Unit 5 Liquids, Solids, and Solutions
Intermolecular Forces (IMFs)
Solutions
Ions in Aqueous Solutions and Colligative Properties
- Describe the difference between and IMF and a bond.
- Describe dipole-dipole forces, hydrogen bonding, and London dispersion forces found within two molecules
- Identify dipole-dipole forces, hydrogen bonding, and London dispersion forces found within two molecules
- Predict the relative strength of IMFs
- How do IMFs affect certain physical properties such as boiling point and melting point.
- Describe the structure of a water molecule
- Explain how the physical properties of water are determined by the structure of water
Solutions
- Distinguish solutions from suspensions and colloids
- Identify and explain physical and chemical factors that affect solubility
- Define concentration terms of molarity, molality, percent by volume.
- Perform calculations using molarity (M) and molality (m)
Ions in Aqueous Solutions and Colligative Properties
- Describe the dissociation of ionic compounds and the ionization of some molecular compounds when they dissolve in water
- Define electrolyte
- Distinguish between strong and weak electrolytes
- Write a net ionic equation using the solubility rules
- Perform calculations with different solution concentrations such as molarity, and molality.
- Discuss effects of temperature, pressure, and structure on solubility.
- Use a solubility chart to determine if a solution is unsaturated, saturated, or supersaturated.
- Define colligative properties and use to calculate boiling point elevation, freezing point depression, and vapor pressure lowering
- Use colligative properties to determine the molar mass of a solute
To gain a better understanding of solubility and the dissolving process please refer to the page on solvation.
Unit 5 handoutsCourse Packet pagesSolutions PowerPoint day 1Solutions PowerPoint day 2Review Solutions |
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