Man you are a solid speaker. I can appreciate when someone talks on a topic being certain of what they are going to say before they say it, while not pausing or using "like". How I've not found these videos earlier is beyond me.
hi, i'm a school teacher here in the Philippines. I really appreciate your videos cause they help me a lot in facilitating my teaching the students here. Keep it coming. God bless
hermest99: On average there would be as many repulsions as attractions. However, attractions move the charges closer thus increasing the attraction whereas repulsions move the charges away diminishing the repulsion. This results in a net attraction. Further this can result in a resonance effect between the molecules that stabilizes the attraction. Google "the strengths of van der waals dispersion forces" to find an excellent explanation of this.
Can you please explain why they are a intermolecular? A molecule is 2 or more atoms joined together by let's say a covalent bond. The London dispersion force acts upon 2 atoms. Shouldn t that make it intramolecular? As a whole does it form a giant molecular structure, or what is holding the london dispersion force formed molecules together, and create a liquid like in the case of liquid argon?
I want to point this out, don't expect this set of videos to teach you things from ground zero , i mean, this playlist assumes some basic previous knowledge on chemistry. Then you will be able to absorb the information accurately
But what determines which of the electrons go back and which ones don't? Won't the randomness of electron position in an orbital also cause them to just repel the other electrons at times? won't the attraction purely based on uncertainty of where they are and the existence of 2 positions of attraction (+-) and (-+) versus two of repulsion (--) and (++) cause a net attraction of zero?
Ron Mignery Tried that, even mailed a professor of chemistry at my university. He didn't know. The professor of particle physics didn't respond to my email so.. that's where the rabbit hole ended. I guess I'll be forever without understanding the London Dispersion Force.
+hermest99 You really have to think about this less as an electron and more as an electron density. You temporarily shift the electron density associated with a given electron orbital. This allows for new interactions/orbital overlap to occur. The polarization takes place because of ionic repulsion but the attractive interaction is more akin to a covalent bond.
***** Even with electron density and seeing electron orbitals as a chance of it being there then there's still the problem of ++, +-, -+ and -- occurring so equal chance of repulsion and attraction. I mailed a chemistry professor of the chemistry department of the uni I'm attending (I'm not in chemistry myself) and he didn't know, so I mailed the university's leading expert on this stuff, and he didn't mail me back. so somehow this is more intricate then it seems.
Hello I just have a question. You said that w/ increased amount of pi-bonds there's an increased attraction due to london dispersion forces. I'm confused b/c thinking about saturated fats vs. unsaturated fats (contains pi-bonds), the saturated fats have a larger london dispersion forces b/c they have more surface or as you called it "contact area." So if you can clear that up, I'd appreciate it. Thanks in advance. Bozeman Science
Just one question Paul. The dispersion force causes an attraction via the induction of the temporary dipole, why is it called a dispersion force? It seems to be doing the opposite; could you clarify this? Thanks.
So, neopentane and N-pentane are composed of the same elements but have different hydrocarbon lattice structures and this massively effects there boiling and cooling points?
Check out this image: en.wikipedia.org/wiki/File:Isosurface_on_molecule.jpg#mediaviewer/File:Isosurface_on_molecule.jpg This is a molecule (zirconocene), where part (left) is rendered using the ball-and-stick model, and part (right) is a representation of the "electron cloud" surrounding it. The term "squashiness" is just an adjective being used to describe the consistency of this cloud. Try to imagine the electron cloud as a big water balloon. The bigger the water ballon, the more "squashy" it will be (think of a golf ball-sized water balloon compared to a basketball-sized one). If you wanted to move most of the water in a basketball-sized water balloon to one side, it wouldn't be a problem at all compared to a little tiny one. That's exactly what polarizability is - the ease of distortion of the electron cloud of a molecule. So the more "squashy" the molecule, the more polarizable it will be.
Darn, this couldn't have come out yesterday. My chemistry teacher set a challenge to do with LDF. But its alright this will help reinforce those ideas. Thanks for the video. Also i was wondering, do the instantaneous dipole moments of electrons have anything to do with their quantum spin?
Your soothing voice creates a sense of false confidence in my ability to succeed in chemistry.
lol
I will not write LOL
This video was 2yrs ago. I'm curious how many of the 370 who liked your comment passed :)
Creative
5 years later I do not remember any of this hahaha
Saving my medical school career one video at a time.
Nathie1230 de
hows the medical school going?
I hope you got into medical school!!!
saving my undergrad pre med career
are you a doctor now?? im so invested lol i remember seeing this comment when i posted mine 5 years ago
Your wish is my command. This is video 16 in a 71-part series on the new AP Chemistry course. I hope to finish sometime this fall.
Holy crap, you did it, thank you for your service to all science students, aspiring scientists, and ultimately, your service to the world.
Man you are a solid speaker. I can appreciate when someone talks on a topic being certain of what they are going to say before they say it, while not pausing or using "like". How I've not found these videos earlier is beyond me.
