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Topic/Objective Unit 1 Matter and measurement Measurement and units Use of significant figures Dimensional analysis Classification of matter Unit 2 Atoms, molecules and ions Atomic theory and atomic structure 1. Evidence for the atomic theory 2. Atomic masses; determination by chemical and physical means 3. Atomic number and mass number; isotopes Naming compounds Unit 3 Stoichiometry Stoichiometry 1. Balancing of equations 2. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants Chemical reactivity Percent composition of compounds Unit 4 Reactions in water and stoichiometry Precipitation reactions Ionic and molecular species present in chemical systems: net ionic equations Oxidation-reduction reactions a. Oxidation number b. The role of the electron in oxidation-reduction Strong, weak and nonelectrolytes Concentration & Stoich Unit 5 Thermochemistry State functions First law of thermodynamics change in enthalpy heat of formation heat of reaction Hess’s law; Unit 6 Thermodynamics Entropy free energy of formation; Section Ch 1 1.4-1.5 1.5 1.6 1.2 2 AP Outline: First half HW Lab HW1: Read Title: Safety and Equipment in lab Ch1, #1, 25, 37, 45, 65 Objective: To teach students proper safety techniques and get them familiar with lab equipment HW1: Read Ch2, 21, 41, 47, 55, 2.1-2.3 HW2: 59, 65, 61, 89 2.4 Title: Qualitative analysis of cations and anions (exp14) Objective: To determine the identity of unknowns by testing for the presence of various ions. 2.5 2.6-2.8 3 3.1 3.3-3.7 HW1: Read CH3, 11, 19, 20, 23, 33 HW2: 43, 49, 51, 59, 71, Title: Soichiometry in synthesis of ionic compound (exp9) Objective: Potassium alum is produced and the percent and theoretical yield of the compound is calculated Title: Empirical formula of a hydrate (exp2) 3.2 3.3 Objective: Find the empirical formula of a hydrate by heating it in a crucible and then determining the moles of the hydrate from mass measurements. 4 4.2 4.2 HW1: Read Ch 4 : 15, 19, 27, 41, 49 HW2: 61, 67, 69, 85, 92 Title: Finding the ratio of moles of reactants in a chemical reaction (exp1) Objective: Find the coefficients for two chemical reactants that appear in a balanced chemical reaction Title: An Activity series (exp20) Objective: The activity series for five metals and three halogens are determined 4.4 4.4 4.3 4.5-4.6 5 5.1 5.2 5.3 5.4 5.5 5.6 HW2: 63, 67, 72, 75, 19 19.1-19.4 HW 1:Read Ch5, 39, 45, 53, 61 HW1: Read Ch 19, 31, 37, 39, 47, Title: Thermochemistry and Hess’s Law. (exp13) Objective: The enthalpy of a reaction is determined from its three different chemical reactions using Hess’s law. Title: Analysis of a coordination compound (exp15) Objective: A coordination compound is synthesized free energy of reaction; Dependence of change in free energy on enthalpy and entropy changes Relationship of change in free energy to equilibrium constants and electrode Unit 7 Electrochemistry Balancing of redox reactions electrolytic and galvanic cells Faraday’s laws; standard half-cell potentials Nernst equation prediction of the direction of redox reactions Batteries & Corrosion Unit 8 Nuclear chemistry nuclear equations half-lives, and radioactivity; chemical applications 19.5 Unit 9 Quantum mechanics Electron energy levels: atomic spectra, quantum numbers, atomic orbitals Unit 10 Bonding Binding forces a. Types: ionic, covalent, metallic b. Polarity of bonds, electronegativities c. Bond energies, enthalpy and chemical reactions Molecular models a. Lewis structures b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds c. VSEPR Unit 11 Gases Laws of ideal gases a. Equation of state for an ideal gas b. Partial pressures Kinetic molecular theory a. Interpretation of ideal gas laws on the basis of this theory b. Avogadro’s hypothesis and the mole concept c. Dependence of kinetic energy of molecules on temperature d. Deviations from ideal gas laws HW2: 51, 53, 55, 63, 19.6 from a transition metal ion that is in solution. The compound is filtered from the solution and tested in various ways to determine the composition of the substance. 19.7 20 20.1-20.2 HW1: Read Ch 20, 9, 11, 13, 19 20.3, 20.9 HW2: 23, 35, 51, 59, 93 20.5 20.4 Title: Electrochemical cells (exp21) Objective: Half cells are constructed using different metals with the zinc half cell chosen as a reference standard with all potentials measured with respects to it. In addition the Nernst equation is used to measure the potential of a nonstandard solution and to find the concentration of a complex ion. 20.6 20.5 20.7-20.8 21 21.1-213 21.4 21.5, 21.9 HW1: Read Ch 21, #11,17, 27 HW2: 29,57, 65 6 HW1: Read CH6,5,25,49,51 HW2: 53, 67, 71, 73 . 8,9 HW1: Read Ch8, #7,19, 37, 61, 65, 69 Title: Molecule building 6.1-6.9 8.1-8.3 Hw2: Read 9.19.6, # 35, 43, 47, 51, 96 8.4 Objective: The Lewis dot structure of different covalent compounds are drawn and the respective models are built using ball and stick model kits. Polarity, molecular shape and bond angles are also determined. 