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Material Type: Exam; Class: INTRO TO CHEMISTRY; Subject: Chemistry; University: SUNY College of Technology at Canton; Term: Fall 2006;
Typology: Exams
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1 Have obtained basic abilities to make observations and measurements in a laboratory situation 2 Have learned the methods of measurement and verification of the theoretical chemical principles learned in the lecture portion of the course. DETAILED LECTURE OBJECTIVES: – The student should be able to: 1 Convert from English units to metric units of measurement and visa versa by the unit conversion method. 2 Calculate the density of a material. 3 Use density as a conversion factor to convert from volume to mass and visa versa. 4 Calculate percent and use percent as a conversion factor. 5 Draw the structure of the atom showing the number of electrons, protons and neutrons for any isotope or ion. 6 State the electron configuration for any atom up to atomic number 36. 7 State the general trends on the periodic chart. (i.e., atomic radius, number of valence electrons, electronegativity, reactivity as a metal or non-metal, ionization energy ) 8 Determine electron configuration from the location of the atom on the periodic chart. 9 Name inorganic chemical compounds. 10 Write the chemical formula of chemical compounds from the oxidation states. 11 Determine molecular mass of compounds. 12 Calculate the number of atoms or formula units of a substance using moles. 13 Calculate the percent composition of a chemical compound. 14 Determine the empirical formula and molecular formula of a compound from the percent composition and/or combustion analysis. 15 Represent a chemical reaction by use of a balanced chemical equation. 16 Predict chemical reactions: composition, decomposition, single replacement, double replacement, and combustion reactions. 17 Calculate amounts of reactants and products in a chemical reaction by using moles of substances (stoichiometry problems) 18 Calculate molarity of a solution and use molarity as a conversion factor. 19 Determine the limiting reactant in a stoichiometry problem. 20 Calculate the concentration of an acid or base by titration. 21 Use the kinetic theory of gases to explain the observed properties of gases. 22 Use the combined gas law and the ideal gas law to calculate the relationship between temperature, pressure, volume, and number of moles of an ideal gas. 23 Apply Dalton’s law of partial pressure to calculations involving mixtures of gases. 24 Calculate the amount of heat a substance absorbs when it undergoes a temperature change. 25 Calculate the amount of heat transfer during a reaction in a calorimeter. 26 Use the first law of thermodynamics (conservation of energy) in calorimeter calculations (q = 0).
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
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:
V. Chemical Reactions VI. Stoichiometry VII. Aqueous Solutions VIII. Gas Laws IX. Atmospheric Gases X. Thermochemistry XI. Chemical Bonding O. DETAILED TOPICAL OUTLINE: I. Unit Conversions, Density, Percent A. Method of problem solving using unit conversion method B. Metric - Metric unit conversions C. Density measurements and using density as a conversion factor D. Percent and percent composition E. Significant figures II. Atomic Theory, Electron Configuration A. Development of the atomic theory B. Number of protons, neutrons, and electrons in different isotopes and different ions C. Atomic mass D. Bohr model of the atom E. Electron configuration and order of filling energy sublevels with electrons F. Orbital diagrams and determining the number of unpaired electrons in an atom G. Quantum numbers III. Periodic Chart A. Classification of the elements: Periodic law and the Periodic Table B. Determining the charge on an atom from the Periodic Table C. Trends on the Periodic Table: atomic radius, ionic radius, electronegativity, reactivity, and ionization energy D. Determination of the electron configuration from the periodic chart IV. Chemical Compounds, Moles A. Concept of the mole to count atoms: Avogadro’s Number B. Naming chemical compounds C. Writing formulas of chemical compounds D. Determination of oxidation states E. Molecular mass V. Chemical Reactions A. Writing chemical equations B. Balancing chemical equations
I. Check-in, safety, Titration Lab, and programming the Excel Spreadsheet II. Density: Determination of the density of a solid and of a liquid and determination of the specific gravity of a solid III. Separation of a Mixture by Physical and Chemical Means IV. Determination of the Formula of a Hydrate V. The Chemistry of a Penny: Determination of the composition and the percent copper in a new penny VI. Analysis of Aspirin by Spectroscopy VII. Types of Chemical Reactions: Observation of chemical reactions and writing the chemical equation representing those reactions VIII. Determination of Calcium Carbonate in Eggshell IX. Identification of a Metal Carbonate or Metal Hydrocarbonate X. Determination of the Molar Mass of a Gas XI. Determining the Heat Capacity of a Metal XII. Thermochemistry
