get the 1.78 D I DONT UNDERSTAND
U didn't show how u calculated it using the formula

[@rayar2323]

2:16, Dipole moment= Charge * Distance of Seperation

[@Cobfhd]

10:02 WHY DO WE CONSSIDER THE C-O to have +1 and -1 charge , please explain that . thank you

[@clotho5437]

Because Carbon needs 1 electron and Oxygen provided that.
You can imagine this as a CH3 + OH molecule if it makes it any easier. The topic is concerned about the separation of these charges when the molecule is formed.

[@clotho5437]

Because Carbon needs 1 electron and Oxygen provided that.
You can imagine this as a CH3 + OH molecule if it makes it any easier. The topic is concerned about the separation of these charges when the molecule is formed.

[@PronycDragon]

you say in the first part that chlorine is much bigger than hydrogen but I thought the trend for atomic radius was that the atoms get bigger as you move to the left and down on the period table??

[@ChemSimplified]

He was referring to the bond dipole between C-Cl and C-H, not the atomic radius of Cl vs H.

[@alainadrouin1222]

where do the charges come from?

[@destinycross7977]

how do you know the electronegativity value ?

[@kritinanishwajoka5423]

According to the pauling scale. You can check somewhere

[@soumaknandi9218]

starts at 8:36

[@vishalchimkode8894]

Have you gone mad?

[@The053199]

How do you decide what charge to use?

[@ruslansaidov2000]

see which element in the molecule is most electronegative, and assign the minus charge to that one.

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[@Cinnaminimonster-3-]

Here cuz my teacher didn’t teach us this but it’s on a test review sooo.

[@l1wlf457]

So why is Bf3 non-polar ?

[@adelijoel5274]

Please what of if the charges are the same

[@The053199]

Then its non polar

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