| Credit- Degree applicable | | Effective Quarter: Fall 2020 | I. Catalog Information
| CHEM 1AH | General Chemistry - HONORS | 5 Unit(s) |
| | (See general education pages for the requirement this course meets.) (Not open to students with credit in CHEM 1A.)
(Admission into this course requires consent of the Honors Program Coordinator.)
Prerequisite: CHEM 25 or CHEM 30A or satisfactory score on Chemistry Placement Test; MATH 114 or MATH 130 or equivalent.
Advisory: EWRT 1A or EWRT 1AH or (EWRT 1AS and EWRT 1AT) or ESL 5. Lec Hrs: 36.00
Lab Hrs: 72.00
Out of Class Hrs: 72.00
Total Student Learning Hrs: 180.00 This course provides an introduction to the structure and reactivity of matter at the molecular level, as well as an application of critical reasoning to modern chemical theory and structured numerical problem-solving. Students will learn the development of molecular structure from rudimentary quantum mechanics, including an introduction to ionic and covalent bonding; chemical problem-solving involving both formula and reaction stoichiometry employing the unit analysis method, and be introduced to thermochemistry and a discussion of the first law of thermodynamics. Additionally, this course is part of the Honors Program.
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| Student Learning Outcome Statements (SLO)
| | | Identify and explain trends in the periodic table. |
| | | Construct balanced reaction equations and illustrate principles of stoichiometry. |
| | | Apply the first law of thermodynamics to chemical reactions. |
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II. Course Objectives | A. | Examine contributions by investigators of diverse cultures and times to the body of chemical knowledge, with an emphasis on physical and chemical conceptual frameworks. |
| B. | Investigate the critical aspects of measurement. |
| C. | Explore the historical development of understanding the structure of the atom. |
| D. | Assess the development of the Periodic Table of Elements in light of modern atomic theory. |
| E. | Differentiate the causes and types of molecular bonding. |
| F. | Appraise the effect of quantum mechanics on formulation of molecular structure. |
| G. | Employ systematic nomenclature to the identification of molecules. |
| H. | Utilize the principles of stoichiometry to analyze compounds, chemical mixtures, and reactions. |
| I. | Examine the prominent characteristics of solutions. |
| J. | Classify the major types of chemical reactions. |
| K. | Apply the essential principles of thermodynamics to chemical systems. |
| L. | Explore in depth advanced topics of general chemistry through problem-solving and/or projects. |
III. Essential Student Materials IV. Essential College Facilities | | Fully equipped chemical laboratory including, at a minimum, the following: consumable chemicals, chemical balances, glassware, molecular models, melting point apparatus, laptops with data acquisition modules, fume hoods, chemical disposal facilities, lockable student storage areas, periodic tables, and laboratory technician. Lecture room with a periodic table. |
V. Expanded Description: Content and Form | A. | Examine contributions by investigators of diverse cultures and times to the body of chemical knowledge, with an emphasis on physical and chemical conceptual frameworks. |
| 1. | Historical development of chemical principles |
| 2. | Application of chemistry to topics such as environmental stewardship and traditional medicine. |
| B. | Investigate the critical aspects of measurement. |
| 1. | Comparison of SI and British systems of units |
| 2. | Problem solving using dimensional analysis |
| 3. | Limitations of measurement and statistical methods |
| a. | Precision versus accuracy |
| C. | Explore the historical development of understanding the structure of the atom. |
| 1. | Historical development of atomic theory |
| a. | Proust's Law of Definite Proportions |
| b. | Dalton's Law of Multiple Proportions |
| d. | Millikan oil drop experiment |
| e. | Thompson cathode-ray tubes |
| f. | Rutherford nuclear deflection experiment |
| a. | Protons, neutrons, and electrons |
| a. | Atomic number, atomic mass, mass number |
| 4. | The Bohr Model of the atom |
| b. | Ground and excited states |
| 5. | Development of modern quantum theory |
| a. | Electromagnetic spectrum |
| b. | Wave-particle duality of light |
| 6. | Implications of elementary quantum mechanics |
