Course Discipline and s2

GAVILAN COLLEGE CURRICULUM DEVELOPMENT

FORM C Modify or Inactivate an Existing Course Date: 12/01/09 Prepared & Submitted by: D. Clark Department: Chemistry Course Discipline and Number: Chem 1A

1. What is the effective term? Fall Spring Summer Year: 2010

2. Inactivate Course(s): (Inactivating a course will remove it from the course catalog. Courses may be re- activated by updating the course and bringing it back to the Curriculum Committee for approval. Transferable courses will need to be re-articulated, should you decide to reactivate the course.)

Reason for inactivation:

3. Modification of the following: (Attach existing course outline, note changes as appropriate. Update Prerequisite/Advisory Form, if appropriate )

Number Hours Prerequisite/Advisory Discipline Title Units Description Content Grading GE Applicability Repeatability Transferability General Update Reinstate Course Cross list course with Other (please describe.)

FROM: Discipline & Number Course Title Units Lec Lab Hours per Hours per week week TO: Discipline & Number Course Title Units Lec Lab Hours per Hours per week week Reason for modification: General update including new text edition.

4. Will this course be offered via distance education? Yes No If yes, fill out Form D – Distance Education form.

5. Routing/Recommendation for Approval Signatures Approval Dept. Approval (Chair Sign) Date Yes ___ No ___

Area Dean Date Yes ___ No ___

Curriculum Committee Chair Date Yes ___ No ___

VP of Instruction Date Yes ___ No ___

Superintendent/President For Yes ___ No ___ District Board CCC Chancellor’s Office Date Yes ___ No ___ (if applicable)

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 GAVILAN COLLEGE CURRICULUM DEVELOPMENT

COURSE OUTLINE

DISCIPLINE: CHEM 1A DEPARTMENT: Chemistry (Discipline and Number) COURSE TITLE: General Chemistry (Maximum of 58 spaces) ABBREVIATED TITLE: GENERAL CHEMISTRY (Maximum of 28 spaces)

SEMESTER UNITS: 5.0 LEC HOURS PER WEEK: 4 LAB HOURS PER WEEK: 3

Classification: Non Credit Category: Occupational Code (SAM): N/A Y Not Applicable, Credit Course N/A TOP Code: 0000.00 LEH Factor: FTE Load:

CATALOG DESCRIPTION: No Change Change

COURSE REQUISITES: List all prerequisites separated by AND/OR, as needed. Also fill out and submit the Prerequisite/Advisory form. No Change Replaces existing Advisory/Prerequisite In addition to existing Advisory/Prerequisite Prerequisite: Co-requisite: Advisory:

GRADING SYSTEM: Select only one: No Change Standard Letter grade Pass/ No Pass Option of a standard letter grade or pass/no pass Non Credit

REPEATABLE FOR CREDIT: (Note: Course Outline must include additional skills that will be acquired by repeating this course.) No Change Credit Course Yes No If yes, how many times? 1 2 3 Non Credit Course Yes No If yes, how many times? 1 2 3 Unlimited (Noncredit only) STAND ALONE: No Change Yes (Course is NOT included in a degree or certificate program) No (Course is included in a degree or certificate program)

METHODS OF INSTRUCTION: No Change

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 RECOMMENDED OR REQUIRED TEXT/S: (The following information must be provided: Author, Title, Publisher, Year of Publication, Reading level and Reading level verification) Required Recommended N/A Author: Title: Publisher: Year of Publication: Required: Required: Required: Required: 1.) J.E. Brady, J.E. 1.) "Chemistry: Matter And 1.) J. Wiley 1.) 2009 Russel, J.R. Holum Its Changes," 5th ed. Publishing 2.) 2007 2.) J.A. Beran 2. "Chemistry In The 2.) J. Wiley Laboratory," 4th ed. Publishing Recommended: Recommended: 1.) 2009 1.) J.E. Braady, J.E. Recommended: Recommended: Russel, J.R. Holum 1.) "Study Guide For 1.) J. Wiley 2.) 2009 Chemistry: Matter And Its Publishing 2.) J.E. Brady, J.E. Changes," 5th ed. Russel, J.R. Holum 2.) J. Wiley 2.) "Student Solutions Publishing Manual For Chemistry: Matter And Its Changes," 5th ed. or other appropriate college level text. ISBN: 978-0-470-28643-2 Reading level of text: 13.0 Verified by: D. Clark 978-0-471-10952-5 grade 978-0-470-18464-6 978-0-470-18465-3 (if available) Other textbooks or materials to be purchased by the student: None

