Real Gases—Not ideal Illustrating two different problems: 1. Gases don’t satisfy the ideal gas equation, because PV/nRT 1 under all conditions. 2. Gases don’t satisfy the ideal gas law, because they all turn into liquids (at the temperatures listed).
van der Waals acoefficient is intimately connected to the temperature at which the gas condenses to form a liquid van der Waals Gas Law
Kinetic theory of everything
Heating Curves: energy deposited into different dynamic modes
Boiling points of various hydrides (and noble gases)
Dipole-dipole interaction between molecules
Dipole-dipole interaction between molecules Like ion-dipole interaction in solution.
A special case of the permanent dipole-permanent dipole interaction: the hydrogen bond Found wherever H is bound to N, O, or F so that the bond is highly polar Electron density on the “back side” of the H atom is very low