2) Determine the molecular polarity (MolecularPolarity) (e.g. dipole) of a species by explaining the molecular geometry and bond polarity. (could be required to fill in [Worksheet for Molecular Polarity]).
Intermolecular Force (IMF)
3) Determine the correct Intermolecular Forces (IntermolecularForces) (IMF) for each type of species (student will need to memorize table). In addition, be able to order species from lowest to highest IMF (either between IMF or within IMF).
4) Know that all substance have London Dispersion forces (LDS), what is it including instantaneous dipole, and why non-polar molecules are only substance that LDS is main IMF. Also, know the other situation that LDS play a major role in determining physical properties/comparison (vary different molar masses).
Physical Properties
5) Using your knowledge of of IMF, explain why a series of different substances (all at same temperature) are in different phases (i.e. solid, liquid, gas). Knowing that a substance can be in different phases, it only has one IMF value.
6) Be able to determine which substance has a higher or lower Boiling point after determining the substance IMF. Knowing that the higher IMF, the higher Boiling point (in general).
Physical Properties: Solubility/solution
7) Using your knowledge of IMF, determine if two substances dissolve/miscible in each other. Know the definition of miscible/immiscible and understand and memorize the phrase (Like dissolves Like) to determine if two substance are dissolve/miscible in each other.
8) Be able to make a drawing and provide an explanation (as discussed in class work) for the following:
a) Polar solute dissolved in a polar solvent
b) Ionic solute dissolved in a polar solvent
c) Non-polar solute dissolved in a non-polar solvent (will use oval for non-polar molecules)
d) Non-polar solute trying to dissolve in a polar solvent.
9a) Be able to define solute and solvent in a particle view manner.
9b) Be able to explain what a unsaturated solution, saturated solution, and saturated solution with undissolved solute (on top or bottom) is in a particle view manner.
9b) What happens to the solubility (amount of solute particles in solvent) of an ionic solute if you increase temperature of the solution.
9b) What happens to the solubility (amount of solute particles in solvent) of a gas solute if you increase temperature of the solution.