CHEM 1210 Chapter Notes - Chapter 12: Partially Ordered Set, Phase Diagram, Atomic Orbital

• School: Ohio State University
• Department: Chemistry
• Course: CHEM 1210
• Professor: A L L

Document Summary

Behavior can change at high pressures and low temperatures due to changes in intermolecular forces. 12-1 intermolecular forces - interaction between molecules from the permanent and momentary unequal distribution of electron density within molecules: van der waals forces are types of intermolecular forces. Chapter 12: intermolecular forces: liquids and solids: electron charge density is the probability that an electron is in a certain region at a given time. Electrons in elongated molecules are more easily displaced and elongated molecules are more polarizable: dipole-dipole interactions. Ice hydrogen bonds hold the water molecules in a rigid, but open structure with a low density. As it melts, some hydrogen bonds are broken allowing molecules to be more compactly arranged leading to an increase in density. Once water attains its maximum density, the density will decrease as temperature increases: other properties affected by hydrogen bonding, dimers are double molecules created from pairs of joined molecules, viscosity trends can be explained by hydrogen bonding.