Chemistry Central Campus

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1 Chemistry Central Campus CHEM 1411 General Chemistry I CRN Spring 2012 Tuesdays, 8:30 11:30 am, in Lab 414 Thursdays, 8:30 11:30 am, in LHSB 416 We will meet for the first time on Tuesday, January 17, in Lab credit course (3 hours lecture + 3 hours lab per week) 96 hours per semester / 16 weeks Instructor: Janis C. Stevenson, Ph.D. Instructor Contact Information: janis.stevenson@hccs.edu or chem1411@sbcglobal.net Phone: Learning Web: Office hours: Before or after class (T/Th) or by appointment. Your performance in my class is very important to me. Please contact me concerning any problems that you are experiencing in this course. Please ask for the help that you need before your course grade is in serious trouble. Course Description: 4-credit course. Core curriculum course. This course is designed for science and engineering majors to study atomic structure, chemical reactions, thermodynamics, electronic configuration, chemical bonding, molecular structure, gases, states of matter, and properties of solutions. Prerequisites: One year of high school chemistry. Must be placed into: Math 0312 (intermediate algebra) or higher College-level reading (or take GUST 0342 as a co-requisite) College-level writing (or take ENGL 0310/0349 as a co-requisite) Important: Strong general math and algebra skills are needed for this course! Course Goals: Students will learn the basic concepts covered for the following topics: atomic structure, the periodic table, chemical nomenclature, chemical reactions, thermodynamics, electronic configuration, chemical bonding, molecular structure, states of matter, and properties of solutions.

2 CHEM 1411 page 2 Student Learning Outcomes A student will: 1. Develop an understanding of basic concepts of chemical measurements and calculations, structures of atoms, molecules, and ions, the periodic table, chemical compound nomenclature, chemical reactions, reactions in aqueous solution, the structure and properties of gases, liquids, and solids, thermochemistry, quantum theory, chemical bonding, and molecular geometry. 2. Build a chemistry vocabulary so that he/she can communicate easily with chemistry professionals. 3. Learn and use a variety of tools, techniques, and strategies to solve problems in chemistry. 4. Practice laboratory skills in working safely, using common lab equipment, making measurements, handling chemicals, running reactions, recording/analyzing/ communicating data, assessing experimental error, and operating scientific instruments. Learning Objectives By the end of this course, a student should be able to do each of the actions listed below. This list of learning objectives is useful to review before each test and the final exam! Chapter 1: Chemistry 1. Define homogeneous mixture, heterogeneous mixture, element, and compound. 2. Differentiate between a physical change and a chemical change. 3. Know the SI base units and the prefixes used with SI units. 4. Calculate the density of a substance. 5. Convert temperatures between the Fahrenheit, Celsius, and Kelvin scales. 6. Use scientific notation for numbers. 7. Determine the correct number of significant figures in a calculation. 8. Distinguish between accuracy and precision. 9. Use dimensional analysis to solve problems and determine the correct units. Chapter 2: Atoms, Molecules, and Ions 1. Describe the structure of an atom in terms of protons, neutrons, and electrons. 2. Define atomic number and mass number for an element and determine them from a periodic table. 3. Understand the definition and the notation for isotopes. 4. Distinguish between metals, metalloids, and nonmetals. 5. Define a period and a group on a periodic table of elements. 6. Identify alkali metals, alkaline earth metals, halogens, and noble gases. 7. Define molecules, ions, cations, and anions. 8. Determine chemical formulas for molecules and ions. 9. Determine the names of simple inorganic ionic and molecular compounds. 10. Define acid, base, and hydrate. 11. Know the names of the first ten straight-chain alkanes. Chapter 3: Mass Relationships in Chemical Reactions 1. Determine the average atomic mass of an element. 2. Define a mole and know Avogadro s number. 3. Calculate the molecular mass and the molar mass of an element or compound. 4. Convert between moles and mass of an element or compound. 5. Calculate the percent composition of a compound. 6. Determine the empirical and molecular formulas of a compound. 7. Write a chemical equation describing a chemical reaction. 8. Balance a chemical equation. 9. Determine the amounts of reactants and products in a given chemical reaction. 10. Identify the limiting reagent in a chemical reaction. 11. Calculate the theoretical yield and percent yield of a chemical reaction. Chapter 4: Reactions in Aqueous Solution 1. Define solution, solute, solvent, and aqueous solution. 2. Define strong electrolyte, weak electrolyte, and nonelectrolytes and give examples.

