Chemistry

Chapter 6 Overview Formula Mass and the Mole Concept Ø Molecules Ø Ionic Compounds Determining Empirical and Molecular Formulas Ø Percent Composition Ø Empirical Formulas Ø Derivation of Molecular Formulas Solutions Ø The Dilution Equation Ø Units of Concentration (Additional Practice) 4 - 5 The Dilution Equation Figure 6.10 Ø Both solutions contain t

CHEM | 1 | Chemistry | lecture notes | Chapter 6 Overview Formula Mas

Chapter 11 Overview The Dissolution Process  The formation of solutions Electrolytes  Types Solubility  Effects due to T and P  Henry’s Law  Solubility Curves Colligative Properties  Molality, Molarity  Vapor Pressure Lowering,  Boiling Point Elevation,  Freezing Point Depression,  Osmotic Pressure Colloids 4 - 1 Units of Concentration 1. Molar

CHEM | 1 | Chemistry | lecture notes | Chapter 11 Overview The Dissol

Chapter 10 Intermolecular Forces  Types  Effect on Boiling Points Properties of Liquids  Adhesive and Cohesive Forces  Viscosity, Surface Tension, Capillary Rise Phase Transitions  Definitions/Types  Heating Curves Phase Diagrams  How to interpret phase diagrams  Supercritical Fluids The Solid State of Matter  Bonding in Solids  Types Lattice

CHEM | 1 | Chemistry | lecture notes | Chapter 10 Intermolecular Forc

Chapter 8 overview • The Ideal Gas Law PV = nRT Related calculaons: n = mass / MM mass = density × V • STP: 1 atm; 0 °C = 273.15 K • Dalton’s Law: P T = P A + P B or P A =X A P T P B =X B P T Related calculaons: X A =P A /P T X B =P B /P T X A + X B = 1 • Kinec-Molecular Theory of gases: All gases , regardless of their molecular mass, have the same average kinec energy at the same temperature

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