Course Outline of Introduction to Chemistry | CHEM 101, Exams of Chemistry

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STATE UNIVERSITY OF NEW YORK COLLEGE OF TECHNOLOGY CANTON, NEW YORK COURSE OUTLINE CHEM 105 - COLLEGE CHEMISTRY I PREPARED BY: NICOLE HELDT SCHOOL OF SCIENCE, HEALTH, AND PROFESSIONAL STUDIES SCIENCE DEPARTMENT MAY 2006 27 Describe the significance of an enthalpy diagram to determine whether it is exothermic or endothermic and to determine the activation energy. 28 Use Hess’s Law of summation of enthalpy of formation to calculate the enthalpy change of a reaction. 29 Describe the structure and composition of the atmosphere. 30 State the sources and the effects of constituents of the atmosphere, such as nitrogen oxides, sulfur oxides, ozone, carbon dioxide, and smog. 31 Draw appropriate Lewis structures for ionic and covalent compounds including resonance contributing structures. 32 Assign formal charges to atoms in a Lewis structure. 33 Determine the most likely to least likely Lewis structure. 34 Identify and draw exceptions to the octet rule in certain covalent Lewis structures. 35 Determine the shapes of covalent molecules by applying Valence Shell Electron Pair Repulsion Theory (VSEPR). 36 Determine if a molecule is a dipole or a non-polar molecule from electronegativity difference and from the shape of the molecule. DETAILED LABORATORY OBJECTIVES: The student should be able to: (Excel Spreadsheets) 1 Write an Excel spreadsheet in order to use it as a data sheet in the laboratory. 2 Program an Excel spreadsheet in order to do the necessary calculations on the laboratory data. 3 Use the computer program, Graphical Analysis (G/A) or Excel to do computer graphing. 4 Titration Lab (a) Be able to perform the titration technique (b) Be able to determine the endpoint of a titration using an indicator (c) Determine the concentration of an acid from the known concentration of a base and the known volumes of both the acid and base. 5 Density Lab (a) Determine the density and the specific gravity of a substance. (b) Determine the density of a solution at different concentrations. (c) Plot a calibration curve of density versus concentration in order to determine the concentration of an unknown solution. 6 Separation of a Mixture (a) Separate a mixture into its components by physical and chemical means. (b) Calculate the percent of each component in a mixture. 7 The Chemistry of a Penny (a) Determine the composition of a U.S. penny. (b) Determine the year that the composition of a U.S. penny was changed. (c) Determine the density of a new U.S. penny. (d) Use the spectrophotometer to determine the absorbance concentration data of a solution in order to plot a absorbance - concentration calibration graph. (e) Use the calibration graph to determine the concentration of an unknown solution. 8 Formula of a Hydrate (a) Determine the percent water of hydration in a compound. (b) Determine the formula of a hydrated material. 9 Types of Chemical Reactions (a) Classify chemical reactions into 5 types: combustion, composition, decomposition, single replacement, and double replacement. (b) Predict and balance chemical reactions that are of the general type mentioned. (c) Make observations to indicate that a chemical reaction has occurred. 10 Determination of Calcium carbonate in Eggshells (a) Use stoichiometry to determine the amount of calcium carbonate in an eggshell from the amount of products that are produced when the eggshell is reacted with a strong acid. (b) Calculate the percent calcium carbonate in the eggshell and compare two different methods for determining its amount. 11 Analysis of Aspirin by Spectroscopy (a) Be able to make solutions of a known Molarity. (b) Be able to dilute solutions and calculate the molarity of those solutions. (c) Be able to use pipettes and volumetric flasks in making solutions. (d) Be able to use spectroscopy to determine the amount of light absorbance of a sample of known concentration and to apply Beer’s Law to show the relationship of absorbance to concentration. (e) Be able to create a standard curve for absorbance versus concentration of know solutions which can be used to determine the concentration of an unknown solution from its measured absorbance (f) Be able to use spectroscopy to analyze the amount of acetylsalicylic acid in over the counter analgesics. 12 Identification of a Metal Carbonate (a) Use physical and chemical properties of a compound to identify what compound that it is. (b) Use stoichiometry calculations to predict how much product should form from a chemical reaction. 13 Determination of the Molar Mass of a Gas (a) Apply Dalton’s Law of Partial Pressure to calculate the total pressure of a gas when collected over water. (b) Measure the factors necessary to define the quantity of a gas: pressure, temperature and volume. (c) Use the laboratory measurements of temperature, mass, pressure and volume to determine the molecular mass of a gas. 14 Specific Heat Capacity Lab (a) Determine the specific heat capacity of several different metals. (b) Define what specific heat is and determine on what factors it depends. (c) Apply the law of conservation of energy to a calorimeter and calculate heat gains and losses from different substances. 15 Thermochemistry (a) Use a calorimeter to calculate the heat given off by a chemical reaction. (b) Use Hess’s Law to determine the heat of a reaction J. TEXTS: General Chemistry: Principles and Modern Applications, Ninth Edition, Petrucci, Harwood and Herring, 2002, Prentice Hall, Inc. Laboratory Manual: College Chemistry I CHEM 105 Laboratory Manual, Leedom and Heldt, Fall 2006, Canton College Duplicating. K. EQUIPMENT: Lecture facilities for 60 students, various demonstration-equipment, computers with word processing, spreadsheet and computer graphing capabilities, and laboratory facilities for 18 students per lab. L. GRADING METHOD: 90 - 100 A 85 - 89 B+ 80 - 84 B 75 - 79 C+ 70 – 74 C 65 - 69 D+ 60 - 64 D < 60 F M. MEASUREMENT CRITERIA/METHODS: 1. Class Grade (quizzes, exams, graded homework) 55 % 2. Laboratory Grade 25 % 3. Comprehensive Final Exam 20 % N. GENERAL TOPICAL OUTLINE: I. Unit Conversions, Density, Percent II. Atomic Theory, Electron Configuration III. Periodic Chart IV. Chemical Compounds, Moles