3 3. Describe hydration. 4. Define solubility and use the solubility rules to determine if a compound is soluble. 5. Determine if a precipitate will form in a chemical reaction. 6. Write molecular, ionic, and net ionic equations for precipitation reactions. 7. Identify Brønsted acids and bases. 8. Describe a neutralization reaction in terms of the reactants and products. 9. Describe an oxidation-reduction reaction and write the half-reactions. 10. Assign oxidation numbers using the basic set of rules provided in this chapter. 11. Classify redox reactions into combination, decomposition, combustion, displacement, and disproportionation reactions. 12. Calculate the concentration of a solution in terms of molarity (M=mol/L). 13. Calculate how much water is needed to dilute a solution to a specified concentration. 14. Describe the process of titration and define the equivalence point. CHEM 1411 page 3 Chapter 5: Gases 1. Describe the characteristics of a gas. 2. Define the pressure of a gas and know the units used to measure pressure. 3. Understand the relationships between the pressure and volume of a gas (Boyle s Law), the temperature and the volume of a gas (Charles s and Gay-Lussac s Law), and the relationship between the volume and moles of a gas (Avogadro s Law). 4. Know the ideal gas equation and how to use it. 5. Calculate partial pressures in a mixture of ideal gases. 6. Describe the kinetic molecular theory of gases. 7. Describe the distribution of molecular speeds as a function of temperature. 8. Understand the application of van der Waals equation for nonideal gas behavior. Chapter 6: Thermochemistry 1. Understand the law of conservation of energy and list different forms of energy. 2. Define heat, exothermic process, and endothermic process. 3. Define system, surroundings, open system, closed system, and isolated system. 4. Define a state function. 5. State the first law of thermodynamics. 6. Calculate the work of gas expansion or contraction. 7. Calculate the change in internal energy, E, of a specified system. 8. Calculate the change in enthalpy, H, of a specified system. 9. Calculate the heat change of a substance based on its specific heat, s, or heat capacity, C. 10. Describe a constant-volume calorimeter and a constant-pressure calorimeter. 11. Calculate the standard enthalpy of reaction based on the enthalpies of formation for products and reactants using the direct method and the indirect method (Hess s Law). 12. Understand the concepts of the heat of solution and the heat of dilution. Chapter 7: Quantum Theory and the Electronic Structure of Atoms 1. Describe a wave in terms of wavelength, frequency, and amplitude. 2. Define an electromagnetic wave and be familiar with the electromagnetic radiation spectrum. 3. Describe Planck s quantum theory: E = hn 4. Use Bohr s Theory of the Hydrogen Atom to calculate the energies that an electron can possess in a hydrogen atom. 5. Explain the emission spectra of various elements. 6. Describe the dual particle and wave nature of the electron. 7. State the Heisenberg uncertainty principle. 8. Describe the four quantum numbers: n, l, m l, and m s. 9. Determine the relationship between the quantum numbers and the atomic orbitals. 10. Know the shapes of the s, p, and d atomic orbitals. 11. Determine the electron configuration of an atom of any element. 12. State the Pauli exclusion principle and Hund s rule. 13. Predict whether an element will be paramagnetic or diamagnetic. 14. Explain how the periodic table is arranged relative to electron configuration.

