<p>Final Topics 2014 Chemistry 300 Mr. Heberton</p><p>This is only a partial list! Please review your original materials and notes for details.</p><p>Unit 8. Stoichiometry Continued: Limiting Reactants  Determine limiting and excess reactants  Determine how much product can be yielded  Percent yield (actual/theoretical)</p><p>Unit 9. Gas Laws  Units for pressure and pressure conversions  STP  Kinetic Molecular Theory  Boyle, Charles, Gay-Lussac and Combined Gas Laws  Ideal Gas Law  Dalton’s Law  Avogadro’s hypothesis and molar volume of a gas</p><p>Unit 10: Nuclear Chemistry  Types of radiation (alpha, beta, gamma)  Half life (and related calculations)  Applications: nuclear power and safety (debate project)  Fission vs. fusion (process, energy, uses)  Balancing nuclear decay equations</p><p>Unit 11A: Covalent Bonding  Bond forming and breaking in terms of energy  Relationship of bonding to valence electrons and electron configuration  Types of bonding and types of compounds (ionic vs. molecular)  Characteristics of covalent bonds and molecular compounds  Lewis dot structures for molecular compounds  Nonpolar covalent vs. polar covalent vs. ionic bonds  Molecular polarity  VSEPR theory o 3D molecular shapes (linear, bent, pyramidal, trigonal planar, tetrahedral)  Intermolecular Forces (IMF) o London dispersion forces o Dipole-dipole forces o Hydrogen bonding o Identifying the IMFs most prevalent in a substance and comparing different substances’ IMFs Unit 11B: States of Matter and Phase Changes  Solids, Liquids and Gases. o Characteristics (include relative shape, volume, compressibility, and motion of particles (i.e. which can flow and why) o How temperature (kinetic energy) and IMF’s control state of matter for a substance  Phase Changes – know all six! o Endothermic vs. Exothermic changes  Heating and cooling curves and concepts  Vapor pressure o Vapor pressure curves</p><p>Unit 12. Solutions  Homogenous mixtures  Concentrated vs. dilute solutions  Types of solutions (unsaturated, saturated)  Factors that affect degree and rate of solubility  Solubility of different substances. o Role of polarity and IMFs  Solubility curves and trends with temperature  Measuring concentration: molarity and molality  Dilution  Colligative properties o BP Elevation and FP Depression calculations</p><p>Unit 13. Kinetics and Equilibrium  Heat flows o Exothermic (out) and endothermic (in)  Potential energy diagrams  Activation energy  Heat of Reaction = ∆H (why there are endothermic and exothermic reactions)  Collision theory o Two requirements for effective collisions (sufficient energy and orientation) o Factors that influence the rate of a reaction  Concept of equilibrium in reversible reactions  Writing equilibrium constant expressions o Calculating Keq and concentrations at equilibrium Unit 14. Acids and Bases  Characteristics of acids and bases  Arrhenius definitions of acids and bases o Identifying acids and bases from formulas  Identifying strong vs. weak acids and bases o Ka (and how it reveals relative strength of acids) o Relative strength as electrolytes  Calculating pH for strong acids and bases  pH “loop” problems  Using indicators  Hydrolysis and pH of salts  Neutralization  Titration</p>