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Advanced Placement Chemistry Outline Summer Assignment Chapter 1 – Introduction Observations and conclusions; properties of matter; physical and chemical changes; elements, compounds, and mixtures; the scientific method; atoms, molecules, and ions; the use of chemical models; chemical symbols and nomenclature; chemical equations; the chemistry of the alkali metals Chapter 2 Measurement SI units; uncertainty in measurement and significant figures; accuracy and precision; systematic and random errors; density; isotopes; calculation of formula masses; Avogadro's constant; the mole Assignments Brown LeMay Summer Assignment - Read Sections 1.3,1.4,1.5 - Do end of Chapter problems 19,21,23,31,35 Read Chapter 2 - Do end of Chapter problems 15,23,25,31,35 Memorize Polyatomic Ions and Solubility Rules – handout. Aug 9-27 Chapter 3 - Stoichiometry stoichiometry, including limiting reagents; theoretical, actual, and percent yield; empirical formulas, percent composition; molecular and structural formulas Chapter 5 - Chemical Thermodynamics: Thermochemistry definition of system and surroundings; state functions [very briefly]; energy, work, and heat [I omit PV work]; temperature, thermal energy, and heat; exothermic and endothermic reactions; energy units; heat capacity and specific heat; calorimetry; enthalpy; Hess's Law Assignments- Brown LeMay – Chapter 3 problems 3,17,21,3.29,3.39,3.51,53,6571,75,77,100 Chapter 5 5,13,15,25,27,33,41, Western Kentucky University Hess’s Law Problem Set Hendrickson Laboratory Experiments (wet labs) Determination of the Empirical Formulas Experiment 5 Brown LeMay Chemical Reactions of Copper and Percent Yield Experiment 6 Brown LeMay Heat of Neutralization Experiment 26 Brown LeMay ****Exam 1**** Aug 30 – Sept 10 Chapter 10 - Gases pressure; Boyle's Law, Charles's Law, and the combined form; absolute zero, standard temperature, and pressure; the ideal gas equation; Dalton's Law; kinetic molecular theory; molecular speeds and Graham's Law; real gases and van der Waal's equation Assignments- Brown LeMay Chapter 10 problems 1,9,19,21,25,29,35,39,45,47,49,51,55,59,65,71,73,75,83 Laboratory Experiments(wet) Determining the Molar Volume Using a Gas Collection Tube (Adapted from Flinn Scientific (page 318 2007 catalog) The Gas Laws Experiment 15 Investigations in Chemistry Henrickson,Hunter,Byrd Graham’s Law Experiment 16 Investigations in Chemistry Henrickson,Hunter,Byrd **** Exam 2***** Aug 13 – Oct 1 Chapter 6- Atomic Structure discovery of the electron and its mass and charge; the nuclear atom; the proton and neutron; the electromagnetic spectrum, including frequency and wavelength; the photoelectric effect [qualitatively]; the Rydberg/Balmer equations; the quantum mechanical model of the atom and the Planck equation; the Bohr model; the Heisenberg uncertainty principle; Schrodinger equation [very brief mention only], electron spin, and the Pauli exclusion principle; quantum numbers [physical meaning only - not extended to knowing quantum "address" of each electron]; shapes of orbitals Chapter 7 - Electronic Structure and the Periodic Table electron configurations (aufbau principle) of atoms and ions; isoelectronic species and properties; the periodic table and periodicity; atomic and ionic radii; ionization energies; electron affinity Laboratory Experiments/Activities Molecular Geometries of Covalent Molecules: Lewis Structures and VSEPR Theory (activity lab experiment 11) Brown LeMay Collection of Gas Over Water(wet lab) – adapted from Flinn Scientific ******Exam 3***** Oct 4-8 Review and Take Quarter Exam Fall Break Oct 11-15th Oct 18 – Nov 12 Chapter 8- Chemical Bonds valence electrons; ionic bonds; Lewis structures; polar and nonpolar bonds; electro negativity; bond length, energy, and order; formal charge; resonance structures; exceptions to octet rule Chapter 9- Molecular Shape and the Theory of Chemical Bonding the VSEPR model; lone pair-lone pair repulsions; polar and nonpolar molecules; dipole momems; valence bond theory, hybridization, and sigma and pi bonds; molecular orbital theory, including shapes