4 CHEM 1411 page 4 Chapter 8: Periodic Relationships Among the Elements 1. Explain why the periodic table is arranged according to atomic number rather than atomic mass. 2. Define a representative element. 3. Explain what valence electrons are. 4. Determine the electron configuration of cations and anions. 5. Identify isoelectronic ions. 6. Predict how effective nuclear charge, atomic radius, and ionic radius vary through the periodic table. 7. Predict how ionization energies vary for the electrons in an element. 8. Define electron affinity and know which elements have high electron affinities. 9. Be familiar with diagonal relationships on the periodic table. 10. Predict whether oxides will be acidic, basic, or amphoteric. Chapter 9: Chemical Bonding I 1. Draw Lewis dot symbols for any representative element. 2. Explain the difference between an ionic bond and a covalent bond. 3. Define single bond, double bond, and triple bond, and predict how bond length varies with type of covalent bond. 4. Explain the octet rule. 5. Compare the properties of ionic and covalent compounds. 6. Define electronegativity and classify bonds as ionic, polar covalent, or covalent based on electronegativity differences. 7. Draw Lewis structures for molecules. 8. Determine the formal charge on an atom in a molecule. 9. Explain the concept of resonance and show how resonance is represented. 10. Know the exceptions to the octet rule: incomplete octets, odd-electron molecules, and expanded octets. 11. Define bond enthalpy and calculate the enthalpy of reaction based on bond enthalpies. Chapter 10: Chemical Bonding II 1. Predict the geometry of a molecule from the Valence-Shell Electron-Pair Repulsion (VSEPR) model. 2. Define dipole moment and predict whether a molecule will be polar or nonpolar. 3. Describe the Valence Bond Theory and determine the type of hybridized orbital used to describe the bonding of a central atom in a molecule. 4. Describe the difference between sigma bonds and pi bonds. 5. Describe Molecular Orbital Theory and draw molecular orbital configurations for simple molecules. 6. Calculate the bond order of a bond in a molecule. 7. Describe delocalized molecular orbitals such as those found in benzene. Chapter 11: Intermolecular Forces and Liquids and Solids 1. Compare the properties of gases, liquids, and solids. 2. Describe the types of intermolecular forces between molecules. 3. Describe hydrogen bonding and its effects on the properties of compounds. 4. Define the surface tension and viscosity of a liquid. 5. Differentiate between cohesion and adhesion. 6. Describe the unusual properties of water. 7. Explain the difference between amorphous and crystalline solids. 8. Draw simple cubic, body-centered cubic, and face-centered cubic structures and calculate the density, unit cell edge length, or number of atoms in a unit cell for a given substance. 9. Use Bragg s law to calculate an atomic spacing in a crystalline compound. 10. Classify crystals into ionic, covalent, molecular, or metallic types. 11. Describe phase changes of a substance and be able to define evaporation, vaporization, boiling, condensation, melting, freezing, sublimation, and deposition. 12. Define critical temperature, critical pressure, and triple point. 13. Draw and use a phase diagram to determine the phase of a compound at a given temperature and pressure or to illustrate phase changes. SCANS or Core Curriculum Statement and Other Standards Credits: 4 for Chem 1411: 3 credits for lecture and 1 credit for lab (not separable)

5 16-WEEK PROPOSED COURSE CALENDAR CHEM 1411 page 5 Week 1: Week 2: Week 3: Week 4: Jan. 17: Welcome, Course Overview, Syllabus, Chapter 1: Chemistry Jan. 19: Chapter 1: Chemistry, cont d Jan. 24: Chapter 2: Atoms, Molecules, and Ions, Lab: Safety Training Jan. 26: Chapter 2: Atoms, Molecules, and Ions, cont d Jan. 31: Chapter 2: cont d, Exp. 1: Measuring Techniques and Calculations Feb. 2: Chapter 3: Mass Relationships in Chemical Reactions Feb. 7: Chapter 3, cont d, Exp. 2: Separation of a Mixture Feb. 9: Chapter 3, cont d / Chapter 4: Reactions in Aqueous Solution Week 5: Feb. 14: Chapter 4, cont d, Test Review (Chapters 1, 2, and 3) Feb. 16: Chapter 4, cont d, take TEST #1 (Chapters 1, 2, and 3) (1 ½ hours) Week 6: Week 7: Feb. 21: Chapter 4, cont d, Exp. 10: Conductivity of Solutions (bring water sample!) Feb. 23: Chapter 5: Gases Feb. 28: Chapter 5, cont d, Exp. 8 : Reactions in Aqueous Solution Mar. 1: Chapter 6: Thermochemistry Week 8: Mar. 6: Chapter 6, cont d / Chapter 7: Quantum Theory, Test Review (Chapters 4 and 5) Mar. 8: Chapter 7 cont d, take TEST #2 (Chapters 4 and 5) (1 ½ hours) *** SPRING BREAK!! MARCH 11-18: No classes *** Week 9: Mar. 20: Chapter 7, cont d, Exp. 12: Heat of Neutralization Measured by Vernier Computer Interface Mar. 22: Chapter 7, cont d / Chapter 8: Periodic Relationships Among the Elements Week 10: Mar. 27: Chapter 8, cont d, Exp. Handout: Colored Flame Lab Mar. 29*: Chapter 9: Chemical Bonding I Week 11: Apr. 3: Chapter 9, cont d, Test Review (Chapters 6, 7, and 8) Apr. 5: Chapter 9 cont d, take TEST #3 (Chapters 6, 7, and 8) (1 ½ hours) Week 12: Apr. 10: Chapter 9, cont d, Exp. Handout: Lewis Structures and Bond Enthalpies Lab Apr. 12: Chapter 10: Chemical Bonding II Week 13: Apr. 17: Chapter 10 cont d, Exp 15: Molecular Geometries of Covalent Molecules Apr. 19: Chapter 11: Intermolecular Forces and Liquids and Solids Week 14: Apr. 24: Chapter 11 cont d, Test Review (Chapters 9, 10, and 11) Apr. 26: Test Review, take TEST #4 (Chapters 9, 10, and 11) (1 ½ hours) Week 15: May 1: Review Chapters 1-6 for Final Exam May 3: Review Chapters 7-11 for Final Exam Week 16: May 8: No class May 10: FINAL EXAM, 8:00 10:00 a.m. Note that starting time is 8:00 a.m.!! Notes: The weeks shown in boxes are those in which a test or exam will be given. * Thursday, March 29, is the last day for course withdrawals at HCC.

