CHE 1302 Lecture Notes - Lecture 2: Intermolecular Force, Hydrogen Bond, Enthalpy
Document Summary
Baker | che 1302 | summer 2017| lecture 2 | page 1. Basically the attraction between positive and negative molecules. Strength of forces/bonds are affected by: distance between molecules, sizes of individual charges. Aka: van der waals or london dispersion. Carbon-hydrogen molecules are pretty darn close to non-polar. Lots of stuff going on in the background (lewis structure, vespr, polarity of molecules, etc. : electrons aren"t always evenly distributed. Even if the imbalance only lasts for a few milliseconds, it"s enough time for the molecule to interact with other molecules. Permanent dipoles in molecules: versus the temporary dipoles seen in dispersion forces. Hydrogen bonded to nitrogen, oxygen, or fluorine. An -oh in a molecule means it will hydrogen bond to anything else that"s willing, regardless of what the. Oh is attached to: typically found in alcohols. Putting sodium chloride (nacl) i water to make salt water. Water molecules rearrange so the negative dipole on the water molecules face the positive.
