![]() In this case it's an even stronger version ofĭipole-dipole interaction that we call hydrogen bonding. Of course, water isĭipole-dipole interaction. Partially charged oxygen, and the partially positive To be some sort of electrostatic attractionīetween those opposite charges, between the negatively So we have a partial negative,Īnd we have a partial positive. Little bit of electron density, therefore becoming Those electrons closer to it, giving the oxygen a partial Oxygen and the hydrogen, I know oxygen's moreĮlectronegative than hydrogen. And once again, if I thinkĪbout these electrons here, which are between the Intermolecular force, and this one's called The intermolecular force of dipole-dipole We have not reached the boiling point of acetone. Is between 20 and 25, at room temperature Point of acetone turns out to be approximatelyĥ6 degrees Celsius. And so there's going to beĪn electrostatic attraction between those two molecules. That opposite charges attract, right? So this negativelyĬharged oxygen is going to be attracted to Positive and negative charge, in organic chemistry we know Molecule is polar and has a separation of ![]() So we get a partial negative,Īnd we get a partial positive. The same thing happens to thisĪcetone molecule down here. We also have aĭifferent poles, a negative and a positive pole here. So we have a polarizedĭouble bond situation here. Molecule, we're going to get a separation of charge, a Little bit of electron density, and this carbon is becoming Those electrons closer to it, therefore giving oxygen a More electronegative, oxygen is going to pull I know that oxygen is more electronegativeĮlectrons in this double bond between the carbon Molecules of acetone here and I focus in on theĬarbon that's double bonded to the oxygen, ![]() And so let's look at theįirst intermolecular force. And so that's different fromĪn intramolecular force, which is the force within a molecule. Intermolecularįorces are the forces that are between molecules. That polarity to what we call intermolecular forces. To see how we figure out whether moleculesĪre polar or nonpolar and also how to apply Whether a covalent bond is polar or nonpolar. Conversely, if you bring the positive side of a permanent dipole near a molecule, the electrons in the molecule will rush towards the positive side, leaving the far side of the molecule with fewer electrons and thus a temporary positive charge.Įlectronegativity, we learned how to determine When the permanent dipole goes away, though, it is more stable for the electrons to spread out again. If you bring something negatively charged near the molecule (like the negative end of a permanent dipole), then the negatively charged electrons will be repelled and will concentrate on the far side of the molecule, making the near side slightly positively charged and the far side slightly negatively charged (ie you've made an induced dipole!). In this terrible metaphor, the people walking around the room are like the electrons evenly spread around a molecule. Conversely, if I brought a bunch of cupcakes there might be a rush for my side of the room, though people would spread out again once the cupcakes were gone. When the skunk leaves, though, the people will return to their more even spread-out state. ![]() ![]() If I bring a smelly skunk into the room from one of the doors, a lot of people are probably going to move to the other side of the room. Suppose you're in a big room full of people wandering around. ![]()
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