CHEMISTRY 1211K Course Syllabus, Fall 2013

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1 CHEMISTRY 1211K Course Syllabus, Fall 2013 Prerequisite: High School Chemistry and Algebra Text: Chemistry: A Molecular Approach by Nivaldo Tro 3rd edition with Mastering General Chemistry Required Laboratory Materials: 1) a stitched binding notebook for laboratory work (note: spiral, cemented, or loose-leaf notebooks are not acceptable!); 2) safety glasses or goggles Instructor: Dr. Doyle Barrow dbarrow@gsu.edu Phone: (404) Office: 434D Kell Hall Office Hours MW 1:15 2:15 (Other times are available by appointment: There is a sign up sheet outside my office) Lecture: MWF 12:00 12:50 Note reguarding office hours: If you come to office hours bring your book, your lecture notes and your attempt at the homework Week Benginning Monday Wednesday Friday August 26 th Orientation/lecture Lecture Quiz I Sept 2 nd Lecture Lecture Quiz 2 Sept 9 th Labor Day Lecture Quiz 3 Sept 16 th Lecture Review Exam I Sept 23 rd Lecture Lecture Quiz 4 Sept 30 th Lecture Lecture Quiz 5 Oct 7 th Lecture Lecture Quiz 6 Oct 14 th Review Exam II Lecture Oct 21 st Lecture Lecture Quiz 7 Oct 28 th Lecture Lecture Quiz 8 Nov 4 th Lecture Lecture Exam III Nov 11 th Lecture Lecture Quiz 9 Nov 18 th Lecture Lecture Quiz 10 Nov 25 th Thanksgiving Break Thanksgiving Break Thanksgiving Break Dec 2 nd Lecture Review Exam IV Dec 9 th Review Exam 1 will cover chapters 1 and 2 Exam 2 will cover chapters 3 and 4 Exam 3 will cover chapters 5 and 6 Exam will will cover chapter 9 plus parts of 7, 8 and 10

2 Chapters will be covered in order The last day to withdraw and receive a W is October 15th, 2013 Final Exam is Monday Dec Learning outcomes Learning outcomes are found on the BOR website and are listed below. Common Student Learning Outcomes for the Core Curriculum Quantitative Reasoning and Mathematics: Quantitative reasoning and mathematics will be characterized by logic, critical evaluation, analysis, synthesis, generalization, modeling, and verbal, numeric, graphic, and symbolic problem solving. Scientific Reasoning: Scientific reasoning will be characterized by understanding and applying scientific method, laboratory techniques, mathematical principles, and experimental design to natural phenomena. Content-based Learning Outcomes for Principles of Chemistry As the result of instruction, we expect students successfully completing the Principles of Chemistry I and Principles of Chemistry II courses to understand and remember the following concepts and principles: Properties of Matter 1. Chemistry is the study of the composition and properties of matter, and how those properties are affected by changes in composition and external conditions. 2. All matter has mass and takes up space, and is composed of particles interacting through forces. The properties of matter depend, in part, on the relative strength of interacting forces. This model of matter is useful for explaining the general properties of the three phases of matter (solid, liquid, gas) and the transitions between phases. Atomic Theory 3. All matter is composed of just over 100 different types of particles, called atoms. Matter may be composed of a single type of atom (an element), or different types of atoms may bond to each other in fixed proportions to form compounds (molecules or crystals). A chemical reaction occurs when atoms rearrange their bonding structures, which may include adding or removing atoms to the basic chemical unit, resulting in new compounds.

3 4. Atoms combine chemically as whole units; therefore, a pure compound may be identified by its chemical formula. Different types of atoms have different relative masses; therefore, the number of particles in a fixed sample of a pure substance may be calculated by dividing by the relative mass of the atoms in the substance. The mole is a unit of measurement that has been defined to expedite the conversion between the mass of a substance and the number of particles in a substance. One mole is the quantity of a substance such that the relative mass of all the atoms in the chemical formula is equal to that mass of the substance in grams. 5. It has proven useful in the study of chemistry to recognize different types or classes of reactions; some examples are replacement, combination, combustion, and acid-base reactions. Thermochemistry: Temperature, Heat and Energy 6. Energy is stored in chemical bonds. Therefore, energy may be absorbed or released as chemical bonds are broken and formed in a chemical reaction. Exothermic reactions release heat as a result of a reaction, resulting in warmer surroundings; endothermic absorb heat in a reaction, resulting in colder surroundings. Enthalpy is a measure of the amount of heat absorbed or released in a chemical reaction. 7. Heat and work are two methods for transferring energy from one substance to another. Heat involves random motions of the particles of a substance; work results from non-random motions. 8. Temperature is a property of matter; it is proportional to the average kinetic energy of the particles of a substance. The addition or removal of heat usually (but not always) results in an increase or decrease in temperature, respectively. However, heat added to or removed from a substance may result in other changes in the energy of the substance besides an increase or decrease in random kinetic energy. The Gaseous State 9. Four fundamental properties of all gases are pressure, volume, temperature, and quantity. These properties are related to each other mathematically in a relatively simple way. Observing two properties at a time while holding the other two constant results in the empirical gas laws; an equation relating all four properties simultaneously is called the ideal gas law. The ideal gas law is a very useful but approximate result; variations have been added to the ideal gas law to make it more closely reflects the behavior of real gasses. 10. Kinetic-molecular theory assumes that an ideal gas consists of point-like particles that only interact when they collide, and conserve kinetic energy before and after a collision. The pressure of gaseous systems is described as collisions of the point-like particles with the walls of

