COURSE SYLLABUS AND INSTRUCTOR PLAN

Transcription

1 WACO, TEXAS COURSE SYLLABUS AND INSTRUCTOR PLAN GENERAL INORGANIC CHEMISTRY I CHEMISTRY , 02, 03 Joe Dean Zajicek SPRING 2012

2 Course Description: Covers the fundamental laws, theories, and concepts of chemistry, methods of writing chemical formulas and equations, structure of the atom and matter, periodic classification related to the properties of typical elements and compounds, and electrolytic dissociation and solutions. Serves as the prerequisite requirement for engineering, medicine, advanced work in chemistry and other fields of science. Prerequisites and/or Corequisites: Credit for, or concurrent enrollment in, MATH 1314 or equivalent, or consent of division director. Course Notes and Instructor Recommendations: Chemistry 1411 is a course designed for majors in the field of science. This course requires a math background of College algebra or its equivalent, with special emphasis on the solution of statement problems. A background in high school chemistry would be very helpful in this course but is not required. This course will require more of study time because of the nature of the subject material in the field of chemistry. A student should spend not less than three for each hour in class, working on understanding the lecture material and working on problem solving. For those students without a high school background in chemistry, you will need to consider additional time to be spent in the study of course material in the area of problem solving. Course notes will be presented by use of PowerPoint slides. Instructor Information: Instructor Name: Joe Dean Zajicek MCC jzajicek@mclennan.edu Office Phone Number: Office Location: Science Bldg. Room 307 Office/Teacher Conference Hours: MW 8:30-9:30 TT 11:00-12:00 Fri. only by special arrangement Other Instruction Information: Required Text & Materials: Title: General Chemistry with Qualitative analysis 2

3 Author: Robinson, Odom & Holtzclaw Edition: 10th Publisher: Houghton Mifflin ISBN: MCC Bookstore Website Methods of Teaching and Learning: Lecture along with student in-class activity, student performances with respect to lab exercises, learning assignments by use of exercise sets, major exams, and some lab quizzes. Course Objectives and/or Competencies: 1. Define the fundamental properties of matter. 2. Classify matter, compounds, and chemical reactions. 3. Determine the basic nuclear and electronic structure of atoms. 4. Identify trends in chemical and physical properties of the elements using the Periodic Table. 5. Describe the bonding in and the shape of simple molecules and ions. 6. Solve stoichiometric problems. 7. Write chemical formulas. 8. Write and balance equations. 9. Use the rules of nomenclature to name chemical compounds. 10. Define the types and characteristics of chemical reactions. 11. Use the gas laws and basics of the Kinetic Molecular Theory to solve gas problems. 12. Determine the role of energy in physical changes and chemical reactions. 13. Convert units of measure and demonstrate dimensional analysis skills. 14. Use basic apparatus and apply experimental methodologies used in the chemistry laboratory. 15. Demonstrate safe and proper handling of laboratory equipment and chemicals. 16. Conduct basic laboratory experiments with proper laboratory techniques. 17. Make careful and accurate experimental observations. 18. Relate physical observations and measurements to theoretical principles. 19. Interpret laboratory results and experimental data, and reach logical conclusions. 20. Record experimental work completely and accurately in laboratory notebooks and communicate experimental results clearly in written reports. 21. Design fundamental experiments involving principles of chemistry. 22. Identify appropriate sources of information for conducting laboratory experiments involving principles of chemistry. 3

4 Course Outline or Schedule: The subject material in Chemistry 1411 will be divided into 9 study units consisting of the topics listed below and into 12 laboratory experiment units. The study units will consist of the following items: 1. A set of objectives, which cover the major concepts on the unit. 2. A reading assignment on the objectives and review of PowerPoint slides; this is required prior to class discussion. 3. Problem solution assignment of some objectives, this involves calculations to solve problems based on chemical concepts. 4. BONUS WORK - This will consist of a set of problems and/or questions, which are assigned with each study unit. This problem and/or question set are located at the end of each set of objectives. 5. Each unit of study will consist of lecture on some of the material by use of electronic slides, along with discussion and study. Upon completion of the units of study, the following will be done 1. A TEST will be taken on the units of study. The test will consist of approximately 35 to 50 questions and/or problems on the100-point test and 20 to 35 questions and/or problems on the 50-point test. 2. The EXERCISE SET for bonus points will be turned in on a given assigned time. STUDY UNITS TO BE COVERED Approx. time for completion of unit 1. Fundamental Concepts 1 Week 2. Symbols, Formulas, Equations and Thermochemistry 2 Weeks Test 1 3. Atomic Structure, Periodic Law and Relationships of Periodic Classification of Elements 2 Weeks Test 2 4. Chemical Bonding: General Concept 1½ Weeks 5. Chemical Bonding: Molecular Orbitals and Molecular Structure 1½ Weeks Test 3 6. Gaseous State, Gas Laws and Gram Molecular Volume 2 Weeks 7. Liquid and Solid States 1 Week Test 4 8. Solution Chemistry and Solution of Electrolytes 2 Weeks 9. Acids, Bases and Salts 1 Week Test 5 THESE UNITS MAY BE USED FOR BONUS WORK 10. Nonmetals 11. The Representative Metals and Semi-Metals 4