STUDENT LEARNING OUTCOMES: 1. Complete this section in a manner that demonstrates student’s use of critical thinking and reasoning skills. These include the ability to formulate and analyze problems and to employ rational processes to achieve increased understanding. Reference Bloom's Taxonomy of action verbs. 2. List the Type of Measures that will be used to measure the student learning outcomes, such as written exam, oral exam, oral report, role playing, project, performance, demonstration, etc 3. Identify which Institutional Learning Outcomes (ILO) apply to this course. List them, by number, in order of emphasis. For example: "2, 1" would indicate Cognition and Communication. (1) Communication, (2) Cognition, (3) Information Competency, (4) Social Interaction, (5) Aesthetic Responsiveness, (6) Personal Development & Responsibility, (7) Content Specific. 4. For GE courses, enter the GE Learning Outcomes for this course. For example "A1, A2". GE Learning Outcomes are listed below.

1) Student Learning Outcomes 2) Measure 3) Institutional 4) GE Learning Learning Outcome (only Outcome required if GE applicable) 1. Demonstrate proficiency in using Measure: Home ILO: 2, 1 GE-LO: B1, B3, scientific notation, significant figures, and work, Quiz and B5, B6, A6 measurement units. Exam Design strategies to approach and solve problems using dimensional analysis. Use the periodic table to gain information about atoms, elements and predict their properties and reactivities. 2. Differentiate among the three basic Measure: Home ILO: 2, 1 GE-LO: B1, B3, classifications of matter: elements, work, Quiz and B5, B6, A6 compounds and mixtures as well as their Exam

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 formation and physical properties. Demonstrate and analyze the concepts of moles and molarity. Identify the major class of reactions, balance equations and predict their products 3. Determine and write the chemical names Measure: Home ILO: 2, 1 GE-LO: B1, B3, and formulas of ionic and molecular work, Quiz and B5, B6, A6 compounds. Exam Develop strategies to approach, comprehend and solve problems involving stoichiometry. Evaluate the chemical properties of electrolytes, acids and bases. 4. Demonstrate and analyze the formation, Measure: Home ILO: 2, 1 GE-LO: B1, B3, products and properties of solutions. work, Quiz and B5, B6, A6 Recognize oxidation-reduction reactions Exam and assignment of oxidation numbers. Writing and balancing equations for oxidation-reduction reactions for both acidic and basic solutions. 5. Distinguish between Measure: Home ILO: 2, 1 GE-LO: B1, B3, exothermic/endothermic reactions and work, Quiz and B5, B6, A6 evaluate chemical systems and thermal Exam properties. To prepare, manipulate and interpret thermochemical equations, enthalpy diagrams and use Hess's Law to calculate enthalpy changes. 6. Distinguish the main features of atomic Measure: Home ILO: 2, 1 GE-LO: B1, B3, theory and apply the fundamental work, Quiz and B5, B6, A6 organization of the atom including the Exam electron orbitals. Relate the electron configuration of elements to their location in the periodic table and the element's corresponding properties. Determine how ionic and molecular compounds are formed from their elements and what factors cause elements to form an ionic or molecular compound. 7. Draw Lewis diagrams for the structures of Measure: Home ILO: 2, 1 GE-LO: B1, B3, molecules and polyatomic ions and deter- work, Quiz and B5, B6, A6 mine the polarity of bonds based upon the Exam difference in electronegetivity. Compare and contrast the Valence Bond and VSEPR theories and predict the geometries of molecules. Compare and contrast Hybrid Orbital and Molecular Orbital theories to explain multiple bonds and the shapes of

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 molecules. 8. Use the Imperical Gas Laws to quantita- Measure: Home ILO: 2, 1 GE-LO: B1, B3, tively describe gaseous behavior. work, Quiz and B5, B6, A6 Explain the Kinetic-Molecular theory of Exam gases and relate it to the properties of gases. 9. Describe the differences between the Measure: Home ILO: 2, 1 GE-LO: B1, B3, intermolecular forces and predict which work, Quiz and B5, B6, A6 forces will affect a given sample and Exam determine its properties. Apply Le Chatelier's principle of dynamic equilibrium to chemical reactions. Explain how atoms, ions or molecules can be arranged in crystalline solids and predict their properties. 10. Collect and analyze laboratory experi- Measure: Home ILO: 2, 1, GE-LO: B4, mental data ans solve related chemical work, Quiz, 4, 6 B7, B8, A5 problems. Exam Examine chemical concepts through peer and Laboratory interaction and written laboratory reports. Reports Relate classroom and laboratory experiences to phenomena outside the classroom.

