A molecule of pyruvate would attract another molecule in three ways:
- London Dispersion Forces- In all molecules polar or non-polar, the electrons in the molecule are shared amongst the atoms, they do this by being in constant motion around the atom. As a result of this at a given time there could be more electrons in a certain area and fewer electrons in an area in another molecule. This creates temporary dipoles, which serve as a very weak force of attraction.
- Dipole-Dipole- In polar molecules there is an uneven distribution of charges in the molecule, creating a positive and negative pole. This then results in the positive end of one dipole molecule, being attracted to the negative end of another, creating a force of attraction.
- Hydrogen Bonding- This is a special type of dipole-dipole that occurs between two polar molecules, with one possessing a hydrogen and another possessing a fluorine, nitrogen, or oxygen. In this attraction the O2, F2, or N2, in this case Oxygen will break its bond to the molecule and reform a covalent bond with the hydrogen of another then it will break and oxygen will re-bond to the molecule, this then keeps on happening creating a very strong bond.
Here you discuss the intermolecular forces of attraction that are active in Pyruvic Acid. As all molecules have London Dispersion Forces, you mention that. All polar molecules have Dipole-Dipole forces, so you mentioned that. Finally, this molecule has the ability for Hydrogen Bonding, a very special type of Dipole-Dipole, and you mentioned that. Push come to shove, you have mentioned all of the intermolecular forces and accurately show by the picture, the forces of dipole-dipole and hydrogen bonding. Excellent.
ReplyDeleteDavid,
ReplyDeleteYou have properly discussed all of the types of bondings that are available for this molecule. Your descriptions and definitions of each of the bonds are accurate and correct. Also, your picture is very well done. You properly show the single and double bonds in their correct space, and the electrons that are around the atom. Everything in the picture is accurate and easy to read. It would have been nice if you color-coded the atoms, but it is very well done and satisfactory without that. Good job overall for the intermolecular forces and the picture.
-Richard Herzig