of molecular orbitals; configurations of diatomic molecules; explanation of paramagnetism of O2 molecule; band theory of bonding in solids; molecular spectra ****Exam 4**** Nov 15 –Dec 10 Chapter 4 - Reactions in Solution . strong, weak, and nonelectrolytes; Arrhenius acids and bases; solubility rules; reactions between ions in solution, including precipitation and neutralization; ionic and net ionic equations; single replacement reactions and an introduction to the activity series; concentration (percents, molarity); dilution and titration calculations Oxidation-Reduction Reactions oxidation numbers, including periodicity and nomenclature; balancing of redox reactions; disproportionation reactions; oxidation by oxygen; metallurgy ****Exam 5**** Dec 13-17 Review for Midterm and Midterm Exam Christmas Break Dec-20 – Jan 2 Jan 3 – Jan 21 Chapter 15 - Chemical Equilibrium chemical equilibrium, equilibrium constants, equilibrium constant expressions, and equilibrium calculations; Le Chatelier's Principle; industrially important equilibrium Chapter 16- Acids and Bases Bf0nsted-Lowry definitions; Kw; pH and other "p" scales; concentration of H+ and OH- in aqueous solution; hydrolysis; the common ion effect; buffered solutions; indicators; titration calculations; polyprotic acids *****Exam 6**** Jan 24-Feb -11 Chapter 17 - More about Equilibria periodicity; Lewis acids and bases; equilibria of complexes [briefly]; solubility product constants; factors influencing solubility of salts; practical applications Chapter 19 - Chemical Thermodynamics: More Enthalpy, Entropy, and Free Energy The laws of thermodynamics; entropy; free energy; temperature and direction of spontaneous change; calculation of delta G from delta H, delta S, or from delta Gf estimation of delta G at different temperatures; estimation of temperature at which the direction of spontaneous changes reverses; delta.G for nonstandard conditions; standard free energy and equilibrium constants ****Exam 7*** ****Quarter Exam*** Feb-14 – March 4 Chapter 20 - Electrochemistry voltaic cells; standard cell potentials; effect of concentration on cell potential; free energy and cell potential; batteries; corrosion; electrolytic cells; stoichiometry and Faraday's Laws; practical applications ***Exam 8**** March 7-18 Chapter 11 - Liquids, Solids, and Changes of State kinetic molecular view of liquids' and solids; intermolecular attractions, including hydrogen bonding and London forces; properties of liquids, such as viscosity, capillary action, etc.; vapor pressure and boiling points; melting points and freezing points; heating and cooling curves; phase diagrams; types of crystals (ionic molecular, covalent network, and metallic) and properties; arrangements of units in crystals [I omit]; crystal structure from x_ray diffraction patterns and the Bragg equation [1 omit]; crystal defects and semiconductors [1 cover briefly] Chapter 13- Solutions Revisited kinetic molecular view of solution process; solubility of solids; effect of temperature on solubility; effect of pressure on solubility {Henry's Law}; molality and mole fraction; Raoult's Law, ideality, distillation, and azeotropes; colligative properties, including osmosis and van't Hof factor; colloids ****Exam 9**** March 21 – April 1 Unit 18 - Chemical Kinetics rates of reactions; rate and concentration; finding rate laws; first order reactions; second order reactions; rate and identity of reactants; rate and solvent; heterogeneous reactions; catalysts; rate and temperature; theory of reaction rates; reaction mechanisms; the steady state approximation Chapter 21 - Nuclear Chemistry the radioactive decay process; induced nuclear reactions; rates of nuclear reactions; nuclear stability; radioactive decay series; energy changes; fission and fusion; biological effects; uses of radioisotopes; synthesis of the elements *****Exam 10**** April 11-15 Unit 22 - Organic Chemistry occurrence; hydrides; stereo isomers [I treat optical isomers lightly]; alkanes; nomenclature, functional groups, mechanisms, synthesis [lightly], polymerization April 28-29 Review for AP Exam **** Final Exam**** April 29th .