Advanced Placement Chemistry Syllabus

Transcription

1 Advanced Placement Chemistry Syllabus Course Description: The College Board describes AP chemistry as a course designed to be the equivalent of the general chemistry course usually taken during the first college year. For some students, this course enables them to undertake, in their freshman year, second year work in the chemistry sequence at their institution or to register in courses in other fields where general chemistry is a prerequisite. Student Assessment: Students will be graded on a standard 10 point scale. Assignments will consist of homework, writing assignments, laboratory work, quizzes, and exams. Students who earn 90% of the points or better will receive a A 80% of the points or better will receive a B 70% of the points or better will receive a C 60% of the points or better will receive a D 59% of the points of lower will receive a F Homework Selected homework problems will be checked. If a student is absent the day the assignment is given they will have a day after they return to hand in the assignment. If the student is absent the day the assignment is due it will be due the day they return. Quizzes/Exams A quiz or exam will be given every other Friday. Quizzes will be worth 25 points and exams will be worth 100 points. There will be a comprehensive exam given every nine weeks. The exam, quiz and homework schedule may change as needed. The students low exam and quiz will be dropped each half year if it helps the students grade. If a student misses an exam or quiz for any reason that will be the exam or quiz dropped. Students may take a quiz or exam early as long as they notify me three days in advance. If a second exam or quiz is missed during the quarter it will be up to the instructors discretion how that exam will be handled.

2 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 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 Common Ions back table of text. Aug 9-26 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 Assignment Stoichiometry /Thermochemistry Chapter 3 problems 5,19,33,37,45,61,77,79,83,91,107 Chapter 5 problems 13,15,19,27,33,43 Handout Hess s Law problems from Western Kentucky University Dr.Henrickson

3 Labs(wet) Experiment 5 Brown LeMay Chemical Formulas Experiment 8 Brown LeMay Gravimetric Analysis of a Chloride Salt ****Exam 1**** Aug 29 Sept 09 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 Assignment Gases Chapter 10 problems 21,29,47,49,51,59,65,71,73,75,83,86,99 Labs(wet) Experiment 15 The Gas Laws Investigations in Chemistry Henrickson,Hunter,Byrd Experiment 16 Graham s Law Investigations in Chemistry Henrickson,Hunter,Byrd Determining the Molar Volume using A Gas Collection Tube Adapted from Flinn Scientific Experiment page Catalog. **** Exam 2***** Sept 12 Sept 23 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 Chapter 6 problems 3,13,19,23,27,43,45,53,55,65,69

4 Chapter 7 problems 5,11, ******Exam 3***** Sept 26th-30 Review and Take Quarter Exam Fall Break Oct 3-7th Oct 10 October 20 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**** Oct 25 Dec 09 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 Review for Midterm and Midterm Exam Christmas Break Dec-19 Jan 2 Jan 3 Jan 20 Chapter 15 - Chemical Equilibrium

5 chemical equilibrium, equilibrium constants, equilibrium constant expressions, and equilibrium calculations; Le Chatelier's Principle; industrially important equilibrium Chapter 16- Acids and Bases Bronsted-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 23-Feb -10 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-13 March 2 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 5-20 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,

6 including osmosis and van't Hof factor; colloids ****Exam 9**** March 21 March 30 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 Unit 22 - Organic Chemistry occurrence; hydrides; stereo isomers [I treat optical isomers lightly]; alkanes; nomenclature, functional groups, mechanisms, synthesis [lightly], polymerization April Review for AP Exam **** Final Exam**** April 29 th.