1. AP CHEMISTRY Notes Chapter 1 Masterton Hurley Matter and Measurments

2. Types of Substances Separating Mixtures 1.Filtration: Mixture passes through a barrier with fine pores leaving the solid on the barrier. 2.Distillation: Liquid vaporizes leaving a residue of the solid behind. 3.Chromatography: Uses solubility and adsorption to separate components.

3. Measured quantities LengthSI unit m meter Tiny distances are measured in nanometers, 10 -9 m VolumeSI unitL Liter 1L = 10 3 mL = 10 3 cm 3 And 1 mL = 1 cm 3 MassSI unitg gram 1Kg = 10 3 g TemperatureSI unit˚C celsius Conveting to Kelvin, K, = ˚C + 273.15

4. Experimental Error Significant Figures Accuracy of tools used determine the significant figures. decigram balance 26.3 g the decigram balance gives you 3 s.f. analytical balance 26.582g the analytical balance gives you 5 s.f. An analytical balance measures accurately to the one thousandth of a gram.

5. Significant figures Multiplying and dividing= the answer has the fewest significant figures. 10.2 x 12.5423 = 127.93146 3sf 6sf reported answer should have 3sf 128 Adding and subtracting= the answer has the least significant place value. 16 - 1.895 = 14.105 Ones thousandths reported answer should be significant to the ones place 14

6. Conversion factors Changing from one unit to another – Multiply your starting value by a conversion factor – Conversion factors have a value of 1 1.376 USD $ = 1.000 Euro € Convert 5.51 € to $ Choose a factor that cancels the initial unit.

7. Convert 89.6 miles/hour to a value in meters per second. 1 mile = 1.609 km 1 Km = 1000 m 1 hr = 3600s Show all work, and cancel units.

8. Properties of substances Intensive property – Can be used to identify a substance, the value is independent of the amount. Ex. Density, Boiling Point. Extensive property – Is dependent upon the amount of substance. Ex. Mass, volume.

9. Identifying substances Chemical properties – Observed when a substance takes part in a chemical reaction. Physical properties – Observed without changing the chemical identity of the substance. Ex. Melting point, boiling point, density, hardness

10. Properties of Substances Densityd=m/v A flask containing 5.00mL of octane has a mass of 25.598g. The empty flask has a mass of 22.138g. What is the density of the octane? What would be the volume of 10.00g of octane?

11. Properties of Substances Solubility – An amount of solute that is dissolved in a solvent. Often expressed as g of solute/ 100 g solvent – Ex. Solubility of Sugar @20˚C = 210g sugar/100g water – A solution of 100g of water with 210g of sugar = saturated – A solution of 100g of water with <210g of sugar = unsaturated – A solution of 100g of water with >210g of sugar = supersaturated

12. Color and Absorption Spectrum Visible light: 400nm – 700nm V I B G Y O R 700nm ultra violet infra red

13. Solving for solubility How much water is required to dissolve 52g of sugar (@20˚C) ? A 20˚C solution contains 25g of sugar and 125 g of water. Is it saturated, unsaturated, or supersaturated?