8.8 8.5 8.6,8.7, 9.5, 9.6, 9.1-9.3 10 10.1-10.5 10.6 10.7-10.8 10.3 10.7 10.9 HW1: Read Ch 10, # 31, 35, 39, 53, HW2: 63, 73 105, Title: Molecular mass of a volatile liquid (exp3) Objective: A small amount of a volatile liquid inside a small test tube and then heated in boiling water until all the liquid vaporizes and fills the tube as excess water escapes. After the gas is cooled, the mass, volume, and pressure is measured to determine the molecular mass of the substance using ideal gas law Title: Determination of the molar volume of a gas (exp 5) Objective: A sample of a solid substance is heated, decomposing it into several products, including a gas. The mass of the gas is determined by the weight difference before and after heating and is then converted to moles. The volume of the gas, the pressure, and the temperature are measured. Topic/Objective Section Ch Unit 12 Liquids and Solids 11 Binding forces 11.2 a. hydrogen bonding 11.2 b. van der Waals (including London dispersion forces) 11.1 c. Relationships to states, structure, and properties of matter 11.3, 11.5, Gases, Liquids and solids from the kinetic-molecular viewpoint 11.8 Phase diagrams of one11.6 component systems Changes of state, including critical points and triple points 11.4 Structure of solids; lattice energies Second half HW Lab HW1: Read Ch11, # 6, 19, 25, 33 HW2: 45, 53, 55, 77, 79 11.7 Unit 13 Properties of solutions Types of solutions and factors affecting solubility Methods of expressing concentration (use of normalities is not tested) Raoult’s law and colligative properties (nonvolatile solutes); osmosis Nonideal behavior (qualitative aspects) Unit 14 Kinetics Concept of rate of reaction Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws Effect of temperature change on rates Energy of activation; the role of catalysts The relationship between the rate-determining step and a mechanism Unit 15 Chemical Equilibrium Concept of dynamic equilibrium, physical and chemical Le Chatelier’s principle equilibrium constants Equilibrium constants for gaseous reactions: Kp, Kc 13 13.1-13.3 13.4 HW1: Read Ch 13, # 21 27, 35, 41 HW2: 43, 47, 57, 65 13.5 Title: Molecular mass by freezing point depression (exp4) Objective: After first determining the freezing point of a pure substance, the freezing point of a solution is determined. The change in freezing point allows calculation of the freezing point depression constant. This constant is then used to help determine the molecular mass of an unknown substance. 13.6 14 14.1-14.2 HW1: Read Ch14, #,21, 23, 27, 29, 14.3-14.4 HW2: 65, 67, 84, Title: Study of the kinetics of a reaction (exp12) Objective: The total rate law for the oxidation of iodide by bromate ion in the presence of an acid is determined. The order for each of the reactants is found by varying the concentration of each reactant individually. Once the rate law is determined then the rate law is calculated and the activation energy is also determined. 14.5 14.5,14.7 14.6 15 15.1, 15.4, 15.7 15.2-15.3, 15.5-15.6 15.2 HW1: Read Ch15, #13, 27, 33, 37 HW2: 43, 45, 49, 51, Title: Determination of the equilibrium constant of an ionic compound (exp10) Objective: The solubility product of calcium hydroxide is determined using calcium nitrate, vinegar and sodium hydroxide. Title: Equilibrium and LeChatelier’s Principle Objective: Students will apply various stresses to a system and use LeChatelier’s principle to predict the effect of the various stresses. Unit 16 Acids and Bases Acid-base reactions concepts of Arrhenius, Brønsted-Lowry, and Lewis coordination complexes; amphoterism 16, 17 16.1 16.2-16.5, 16.11 HW2: 65,87,93, 101 17.5 HW3: Read Ch 17, # 21, 31, 33, 41 Equilibrium constants for reactions in solution (1) Constants for acids and bases; pK; pH (2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds (3) Common ion effect; buffers; hydrolysis Unit 17 Organic Chemistry Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties) structural isomerism of simple organic molecules and coordination complexes Review Lab Work after exam HW1: Read Ch16, # 29, 37, 43, 55 Title: Determination of the dissociation constant of weak acids (exp7) Objective: A small amount of unknown acid is dissolved in distilled water with half of the resulting solution poured into a different container. Sodium hydroxide is added to the solution to neutralize it, forming a solution of the salt of the acid. The acid and salt solution are then combined and the pH is measured using a pH meter with the pH equaling the pKa. HW4: 65, 73, 81, 96, 16.6-16.8 17.6-17.7 17.1-17.3 25 25.1-25.6 HW1: Read Ch 25, # 11, 17, 21 HW2: 23, 25, 27 Title: Preparation of Esters (exp22) Objective: A number of different esters are prepared, distilled, and purified by shaking it with a saturated solution of sodium carbonate. The theoretical yield is then calculated and the percent yield determined based on the amount actually prepared. 25.3 Handouts AP Exam Title: Qualitative analysis of anions Objective: Students will analyze solutions to determine the presence of 6 common anions. Title: Liquid chromatography Objective: A mixture of Kool-Aid is separated using chromatography and is then measured to allow the calculation of the resolution, selectivity and efficiency of the process. Title: Standardization of a solution using a primary standard Title: Redox titration Title: ID of correct indicator Title: Buffer solutions Title: Analytical gravimetric determination