5 UNIT OUTLINE I. FUNDAMENTAL CONCEPTS A. Time: Three class, with nine preparation 1. Chemistry and its scope 2. Matter and energy 3. Law of conservation of matter 4. Law of conservation of energy 5. Matter-Energy relationship 6. Physical states of matter 7. Chemical and physical changes 8. Chemical and physical properties 9. Varieties of matter a. element b. compound c. mixture 10. Atoms and molecules 11. The scientific method 12. Fundamental units of measure in chemistry a. conversion of these units and their relation to the English system 13. Temperature conversions 14. Calorimeter and heat calculations II. SYMBOLS, FORMULAS, EQUATIONS and THERMOCHEMISTRY A. Time: Six class, with eighteen preparation 1. Symbols and formulas 2. Chemical equations 3. Balancing equations 4. Atomic mass and the Law of Dulong and Petit 5. Formula mass, molecular mass, mole 6. Calculation of percentage of composition 7. Derivation of formula from analytical data 8. Chemical stoichiometry and its application 9. Stoichiometry of heat changes in chemical reactions 10. Solution concentration and titration III. STRUCTURE OF ATOMS, PERIODIC CLASSIFICATION, AND THE RELATIONSHIP OF THE ELEMENTS 5

6 A. Time: Six, with eighteen preparation 1. Fundamental particles a. electron b. proton c. neutron 2. Radioactivity 3. The nuclear atom a. atomic number b. composition of nucleus c. atomic weight scale 4. Bohr model of atom 5. Quantum mechanical model of atom 6. Electronic structure of atom based on electron distribution 7. Periodic table a. Variation of properties within periods and groups IV. CHEMICAL BONDING A. Time: Four class, with thirteen preparation 1. Valence 2. Chemical bonding by electron transfer (ionic bond) 3. Electronegatives of the elements to predict type of bond 4. Chemical bonding by sharing electrons a. nonpolar covalent b. coordinate covalent (dative) 5. Determination of the number of covalent bonds occurring between atoms using Lewis structure 6. Resonance in bonding 7. Polarity as related to bonding 8. Assignment of oxidation numbers in compounds 9. Formula writing from use of oxidation numbers 10. Nomenclature of chemical compounds 11. Calculations involving bond energy 6

7 V. MOLECULAR ORBITAL THEORY AND MOLECULAR STRUCTURE A. Time: Four class, with thirteen preparation 1. Molecular orbital theory with respect to covalent bonding 2. Use of molecular orbitals energy diagram to predict stability of bonds between homonuclear and heteronuclear diatomic molecules and bond order 3. Predict molecular structure using the VSPR theory 4. Predict the type of hybridization occurring in bonding and the state of multiplicity of bonds due to this hybridization VI. GASEOUS STATE OF MATTER: THE KINETIC MOLECULAR THEORY A. Time: Six class, with eighteen preparation 1. General behavior of gases 2. Boyle's Law 3. Kelvin temperature scale 4. Charles' Law 5. Dalton's Law of Partial Pressures 6. Graham's Law of Diffusion 7. Calculations involving gas laws 8. Kinetic-Molecular Theory of gases 9. Relation of gas behavior to Kinetic-molecular theory 10. Deviation of gases to the laws 11. Ideal Gas 12. Avogadros' Law of gases 13. Molar volume of gases 14. Determination of molecular mass of gases by Vapor density 15. Volume relationship in chemical equations 16. Ideal gas law equation and its application in calculations 17. Deviation from ideal gas law VII. LIQUID AND SOLID STATES OF MATTER A. Time: Three recitation, with nine preparation 7

