London Dispersion Forces & Temporary Dipole - Induced Dipole Interactions - Intermolecular Forces
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- Опубликовано: 30 окт 2017
- This chemistry video tutorial provides a basic introduction into london dispersion forces also known van der waals forces. London dispersion forces arises from the electrostatic interactions between temporary dipoles and induced dipoles. A dipole is a polarized particle that contains a separation of charge - one part of the particle is partially positive and the other part is partially positive. Polar molecules contain permanent dipoles. Nonpolar molecules do not usually contain a dipole moment but can become a temporary dipole due to the distortion of the electron cloud. Atoms and molecules with a large number of electrons are highly polarizable, that is, they have a higher probability of turning into a temporary dipole. A dipole can cause another molecule to turn into a temporary dipole. This is known as an induced dipole. The interactions between temporary instantaneous dipoles and induced dipoles are known as van der waals interactions or london dispersion forces. Large molecules have a high amount of london dispersion forces and therefore have higher boiling points than smaller molecules. Boiling point is directly related to the amount of van der waal interactions among molecules.
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Repetition in the description of partial positive... the latter should have been partially negative. To all those who may be confused
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I think the temporary polar molecule induces the other molecule due to dipole moment which pushes the electrons in the induced molecule
not because the electrons are attracted to the positive charge of the inducing molecule as they should have been more attracted to the positive charge of the induced molecule as it is nearer
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Facts bro
So ldr only occurs in between diatomic molecules is it?
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To the Organic Chemistry Tutor 🍻
Can induced dipoles be considered temporary dipoles as well?
Yes, cauz when we take away the non-polar atom away from polar atom,induced dipole will be vanished.
Hi, why cycloalkanes have higher boiling point and greater LDF compare to chain alkanes?
Electron delocalization?
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I really didn't get the part where the atom becomes a dipole, why did the electrons become 8? Where the atom before the atom that is being a dipole has 6 positive and negative charge.
i think that is Delta symbol
the delta symbol with a positive means that one side is slightly positive whereas if it has a negative symbol near it, that side is slightly negative
Which have more solubility in water
Dipole dipole molecule or dipole induced dipole?
dipole-dipole because it occurs in polar molecules and water is a polar molecule. therefore molecules with dipole-dipole interaction are more soluble in water
Thanks
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You forgot to mention why boiling point of noble gases increase with the decrease in electrons
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You'd think more surface area allows more heat to be absorbed, but apparently not
It's because intermolecular forces occur on the surface of the atom or molecule, so the larger the surface area the more room for the intermolecular forces meaning a higher melting and boiling point.
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I'm here cause I have an oral exam today and I forgot how to explain dispersion forces
you wronged F2 electrons is suppose to be 81 not 18
Are we all doing some last minute revision??
Quiz starts at 2pm and its 11: 32am
The notion that the more electrons you have will increase the probability that 1 side will be unevenly distributed seems counterintuitive. For instance, if you flip a coin twice the chances of getting heads 100% of the time is relatively high (let the coin represent helium with only 2 electrons and heads represent the electrons existing on the same side of the atom). Whereas If you flip a coin 53 times (like iodine) the chances of getting heads 100% of the time (or anywhere close) is very low. Therefore the more electrons an atom has should increase the likelihood that the electrons are evenly distributed the majority of the time as a % value, which in turn should lower the LDF of the atom?
It might be because helium has low numbers of electrons so the nucleus can attract them and keep them evenly distributed. Unlike Iodine which has 53 electrons so for e.g if a polar molecule comes near it Iodine nucleus will have a hard time attracting all the electrons and keeping them in their place.
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