GENERAL EDUCATION LEARNING OUTCOMES AREA A Communications in the English Language After completing courses in Area A, students will be able to do the following: A1. Receive, analyze, and effectively respond to verbal communication. A2. Formulate, organize and logically present verbal information. A3. Write clear and effective prose using forms, methods, modes and conventions of English grammar that best achieve the writing’s purpose. A4. Advocate effectively for a position using persuasive strategies, argumentative support, and logical reasoning. A5. Employ the methods of research to find information, analyze its content, and appropriately incorporate it into written work. A6. Read college course texts and summarize the information presented. A7. Analyze the ideas presented in college course materials and be able to discuss them or present them in writing. A8. Communicate conclusions based on sound inferences drawn from unambiguous statements of knowledge and belief. A9. Explain and apply elementary inductive and deductive processes, describe formal and informal fallacies of language and thought, and compare effectively matters of fact and issues of judgment and opinion.

AREA B Physical Universe and its Life Forms After completing courses in Area B, students will be able to do the following: B1. Explain concepts and theories related to physical and biological phenomena. B2. Identify structures of selected living organisms and relate structure to biological function. B3. Recognize and utilize appropriate mathematical techniques to solve both abstract and practical problems. B4. Utilize safe and effectives laboratory techniques to investigate scientific problems. B5. Discuss the use and limitations of the scientific process in the solution of problems. B6. Make critical judgments about the validity of scientific evidence and the applicability of scientific theories. B7. Utilize appropriate technology for scientific and mathematical investigations and recognize the advantages and disadvantages of that technology. B8. Work collaboratively with others on labs, projects, and presentations. B9. Describe the influence of scientific knowledge on the development of world’s civilizations as recorded in the past as well as in present times.

AREA C Arts, Foreign Language, Literature and Philosophy After completing courses in Area C, students will be able to do the following: C1. Demonstrate knowledge of the language and content of one or more artistic forms: visual arts, music, theater, film/television, writing, digital arts.

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 C2. Analyze an artistic work on both its emotional and intellectual levels. C3. Demonstrate awareness of the thinking, practices and unique perspectives offered by a culture or cultures other than one’s own. C4. Recognize the universality of the human experience in its various manifestations across cultures. C5. Express objective and subjective responses to experiences and describe the integrity of emotional and intellectual response. C6. Analyze and explain the interrelationship between self, the creative arts, and the humanities, and be exposed to both non-Western and Western cultures. C7. Contextually describe the contributions and perspectives of women and of ethnic and other minorities.

AREA D Social, Political, and Economic Institutions After completing courses in Area D, students will be able to do the following: D1. Identify and analyze key concepts and theories about human and/or societal development. D2. Critique generalizations and popular opinion about human behavior and society, distinguishing opinion and values from scientific observation and study. D3. Demonstrate an understanding of the use of research and scientific methodologies in the study of human behavior and societal change. D4. Analyze different cultures and their influence on human development or society, including how issues relate to race, class and gender. D5. Describe and analyze cultural and social organizations, including similarities and differences between various societies.

AREA E Lifelong Understanding and Self-Development After completing courses in Area E, students will be able to do the following: E1. Demonstrate an awareness of the importance of personal development. E2. Examine the integration of one’s self as a psychological, social, and physiological being. E3. Analyze human behavior, perception, and physiology and their interrelationships including sexuality, nutrition, health, stress, the social and physical environment, and the implications of death and dying.

AREA F Cultural Diversity After completing courses in Area F, students will be able to do the following: F1. Connect knowledge of self and society to larger cultural contexts. F2. Articulate the differences and similarities between and within cultures.

