Course CRN Credits Days Time Start - End Dates Location Schedule Type

Transcription

1 MONTGOMERY COLLEGE Physical Science Department Takoma Park Campus Instructor: Solomon Teklai CH 101 Principles of Chemistry (I) CH101 Syllabus for Spring 2010 Phone: (240) Office hours: Tu & Th 4:25-4:55pm Dept. phone: (240) Th. 9:30 10:30 am Wed & Fri 11:00-11:30am Office location: SN315 or by Appointments or just stop by my office Course CRN Credits Days Time Start - End Dates Location Schedule Type CH MWF 10:00 am - 10:50 am 01/25/10-05/16/10 SN 309 Lecture Course Description: First of two related courses (with CH 102), this course includes concepts of atomic structure, periodic system, chemical bonding, nomenclature, stoichiometry, weight relationships, kineticmolecular theory, gases, liquids and solids, solutions, chemical reactions, and thermochemistry. (NSLD) PREREQUISITE: Within the past five years, a grade of C or better in either one year of high school chemistry or in CH 100A, or consent of department. PRE- or COREQUISITE: MA 101 or MA 103. Assessment levels: EN 101/101A, RD 120. Three hours lecture, one hour discussion, three hours laboratory each week. TEXT: Chemistry, A Molecular Approach, by Nivaldo J. Tro ISBN: ISBN: Available at Reference Desk in Library LAB MANUAL: Slowinski, Wolsey, and Masterton, Chemical Principles in the Laboratory, 8th or 9 th Ed., Saunders, 2005 or ISBN Or ISBN 13: OPTIONAL: Study Guide, Solutions Manual (Available Reference Desk, Library), gloves for laboratory work must be supplied by student. GOGGLES: OSHA approved chemistry goggles are required for working in laboratory. NOT PERMITTED FOR TESTS OR QUIZZES: Graphing Calculators INFORMATION: There will be four tests and the percentage grade on the final exam; the best three grades of these five grades will be used to calculate the final grade. There will be a quiz most every week in which there is no test. From more than 8 quizzes the best 8 quiz scores will be used in computing your grade. There are no make-up quizzes or tests. All electronic communications will be taken through Montgomery College accounts; therefore, all students are required to activate their Montgomery College accounts. Check for study guide and sample exam questions on mymc POINT DISTRIBUTION: 3 hour 100 points each 40% Online or in class quizzes and assignments 10% Laboratory grade 25% Final exam 25% Total 100% 1

2 FINAL COURSE GRADE: A 90% and above B 80% - 89% C 70% - 79% D 60% - 69% F below 60% Important Dates: JAN - 31 Last day to drop classes and get a refund FEB-14 Last day to drop a course without a grade being recorded, change from credit to audit, or change from audit to credit APR-18 Last day to drop classes with a grade of "W" Exam Exam I on 2/22, Exam-II on 3/24, Exam-III on 4/16, & Exam IV 5/3 Final Exam May 10 from 10:15am-12:15pm Look for the final Exam date on the MY MC website for your other classes Withdrawal from a course is the responsibility of the student. Classroom Policies: Attendance: You are expected to attend all classes. If you have more than two unexcused absences during the semester, you may be dropped from the class. Academic Honesty: You are expected to be honest in reporting your laboratory results and when taking any kind of tests. Any dishonesty in the classroom, such as copying someone else s results or using notes or books during testing, may result in a zero grade. Classroom Conduct: You are expected to behave appropriately in an academic setting. Any use of inappropriate language in the classroom will be grounds for disciplinary action. Support Services: There are several support services available to help you in this course. These are available at the Math Science Learning Center and Library. A student who may need an accommodation due to a disability should make an appointment to see me during my office hours. A letter from Disability Support Services (DSS) authorizing your accommodations will be needed. The DSS office is located in room 122 Student Services Pavilion and may be called on or 1480 and TTY If you are a veteran or on active or reserve status and you are interested in information regarding opportunities, programs and/or services, please visit the Combat2College website at and/or contact Joanna Starling /SV103 or Joanna.starling@montgomerycollege.edu. Tobacco Free Policy: On August 1, 2008, Montgomery College implemented a Smoke and Tobacco Free Policy which prohibits smoking or the use of other tobacco products on any of its campuses or other property. Students who smoke or use tobacco products will be considered in violation of the student conduct code and their behavior will be reported to the Dean of Student Development s office for the appropriate disciplinary action including probation, suspension, or dismissal. If you have any questions about this new policy, please contact the Vice President and Provost s Office, the Office of the Dean of Student Development or the Campus Security Office. Cancellation of Classes: If classes are cancelled due to inclement weather, information will be available by calling or listening to local television and radio stations.. To access assignments on students must: 1. Register at using the registration code that is in their Student Access Kits. 2. Log out of the registration process and go to again. 3. Log in at 2