7 years later and still saving the day 👏
Explained it better than my chem teacher 😔 thank u for ur service
In which School you are ?
@@RoshanKumar-up7rs hogwarts
Very helpful! And way easier to understand than a textbook!
but the forces of friendship are stronger than any other!
your profile pic is haunting
Not at all
You seem so friendly and I can thank you enough for how much you've helped me in chemistry :)
hi, i'm a school teacher here in the Philippines. I really appreciate your videos cause they help me a lot in facilitating my teaching the students here. Keep it coming. God bless
r u still a teacher
hermest99: On average there would be as many repulsions as attractions. However, attractions move the charges closer thus increasing the attraction whereas repulsions move the charges away diminishing the repulsion. This results in a net attraction. Further this can result in a resonance effect between the molecules that stabilizes the attraction. Google "the strengths of van der waals dispersion forces" to find an excellent explanation of this.
Your short 5 minute video helped more than 70 minutes of class in chem
Soooo helpful. Your videos have been my grade savers since sophomore year of high school... Thanks so much :3
You really cleared up how non-polar substances are dissolved. Thank you.
ty for this video , really organized and helpful in learning the concept.
Congrats on 90k subscribers and thanks as always.
hey its been 10 years how is life
this is so helpful all videos use very weird words but this video actually breaks everything down
Great, I have been reading about the London length of the protons in neutron stars and the electron seas that surround them. Thanks for loading this.
i need time to process this :D i had to go back like 10 times. but still, it's good! thanks!
hey hows life 10 years later. man its been a long time
Very clearly explained, easy to understand even with 2x speed. Great job
Originally, I am confused about London dispersion force. After your video, i totally understand how it works! Thanks a lot Mr. Andersen!:)
Thank You, Professor Andersen! Your videos are so helpful and detailed.
Nice! "
I was trying to learn these forces from 1 month but u made it easy". "Thanks"
This is the best video I found for this topic!
Dwija Parikh
Dwija Parikh
Thankyou! Being able to see the atoms in motion really helps.
Very good, the pentanes example is excellent. Looking at previous comments, it seems that mentioning the correlation of electron motion will help.
So thankful to you sir. My teacher is awful and you just explained that with so much ease.
You are a good teacher well👍👍👍👍. Your animation classes are helping to understand the concepts very well.Thank you so much
I have a test tomorrow, and you just made everything better
Your voice is amazing 😭
You're a life-saver, explained it so well. Thank you!
What a fabulous video. This is one of the best.
Can you please explain why they are a intermolecular? A molecule is 2 or more atoms joined together by let's say a covalent bond. The London dispersion force acts upon 2 atoms. Shouldn t that make it intramolecular? As a whole does it form a giant molecular structure, or what is holding the london dispersion force formed molecules together, and create a liquid like in the case of liquid argon?
I really like the way things are explained in such a simple and clear manner:)
Watched your videos in high school and now I'm back watching them in Uni cos I forgot a lot of things LOL
Thank you dude!! You explained really nice! Now I able to understand the whole concept.
You explained it so good. Thank you so much
I want to point this out, don't expect this set of videos to teach you things from ground zero , i mean, this playlist assumes some basic previous knowledge on chemistry. Then you will be able to absorb the information accurately
Great video for anyone studying cell biology / DNA / Proteins to watch
I miss that sound track on biology vids. And as always you are utterly and amazingly awesome
Great explanation sir
That was amazing! The visual really helped!
But what determines which of the electrons go back and which ones don't? Won't the randomness of electron position in an orbital also cause them to just repel the other electrons at times? won't the attraction purely based on uncertainty of where they are and the existence of 2 positions of attraction (+-) and (-+) versus two of repulsion (--) and (++) cause a net attraction of zero?
+hermest99 Google "intermolecular bonding - van der waals forces" for a more direct answer to your question.
Ron Mignery Tried that, even mailed a professor of chemistry at my university. He didn't know. The professor of particle physics didn't respond to my email so.. that's where the rabbit hole ended. I guess I'll be forever without understanding the London Dispersion Force.
+hermest99 You really have to think about this less as an electron and more as an electron density. You temporarily shift the electron density associated with a given electron orbital. This allows for new interactions/orbital overlap to occur. The polarization takes place because of ionic repulsion but the attractive interaction is more akin to a covalent bond.
***** Even with electron density and seeing electron orbitals as a chance of it being there then there's still the problem of ++, +-, -+ and -- occurring so equal chance of repulsion and attraction. I mailed a chemistry professor of the chemistry department of the uni I'm attending (I'm not in chemistry myself) and he didn't know, so I mailed the university's leading expert on this stuff, and he didn't mail me back. so somehow this is more intricate then it seems.
he went through it fast, but helpful over all
Beautifully explained. Thank you
Great Job man!This is exactly what i wanted.Thanks a bunch.
