01.0_lecture1.ppt

Welcome to Chemistry 132 Fall 2008 Section 2 Dr. Layman Course Instructor Dr. Layman Office: PCB 3140 Office Hours: MWF 10:00 AM ? 11:00 AM Problem Sessions: TBA Tel: 568-1656 laymanka@jmu.edu Course Information Syllabus ? please read it carefully! Blackboard ? check it frequently for daily PowerPoint slides, weekly CSB assignments, and announcements. Grading Scheme No make-up activities Hour Exams (55%): Wednesday, September 17, 9:00 AM ? 10:00 AM Wednesday, October 8, 9:00 AM ? 10:00 AM Wednesday, October 29, 9:00 AM ? 10:00 AM Friday, November 21, 9:00 AM ? 10:00 AM Lowest Hour exam will be dropped In-Class Activities (10%): Workshops 1 excused workshop absence CPS (a.k.a. Clickers) 90% answering, 10% correct 4 lowest scores will be dropped CSB (10%): CSB is useful but insufficient Final Exam Friday, December 12, 2008 at 8:00-10:00 AM Cumulative (Chem 131 and Chem 132) Quizzes There will be NO quizzes? I hear a Cell Phone!!! Cell phones should be muted and stored in your pocket or backpack AT ALL TIMES during class. A ringing cell phone is my signal to administer a Quiz at the next available quiz section. UNLESS Index Cards-- Front Name Year Major Dorm Random Fact Index Cards-- Back Math classes completed Math classes in which you are currently enrolled Why are you taking this course? It?s required for my major. It fit into my schedule. It was one of the few courses that wasn?t filled. Why are you taking chemistry? Why is chemistry unique? understanding the natural world at the molecular level biology earth sciences physics Color: fireworks, gemstones, and pigments fireworks: molecular emission BaCl2 green SrCl2 red gems & pigments: molecular absorption Sapphires Blue = Ti, Fe Purple = V Green, yellow = Fe Pink = Cr Ruby Red = Cr Molecular recognition for disease detection no complement complement Problems for chemists Energy conversion - batteries, solar, nuclear Environment - remediation Materials - sports equipment, medical implants, iPods Medicine - transport, regulation, drug discovery & delivery Where do we start? Economics Chemistry Oceanography Atmospheric Sciences Physics Medicine Governments Geology Anthropology Biology Astronomy Politics People Objectives for Chemistry 132 continue to understand the world from an atomic and molecular level perspective REACTIONS 1. How quickly do reactions occur? 2. What remains when the reaction is done? 3. What is the driving force? 4. How can we explain reactions at a molecular level? 132: higher expectations CONTENT MASTERY learn vocabulary & quantitative relationships read work problems interconnect ideas & visualize the molecular level explain macroscopic phenomena in molecular terms transfer ideas to new problems apply and integrate concepts + UNDERSTANDING Why is chemistry challenging to many people? the molecular world isn?t visible quantitative relationships symbols molecular level pictures words chemistry uses many languages What do you need to do to succeed? How would you approach this if you were playing an instrument or a sport? observe the skill drill scrimage / rehearse compete / perform discussion class & book CSB & book problems problems & workshop exam class & problems Things that make a difference mastery of stoichiometry is essential for success (ch. 3, 4) working problems is essential CSB drills the basics - it isn?t enough attitude matters! (don?t psych yourself out of succeeding) do a little every day sleep affects performance Wednesday - advice for studying Homework It?s not there because I want to waste paper CHEMISTRY 132: GENERAL CHEMISTRY II CSB Homework, Review Material and Suggested Textbook Problems CSB due dates will be announced in class. Learning objectives are posted at http://csm.jmu.edu/chemistry/courses/genchem/. Chapter 13:  The Properties of Solutions Review Section 12.3: Types of Intermolecular Forces Online ChemSkill Builder:  Unit 15 Sections 1-5. Text Questions: 4,6,10,17,20,24,31,33,41,45,47,51,53,64,66,68,72,85. Chapter 16: Kinetics: Rates and Mechanisms of Chemical Reactions Online ChemSkill Builder: Unit 16 Sections 1-6. Text Questions: 8, 