3 You will be asked for a course ID and a student ID. The student ID can be anything you please; for example, use your last four digits of university ID For your course, the course ID should be: MCTEKLAI24735 Once you have done that, you will be enrolled. MCTEKLAI24735 Remember, to get credit, you must do the assignments in the Assignment List, do not work in the Study Area to earn credit. # Outcome 1. Use dimensional analysis as a technique for solving problems and report the answer with the appropriate number of significant figures. 2. Do mole and stoichiometry calculations. 3. Analyze and solve various problems that include a combination of concepts from various chapters. 4. Predict the quantitative behavior of gases and solutions. 5. Determine solution concentrations and calculate the amounts of materials involved in solution reactions. 6. Calculate the magnitude and direction of heat flow for physical and chemical changes. 7. Name and write symbols for elements, ions, and compounds. 8. Write balanced molecular, ionic, and net ionic equations and predict the products of various types of reactions. 9. Identify chemical and physical properties. 10. Describe the major components of the atom and their location in the atom. 11. Predict the qualitative behavior of gases, liquids, solids, and solutions. 12. Use the Periodic table to predict relative properties of elements and formulas of compounds, formula masses, electron configuration, and periodic trends. 13. Predict the types of intramolecular forces within a substance and intermolecular forces between substances and in solution. 14. Use types of chemical bonding and Lewis dot structures to predict the geometry, polarity, and properties of compounds. 15. Describe the chemical bonding between atoms on the basis of atomic structure. 16. Locate safety equipment and work safely in the laboratory. 17. Demonstrate proper waste disposal. 18. Successfully use chemistry laboratory techniques such as filtration, collection of gases, precipitation, weighing, titration, etc. 19. Make observations, collect and interpret data, and do calculations. 20. Apply chemical principles to explain results. CH 101 Chemistry, A Molecular Approach, by Nivaldo J. Tro Learning Objectives WEEK TEXT CHAPTER OBJECTIVES LAB Chapter 1 Matter, Measurement, and Problem Solving Check-in, Lab Week #1 Safety, 1. Differentiate between the three states of matter. Measurement & 2. Distinguish between elements, compounds, and mixtures. Significant 3. Give the symbols and names for elements 1-38, and selected others. Figures 4. Distinguish between physical and chemical properties and between physical and chemical changes. 5. Convert temperatures among the Fahrenheit, Celsius, and Kelvin scales. 6. Perform calculations involving density. 7. Report and determine the number of significant figures in a measurement. 8. Express the result of a calculation with the proper number of significant figures. 9. Know the SI units of measurement and prefix multipliers. 10. Convert between units using dimensional analysis. 3