| a. | Heisenberg Uncertainty Principle |
| c. | The Born interpretation |
| h. | Extension to polyelectronic atoms |
| 7. | Electronic configurations |
| c. | Pauli Exclusion Principle |
| D. | Assess the development of the Periodic Table of Elements in light of modern atomic theory. |
| 1. | History of the Periodic Table |
| 2. | Periodic trends of the elements |
| 3. | Survey of elemental groups |
| E. | Differentiate the causes and types of molecular bonding. |
| 1. | Types of chemical bonds |
| 2. | Relationship of bond type to electronegativity |
| F. | Appraise the effect of quantum mechanics on formulation of molecular structure. |
| 1. | Lewis structures of organic and inorganic substances |
| b. | Exceptions to the octet rule |
| b. | Hybridization of atomic orbitals in organic and inorganic molecules/ions |
| 3. | Molecular orbital theory |
| a. | Bonding and antibonding orbitals |
| b. | Sigma and pi bonds in simple organic molecules such as alkanes, alkenes, alkynes, and aromatics |
| e. | Homonuclear diatomic molecules |
| f. | Heteronuclear diatomic molecules |
| g. | Delocalized bonding in organic molecules such as benzene |
| G. | Employ systematic nomenclature to the identification of molecules. |
| 1. | Ionic compounds with fixed cation charge |
| 2. | Ionic compounds with variable charge cations |
| 3. | Binary covalent compounds |
| 5. | Simple organic substances |
| H. | Utilize the principles of stoichiometry to analyze compounds, chemical mixtures, and reactions. |
| 1. | Historical development of stoichiometry |
| a. | Law of Conservation of Mass |
| 3. | Percent composition of compounds |
| a. | Calculation from combustion analysis |
| b. | Calculation from given masses |
| 4. | Determine compound formulas |
| 5. | Balance simple chemical equations |
| 6. | Identify limiting reagents |
| 7. | Calculate percent yield |
| I. | Examine the prominent characteristics of solutions. |
| 1. | Homogeneous versus heterogeneous mixtures |
| 3. | Strong and weak electrolytes |
| J. | Classify the major types of chemical reactions. |
| 1. | Precipitation reactions |
| b. | Complete ionic equations |
| 3. | Oxidation-reduction reactions |
| b. | Balancing oxidation-reduction reactions |
| 4. | Combustion reactions in organic substances such as hydrocarbons and alcohols |
| K. | Apply the essential principles of thermodynamics to chemical systems. |
| b. | Chemical and mechanical |
| 3. | First Law of Thermodynamics |
| a. | Exothermic versus endothermic processes |
| b. | Constant pressure versus constant volume |
| L. | Explore in depth advanced topics of general chemistry through problem-solving and/or projects. |
| 1. | Typical problem solving topics may include but are not limited to any of the following: |
| a. | Determine the solutions to the one-dimensional particle-in-a-box electron wavefunctions. |
| b. | Derive an expression for enthalpy from general thermodynamic relationships. |
| 2. | Typical project topics may include but are not limited to any of the following: |
| a. | Explore the historical development of atomic theory from the Greek notion of atomism through to the modern quantum model of atomic structure. |
| b. | Investigate the relationship between hybridization, bonding, and structure in delocalized and/or organic molecules. |
| c. | Investigate the role of molecular orbital theory in the spectroscopy of small molecules. |
VI. Assignments | 1. | Required readings from the textbook in preparation for the scheduled lecture. This may include entire chapters or sections from the chapters covering topics included in this outline. |
| 2. | Required readings from the laboratory manual as a preparation for the scheduled experiment in order to provide students with familiarity about the specific laboratory protocols and related safety precautions necessary for successful completion of the experiment. |
| 1. | Homework assignments based on classroom discussion/lecture may include answering questions from end-of-chapter exercises or other sources as deemed appropriate by the instructor. |
| 2. | Periodic quizzes and mid-term examinations based on material discussed in lectures and/or reading assignments |
| 1. | Pre-lab exercise: The pre-lab assignment for the scheduled laboratory experiment to be completed prior to beginning of each new experiment. This assignment may be identical to that provided in the laboratory manual or substituted with other appropriate assignments determined by the instructor. |