6 CHEM 1411 page 6 Instructional Methods Lectures, problem-solving sessions, demonstrations, hands-on laboratory activities, and active student participation exercises will be used to teach the concepts and practice the skills essential to this chemistry course. Student Assignments 1. Homework Assignments Students are responsible for reading and working to comprehend Chapters 1-11 in the textbook. Please read the chapter before the initial lecture on that chapter is given. Homework is assigned to help you learn the concepts and practice the problem-solving skills needed for this course. The homework is essential to preparing you for the tests and the final exam. Homework assignments are to be written clearly on paper, showing all the calculations and/or reasoning used to reach the answer. If an answer is reported without the necessary calculations, you will not receive full credit for the problem. Each homework assignment must be turned in to the instructor for grading on the specified due date. Late homework will not be accepted with one exception: if a student is absent due to illness or personal emergency, the student may turn the homework assignment in at the beginning of the first period that the student returns to class. Assignments that are not turned in on time will receive a grade of zero (0). While you may work with other students on the homework assignments if you so choose, do not copy someone else s work and/or do not allow someone else to copy your work since this defeats the learning value of the homework. The lowest homework score will be dropped from your grade calculation. All of the other homework grades will be averaged together. The homework grade average will count as 10% of your overall course grade. There are two versions of the Chemistry textbook by Raymond Chang in common use: the 10 th edition (recommended) and the 9 th edition (acceptable). There are differences in some of the problem numbers between the two versions. Make sure you refer to the correct problem listing for the textbook edition you have. The proposed homework assignments and due date schedule are shown on the next page. The instructor reserves the right to modify these assignments or due dates if necessary and will communicate these changes clearly in class and on the learning web site.

