Office hours: Before or after class on Sat by appointment.

Transcription

1 Biology and Physical Sciences Department Central Campus CHEM General Chemistry I CRN Spring 2011 Central Campus - Room LHSB 416 9:00-12:00 Sat Lab LHSB :01-15:00 Sat 3 hour lecture course / 3 hour Lab per week/ 16 weeks Regular semester Instructor: Kareem Khan, MS, PhD Instructor Contact Information: abdul.khan4@hccs.edu Phone: (713) (office) Learning Web: Office hours: Before or after class on Sat by appointment. 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) Course Goal 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. Student Learning Outcomes A student will:

2 CHEM 1411 page 2 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 sophisticated scientific instruments. 5. Increase his/her confidence in learning chemistry to help the student succeed in higher-level courses. Learning objectives By the end of this course, a student should be able to do the following at a minimum: 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 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.

3 CHEM 1411 page 3 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. 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 for a dilution to a specified concentration. 14. Describe the process of titration and define the equivalence point. 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.

4 CHEM 1411 page 4 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 = h 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. 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 varies through the periodic table. 7. Predict how atomic radius varies through the periodic table. 8. Predict how ionic radius varies through the periodic table. 9. Predict how ionization energies vary for the electrons in an element. 10. Define electron affinity and know which elements have high electron affinities. 11. Be familiar with diagonal relationships on the periodic table.

5 CHEM 1411 page 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 for a chemical 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: dipole-dipole, dipole-induced dipole, and dispersion forces. 3. Describe hydrogen bonding and its effects on 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.

6 CHEM 1411 page Describe phase changes of a substance and be able to define evaporation, vaporization, boiling, condensation, melting, freezing, sublimation, and deposition. 12. Define critical temperature and critical pressure. 13. Define triple point. 14. 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 Credit: 4 (3 for theory lecture and 1 for lab, Theory and Lab are inseperable so when the final grades submitted it will be the cumulative grades)

7 CHEM 1411 page 7 Course calendar 22-Jan 29-Jan 5-Feb 12-Feb 19-Feb 26-Feb 5-Mar Welcome, Course Overview, Syllabus, Chapter 1: Chemistry Exp. 1 Lab Safety Training Chapter 2: Atoms, Molecules, and Ions; Exp. 2: Separation of the Components in an Inorganic Mixture pp: 15 Chapter 8: Periodic Relationships Among the Elements; Exp. 10: UV-Vis Spectroscopy Detection of Caffeine pp:111 Test Review (Chapters 1, 2, 8): Exp. 3: The Iron-Copper Molar ratio: Single replacement reaction and limiting reagent pp:29 TEST #1 (Chapters 1, 2, and 8) - Chapter 3: Mass Relationships in Chemical Reactions Chapter 4: Reactions in Aqueous Solution ; Exp. 5: Reactions in Aqueous Solution pp: 53 Test Review (Chapters 3, 4): Exp 6: Determine the retention Time for EtOH, Acetic Aicd & Ethyl Acetate pp: Mar TEST #2 (Chapters 3, 4) ; Chapter 5: Gases 19-Mar *** Spring Break!! MARCH 14-22: No classes *** 26-Mar Chapter 6: Thermochemistry ; Exp. 8: Heat of Neutralization pp: 87 2-Apr Chapter 7: Quantum Theory ; Test Review (Chapters 5, 6, 7) 9-Apr TEST # 3 (Chapters 5, 6, 7) ; Chapter 9: Chemical bonding I: Basic concepts 16-Apr *** Easter Holiday - School Closed *** 23-Apr Chapter 10: Chemical Bonding II ; Chapter 11: Intermolecular Forces and Liquids and Solids 30-Apr TEST # 4 (Chapters 9, 10, 11) ; Student presentation 7-May ** FINAL COMPREHENSIVE EXAM, 10:00 am 01:00 p.m. ** April 21 is the last day for course withdrawals till 4:00pm Instructor reserves the right to make changes in the syllabus if he feels the need to do so.

8 CHEM 1411 page 8 Instructional Methods Face to face 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 It is advised that read the chapter before coming to the class. Homework is assigned to help you learn the concepts and practice the problemsolving 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. 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. No food or drink is allowed in the laboratory at any time. Students are expected to read and understand the laboratory experiment before coming to the lab. Pre-lab questions are will be graded and should be handed over before starting the Experiment.