8 1. General properties of liquids and kinetic molecular theory of liquids 2. Vapor pressure and boiling points of liquids 3. Intermolecular forces in liquids 4. Surface tension 5. Critical temperature and pressure 6. Heat of vaporization and fusion 7. General properties of solids and kinetic molecular theory of solids 8. Crystalline solids a. types and structural units 9. Prediction of atoms per unit cell, radius ratio rule of ionic compounds 10. Use of lattice energies in study of ionic compounds 11. Crystal defects 12. X-ray diffraction in analysis of crystals 13. Lattices energies 14. Amorphous solids 15. Vapor pressure solids and melting point of solids VIII. SOLUTIONS A. Time: Six class, with eighteen preparation 1. General properties of solutions 2. Kinds of solutions and examples of each 3. Effects of certain factors on various solutions 4. Azeotrophic mixtures 5. Saturated, unsaturated, and supersaturated conditions for solutions 6. Concentrations of solutions 7. Calculations in the determination of solution concentrations 8. Effects of solute upon the properties of solvents 9. Determination of the molecular mass of solutes by the solution method 10. Solutions and electrolytes a. mechanism of dissolution of ionic and covalent compounds b. ion activity, activity coefficient 11. Colloid chemistry 8

9 a. properties of a colloidal system b. type of colloidal systems c. brownian movement d. adsorption properties IX. ACIDS, BASES AND SALTS A. Time: Three class, with nine preparation 1. Various concepts of acids and bases 2. Strength of acids and bases 3. Properties of acids and bases 4. Methods of formation of acids and bases 5. Neutralization 6. Types, solubility, and properties of salts 7. Preparation of salts 8. Determination of solution concentration by titration process The following will be covered as an outside reading assignment - Bonus work X. NONMETALS A. The student should develop an understanding of: 1. Chemical characteristics of nonmetals 2. Allotropic forms of carbon and phosphorous 3. Carbon a. occurrence b. properties 4. Preparation, properties, and uses of oxides of carbon 5. Preparation, properties, and uses of carbonic acid, its salts and various compounds containing carbon 6. Nitrogen a. properties, preparation and uses 7. Ammonia a. properties, preparation and uses 8. Oxygen compounds of nitrogen 9. Salts of nitrogen and their properties 10. Acids of nitrogen and their properties 11. Phosphorus a. preparation, properties and uses 12. Phosphine 13. Halides of phosphorus and their compounds 14. Oxides of phosphorus and their compounds 15. Acids of phosphorus and their compounds 9

10 16. Properties and uses of noble gases 17. Production of noble gases 18. Some compounds; their structure, properties and uses of noble gases 19. Oxygen and hydrogen a. occurrence b. physical and chemical properties c. preparations 20. Basic and acidic anhydrides 21. Ozone a. allotrophy b. physical and chemical properties c. preparation and uses 22. Uses of hydrogen and oxygen 23. Occurrence and method of extraction of sulfur 24. Properties of the elements of the sulfur family 25. Uses of elements of the sulfur family 26. Sulfur a. properties b. allotropic forms 27. Sulifdes, selenides, tellurides 28. Oxides of sulfur family 29. Acids of sulfur family a. properties and preparation 30. Occurrence of halogens 31. Preparation, properties, and uses of halogens 32. Preparation, properties, and uses of hydrogen halides 33. Oxyacids of the halogens and their salts XI. REPRESENTATIVE METALS AND SEMI-METALS A. The student should develop an understanding of: 1. Occurrence, preparation, properties and uses of the metals 2. Important compounds of the metals a. preparation, properties and use 3. Occurrence, preparation, properties and uses of semi-metals 4. Crystals of semi-metals a. characteristics, shape and bonding 5. Solar cell a. basic units b. function in production of electrical energy XII. LABORATORY A. Time: Fifty-six of laboratory work (4 weekly) 10

11 B. Topics to be covered are those which will parallel lecture. EXERCISE TITLES Skills & Measurements Identification of Substance Physical and Chemical Changes Determination of Empirical Formula Water of Hydration Purity of Sodium Bicarbonate Atomic Mass from Calorimetry Chemical Activity of Metals Physical Behavior of Gases Molar Mass of a Substance (Vapor Density Method) Solutions and Solubility Molecular Mass by Solution Method Acid-Base Titrations If the schedule listed above is subject to a change the student will be notified about changes one week in advance in class. Course Grading Information: TESTING A test will be given after the completion of study for an assigned study unit. The test will be basically OBJECTIVE type questions, such as multiple choice, completion, true-false, matching and then there will be some of a short essay type, along with problem solution. The testing time will be announced approximately 1 week in advance of the completion of lecture material covered on the test. A minimum score of 70 on a 100-point and 35 on a 50-point test must be obtained in order to pass, if the score is less than these points, a retest may be taken. The retest MUST be taken within ONE WEEK from the day on which the first test was given and the maximum score, which can be obtained, will be 70 or 35 points. GRADING PROCEDURE Grading will be on a point basis, each study unit test will have a value of 100 or 50 points. The laboratory experimental units have the points listed for each experiment from 10 t0 20 points. The following percentages of the total point will result in a grade of (90%) A (80%) B 11

