Class: PRINCIPLES OF CHEMISTRY MWF 10:30AM 11:20AM CB1 121 Office CH 226 Phone 407-823-1167 Email david.roberts@ucf.edu Recitation Session: - T - 12:30PM - 1:20PM - CB1 105 Recitation Session: CHS 1440.0022 PRINCIPLES OF CHEMISTRY - T - 3:30PM - 4:20PM - CB1 319 Recitation Session: CHS 1440.0023 PRINCIPLES OF CHEMISTRY - R 10:30AM 11:20AM CB1 103 Recitation Session: CHS 1440.0024 PRINCIPLES OF CHEMISTRY R -11:30AM - 12:20PM - CB1 103 Recitation Session: CHS 1440.0025 PRINCIPLES OF CHEMISTRY R - 1:30PM - 2:20PM - CB1 103 Principles of chemistry is a one semester college course. This satisfies UCF general chemistry degree requirement, with an emphasis on materials and their application to engineering systems. You'll begin with an exploration of the fundamental relationship between electronic structure, chemical bonding, and atomic order, then proceed to the chemical properties of "aggregates of molecules," including crystals, metals, semiconductors, solutions and acid-base equilibria, polymers, and biomaterials. Real-world examples are drawn from industrial practice (e.g. semiconductor manufacturing), energy generation and storage (e.g. automobile engines, lithium batteries), emerging technologies (e.g. photonic and biomedical devices), and the environmental impact of chemical processing (e.g. recycling glass, metal, and plastic). Is This Course for Me? This is not "just a chemistry class" - it's a chemistry-centered class that integrates examples from the world around us, in the arts and humanities, the human stories behind the science, and applications to engineering and emerging technologies. Learning Objectives Upon successful completion of CHS 1440, students will have accomplished the following general learning objectives. General Predict the properties and interactions of chemical substances by understanding their composition at the atomic level, making connections to structure, bonding, and thermodynamics as necessary. Determine and apply principles of materials science (specifically microstructure design and selection) to the selection of materials for specific engineering applications. Expectations How much time will this class take? At UCF, this class meets 3 times per week, with three one-hour lectures by Mr. Roberts, and onehour recitation sessions divided into several sections. Can I work with others? Homework: At UCF, homework for this course is not graded. You should consider working assigned owl problems to be an essential part of developing your knowledge. At UCF, working together in
groups on is common and even encouraged. If you'd like to connect with others working on this course. Self-Assessment: The self-assessment and exam portions you should work on your own.. They are intended for you to demonstrate your mastery of the material. You should work these problems on your own, closed-book, using only a calculator, a periodic table and list of fundamental constants. Required Textbook and Supplies Chemistry for Engineering Students, 3rd edition, Lawrence Brown and Thomas Holme (Brooks/Cole-Cengage Learning) The book is available in a number of formats: Traditional hardcover textbook, Loose leaf textbook including e-book access and OWL access code You should choose whichever format you believe will work best for you. You will have an option of using OWL to do additional practice problems, but those will not count for course credit. Class Information and Announcements Announcements regarding schedule changes or other developments will be made in class at the earliest possible time. Information will also be available electronically via e-mail and the web. The class website can be found at UCF online on Canvas. This site offers a broad array of class information, including copies of the slide files used in class, old exams, and announcements. Course-related email: I will often distribute class announcements by email. The only simple way to do this is through the Canvas system, which lets me send mail to the entire class roster. So any message I send out concerning class announcements will always go to your Canvas address. Please be sure to check that account regularly, or to set up a forwarding instruction if you prefer. Course Evaluation: Weekly Quizzes: These short quizzes are representative of the homework in classes, and an indication of the knowledge you should have in preparing for the exam and will be given in recitation. 3 Exams and Exam Problems: Exam will take place at logical breaks in the course( See Schedule).These problems based on homework and quizzes verify that you've developed the appropriate depth of understanding and application. Missed Exams There will be no regularly scheduled make-up exams. In the event that you miss an exam due to a university-approved absence, you should consult with me as soon as possible to discuss your situation. If possible, you should discuss your absence with me before the exam is given. Final Exam The Final Exam will be a two-hour and 50 minutes, 150-point test covering all material taught during the Semester according to the university s final exam schedule.