7 Homework from the 10 th edition of the Chemistry textbook by Raymond Chang, HW Due Chapter Problems 1 Tu, 1/ , 1.9, 1.12, 1.16, 1.22, 1.24, 1.29, 1.34, 1.35(a,b,c), 1.40 CHEM 1411 page 7 2 Tu, 2/ , 2.16, 2.18, 2.21, 2.22, 2.26, 2.36, 2.50, 2.58(not f), 2.60, 2.74, Tu, 2/ , 3.14, 3.16, 3.20, 3.24(b,d,f), 3.44, 3.48, 3.52, 3.60(a,c,e,g,i), 3.66, 3.83, Tu, 2/ , 4.18, 4.20, 4.22(a+c), 4.32, 4.44(c+d), 4.50, 4.54, 4.56, 4.59, 4.62, Tu, 3/ , 5.14, 5.18, 5.19, 5.22, 5.23, 5.32, 5.34, 5.40, 5.52, 5.63, Tu, 3/ , 6.18, 6.20, 6.26, 6.33, 6.34, 6.54, 6.57, 6.62, Tu, 3/ , 7.8, 7.16, 7.20, 7.52, 7.56, 7.58, 7.66, 7.76, 7.78, Tu, 4/ , 8.12, 8.20, 8.28, 8.30, 8.35, 8.38, 8.44, 8.52, 8.56, 8.62, Tu, 4/ , 9.16, 9.36(use Fig 9.5), 9.40, 9.44, 9.46, 9.48, 9.54, 9.64, 9.72, Tu, 4/ , 10.10, 10.14, 10.24, 10.36, 10.46, 10.52, 10.53, 10.80, Tu, 4/ , 11.10, 11.12, 11.16(explain why!), 11.27, 11.38, 11.42, 11.44, 11.48, 11.49, 11.54, 11.59, Homework from the 9 th edition of the Chemistry textbook by Raymond Chang, HW Due Chapter Problems 1 Tu, 1/ , 1.9, 1.12, 1.16, 1.22, 1.24, 1.29, 1.34, 1.35, Tu, 2/ , 2.16, 2.18, 2.21, 2.22, 2.26, 2.36, 2.50, 2.58, 2.60, 2.70, Tu, 2/ , 3.14, 3.16, 3.20, 3.24(b,d,f), 3.44, 3.48, 3.52, 3.60(a,c,e,g,i), 3.66, 3.83, Tu, 2/ , 4.18, 4.20, 4.22(a+c), 4.32, 4.44(c+d), 4.50, 4.54, 4.56, 4.59, 4.62, Tu, 3/ , 5.14, 5.18, 5.19, 5.22, 5.23, 5.32, 5.34, 5.40, 5.52, 5.63, Tu, 3/ , 6.18, 6.20, 6.26, 6.34, 6.35, 6.54, 6.57, 6.62, Tu, 3/ , 7.8, 7.16, 7.20, 7.52, 7.56, 7.58, 7.66, 7.76, 7.78, Tu, 4/ , 8.12, 8.20, 8.28, 8.30, 8.35, 8.38, 8.44, 8.52, 8.56, 8.62, Tu, 4/ , 9.16, 9.36(use Fig 9.5), 9.40, 9.44, 9.46, 9.48, 9.54, 9.64, 9.72, Tu, 4/ , 10.10, 10.14, 10.24, 10.38, 10.46, 10.52, 10.53, 10.80, Tu, 4/ , 11.10, 11.12, 11.16(explain why!), 11.27, 11.38, 11.42, 11.44, 11.48, 11.49, 11.54, 11.59, 11.94

8 CHEM 1411 page 8 2. Laboratory Assignments Experiments will be carried out in laboratory sessions in order to reinforce the chemical concepts being studied and to develop important hands-on laboratory skills. Safety training will be provided so that students will be prepared to work safely. Safety is the top priority in the laboratory and the safety procedures must be followed at all times. Safety goggles must be worn during all laboratory work. Points will be deducted from the laboratory grade if the instructor must remind a student to put on safety goggles. No food or drink is allowed in the laboratory at any time. Any student who does not follow the safety procedures will not be allowed to do the lab experiments and will receive a grade of zero (0) for the laboratory portion of the course grade. For most labs, students will be asked to read and understand the laboratory experiment before coming to the lab. Pre-lab questions may be assigned. There are no make-ups for any laboratory experiment. A grade of zero (0) will be given for any labs you miss. You will be allowed to drop one lab grade during the semester so it is possible to miss one lab experiment due to illness or personal situation without decreasing your grade. You are responsible for arriving on time for lab. If you are late to class and you miss the discussion of lab procedures and safety precautions provided by the instructor, you have yourself become a safety hazard and you will therefore likely receive a grade of 0 (zero) for that lab. Your lab grade will be based on your attendance, participation, attention to safety, performance (including following directions and cleaning up), and lab assignments. Your lab grade will count as 10% of your final course grade. 3. Quizzes Quizzes will be given at the very beginning of class (to encourage punctuality) and are designed to check that the students are keeping up with the textbook reading and are able to utilize the material in the textbook (text, tables, figures, sample problems). Missed quizzes will be recorded as a zero (0) in the gradebook and there are no makeups for any quiz. The two lowest quiz grades will be dropped. The scores on your quizzes will be totaled and then divided by the total number of possible points on the quizzes and converted to a percentage. This quiz grade will count as 6% of your final course grade.

