Important - Important: 1. Read this material thoroughly if...

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Important: 1. Read this material thoroughly if you expect to try for advanced placement and extra credit which counts towards graduation. 2. Study the topics listed in the attached outline. 3. Work many practice problems listed at the end of the corresponding chapters in textbooks. 4. Come to the examination rested. No one can do well on an exam when excessively fatigued. You should therefore try to rest before taking the exam for credit. If your trip to campus requires travel into the late hours of the night, or a very early departure form your home, you might be advised to allow for one nights rest in the Lafayette area before taking the examination. Many students who are unsuccessful with the examination tell us that failure to take this advice contributed to their inability to complete the examination successfully. Please consult your advanced credit schedule or your academic advisor for both the time and place of the examination. PURDUE UNIVERSITY Chemistry 112 Study Guide This study guide lists the topics or terms that should be mastered before you attempt the examination for credit in Chemistry 112. The material can be found in a number of books on the market. A list of possible textbooks is given below. Attached is a sample Chemistry 112 final exam along with the answers. Suggested Texts for study: Fundamentals of Chemistry, by Ralph Burns, 2nd edition, Prentice Hall. Fundamentals of General, Organic, and Biological Chemistry, by John Holum, Wiley. Chemistry, The Central Science, by Brown, Lemay, Bursten, Prentice Hall. Chemistry Principles and Practice, by Reger, Goode, Mercer, Saunders. Other Resources: Throughout the year, Chemistry 112 final exams (only) are on file at the Stewart Copy Center (STEW G-66). During the Fall and Spring semester; old Chemistry 112 hourly exams are available in the Chemistry Resource Room (WTHR 117). 2 Gases Atmosphere Kinetic Molecular Theory Kinetic Energy Atmospheric Pressure, definition and units Boyles' Law, Charles's law, Gay-Lussac's Law, Combined Gas Law Standard Temperature and Pressure (STP)
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Molar Volume and Gas Density Ideal Gas Law; universal gas constant Real Gases Dalton's Law of partial Pressures Vapor Pressure Gas Stoichiometry Diffusion Liquids and solids Intramolecular forces - bonding types Intermolecular forces - attractions of molecules one for another - as a group called van der Waals hydrogen bonding Dispersion forces (London forces) Dipole forces Vaporization and condensation Boiling point Heat of Vaporization, Heat of fusion, specific heat Heating and cooling curves Amorphous solids, crystalline solids (ionic, molecular, covalent network, metallic) 3 Solutions Homogeneous, heterogeneous Solute, solvent Miscible, immiscible, soluble, insoluble, concentrated, dilute, hydration, solvation Effects of temperature and pressure on solubility Saturated and unsaturated Solubility of gases in liquids Solution Concentration Expressions: Molarity, percent by volume, percent by mass, parts per million (ppm), parts per billion
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This note was uploaded on 04/03/2011 for the course CHEM 112 taught by Professor Harwood during the Spring '11 term at Purdue.

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Important - Important: 1. Read this material thoroughly if...

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