4 HW on Ch-1 Page- 40 problems 69, 71, 75, 77, 79, 83, 89, 91, Chapter 2 Atoms and Elements 1. Describe the various aspects of modern atomic theory. 2. List and describe the major subatomic particles in terms of relative charge, mass, and location in an atom. 3. Use atomic number and mass number to describe the composition of an atom. Week #2 Chapter 2 Atoms and Elements 4. Calculate the average atomic mass of an element given its distribution of isotopes and isotopic masses. 5. Give the charges of the ions of the main group elements. 6. Locate, name, and identify members of the various groups, periods, and types of elements on the periodic table. 7. Interconvert molar mass, moles, and number of particles for elements. HW on Ch-2 Page- 79 problems 53, 55, 59, 60, 61, 62, 63, 65, 69, 71, 73, 74, 77, 78, 79, 80, 81ab, 82ab, 83, 84, 85ab Week #3 Chapter 3 Molecules, Compounds and Chemical Equations 1. Identify a substance as ionic or molecular from its formula. 2. Name ionic and molecular compounds. 3. Calculate formula masses and molar masses of compounds. 4. Interconvert molar mass, moles, and numbers of particles for compounds. 5. Calculate the percent composition by mass of a compound from its formula. 6. Determine the empirical formula for a compound from percent composition data. 7. Determine the molecular formula of a compound from its molar mass and empirical formula. 8. Write and balance chemical equations HW on Ch-3 Page- 124 problems 33, 34, 35, 36, 37, 39, 41, 43, 45, 46, 49, 51, 52, 53, 54, 55, 57, 59, 60, 65, 75ab, 77ab, 79, 81, 85, 87, 94, 97, 98, 99, 100 Week #4 Chapter 4 Chemical Quantities and Aqueous Reactions 1. Do calculations involving the stoichiometry of a reaction. 2. Identify limiting and excess reagents in a reaction mixture. 3. Calculate the theoretical and percent yields for reactions with a limiting reactant. 4. Interconvert molarity, moles, and volume. 5. Make dilution calculations. 6. Make stoichiometry calculations for reactions in aqueous solution. Exp-1 The density of Liquids and Solids Exp-3/ Handout Fractional Crystallization Exp-6 Properties of hydrates HW on Ch-4 Page- 177 problems 25, 27ab, 33ab, 37ab, 41a, 43ab, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 68, 69, 70, 71, 75, 77, 79, 81, 83, 85, 86, 87, 89 Exam I on 2/22, ( Chapter 1, 2, 3 & part of 4 ) Week #5 8. Classify substances as electrolytes (strong or weak) or nonelectrolytes. 9. Use solubility rules to determine if a precipitate forms and if so, the identity of the precipitate when two solutions are mixed. 10. Identify common strong and weak acids and bases. 11. Write and balance molecular, ionic, and net ionic equations for precipitation reactions and acid-base reactions. 12. Assign oxidation numbers to each atom in a compound. 13. In a redox reaction, identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent. 14. Identify reaction types: precipitation, acid-base, and oxidation-reduction. Week #6 Chapter 5 Gases 1. Interconvert units of pressure. 2. Use the empirical gas laws in calculations. Exp-24 A/Handout Standardization of a basic solution Exp-30 Determination of Iron with 4