CONTENT, STUDENT PERFORMANCE OBJECTIVES, AND *OUT-OF-CLASS ASSIGNMENTS: HOURS *e.g., essays, library research, problems, projects required outside of class on a 2 to 1 basis for Lecture units granted. 10 Hours Chapter-1 Fundamentals of Chemical Change The scientific method. Matter, energy and chemical changes. Measured quantities and their units. Computations, dimensional analysis and significant figures. Properties of substances; density and specific gravity. Homework problems from text and instructor. Laboratory Experiment: Locker Check-In and Safety.

Demonstrate proficiency in using scientific notation, significant figures, and measurement units. Design strategies to approach and solve problems using dimensional analysis.

18 Hours Chapter-2 The Periodic Table and Some Properties of the Elements Elements, compounds and mixtures. Atoms, chemical symbols, formulas and equations. The structure of matter; atoms and subatomic particles. Periodic law and the periodic table. Metals, nonmetals and metalloids. Reactions of the elements; formation of ionic and molecular compounds. Properties of ionic and molecular compounds. Ionic and molecular nomenclature. Homework problems from text and instructor. Laboratory Experiment: Techniques and Measurements.

Use the periodic table to gain information about atoms, elements and predict their properties and reactivities.

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 Differentiate among the three basic classifications of matter: elements, compounds and mixtures as well as their formation and physical properties. Determine and write the chemical names and formulas of ionic and molecular compounds.

18 Hours Chapter-3 Stoichiometry: Quantitative Chemical Relationships The mole concept. Measuring moles of elements and coumpounds. Emperical and molecular formulas. Percentage composition. Writing and balancing chemical equations. Using chemical equations in calculations. Limited reactant calculations. Theoretical yield and percentage yield. Reactions in solutions and molar concentration. Stoichiometry of reactions in solution. Homework problems from text and instructor. Laboratory Experiment: Emperical Formula of an Oxide.

Identify the major classes of chemical reactions, balance equations and predict their products. Demonstrate and analyze the concepts of moles and molarity. Develop strategies to approach, comprehend and solve chemical problems involving stoichiometry.

10 Hours Chapter-4 Reactions Between Ions in Aqueous Solutions Electrolytes and nonelectrolytes. Equations for ionic reactions. Predicting reactions that produce precipitates. Strong and weak acids and bases. Acid-Base neutralization. Ionic reactions that produce gases. Predicting when ionic reactions actually occur. Stoichiometry of ionic reactions. Homework problems from text and instructor. Laboratory Experiment: Limiting Reagents.

Evaluate the chemical properties of electrolytes, acids and bases. Demonstrate and analyze the formation, products and properties of solutions.

18 Hours Chapter-5 Oxidation-Reduction Reactions Oxidation-reduction reactions. Balancing redox equations by the ion-electron method. Reactions of metals with acids. Displacement of one metal by another from compounds. Molecular oxygen as an oxidizing agent. Stoichiometry and redox reactions. Homework problems from text and instructor. Laboratory Experiment: Reaction Types.

Recognize oxidation-reduction reactions and assignment of oxidation numbers. Writing and balancing equations for oxidation-reduction reactions for both acidic and basic solutions.

18 Hours Chapter-6 Energy and Thermochemistry Kinetic and potential energy. The kinetic theory of matter. Energy changes in chemical reactions. The First Law of Thermodynamics: heat and work. Measuring energy changes; calorimetry. Enthalpy changes in chemical reactions. Combining thermochemical equations; Hess's Law. Standard heats of formation and Hess's Law.

Homework Problems from text and instructor. Laboratory Experiment: Cation Identification.

Distinguish between exothermic/endothermic reactions and evaluate chemical systems and thermal properties. To prepare, manipulate and interpret thermochemical equations, enthanlpy diagrams and use Hess's Law to calculate enthalpy changes.

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 10 Hours Chapter-7 Atomic and Electronic Structure Electromagnetic raqdiation. Atomic spectra and the Bohr model of the hydrogen atom. Wave properties of matter and wave mechanics. Electron spin and the Pauli Exclusion Principle. Electronic structures of multielectron stoms. Electron configurations and the periodic table. Unexpected electron configurations. Shapes of the atomic orbitals. Variation of atomic properties with electronic structure.

Homework Problems from text and instructor. Laboratory Experiment: Calorimetry.