This was fantastic . I liked the video and understood it very well
I finally feel I understand the London dispersion forces. Thank you!
Very helpful sir. Keep it up👍
I liked your way of teaching
Is the London Dispersion Force same as the van der Waals force?
Wish every school and collage have professor like him.
You have saved my life in 2017
Now it’s almost 2021!
Hello I just have a question. You said that w/ increased amount of pi-bonds there's an increased attraction due to london dispersion forces. I'm confused b/c thinking about saturated fats vs. unsaturated fats (contains pi-bonds), the saturated fats have a larger london dispersion forces b/c they have more surface or as you called it "contact area." So if you can clear that up, I'd appreciate it. Thanks in advance. Bozeman Science
Thanks for the great video! It was very clear and understanding, and I appreciate your videos.
Brilliant teaching style
Easier than text book
Thank u soo much
Yes, I learned what london forces are. Thank you for the video
Just one question Paul. The dispersion force causes an attraction via the induction of the temporary dipole, why is it called a dispersion force? It seems to be doing the opposite; could you clarify this? Thanks.
Excellent video.. well said...great animation. .
Just one small doubt why does London forces increase with Pi bond....
Daipayan hati electrons are loosely held in pi bonds.Hence greater polarisability.
it's awesome man..I just got full in chemistry.. tq a lot 😊😊😊😊😊
so how do you know if a London dispersion has occurred? if it's a ionic bond or non polar covalent?
+Emily S. London dispersion happens in nonpolar molecules.
Thank you so much! you explained this topic in a very interesting way
So, neopentane and N-pentane are composed of the same elements but have different hydrocarbon lattice structures and this massively effects there boiling and cooling points?
Yeah the surface area of the N-pentane is more than that of neo-pentane so the B.P. for N-pentane is more than that of its isomer
Excellent I appreciate yourteaching really really👌👌
Thank You Helped so much studying for finals
Thank you it helped me a lot. You had explained it in a nice manner.
What's the difference between London dispersion forces and Van der Waals forces?
nice explanation man.
Thank you for a such elegant and clear explanation. Is there a mathematical equivalent to to dipole moment for London forces?
VERY WELL explained! Cheers!
Thanks a lot! it's very helpful and interesting. i really love your video.
Is HCl has london forces? can HCl has a temporary dipole ?
man I always watch your videos.. keep up the great work, I will be back!:)
btw. is london dispersion force the same as dispersion force?
Yes, these are actually dispersion forces named after their founder Fritz London
whats the difference between london dispersion forces and van der waals forces
Mr Anderson, how is the matrix?
thank you very much for that. I am a Saudi master student study in Germany 👏🏻👏🏻👏🏻👏🏻👏🏻👏🏻👏🏻👏🏻👏🏻👏🏻
great illustrations
Wow hats of to you....nice explanation friend.........
So the positive nucleus will attract negative electrons?
Thank you! My chemistry project is saved.
Bravo! I feel like cheering :)
This is amazing! Thank you very much sir!
sorry am not clearly about contact area. can u explain again?
Is LDF the same as Van Der Waals?
Mr. Anderson can you please do a video of you doing Simon Says??? Pleeease!!
THANK YOU FOR THIS I LOVE YOU
Thank you! Great explanation.
Extremely helpful! Thanks!
SO HELPFUL, THANK YOU!
Great explanation
thank you very much !!!
Really Good Work :D
What would London Force do to polar molecules?
Wonderful video :D Thanks!
Why are hydrocarbon compounds apo?
Mr anderson can i know which books did you use for learning this concept
Polarisability is the "squashiness" of a molecule? Can anyone describe this a lil better?
Check out this image:
en.wikipedia.org/wiki/File:Isosurface_on_molecule.jpg#mediaviewer/File:Isosurface_on_molecule.jpg
This is a molecule (zirconocene), where part (left) is rendered using the ball-and-stick model, and part (right) is a representation of the "electron cloud" surrounding it. The term "squashiness" is just an adjective being used to describe the consistency of this cloud. Try to imagine the electron cloud as a big water balloon. The bigger the water ballon, the more "squashy" it will be (think of a golf ball-sized water balloon compared to a basketball-sized one). If you wanted to move most of the water in a basketball-sized water balloon to one side, it wouldn't be a problem at all compared to a little tiny one. That's exactly what polarizability is - the ease of distortion of the electron cloud of a molecule.
So the more "squashy" the molecule, the more polarizable it will be.
Such a good explanation! Thanks Shaheen :)
Darn, this couldn't have come out yesterday. My chemistry teacher set a challenge to do with LDF. But its alright this will help reinforce those ideas. Thanks for the video.
Also i was wondering, do the instantaneous dipole moments of electrons have anything to do with their quantum spin?
I don't suppose you've done a more advanced video on this?
Thank you, this was really helpful :)
pleases upload the vedios for van der waal forces