Noncovalent Forces

Structural Biochemistry/Chemical Bonding/Noncovalent bonds
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Ciferri and A. Perico, Eds. Schneider Binding mechanisms in supramolecular complexes Angew. Quantifying Hydrogen Bonding J.

Retrieved 11 November Noncovalent Forces. Otero de la Roza, G.


Maharramov, K. Mahmudov, M. Kopylovich, A.

Noncovalent Forces (Challenges and Advances in Computational Chemistry and Physics)

Hobza and K. Res , 48 , — Angewandte Chemie International Edition.

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So this is a polar molecule as well. And so the boiling point of acetone turns out to be approximately 56 degrees Celsius. Richard F. Metal aromaticity. Sastry is a J.

Compendium of Chemical Terminology. Opinion Coll. Interface Sci. Molecular Shape and the Hydrophobic Effect Annu. Water-Mediated Hydrophobic Interactions Annu. M Eur. Physical J. Biedermann, W. Nau and H. ChemPages Netorials. University of Wisconsin - Madison. Retrieved 27 October Metal Ions in Life Sciences.

Berlin: de Gruyter GmbH. Biochemistry 4th ed. The organic chemistry of drug design and drug action 2. Amsterdam [u. Chemical bonds.

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1st International Conference on Noncovalent Interactions

Namespaces Article Talk. Views Read Edit View history. By using this site, you agree to the Terms of Use and Privacy Policy. Intermolecular forces are the forces that are between molecules. And so that's different from an intramolecular force, which is the force within a molecule. So a force within a molecule would be something like the covalent bond. And an intermolecular force would be the force that are between molecules.

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And so let's look at the first intermolecular force. It's called a dipole-dipole interaction. And let's analyze why it has that name. If I look at one of these molecules of acetone here and I focus in on the carbon that's double bonded to the oxygen, I know that oxygen is more electronegative than carbon. And so we have four electrons in this double bond between the carbon and the oxygen. So I'll try to highlight them right here.

And since oxygen is more electronegative, oxygen is going to pull those electrons closer to it, therefore giving oxygen a partial negative charge. Those electrons in yellow are moving away from this carbon. So the carbon's losing a little bit of electron density, and this carbon is becoming partially positive like that. And so for this molecule, we're going to get a separation of charge, a positive and a negative charge. So we have a polarized double bond situation here.

We also have a polarized molecule. And so there's two different poles, a negative and a positive pole here.

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And so we say that this is a polar molecule. So acetone is a relatively polar molecule. The same thing happens to this acetone molecule down here.

Intermolecular forces

So we get a partial negative, and we get a partial positive. So this is a polar molecule as well. It has two poles. So we call this a dipole. So each molecule has a dipole moment. And because each molecule is polar and has a separation of positive and negative charge, in organic chemistry we know that opposite charges attract, right? So this negatively charged oxygen is going to be attracted to this positively charged carbon.

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And so there's going to be an electrostatic attraction between those two molecules. And that's what's going to hold these two molecules together. And you would therefore need energy if you were to try to pull them apart. And so the boiling point of acetone turns out to be approximately 56 degrees Celsius. And since room temperature is between 20 and 25, at room temperature we have not reached the boiling point of acetone. And therefore, acetone is still a liquid. So at room temperature and pressure, acetone is a liquid. And it has to do with the intermolecular force of dipole-dipole interactions holding those molecules together.

And the intermolecular force, in turn, depends on the electronegativity. Click OK to close the Internet Options popup. Chrome On the Control button top right of browser , select Settings from dropdown.

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