Distinguish the main features of atomic theory and apply the fundamental organization of the atom including the electron orbitals. Relate the electron configuration of elements to their location in the periodic table and the corresponding properties of many elements.

18 Hours Chapter-8 Chemical Bonding: General Concepts Electron transfer and the formation of ionic compounds. Wlectron bookkeeping and Lewis symbols. Electron sharing and the formation of covalent bonds. Some important compounds of carbon. Electronegativity and the polarity of bonds. Electronegativity and the reactivities of metals and nonmetals. Drawing Lewis structures and the Octet Rule. Formal charge and the selection of Lewis structures. Resonance; when a single Lewis structure fails. Coordinate covalent bonds.

Homework Problems from text and instructor. Laboratory Experiment: Spectrophotometric Iron Analysis.

Determine how ionic and molecular compounds are formed from their elements and what factors cause lelements to form ionic and molecular compounds. Draw Lewis diagrams for the structures of molecules and polyatomic ions and determine the polarity of bonds based upon the differences in electronegativity.

18 Hours Chapter-9 Chemical Bonding and Molecular Structure Common molecular structures and geometry. Predicting the shapes of molecules; VSEPR Theory. Molecular shapes and molecular polarity. Wave mechanics and covalent bonding; Valence Bond Theory. Hybrid orbitals. Double and triple bonds. The Molecular Orbital Theory. Delocalized molecular orbitals. Bonding in solids.

Homework Problems from text and instructor. Laboratory Experiment: Chemical Periodicity.

Compare and contrast the Valence Bond and VSEPR theories. Compare and contrast Hybrid Orbitals and Molecular Orbital theories to explain multiple bonds and the shapes of molecules.

10 Hours Chapter-10 Properties of Gases Properties common to all gases. Pressure; its measurement and units. Pressure-, Volume-, Temperature- relationships for a fixed amount of gas. The Ideal Gas Law. Stoichiometry of chemical reactions between gases. Dalton's Law of Partial Pressure. Grahamn's Law of Effusion. Kinetic theory and the gas laws. Real gases; deviations from the Ideal Gas Law.

Homework Problems from text and instructor. Laboratory Experiment: Hard Water Analysis.

Use the gas laws to quantitatively describe gaseous behavior. Explain the Kinetic-Molecular Theory of Gases and relate it to the properties of gases.

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 14 Hours Chapter-11 Intermolecular Attractions and the Properties of Liquids and Solids Why gases differ from liquids and solids. Intermolecular attractions. Some general properties of liquids and solids. Changes of state and dynamic equilibrium. Vapor pressures of liquids and solids. Boiling points of liquids. Energy changes during a change of state. Dynamic equilibrium and Le Chatelier's Principle. Phase diagrams. Crystalline solids and X-ray diffraction. Crystal types and their physical properties. Noncrystalline solids.

Homework Problems from text and instructor. Laboratory Experiment: Molar Mass of a Volatile Liquid.

Describe the differences between the intermolecular forces and predict which forces will affect a given sample and determine its properties. Apply Le Chatelier's principle of dynamic equilibrium. Explain how atoms, ions or molecules can be arranged in crystalline solids and predict their properties.

2 Hours Final Examination (cumulative) Comprehensive over the entire course with evaluation of each of the areas previously examined.

Hours Hours Hours Hours Hours

METHODS OF EVALUATION: CATEGORY 1 - The types of writing assignments required: Percent range of total grade: 20 % to 30 % Written Homework Reading Reports Lab Reports Essay Exams Term or Other Papers Other: Extra credut report on a Chemistry topic. If this is a degree applicable course, but substantial writing assignments are not appropriate, indicate reason: Course is primarily computational Course primarily involves skill demonstration or problem solving CATEGORY 2 -The problem-solving assignments required: Percent range of total grade: 70 % to 80 % Homework Problems Field Work Lab Reports Quizzes Exams Other: CATEGORY 3 -The types of skill demonstrations required: Percent range of total grade: % to % Class Performance/s Field Work

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010 Performance Exams CATEGORY 4 - The types of objective examinations used in the course: Percent range of total grade: % to % Multiple Choice True/False Matching Items Completion Other: CATEGORY 5 - Any other methods of evaluation: Percent range of total grade: % to %

05fac630fb64f9ea176a25052f7c047f.doc Revised: 2/25/2010