12 (70%) C (60%) D BONUS POINTS can be obtained by the following ways: 1. Exercise sets. A maximum of 2 points per set 2. Study units 10 and 11. A quiz can be taken on units 10 and 11 and if a score of 35 is obtained on a 50-point test, ten bonus points will be given for Unit 10 and five bonus points for Unit 11. To obtain these bonus points on the study units the test must be taken prior to the beginning of FINAL PREPARATION WEEK. Your laboratory grade will be determined on a point basis. Exercises marked with R will be reported by use of a report form which is found in your laboratory manual; those exercises marked with Q will be reported by way of a short test which will be composed from observation and prelab questions within and at the end of the experiment. On some of the exercises; calculations, tables and/or graphs will be completed and turned in along with a short test. All prelab questions on each experiment must be completed before performing the lab. Six prelab question sets will be turned in from six of your experiments, if completed on the assigned time with proper answers, there will be a bonus of 1 point for each prelab question set. The QUIZ will be given at the beginning of the next scheduled lab meeting or after completion of the experiment. The quiz will contain from 5 to 10 questions. The REPORTS will be completed during the lab experimentation and turned in upon completion of the experiment by placing the report in a designated folder. Students who turn in work which has been copied, both individuals (the student who copied the work and the student who provide the work to be copied) will not receive are grade for the work. Late Work, Attendance, and Make Up Work Policies: NO make-up test will be given for an assigned test that was missed due to an absence which does not meet the college attendance policy; only a retest will be given. The retest MUST be taken within ONE WEEK from the day on which the first test was given and the maximum score, which can be obtained, will be 70 or 35 points. All work on exercise sets is due on date assigned in order to receive a grade. ALL LAB WORK MISSED ON THE DATES ASSIGNED, MUST BE MADE UP WITHIN ONE WEEK FROM THE DATE ASSIGNED IN ORDER TO RECEIVE A GRADE ON THAT EXERCISE, IF ABSENCE FROM LAB MEETS THE COLLEGE ATTENDANCE POLICY. To make-up a missed lab, the following must be done (1) Read lab exercise and review the PowerPoint slides on the exercise missed (2) Set up a time with the instructor to complete the experiment. 12

13 ALL LABORATORY WORK MUST BE COMPLETED BY FINAL PREPARATION WEEK, NO LAB WORK WILL BE DONE AFTER THIS DATE. Student Behavioral Expectations or Conduct Policy: Students are expected to maintain classroom decorum that includes respect for other students and the instructor, prompt and regular attendance, and an attitude that seeks to take full advantage of the education opportunity. MCC Academic Integrity Statement: The Center for Academic Integrity, of which McLennan Community College is a member, defines academic integrity as a commitment, even in the face of adversity, to five fundamental values: honesty, trust, fairness, respect, and responsibility. From these values flow principles of behavior that enable academic communities to translate ideals into action. Individual faculty members determine their class policies and behavioral expectations for students. Students who commit violations of academic integrity should expect serious consequences. For further information about student responsibilities and rights, please consult the McLennan website and your Highlander Student Guide. Academic Integrity Statement: Students who commit violations of academic integrity by turning in work which has been copied, both individuals (the student who copied the work and the student who provide the work to be copied) will not receive are grade for the work. MCC Attendance Policy: Regular and punctual attendance is expected of all students, and each instructor will maintain a complete record of attendance for the entire length of each course, including online and hybrid courses. Students will be counted absent from class meetings missed, beginning with the first official day of classes. Students, whether present or absent, are responsible for all material presented or assigned for a course and will be held accountable for such materials in the determination of course grades. Please refer to the Highlander Guide for the complete policy. The attendance policy for Chemistry 1411, if a student s absences reaches 25% (23 hrs) of the total contact in this course before the student-initiated withdrawal date, they will be dropped from the course. A student must officially withdraw from the course in order to receive 13

14 a W, before the student-initiated withdrawal date. After this date a student can not drop the course. A student is considered tardy to class after the class begins, no excuses will be accepted for tardiness, if the student is tardy by 15 minutes, they will be considered absent. No CELL PHONES OR PAGERS, cell phone or pager must be turned off before entering class, if a student s cell phone or pager sounds or is used during class, you must leave the class and will be counted absent from class. ADA Statement: In accordance with the requirements of the Americans with Disabilities Act (ADA), and the regulations published by the United States Department of Justice 28 C.F.R (a), MCC s designated ADA co-coordinators, Mr. Gene Gooch - Vice President, Finance and Administration and Dr. Santos Martinez Vice President, Student Services shall be responsible for coordinating the College s efforts to comply with and carry out its responsibilities under ADA. Students with disabilities requiring physical, classroom, or testing accommodations should contact Ms. Renee Jacinto, Disabilities Specialist, at or rrjacinto@mclennan.edu. 14