Schedule: Dates-Week of and Readings Lecture /Class Activities August 18 1-3 define the words atom and molecule in your own words. paraphrase the atomic theory of matter. recognize various representations for molecules, including formulas, models, and structural drawings. obtain a correct chemical formula from a line drawing of an organic molecule. perform simple unit conversions and numerical calculations involving numbers in scientific notation and/or units with common metric prefixes. explain the definition of a mole in your own words. calculate the molar mass of a substance from its chemical formula. interconvert between mass, number of molecules, and number of moles. calculate the mass % composition of a substance from its chemical formula. determine a chemical formula from elemental analysis data ( i.e., from % composition). August 25 4-6 recognize some common types of chemical reactions (decomposition, combustion, etc.). explain balancing a chemical equation as an application of the law of conservation of mass. list at least 3 quantities which must be conserved in chemical reactions. write balanced chemical equations for simple reactions, given either an unbalanced equation or a verbal description ( i.e., nitrogen and hydrogen gases react under appropriate conditions to form gaseous ammonia (NH 3)). interpret chemical equations in terms of both moles and molecules.. define the concentration of a solution, and calculate the molarity of solutions from various data. distinguish between electrolytes and non-electrolytes, and explain how their solutions differ. describe the species expected to be present (ions, molecules, etc.) in various simple solutions. recognize some ionic compounds from their formulas. calculate the amount of product expected to be formed in a chemical reaction, given the amounts of reactants used. ("Amount" might refer to either mass or number of moles.) calculate the amount(s) of reactants which need to be used in a chemical reaction in order to produce a specified amount of product. ("Amount" might refer to either mass or number of moles.) September 1 7-9 Exam 1: 9/3 write both molecular and ionic equations for solution reactions. define acid and base. identify some common acids and bases.
distinguish between strong and weak acids or bases, and describe the species expected to be present in their solutions. write equations for acid-base reactions. calculate solution concentrations from titration data. perform stoichiometric calculations involving reactions in solutions, including precipitation reactions. September 8 10-12 demonstrate your mastery of the material from Classes 1-8. perform simple gas calculations. state the postulates of the kinetic theory of gases. describe how the postulates of kinetic theory account for the gas laws (qualitatively). identify conditions under which gases might behave non-ideally. describe the Maxwell-Boltzmann distribution of speeds, and the effect of temperature and molar mass on molecular speed. September 15 13-15 t describe waves in terms of frequency, wavelength, and amplitude. interconvert between frequency, wavelength, and amplitude for light. describe interference as a wave property. relate properties of light such as color and brightness to wave characteristics (i.e., lambda, nu, etc.). describe the photoelctric effect by stating what sort of experiment is involved and what results are seen. explain how the results of the photoelectric effect experiment are consistent with a photon model of light. use the Planck equation to calculate the energy of a photon from wavelength or frequency. September 22 16-18 describe in your own words what is seen when atoms absorb or emit light. use conservation of energy ideas to explain how the observation of atomic spectra implies that atoms have quantized energies. draw an energy level diagram for a simple atom. use an energy level diagram to predict the wavelengths or frequencies of light an atom will absorb or emit, or use the observed wavelengths or frequencies to determine the allowed energy levels define ionization energy. appreciate that the idea of energy levels has its origins in measurable experimental data. describe what happens in photoelectric spectroscopy, and explain how the results show that electrons in atoms have only certain allowed energies. given a photoelectron spectrum, determine the element to which the data correspond paraphrase the uncertainty principle. recognize how quantum numbers arise as a consequence of the wave model. define the term "orbital."
