Course InformationLecture CalendarLaboratory CalendarChemistry Topics CoveredIntroductory LectureAtoms and MoleculesChemical CalculationsGasesThermochemistryChemical ThermodynamicsPhase TransitionsChemical EquilibriumAcids and BasesKineticsQuantum TheoryTransition MetalsPeriodic TrendsLewis StructuresMolecular GeometriesChemical BondingChem 2090 Calendar and SyllabusJohn A. MarohnAugust 28, 20201. Course Information• Instructor and Course Director: Dr. John A. Marohn, Professor, [email protected]• Laboratory Director: Dr. Cynthia Kinsland, Senior Lecturer, [email protected]• Course administrator: Mr. Steve Hutchison, Undergraduate Program Assistant,[email protected]• Textbook: Atkins 7e: Chemical Principles: The Quest for Insight. Peter Atkins, LorettaJones, and Leroy Laverman (w.h. freeman, Macmillan Learning, New York, 2016). ISBN-13: 978-1-3192-4106-3 (epub).• Alternate textbook: General Chemistry, 4th edition. D. A. McQuarrie, P. A. Rock, and E. B.Gallogly (University Science Books, 2011)2. Lecture Calendarending wk. lecture topic textbook section(s) ending lect. no. of lect.1 Introductory Lecture (Marohn notes) 1 12 Atoms and Molecules A and B 3 23 Chemical Calculations E, F, G.3, H, J, L, and M 7 44 Gases 3A to 3D 10 36 Thermochemistry 4A to 4E 15 57 Chemical Thermodynamics 4F to 4J 19 48 Phase Transitions 5A and 5B 20 19 Chemical Equilibrium 5G to 5J 23 39 Acids and Bases J, 6A to 6D, 6F to 6H 24 19 Kinetics 7A and 7B 25 111 Quantum Theory 1A to 1F 31 5.514 Transition Metals 9C and 9D 32 1.514 Periodic Trends 1F and 9A.1 34 215 Lewis Structures 2A to 2D 36 1.515 Molecular Geometries 2E 36 0.516 Chemical Bonding 2F and 2G 39 313. Laboratory CalendarExperiments run on a Wednesday to Tuesday cadence.ending wk. laboratory topic start end3 Check In and Safety 09/09 09/154 Density and Thermometry 09/16 09/225 Determination of Chemical Formulae 09/23 09/296 Recycling Aluminum 09/30 10/067 Complex Iron Salt Synthesis 10/07 10/138 Optical Spectroscopy 10/14 10/209 Acid Titration 10/21 10/2710 Copper in a Penny 10/28 11/0311 Gas Laws + Check Out 11/04 11/1015 Chemical Kinetics (virtual) 12/02 12/084. Chemistry Topics Covered4.1. Introductor y LectureI will explain, using real-world examples, why an engineer should be interested in learning chem-istry.4.2. Atoms and MoleculesSources• Text: A, B• Alt. text: 1.5 to 1.9, 2.1 to 2.5, 2.9 to 2.12, 2.6, 2.8Concepts• Units of Energy• Accuracy and Percentage Error• Precision and Significant Figures• Dimensional Analysis• Elements and Chemical Symbols• States of Matter• The Law of Constant Composition• Dalton’s Atomic Theory• The Nucleus• Protons, Neutrons, and Electrons• Isotopes• Ions• Molecules• Atomic and Molecular Mass24.3. Chemical CalculationsSources• Text: E, F, G.3, H, J, L, M• Alt text: 11.1 to 11.8, 11.10, 11.11, 12.1, 12.2, 10.3, 12.6, 12.7Concepts• The Concept of Mole• Avogadro’s Number• Simplest Formula• Determination of Atomic Mass• Molecular Formulas• Combustion Analysis• Coefficients in Chemical Equations• Stoichiometry• Limiting Reagent• Percentage Yield• Solutions• Molarity• Acids