| 2. | Report: Data obtained in laboratory exercises are to be entered in the assigned laboratory manual or a laboratory notebook. Necessary calculations required to obtain the final results from the experiment must be completed in the manual or the notebook as to be determined by the instructor. Detailed lab reports incorporating results and discussions from the experiment will be required. |
| D. | Collaborative activities requiring conversation in small groups. |
| E. | The honors project assignment should include completion of additional sets of advanced problems that require a deeper understanding of the topics and/or a written research report which may include an oral presentation. |
VII. Methods of Instruction | | Lecture and visual aids
Discussion of assigned reading
Discussion and problem solving performed in class
Quiz and examination review performed in class
Homework and extended projects
Collaborative learning and small group exercises
Laboratory experience which involve students in formal exercises of data collection and analysis
Laboratory discussion sessions and quizzes that evaluate the proceedings weekly laboratory exercises
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VIII. Methods of Evaluating Objectives | A. | Homework assignments based on end-of-chapter problems from the primary text will be evaluated for completion to test comprehension of lectures. |
| B. | Periodic quizzes will be used to test the comprehension of topics covered during the lecture and will be evaluated for accuracy of responses. |
| C. | A minimum of two mid-term examinations will be used to evaluate the ability of students to a) solve problems, b) outline various concepts covered in the lecture, and c) demonstrate an understanding of reading assignments. These will be evaluated for accuracy to assess student progress in achieving various learning outcomes. |
| D. | A comprehensive final examination in any chosen format (multiple choice questions or free response) will be based on all the course material covered during the entire quarter and evaluated for accuracy of responses. |
| E. | Pre-lab assignments will be evaluated for completeness and level of preparedness required for safe and timely execution of laboratory protocols and experiments. |
| F. | Report sheets and/or laboratory reports will be evaluated for successful completion of laboratory experiments as well as accuracy of data analysis and interpretation. Students will work both individually and collaboratively towards the completion of the laboratory experiments. |
| G. | A comprehensive laboratory examination or periodic quizzes will be used to evaluate the student understanding of the various concepts discussed in the different experiments performed during the course. Concepts evaluated will include: a) general laboratory protocol b) comprehension of data analysis and interpretation and c) critical thinking as it pertains to the scientific method |
| H. | The honors advanced problems and research report would be evaluated for accuracy of response, depth of analysis, critical thinking skills, and a comprehensive discussion of the research topic. |
IX. Texts and Supporting References | A. | Examples of Primary Texts and References |
| 1. | Silberberg and Amateis. Chemistry: The Molecular Nature of Matter and Change, 8th edition. McGraw-Hill, 2018. ISBN 978-1-259-63175-7. |
| 2. | De Anza Chemistry Department General Chemistry Laboratory Manual (https://www.deanza.edu/chemistry/Chem1A.html) |
| B. | Examples of Supporting Texts and References |
| 1. | Silberberg, Martin. Student Solutions Manual: Chemistry: The Molecular Nature of Matter and Change, 8th edition. McGraw-Hill, 2018. ISBN 978-1259916250 |
X. Lab Topics | 1. | Maintaining a laboratory notebook |
| 2. | Writing laboratory reports |
| 1. | Materials safety data sheets (MSDS) |
| a. | Separation of waste streams |
| b. | Proper disposal methods |
| c. | Environmental hazards of improper waste disposal |
| a. | Maintaining laboratory cleanliness |
| c. | Segregation of chemicals by hazard |
| b. | Limiting chemical exposure |
| e. | Proper use of fire extinguishers |
| 1. | Proper ignition of Bunsen burners |
| 1. | Gravimetric analysis of a hydrate |
| 2. | Relationship of endpoint to equivalence point |
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