9 CHEM 1411 page 9 4. Tests Four tests, each one covering two or three chapters, will be given in this course. There are no make-ups for any test. If you miss a test for any reason, you will receive a grade of zero (0) on it. You will be allowed to drop the lowest of the four test grades. If you miss a test, then this is the test grade that will be dropped. Each of the other three tests will count as 18% of your course grade for a total of 54%. 5. Final Exam A common final exam covering all 11 chapters will be given to all CHEM 1411 classes. There are no make-ups for the final exam and this final exam score cannot be dropped. If you miss the final exam, you will receive a grade of zero (0) on it. The final exam score will count as 20% of your course grade. Assessments Homework Lab Assignments Quizzes Tests Final Exam: 10% of your final grade (the lowest homework score is dropped) 10% of your final grade (the lowest lab score is dropped) 6% of your final grade (the lowest two quiz scores are dropped) 54% of your final grade (the lowest of the four test scores is dropped; each of the other three tests counts for 18% of your final grade) 20% of your final grade (this is a system-wide comprehensive final) Instructional Materials 1. Textbook: Chang, Raymond (2010) Chemistry (10 th Edition), Boston, MA: McGraw- Hill. (Need Chapters 1 through 11) Important Note: If you plan on purchasing or renting the textbook on-line, please check when you will receive the textbook. We will start using the textbook the first week of class and you will quickly fall behind if you have to wait more than a week for your book to be delivered. 2. Lab Manual: Laboratory Manual for Chem 1411 General Chemistry I by Gholam Pahlavan, Yiyan Bai, and William Askew 3. Safety Goggles (Note: safety glasses are not adequate you must have goggles) 4. Calculator: must have scientific notation, exponent, and logarithm (log and ln) functions. For tests, you must have an actual calculator - you are not permitted to use a calculator application on a cell phone, I-Touch, or other such device.

10 POLICY STATEMENTS CHEM 1411 page 10 ADA: Services to Students with Disabilities Any student with a documented disability (e.g. physical, learning, psychiatric, vision, hearing, etc.) who needs to arrange reasonable accommodations must contact the Disability Services Office at the respective college at the beginning of each semester. Faculty is authorized to provide only the accommodations requested by the Disability Support Services Office. To visit the ADA Web site, log on to click Future Students, then scroll down the page and click on the words Disability Services. For questions, please contact Jaime Torres ( ) or Martha Scribner ( ) at Central Campus or the Disability Counselor at your campus. Academic Honesty Students are responsible for conducting themselves with honor and integrity in fulfilling all course requirements. You are expected to be familiar with the University's Policy on Academic Honesty, found in the HCC catalog. If you are charged with an offense, pleading ignorance of the rules will not help you. Cheating on a test in any form (copying from another student or collaborating with another student during a test, sharing a calculator, using unauthorized materials or cell phones during the test, knowingly obtaining or using a test that has not yet been administered, or other forms of dishonesty) will result in a grade of 0 (zero) on the test for a first offense and a failing grade (F) for the entire course for a second offense. In addition, college officials may recommend probation or dismissal from the College System (see the Student Handbook at for Current Students). Attendance Policy Class Attendance You need to come to all class and lab sessions to do well in this chemistry course! Class attendance is checked daily and you are expected to attend all lectures and labs. Missing a single class or lab may make it difficult to catch up again. If you anticipate that you will miss 3 or more class and/or lab sessions during this semester, this is not the right semester for you to take Chem Absences in this course can cause you to fall behind very quickly and set your course grade on a downward spiral. There are no make-ups for any lab session, quiz, test, or final exam. If you are ill or have a personal emergency that causes you to miss 2 or more class or lab sessions in a row, please notify the instructor by ( janis.stevenson@hccs.edu or chem1411@sbcglobal.net ). If you miss any class, including one during the first week, you are responsible for all material missed. It is a good idea to find someone in class who would be willing to share class notes or discuss missed topics with you if you are absent.

