The treatment in Problem P15C.4 applies only to one-dimensional solids. In three dimensions, the variation of density of states is more like that shown in Fig. 15.1. Account for the fact that in a three-dimensional solid the greatest density of states is near the centre of the band and the lowest density is at the edges.
Chapter 13: Physical Properties of Solutions Solutions: homogeneous mixtures of two or more pure substances; the solute is uniformly dispersed throughout the solvent if the solvent is H2O then the solution is aqueous solution = solute + solvent unsaturated solution: contains less solute than the solvent has the capacity to dissolve at a specific temperature saturated solution: contains the maximum amount of solute that will dissolve in a solvent at a specific temperature solubility:amount of solute dissolved in a given volume of a saturated solution at a specific temperature supersaturated solution: contains more dissolved solute than is present in a saturated solution and are generally unstable Solution Formation Process: solvation: solute molecules separated from each other and surrounded by solvent molecules depends on interactions: solute-solute, solvent-solvent, solute-solvent Energy Changes in Solution Formation: Solute-Solvent Interactions: “like dissolves like” polar substances tend to dissolve in polar solvents non polar substances tend to dissolve in non polar solvents miscible: mixing in all proportions immiscible, if not methanol is miscible with water but hexanol is almost insoluble in water. why answer: methanol is polar but hexanol is almost non polar Concentration Units: molarity: M = moles of solute/liters of solution temperature d
