Dipole Induced Dipole IMF
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- Опубліковано 6 лис 2019
- Explanation and example of dipole induced-dipole intermolecular force. (Polar and nonpolar molecules) Note: There is a correction. Ion-Dipole intermolecular forces are stronger than hydrogen bonding.
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hi, I have a question. Shouldn't ion-dipole interactions be stronger than h-bonding interactions because in ion-dipole interactions the molecules that are interacting are one with a formal charge and a partial charge so wouldn't it be a little bit stronger than h-bonding interactions which are just between molecules with partial charges ? Thank you so much for this video and for any help :)
Hi Suraiyanishat, YES! Good catch. Here is a video with the correction. Thanks:)
ua-cam.com/video/-wxb-Qsjlzo/v-deo.html
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Hi I understand that the larger the molecule the more polarizable hence the more soluble but how come chlorine and fluorine which are way smaller than iodine is more soluble. Thank you
shalom onyenekwe : Hi Shalom:). Iodine (I2) will be more soluble than chlorine (Cl2) or fluorine (F2) because it has greater surface area. I think your may be referring to the acids HCl, HF and HI. HCl and HI are both strong acids and completely ionize in water (dissolve if you will). HCl is considered a stronger bond than HI because of the stronger electro negativity and smaller atomic radius (greater coulombic attraction) of chlorine compared to iodine. As bond strength increases the acidity decreases. So HCl has the greater bond strength and lower acidity compared to the weaker bond strength and greater acidity of HI. HF is a weak acid and only partially ionizes. This is in fact because fluorine has the greatest electro negativity and smallest atomic radius of the halogens so it is more attracted to the hydrogen than the water molecule. I hope that helps!
My textbook calls it "induced-dipole induced-dipole forces." Is this different than the dipole induced-dipole forces you describe here?
Hi Mark, induced dipole induced dipole is the same thing as London dispersion forces. I’ll send the link to that video. Dipole- induced dipole is different. It is unique to polar and non polar molecules interacting.
London dispersion forces, same thing as induced dipole- induced dipole: ua-cam.com/video/KsURyiGzg6g/v-deo.html
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Hi Bts - viminkook, I am glad you liked it! Thank you for your comment☺
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Hi! If this is so why aren't covalent compounds soluble in water. Please answer 😔😔😔
Covalent compounds like methane why aren't the soluble in water.. If the water can induce the dipole on non polar molecules
shalom onyenekwe: Hi Shalom! It depends on how easily polarizable the covalent compound is. Iodine has a large surface area so it is more easily polarized than the smaller methane molecule. Therefore iodine has a more easily induced dipole and is more soluble than methane.
shalom onyenekwe: Shalom here is a video on polarizability. Start at 5 minutes 30 seconds ua-cam.com/video/KsURyiGzg6g/v-deo.html Thanks!!
@@OldSchoolChemistry Thank you so much 💕
Hello again. How come Hydrogen bonding is stronger than Ion Dipole? I thought that since Ion Dipole has a full charge, it allows it to have stronger interaction = stronger bond than the hydrogen bonding.
You are correct! I made a mistake. Here is a video with the correction. Thank you!
ua-cam.com/video/-wxb-Qsjlzo/v-deo.htmlsi=xaFXe1oCj2bObySG
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Hi Madot, I hope it was helpful and your chemistry experience is positive. Thanks for leaving a comment.
Hey is induced dipole and spontaneous dipole same??
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Hi Fasseh, I have not heard of "spontaneous dipole." I can tell you that induced dipole is temporary and not permanent which would liken it to the word "spontaneous." I hope that helps!
@@OldSchoolChemistry soory instantaneous dipole.it is also temporary,are they same??
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4:02 I believe this is incorrect; ionic forces should be strongest, followed by hydrogen bonding (which is a type of dipole-dipole interaction), followed by other dipole-dipole interactions.
Hi Joseph, Ionic bonding and covalent bonding are comparisons on intramolecular forces. Intermolecular forces (hydrogen bonding, dipole-dipole, LDF) are within covalent bonds. To compare ionic bond strength use coulomb's law. Here are two videos to clarify: ua-cam.com/video/liU29Lt0eoE/v-deo.html
ua-cam.com/video/PAmdB8LBU7g/v-deo.html
@@OldSchoolChemistry Thanks for the response! I'm referring to intermolecular forces. At the timestamp noted above (4:02), you mention "so hydrogen bonding, and then the next strongest would be ion-dipole..." However, many other sources have the opposite ordering. Here are two: sites.duke.edu/thepepproject/module-1-acids-bases-and-cocaine-addicts/teacher-notes-chemical-bonds-and-forces/ (bottom of page under "Intermolecular forces" section), and chemistry.bd.psu.edu/jircitano/IMforces.html (bottom of page under "Trends in the forces" section). Let me know if you can clear up the confusion. Appreciate the videos!
Joseph Edappully Hi Joeseph, Thank you for your thoughtful reply. I will watch those early next week and reply. Thanks again!
@@josephedappully1482 Hi Joseph, I stand corrected. Thank you for that. I will have to make a new video;) Thanks again!
@@leanthink1 No problem! A lot of content creators just put a little panel/image up with the correction at the time where the mistake was made so they don't have to redo the whole video, but perhaps you already know that. I know it can take a lot of time/effort to make these videos. Thanks for making them!
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