11 CHEM 1411 page 11 Make-Up Policy Homework must be turned in on the assigned due date. If a student is absent due to illness or personal emergency on the homework due date, the student may turn in the homework assignment at the beginning of class of the first class session the student attends following the absence. No credit is given for homework that is turned in late. No make-ups are allowed for any lab session, quiz, test, or final exam. EGLS 3 Evaluation for Greater Learning Student Survey System At Houston Community College, professors believe that thoughtful student feedback is necessary to improve teaching and learning. During a designated time, you will be asked to answer a short online survey of research-based questions related to instruction. The anonymous results of the survey will be made available to your professors and division chairs for continual improvement of instruction. Look for the survey as part of the Houston Community College Student System online near the end of the term. HCC Course Withdrawal Policy If you feel that you cannot complete this course, you will need to withdraw from the course prior to the HCC official final date of withdrawal deadline. For the Spring 2012 semester, this deadline is Thursday, March 29. Please be aware in making your decision that students are allowed no more than SIX (6) total course withdrawals throughout their educational career in obtaining a certificate and/or degree. To help students avoid having to drop/withdraw from any class, HCC has instituted an Early Alert process by which your professor may alert you and HCC counselors that you might fail a class because of excessive absences and/or poor academic performance. It is your responsibility to visit with your professor or a counselor to learn about what, if any, HCC interventions might be available to assist you tutoring, child care, financial aid, job placement, etc. to stay in class and improve your academic performance. If you withdraw from a course, you will receive a W on your transcript for the course. If you do not withdraw before the deadline, you will be assigned the grade you earned in the course. If you quit attending class without officially withdrawing, you will receive a grade of FX, which is a failing grade resulting from lack of attendance. Repeat Course Fee The State of Texas encourages students to complete college without having to repeat failed classes. To increase student success, students who repeat the same course more than twice are required to pay extra tuition. The purpose of this extra tuition fee is to encourage students to pass their courses and to graduate. Effective fall 2006, HCC will charge a higher tuition rate to students registering the third or subsequent time for a course. If you are considering course withdrawal because you are not earning passing grades, confer with your instructor/counselor as early as possible about your study habits, reading and writing homework, test taking skills, attendance, course participation, and opportunities for tutoring or other assistance that might be available.

12 CHEM 1411 page 12 Classroom Behavior You have a shared responsibility with your instructor and your classmates to develop and maintain a positive learning environment for everyone. Your instructor takes this responsibility very seriously and will take action to address the behavior of any student who is hurting the learning environment. As a fellow learner, you are asked to respect the learning needs of your classmates and to assist your instructor in this critical goal. Electronic Devices in the Classroom In order to maximize learning and minimize distractions in the classroom and lab: Please bring your calculator to every class and lab session. Cell phones must be silent or off during all lectures and labs. During tests, cell phones must be turned off and stored out of sight. No text messaging on cell phones is to be done during class or lab. During the class break, you may take care of any phone or text communications. Laptop computers are not to be used during class for any reason. No headphones or ear buds are to be worn during class or lab. Cameras and recording devices are not allowed. Instructor Responsibilities As your instructor, it is my responsibility to: Supply and explain the course syllabus describing the topics to be covered, the grading scale and detailed grading formula explaining how student grades are to be calculated, the required course materials, and the class policies. Provide laboratory safety training. Cover the topics in textbook chapters 1-11 and answer questions on the material. Facilitate an effective learning environment through lectures, class activities, and laboratory work. Assess student performance on homework assignments, laboratory work, quizzes, tests, and the final exam. Arrange to meet with individual students before and after class as needed. Assign final course grades according to the grading formula given. Student Responsibilities To be successful in this class, it is the student s responsibility to: Attend class and lab regularly, missing no more than 3 sessions for the semester. Be on time for lecture and lab; if you are late to a lab session and miss the discussion of lab procedures and safety precautions, you may receive a 0 (zero) for that lab session. If you are late to lecture and miss a quiz, you will receive a 0 (zero) on that quiz. Obtain the required textbook, lab manual, safety goggles, and calculator. Follow all lab directions and work safely in the laboratory. Listen carefully and actively participate in class and lab exercises. Read and comprehend the textbook. continued on next page

13 CHEM 1411 page 13 Student Responsibilities, continued Make time in your busy schedule outside the classroom to study chemistry and keep up with the coursework. Complete the required reading, homework, lab assignments, quizzes, tests, and final exam. Ask for help when there is a question or problem. Utilize the free tutoring services if you need additional help. Determine and make up if possible what was missed during an absence. Analyze and learn from mistakes on assignments, quizzes, and tests. Keep copies of all paperwork, including this syllabus, every handout, and all assignments. Grading Grading Scale % = A 80-89% = B 70-79% = C 60-69% = D Below 60% = F Grading Percentages Homework: 10% of your final grade Labs: 10% of your final grade Quizzes: 6% of your final grade Test A: 18% of your final grade The lowest of the four Test B: 18% of your final grade test scores is dropped. Test C: 18% of your final grade Final Exam: 20% of your final grade Note: Cannot be dropped. Total: 100%