First Semester Review Name: AP Chemistry 7 points DUE AT EXAM (Thurs., 1/25/18) Date: The AP Chemistry Semester Exam on January 25, 2018, will cover textbook Chapters 3 through 10, our labs, and any additional handouts we have used. - exam will be mostly multiple-choice questions (50-75) with some writing/short answer/math (5-15) - bring this review to the exam *POINTS AWARDED FOR THIS REVIEW FOR COMPLETION OF THE NUMBERED PROBLEMS.* Labs: - Be ready to answer multiple-choice and written questions about any and all of the labs we have done this semester. Related review questions from the textbook are listed for each lab: Lab #1: Percent of water in a hydrate (set-up, calculations) 1) p. 125 #139 2) p. 124 #123 Lab #2: Iodine clock reaction (molarity calculations, dilution, accuracy, precision) 3) p. 173 #35
Lab #3: Net ionic equations (how to write the net ionic equation given any two reactants) 4) p. 173 #45 5) p. 173 #49 Lab #4: Percent of iron in an iron pill (balancing a redox reaction using half-reactions, doing calculations using redox reactions) 6) p. 175 #81 7) p. 176 #87
Lab #5: Stoichiometry of a reaction using unknowns (graphical analysis, limiting reactant, excess reactant, meaning of coefficients in an equation) 8) p. 123 #99 9) p. 123 #107 Lab #6: Molar volume of a gas (set-up, calculations, especially collecting gas over water) 12) p. 229 #87 13) p. 229 #89
Lab #7: Gravimetric analysis (set-up, procedure, calculations) 10) p. 177 #103 11) p. 178 #119 Lab #8: Hand warmer challenger (calorimeter set-up, calculations [q=mcät]) 14) p. 278 #61 15) p. 278 #63
Lab #9: Hess s law (Hess s Law calculations, calorimeter calculations) 16) p. 278 #67 17) p. 279 #73 18) p. 280 #99
Lab #10: Blue sports drink analysis (how a spectrophotometer works; wavelength; absorbance; relationship between absorbance and concentration) 19) If a solution s concentration is higher, will it have a higher absorbance? Why or why not? 20) How would you determine the concentration of an unknown given a spectrophotometer and some known samples? Lab #11: Percent of copper in brass (balancing redox reactions; relationship between concentration and absorbance) 21) p. 177 #105 22) p. 177 #111
Lab #12: VSEPR (know all the names of the molecular shapes, how to draw them, and the major angles) 23) p. 397 #103 Lab #13: Chromatography (types of intermolecular forces in liquids and how that relates to major properties [solubility, boiling point, etc.]) Lab #14: Bonding and types of solids (types of intermolecular forces in metallic, ionic, nonpolar covalent, and polar covalent solids; major properties [solubility, conductivity, melting point, etc.]) 24) p. 488 #33 25) p. 488 #35 26) p. 490 #79 27) p. 494 #121
Other vocabulary and topics to review (use notes, textbook, old study guides, and handouts): stoichiometry calorimetry calculations (constant pressure balancing equations only; q = mcät) limiting reactant specific heat capacity limiting reactant problems Hess s Law problems excess reactant standard enthalpy of formation calculations solution (given tables) solute standard states solvent EMR aqueous solutions wavelength and frequency calculations (c=ëí) molarity energy calculations (E=h í) molarity calculations Bohr Model vs. quantum mechanical model standard solution Heisenberg Uncertainty Principle use of a volumetric flask quantum numbers mass of solute needed to make a solution orbitals dilution calculations (V 1 M 1 = V 2 M 2 ) orbital shapes precipitation reactions and calculations orbital diagrams (arrows) solubility rules Pauli Exclusion Principle predict if two solutions will produce a Dmitri Mendeleev precipitate electron configurations (superscripts) net ionic equations valence electrons spectator ions chemical family names acid-base reactions ionization energy (definition, trends using neutralization reactions and calculations periodic table) [p.175 #69] atomic radius (definition, trends using periodic titration table) oxidation-reduction reactions (redox) metals, non-metals, and metalloids oxidation states (oxidation numbers) bond polarity (using arrows and ä) rules for assigning oxidation numbers electronegativity (definition, trends using oxidation periodic table) reduction ionic radius (concept, trends using periodic writing and balancing half-reactions table) [p. 339 #129] resonance cation properties of gases anion pressure (units, conversion, definition) isoelectronic temperature conversion (K to C, C to K) lattice energy (definition, comparison using STP charge and size) [p. 395 #53] gas law calculations (Boyle s Law, Charles s reaction enthalpy from average bond energy Law, Gay-Lussac s Law, Combined Gas Law) tables ideal gas law calculations Lewis structures molar mass of a gas calculations exceptions to the octet rule gas stoichiometry calculations VSEPR shapes Dalton s Law of Partial Pressures calculations hybridization (sp, sp 2, sp 3, dsp 3, d 2 sp 3 ) [p. 431 collecting a gas over water #29] kinetic molecular theory intermolecular forces (ionic, dispersion, energy dipole-dipole, hydrogen bonding) law of conservation of energy types of solids (atomic, metallic, ionic, potential energy molecular/covalent, network covalent) kinetic energy like dissolves like general rule endothermic exothermic system surroundings heat vs. temperature enthalpy