11,12,14,16,19,20,21,22,24,26,29,31,33,36,38,40,42,50,52,57,58,59,60,61,63,69,77 Chapter 17:  Equilibrium:  The Extent of Chemical Reactions Review Section 3.5: Fundamentals of Solution Stoichiometry (Examples: 12-15) Online ChemSkill Builder: Unit 6 Sections 1, 4 and Unit 17 Sections 1-5. Text Questions:  1,4,6,10,11,13,15,18,20,22,24,26,27,31,32,34,36,40,42,44,47,51,55,57,60,62,68,69,77,80. Chapter 18: Acid- Base Equilibria Review Section 4.4: Acid -Base Reactions Online ChemSkill Builder: Unit 6, Section 2, Unit 18 Sections 1-5 and Unit 19 Section 1. Text Questions: 5,7,9,11,16,18,20,30,32,34,38,45,49,54,62,64,72,79,88,92,94. Chapter 19: Ionic Equilibria in Aqueous Systems Solutions Review Section 4.3: Precipitation Reactions Online ChemSkill Builder: Unit 19 Sections 2-5 and Unit 20 Sections 1-4. Text Questions: 2,4,7,9,13,17,19,21,28,30,35,37,39,41,44,45,46,48,50,54,56,58,60,65,66,70,74,76,95. Chapter 20: Thermodynamics: Entropy, Free Energy, and the Direction of Change Review Sections 6.1-2 & 6.4-6: Thermochemistry Online ChemSkill Builder: Unit 8 Sections 5-6 and Unit 21 Sections 1-5. Text Questions: 2,5,8,10,12,14,16,18,20,22,25,26,27,29,31,36,38,39,41,43,45,49,51,53,54,58,60,62,64,75,78 Chapter 21: Electrochemistry: Chemical Change and Electrical Work Review Sections 4.5 & 4.6: Oxidation-Reduction (Redox) Reactions & Elements in Redox Reactions Online ChemSkill Builder: Unit 10 Sections 1-4 and Unit 22 Sections 1-5. Text Questions: 2,5,7,12,17,18,20,22,27,29,33,29,42,45,47,53,62,66,70,76,84,94,105. Chapter 23: Nuclear Reactions and Their Applications Review Section 2.5: Atomic Theory Today Online ChemSkill Builder: Unit 23 Sections 1-4 Text Questions: 1,2,4,6,8,10,12,18,20,22,24,26,33,38,40,48,50,53,60,62,65,68\ Extra Credit up to 1 extra points on each hour exam twice during the semester ? video or similar ? how it relates to the last class ? chemical explanation Wednesday?s Clicker Question: My black lab is named after a periodic element. Her name can be shortened to my grandmother?s name. In addition, she shares the same name (when shortened) as the individual that said ?Wherever you go, I will go.? What is her name? Molybdenum shortened to Molly Potassium shortened to Kay Californium shortened to Callie Ruthenium shortened to Ruth Samarium shortened to Sam 1 additional CPS drop for answering; 2 additional CPS drops if answer is correct Questions? For Wednesday Review chapter 3 Review section 12.3 Read sections 13.1 - 13.2 Learning objectives Learn how to construct molecular level pictures Know the difference in pure substances and solutions Understand the difference between types of intermolecular forces, bonds, and their relative strengths Understand the factors that affect melting/boiling point, vapor pressure, and solubility CSB Assignment 1: Unit 15(all) Wed, 3 Sept, 8 AM Layman, CHEM132 2F08 Molecular level pictures s vs. l vs. g vs. aq What?s the difference? CH2CH2OH(s) CH2CH2OH(l) CH2CH2OH(g) CH2CH2OH(aq) Why do things exist as liquids or solids? Intermolecular Forces 131 Review of Terms Dipole ? Polarity Polarizability ATTRACTIVE FORCES Intramolecular forces bonding forces These forces exist within each molecule. They influence the chemical properties of the substance. Intermolecular forces nonbonding forces Electrostatic interactions between molecules. They influence the physical properties of the substance. Enthalpy: the dummy?s definition Heat energy associated with bonding changes Breaking a bond: H2 ? H + H Making a bond: H + H ? H2 Phase Transitions and Intermolecular Forces Strength of Intermolecular Forces High boilng point/melting point Or High DHvap/DHfus = Strong Intermolecular Interactions Low boilng point/melting point Or Low DHvap/DHfus = Weak Intermolecular Interactions London Dispersion Forces Temporary dipole for a very short time. Induced dipole developed from interaction with neighbor. Dipole Forces Hydrogen Bonding H2Te H2Se H2S H2O SbH3 AsH3 NH3 PH3 Aqueous - it?s just a type of solution! What is a solution? What can make a solution? Sapphires Blue = Ti, Fe Purple = V Green, yellow = Fe Pink = Cr Ruby Red = Cr