1. Overview of Matter

2. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes

3. Mixtures Variable combination of 2 or more pure substances. HeterogeneousHomogeneous

4. Pure Substances Element –composed of identical atoms –EX: copper wire, aluminum foil

5. Pure Substances Compound –composed of 2 or more elements in a fixed ratio –properties differ from those of individual elements –EX: table salt (NaCl)

6. Endothermic – energy absorbed Exothermic – energy released

7. Physical Properties of Matter Melting Points Boiling Points Density Solubility

8. Melting and Boiling Points Use the Reference Tables to determine the following: –Rank the following substances from smallest melting point to largest melting point: H 2 O, N 2, iron, lead, O 2, C 12 H 22 O 11

9. Reference Tables con’t What is the state of matter (solid, liquid, or gas) will each of the following substances at the given temperature? a. chlorine at -25 o C b. ethanol at 0 o C c. sodium chloride at 1500 o C d. methanol at -100 o C e. sulfur dioxide at 10 o C

10. Density Using the reference tables, determine the following: –Rank the following substances from greatest density to smallest density: H 2 O, Mg, C 6 H 14, Pb, methanol, NaCl

11. Reference Tables con’t What is the mass of 36.5 mL of ethanol? What is the volume of 50.0 g of molten lead? You have 100.0 cm 3 of glucose and sucrose. Which sample has the greatest mass? Support answer with calculations.