1. Lecture 3712/7/05

2. Section 1 Density Atomic composition Isotopes Moles Periodic Table Ionic vs. molecular compounds Predicting Naming Weight percentage Empirical formula

3. Section 2 Stoichiometry Limiting reactant Theoretical and percent yield Solutions Gas laws KMT Real Gases

4. Section 3 Light as energy Bohr atom Quantum numbers Electron configuration Periodic trends Lewis dot structures Formal charge Bond polarity

5. Section 4 Bond Order Molecular Geometry Molecular Polarity IMF Surface tension Changes in state Phase diagrams Solids Colligative Properties

6. 15-112 The osmotic pressure of human blood at 37 °C is 7.7 atm. Calculate what the molarity of a glucose solution should be if it to be safely administered intravenously.

7. 15-117 Maple syrup sap is 3% sugar (sucrose) and 97% water by mass. Maple syrup is produced by heating the sap to evaporate a certain amount of water. A) Describe what is happening to the composition and boiling point. B) If the finished product boils 4 °C higher than the original sap, calculate the concentration of sugar in the final product.

8. Compare the boiling point temperature of: 0.10 mol/kg sucrose solution 0.10 mol/kg KCl solution 0.10 mol/kg MgCl 2 solution

9. Practice Give formula for: Nitrate Sulfate

10. Practice What is the charge on each ion? K 2 S (NH 4 ) 3 PO 4

11. Fill in the table: Symbol # of protons # of neutrons # of electrons