5 3. Use the ideal gas law in calculations. Permanganate 4. Use the ideal gas law to calculate the molar mass or density of a gas. 5. Use Dalton's law to calculate the partial pressure of gas in a mixture. 6. Solve stoichiometry problems involving gas volumes. 7. Use the Kinetic-Molecular Theory to explain each of the gas laws. 8. Use Graham's law of effusion to relate the relative rates of effusion of two gases. 9. State and explain the conditions under which a gas behaves more ideally. HW on Ch-5 Page- 230 problems-29, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 59, 61, 63, 65, 67, 69, 71, 73, 75, 77, 79, 81, 83, Week #7 Spring Break 3/15-3/20 3/15-3/20 Week #8 Chapter 6 Thermochemistry 1. Define potential energy and kinetic energy. 2. Define and do calculations with internal energy, heat, and work. 3. Use calorimetry to determine the specific heat of a substance or an enthalpy change for a reaction. 4. Write and manipulate thermochemical equations. 5. Determine if a reaction is endothermic or exothermic from its enthalpy change. 6. Apply Hess's Law to calculate the enthalpy change for a reaction. 7. Identify standard conditions and calculate enthalpy changes from standard enthalpies of formation. HW on Ch-6 Page- 274 problems 31, 33, 35, 37, 39, 41, 45, 47a &b 49,51, 53, 55, 56, 61, 65, 69, 71, 72, 73, 77, 79, 83, Week #9 Chapter 7 The Quantum- Mechanical Model of the Atom 1. Interconvert wavelength and frequency and the energy of electromagnetic radiation. 2. Compare the energy, wavelength and frequency of electromagnetic radiation. 3. Explain the wave/particle nature of matter and energy. 4. Relate quantum numbers to the size, shape, and energy of atomic orbitals. 5. Sketch the s, p, and d orbitals. Exam-II on 3/24 ( Chapter 4 6 ) Week #10 Chapter 8 Periodic Properties of the Elements 1. Explain the Pauli Exclusion Principle and the Aufbau Principle. 2. Write the electron configuration and use Hund's Rule to write the orbital diagram for an atom. 3. Correlate the electron configuration of an atom with its position in the periodic table. 4. Use the periodic table to identify the valence shell electron configuration for an atom. 5. Explain how effective nuclear charge can be approximated. 6. Explain the general trends in size, ionization energy, electron affinity and metallic character for atoms. 7. Given a set of atoms, determine the order of atomic size, ionization energy, electron affinity and metallic character. 8. Write the electron configuration for ions. 9. Determine the relative sizes of a given set of ions. Week #11 Chapter 9 Chemical Bonding I: Lewis Theory 1. Use Lewis electron dot structures to represent the formation of an ionic compound. 2. Use Coulomb's law to give relative lattice energies for ionic compounds. 3. Use relative electronegativity values to identify a bond as ionic, polar covalent, or pure covalent. Predict which of two bonds is more polar. 4. Indicate the direction of the polarity of a polar bond. 5. Write Lewis structures for covalent compounds and polyatomic ions, including exceptions to the octet rule. 6. Write resonance forms for covalent compounds where appropriate. 7. Assign formal charges to atoms in Lewis structures and use them to determine the most likely Lewis structure. 8. Relate bond order and bond length. 9. Estimate H from bond energies. Exp-35 Spot Tests for Some Common Ions Handout Weights of Pieces of Magnesium Exp-14 Heat Effects and Calorimetry Handout Determination of Iron in a Vitamin Pill Week #12 Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital 5

6 Theory 1. Use the VSEPR model to predict the geometry of simple molecules and polyatomic ions. 2. Determine the polarity of a molecule from its Lewis structure and molecular geometry. 3. Assign the types of hybrid orbitals used by atoms in a simple molecule or polyatomic ion. Describe the formation of sigma and pi bonds from atomic orbitals and identify them in Exp Alkaline Earths and Halogens molecules. 5. Describe the delocalization of electrons Exam-III on 4/14, ( Chapter 7 9 & part of 10 ) Week #13 Chapter 11 Liquids, Solids, and Intermolecular Forces 1. Identify the types of intermolecular forces present between molecules. 2. Based on intermolecular forces, predict the relative boiling points of substances. 3. Calculate the heat required for a phase change for a given mass of a substance. 4. Explain the relative values of the physical properties of liquids (vapor pressure, surface tension, and viscosity). 5. Use the heat of vaporization and hear of fusion in heating curve calculations. 6. Use the phase diagram to describe physical changes as temperature or pressure changes. 7. Sketch a phase diagram, labeling the axes and each of the regions, and locate the triple point, critical point, normal melting point, and the normal boiling point. 8. Identify types of crystalline solids and explain their relative melting points. Week #14 Chapter 12 Solutions 1. Explain the phrase "like dissolves like," and predict the relative solubilities of specific solutes in various solvents. 2. Explain the energetics of solution formation. 3. Explain temperature and pressure effects on the solubility of gases. 4. Define and perform calculations with the concentration units: mass percent, ppm, ppb, mole fraction, molarity, and molality. 5. Define and give examples of colligative properties of solutions. 6. Perform calculations involving boiling point elevation and freezing point depression data. 7. Determine and use the van thoff factor for ionic solutions. Exp-13 Geometrical Structure of Molecules Lab Practical Exam, Check-out Exam IV 5/3 ( Chapter ) Week #15 Final Exam May 10 from 10:15am-12:15pm 6