and Bases• Acid-Base Titrations• Formula Mass from Titration Data4.4. GasesSources• Text: 3A to 3D• Alt text: 13.1 to 13.11Concepts• Measurements of Pressure• Atmospheric Pressure• Boyle’s and Charles’s Law• Avogadro’s Law• Idea-Gas Equation• Determination of Molecular Mass• Partial Pressures• Maxwell-Boltzmann Distribution• Kinetic Theory and Root-Mean-Square Speed• Graham’s Law of Effusion4.5. ThermochemistrySources• Text: 4A to 4E3• Alt text: 14.1 to 14.4, 14.8, 14.9, 14.5, 14.7, 14.6Concepts• Energy, Work, and Heat• Enthalpy• Enthalpy and Energy of Reaction• Enthalpy Changes• Calorimetry• Bomb Calorimeters• Molar Enthalpy of Formation• Heat Capacity• Molar Bond Enthalpies4.6. Chemical ThermodynamicsSources• Text: 4F to 4J• Alt text: 23.1 to 23.10Concepts• Spontaneity of Reactions• Second Law of Thermodynamics• Entropy and Disorder• Entropy and Molecular Structure• Entropy Changes for Reactions• Gibbs Free Energy of Reaction and Spontaneity of Reactions• Gibbs Free Energy of Reaction and the Reaction Quotient• Relation of Gibbs Free Energy to Standard Gibbs Free Energy• Gibb’s Energies of Formation• The van’t Hoff Equation4.7. Phase TransitionsSources• Text: 5A, 5B• Alt text: 15.1 to 15.3, 15.6 to 15.8, 23.10, 15.4Concepts• Molecules in Liquids and Solids• Heating Curves• Fusion and Vaporization• Vapor Pressure• Relative Humidity• Phase Diagrams• The van’t Hoff Equation• Intermolecular Forces44.8. Chemical EquilibriumSources• Text: 5G to 5J• Alt text: 19.1 to 19.9Concepts• The Connection Between Equilibrium and Thermodynamics• Attainment of Equilibrium• Dynamic Equilibrium• Equilibrium-Constant Expressions• Pressure Equilibrium Constants• Equilibrium Calculations• Properties of Equilibrium Constants• Le Chatlier’s Principle, Qualitative• Le Chatlier’s Principle, Quantitative• Approach to Equilibrium4.9. Acids and BasesSources• Text: J, 6A to 6D, 6F to 6H• Alt text: 20.1 to 20.3, 20.5 to 20.9, 21.1, 21.2Concepts• Acids and Bases• Ion-Product Constant• Strong Acids and Bases• pH and Acidity• Weak Acids and Bases• Ka and Acid Strength• Successive Approximations• Henderson-Hasselbalch Equation• Buffers4.10. KineticsSources• Text: 7A to 7B• Alt text: 17.1 to 17.5, 17.8, 17.9Concepts• Reaction Rates• Rates and Time• Initial Rates• First-Order Reactions5• Half-Lift of First-Order Reactions• Second-Order Reactions• Half-Life of Second-Order Reactions4.11. Quantum TheorySources• Text: 1A to 1F• Alt text: 4.3 to 4.9, 5.1 to 5.8Concepts• Electromagnetic Spectrum• Line Spectra of Atoms• Standing waves vs traveling waves• The Electromagnetic Spectrum• The Photoelectric Effect• Photons• X-ray Diffraction• Electron Diffraction• Wave-Particle Duality• The Bohr Model• De Broglie Wavelength• Heisenberg Uncertainty Principle• Schrodinger Equation• Particle in a Box• Quantization• Electronic Transitions• Quantum Theory for Atoms• The Stern-Gerlach Experiment• Electron Spin• Atomic Energy States• Principle Quantum Number• Azimuthal Quantum Number• Magnetic Quantum Number• Hydrogen Atom Wavefunctions• Multielectron Atoms• Pauli Exclusion Principle• Electron