9 CHEM 1411 page 9 There are no make-ups for any laboratory experiment. Your lab grade will be based on your attendance, participation, attention to safety, performance (including following directions and cleaning up), lab reports, pre-lab and post-lab questions. See syllabus for schedule of experiments Note: Assignments have been developed that will enhance your learning. To better understand a topic, you will be given assignments on key information that you will need to remember for your success in course. 3. 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. Assessments Total grades are distributed in the following way (see table below) Test I 15% Test II 15% Test III 15% Final Test 20% Lab 20% Home work 10% Attendance 5% Bonus presentation 10% Note: All score counts shown above reflect the proportion to over all score of 100. For the tests, the lowest of the four test scores is dropped. Final grade is system wide comprehensive exam, it is mandatory to take this exam for qualifying the course grades. To participate in bonus grade is optional, but class teacher will consider attendance and lab performance of the students before allowing for participation.

10 CHEM 1411 page 10 Instructional Materials Text book: Chemistry by Chang, the 10 th edition published by McGraw Hill (ISBN: ) Useful links: Free Textbook HomePage: Choose 10th edition; then select Resources for free materials (animations, tutorials, quizzes) ChemSkilBuilder: Codes are furnished with new textbooks: More, you can also look at the options on: Lab Book: Chemistry 1411/1412 Laboratory Manual with Instrumental Analysis by Yiyan Bai, Shuhsien Batamo, Carolyn Judd, Dongning Lu, and Shamsuddin Shaikh publisher Houston Community College Central campus (ISBN: ) Note: You must have scientific calculator. 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. HCC Policy Statement - ADA Services to Students with Disabilities Students who require reasonable accommodations for disabilities are encouraged to report to Dr. Becky Hauri at to make necessary arrangements. Faculty is only authorized to provide accommodations by the Disability Support Service Office HCC Policy Statement: Academic Honesty A student who is academically dishonest is, by definition, not showing that the coursework has been learned, and that student is claiming an advantage not available to other students. The instructor is responsible for measuring each student's individual achievements and also for ensuring that all students compete on a level playing field. Thus, in our system, the instructor has teaching, grading, and enforcement roles. You are expected to be familiar with the University's Policy on Academic Honesty, found in the catalog. What that means is: If you are charged with an offense, pleading ignorance of the rules will not help you. Students are responsible for conducting themselves with honor and integrity in fulfilling course requirements. Penalties and/or disciplinary proceedings may be initiated by College System officials against a student accused of scholastic dishonesty. Scholastic dishonesty : includes, but is not limited to, cheating on a test, plagiarism, and collusion. Cheating on a test includes: Copying from another students test paper; Using materials not authorized by the person giving the test; Collaborating with another student during a test without authorization;

11 CHEM 1411 page 11 Knowingly using, buying, selling, stealing, transporting, or soliciting in whole or part the contents of a test that has not been administered; Bribing another person to obtain a test that is to be administered. Plagiarism means the appropriation of another s work and the unacknowledged incorporation of that work in one s own written work offered for credit. Collusion mean the unauthorized collaboration with another person in preparing written work offered for credit. Possible punishments for academic dishonesty may include a grade of 0 or F in the particular assignment, failure in the course, and/or recommendation for probation or dismissal from the College System. (See the Student Handbook) HCC Policy Statements Class Attendance - It is important that you come to class! Attending class regularly is the best way to succeed in this class. Research has shown that the single most important factor in student success is attendance. Simply put, going to class greatly increases your ability to succeed. You are expected to attend all lecture and labs regularly. You are responsible for materials covered during your absences. Class attendance is checked daily. Although it is your responsibility to drop a course for nonattendance, the instructor has the authority to drop you for excessive absences. If you are not attending class, you are not learning the information. As the information that is discussed in class is important for your career, students may be dropped from a course after accumulating absences in excess of 12.5% hours of instruction. The six hours of class time would include any total classes missed or for excessive tardiness or leaving class early. You may decide NOT to come to class for whatever reason. As an adult making the decision not to attend, you do not have to notify the instructor prior to missing a class. However, if this happens too many times, you may suddenly find that you have lost the class. Poor attendance records tend to correlate with poor grades. If you miss any class, including the first week, you are responsible for all material missed. It is a good idea to find a friend or a buddy in class who would be willing to share class notes or discussion or be able to hand in paper if you unavoidably miss a class. Class attendance equals class success. HCC Course Withdrawal Policy If you feel that you cannot complete this course, you will need to withdraw from the course prior to the final date of withdrawal. For the Spring 2011 semester, this is Thursday, April 21, Before, you withdraw from your course; please take the time to meet with the instructor to discuss why you feel it is necessary to do so. The instructor may be able to provide you with suggestions that would enable you to