state the meanings of the quantum numbers n, l, ml, and ms, and list the allowed values for each quantum number. identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa. list the number of orbitals of each type (1s, 3p, etc.) in an atom. September 29 19-21 Exam-2 October 1 define the following properties of atoms: atomic radius, ionization energy, electron affinity. state how the above properties vary with position in the periodic table. explain the periodic variation of atomic properties in terms of orbitals and shielding. list several physical properties which distinguish metals and non-metals. use electron configurations to explain why metals tend to form cations while non-metals tend to form anions. define electronegativity, and state how electronegativity varies with position in the periodic table. recognize how quantum numbers arise as a consequence of the wave model. identify/predict polar, non-polar, and ionic bonds by comparing electronegativities. write Lewis electron structures for simple molecules or ions. October 6 22-24 write Lewis electron structures for simple molecules or ions. describe chemical bonding in simple molecules using a model based on the overlap of atomic orbitals. recognize some of the limitations of this simple model appreciate that molecular geometries can be measured experimentally. state how hybridization reconciles observed molecular shapes with the orbital overlap model. predict the geometry of a molecule from its Lewis structure. rationalize common molecular geometries in terms of orbital overlap and hybridization. October 13 25-27 use models (real and/or software) to help visualize the common molecular shapes. use the basic shapes we've examined to determine the geometry of larger molecules. explain the formation of multiple bonds in terms of overlap of a combination of hybridized and unhybridized atomic orbitals. identify sigma and pi bonds in a molecule, and explain the difference between them explain how band diagrams can be used to represent the bonding in an extended solid structure. draw band diagrams for metals and insulators identify a material as metal or insulator from its band diagram. explain how the electrical properties of metals and insulators are related to
their chemical bonding. October 20 28-31 use tabulated bond energies to obtain approximate values of ΔE for chemical reactions. define exothermic and endothermic in your own words. explain (in your own words) the significance of kinetic and thermodynamic factors in controlling chemical reactions. define work and heat using the standard sign conventions explained in your book. define state functions, and explain their importance. state the first law of thermodynamics in word and in equation forms. use experimental data to obtain values for ΔE for a chemical reaction. use experimental data to obtain values for ΔE and ΔH for chemical reactions. define ΔH f. write formation reactions for compounds. October 27 32-35 explain Hess's Law in your own words. calculate the amount of energy liberated or consumed in chemical reactions from tabulated data. obtain thermodynamic data (i.e., ΔH f) from lab measurement explain entropy in your own words in terms of atomic and molecular order. deduce the sign of ΔS for many chemical reactions by examining the physical state of the reactants and products. state the Second Law of Thermodynamics, in words and equations, and use it to predict spontaneity. state the Third Law of Thermodynamics. use tabulated data to calculate ΔS for a chemical reaction.. state the Third Law of Thermodynamics. use tabulated data to calculate ΔS for a chemical reaction. use tabulated data to predict the spontaneity of a chemical reaction. derive the relationship between the free energy change of a system and the entropy change of the universe. use tabulated data to calculate the free energy change for a chemical reaction. explain the role of temperature in determining whether a reaction is spontaneous. use tabulated data to determine the temperature range for which a reaction will be spontaneous. November 3 36-38 Exam -3: November 5 define the rate of a chemical reaction, and express the rate in terms of the various reactants or products. use experimental data to determine rate laws for reactions by the method of initial rates.
use experimental data to determine rate laws for reactions using graphical methods. distinguish between elementary reactions and multi-step reactions. find the rate law predicted for a particular reaction mechanism. November 10 39-41 explain (in your own words) the significance of the terms in the Arrhenius equation based on collision theory. calculate the activation energy for a reaction from experimental data. realize that equilibrium is dynamic, and that at equilibrium, the forward and backward reaction rates are equal. Be able to state these ideas in your own words.. November 17 November 24 December 2 42-44 Thanksgiving 45-47 define the equilibrium constant for a reversible reaction. calculate equilibrium constants from experimental data. calculate the new equilibrium composition of a system after an applied stress. explain the connection between K eq and ΔG. December 9 Final Financial Aide Statement: Institutions must now verify that every student enrolled in every course has met this standard, and we must be able to gather that information as soon as possible but by no later than the middle of the second week of the course (August 27 in the case of the Fall 2014 semester) As of Fall 2014, all faculty members are required to document students' academic activity at the beginning of each course. In order to document that you began this course, please complete the following academic activity Financial Aide Activity by the end of the first week of classes, or as soon as possible after adding the course, but no later than August 27. Failure to do so will result in a delay in the disbursement of your financial aid.
Important Dates: Classes Begin: Monday, August 18, 2014 Withdrawal: Monday, October 27, 2014 11:59 PM Final Examination Period: December 8, 2014 10-1250