12 CHEM 1411 page 12 complete the course. Your success is very important. Beginning in fall 2007, the Texas Legislature passed a law limiting first time entering freshmen to no more than SIX 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 online tutoring, child care, financial aid, job placement, etc. to stay in class and improve your academic performance. If you plan on withdrawing from your class, you MUST contact a HCC counselor or your professor prior to withdrawing (dropping) the class for approval and this must be done PRIOR to the withdrawal deadline to receive a W on your transcript. **Final withdrawal deadlines vary each semester and/or depending on class length, please visit the online registration calendars, HCC schedule of classes and catalog, any HCC Registration Office, or any HCC counselor to determine class withdrawal deadlines. Remember to allow a 24-hour response time when communicating via and/or telephone with a professor and/or counselor. Do not submit a request to discuss withdrawal options less than a day before the deadline. If you do not withdraw before the deadline, you will receive the grade that you are making in the class as your final grade. 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. Classroom Behavior As your instructor and as a student in this class, it is our shared responsibility to develop and maintain a positive learning environment for everyone. Your instructor takes this responsibility very seriously and will inform members of the class if their behavior makes it difficult for him/her to carry out this task. As a fellow learner, you are asked to respect the learning needs of your classmates and assist your instructor achieve this critical goal. Use of Camera and/or Recording Devices As a student active in the learning community of this course, it is your responsibility to

13 CHEM 1411 page 13 be respectful of the learning atmosphere in your classroom. To show respect of your fellow students and instructor, you will turn off your phone and other electronic devices, and will not use these devices in the classroom unless you receive permission from the instructor. Use of recording devices, including camera phones and tape recorders, is prohibited in classrooms, laboratories, faculty offices, and other locations where instruction, tutoring, or testing occurs. Students with disabilities who need to use a recording device as a reasonable accommodation should contact the Office for Students with Disabilities for information regarding reasonable accommodations Instructor Requirements As your Instructor, it is my responsibility to: Provide the grading scale and detailed grading formula explaining how student grades are to be derived Facilitate an effective learning environment through class activities, discussions, and lectures Description of any special projects or assignments Inform students of policies such as attendance, withdrawal, tardiness and make up Provide the course outline and class calendar which will include a description of any special projects or assignments Arrange to meet with individual students before and after class as required To be successful in this class, it is the student s responsibility to: Attend class and participate in class discussions and activities Read and comprehend the textbook Complete the required assignments and exams: Bloom s Taxonomy Analysis, Educational Philosophy Paper, Midterm Exam, Final Exam, Field Study Ask for help when there is a question or problem Keep copies of all paperwork, including this syllabus, handouts and all assignments Complete the field study with a 70% passing score Program/Discipline Requirements The Field Study is a discipline requirement of EDUC The field study is essential in your deciding if education is the right career path for you. The field study also reinforces what you are learning in class by connecting theory to the real world of education. This assignment is very important and as such, it must be completed with 70% of possible points or you will not receive a passing grade in this class. Grading Your instructor will conduct quizzes, exams, and assessments that you can use to determine how successful you are at achieving the course learning outcomes (mastery of course content and skills) outlined in the syllabus. If you find you are not mastering

14 CHEM 1411 page 14 the material and skills, you are encouraged to reflect on how you study and prepare for each class. Your instructor welcomes a dialogue on what you discover and may be able to assist you in finding resources on campus that will improve your performance. Grading Scale = A = B = C = D Below 60 = F