4 the container. The ideal gas law may be derived from the assumptions of the theory and the application of classical mechanics to a large aggregate of point-like particles. 11. Measurements made on gaseous systems have lead to the identification of an absolute temperature scale. The lowest possible temperature in this scale is zero, designated as absolute zero. An ideal gas (in theory) would possess no energy at absolute zero, and therefore exhibits no pressure and have no volume. Atomic Structure 12. Experimental evidence supports the concept of a nuclear atom: a positively charged core which occupies less than 1% of the volume of the atom surrounded point-like negatively charged electrons. The positively charged core, or nucleus, is very massive compared to the electrons surrounding it. The motion of the electrons is unspecified: they do not travel around the nucleus in regular or predictable paths, but out best mathematical model suggest they are most likely to be found in specific regions of space known as orbitals. 13. A useful model of the nucleus suggests it is composed of positively charged protons and neutral neutrons, held together by a 'strong force'. The number of protons determines the type of atom; the sum of protons and neutrons determines the relative mass of the atom. 14. Chemical bonding involves a balance of attractive and repulsive forces between the electrons and nuclei. Most descriptions of bonding characterize chemical bonds in terms of the electrons only. Electrons can be described by quantum numbers, which identify the mostly likely locations of the electrons in space and also their relative energies. Quantum numbers are very helpful in explaining the number and types of bonds that an atom may form with other atoms. Periodicity and Chemical Bonding 15. The structure of the periodic chart is the result of electron quantum numbers. The outermost electrons (valence electrons) in a column have certain quantum numbers that are the same, and therefore those elements generally bond and behave chemically in similar ways. An orbital may hold either 0, 1, or 2 electrons, but never more than two electrons. Elements in a row, or period, of the Chart are generally adding electrons to a set pf orbitals with the same 'principal' quantum numbers. The start of a new period represents a significant increase in the energy of an electron compared to the previous period. 16. Experimental evidence has shown that the last column of the periodic table contains a set of mainly unreactive atoms: the noble gases. They share the common property of having completely filled orbitals in their valence shell. This configuration results in an energetically stable atom. One guiding principle of chemical bonding is that attaining the same 'electron

5 configuration' as the noble gasses is desirable, and is often a consequence for atoms in a compound after a chemical reaction. 17. Chemical bonds that result in the transfer of electrons from one atom to another are called ionic bonds; chemical bonds that result from the sharing of electrons are called covalent bonds. The transfer of electrons results in the formation of charged chemical species, called ions. Most chemical bonds are neither purely ionic nor purely covalent in nature. Covalent bonds are often imagined to be the end result of the overlap of atomic orbitals, leading to a new set of 'molecular' orbitals. 18. A method of accounting for valence electrons and their known properties has been developed which is able to help predict bonding patterns in many small molecules and ions (Lewis structures). Geometry, Molecular Structure, and Properties 19. Application of the basics of electrostatic repulsion leads to a systematic method for determining the equilibrium geometry of a molecule. Geometry, bond strength, the distribution of charge (dipoles), and the resulting intermolecular forces determine the properties of pure substances in the liquid and solid states. 21. Process-based Learning Outcomes for Principles of Chemistry As the result of instruction, we expect students successfully completing the Principles of Chemistry I and Principles of Chemistry II courses to be able to successfully complete the following tasks: 1. Write correct formulas for compounds from their names, and vice versa. Identify the meaning of a chemical formula. 2. Balance simple chemical reactions. Explain or interpret the meaning of the coefficients of a balanced chemical reaction and any subscripts. 3. Report numerical answers to word problems using the correct number of significant figures, and evaluate the error in a measurement or calculation. 4. Solve word problems based on realistic chemistry situations, using appropriate mathematical equations associated with the subject at hand and correctly substituting data found in the word problem in the equation(s) in order to solve for an unknown quantity.

6 5. Use dimensional analysis to perform mathematical operations, such as converting between the mass and moles of substances using data obtained from the periodic chart, chemical formulas, and balanced equations. 6. Communicate ideas and concepts using appropriate grammatical forms in both oral and written formats. Furthermore, as a laboratory science, we expect all students who have completed the Principles of Chemistry sequence to: Recognize the importance of safety in a chemistry laboratory and practice appropriate safety rules and policies whenever conduction an experimental investigation. We also expect all students to have had personal experience with the following tasks: 1. Measure and transfer liquids using a beaker, graduated cylinder, volumetric flask, and pipette. 2. Determine the mass of a substance on a balance. 3. Use a burette to perform a titration. 4. Create a solution of known concentration. 5. Observe the effects of a chemical reaction. 6. Classify materials as acids or bases. 7. Use spectrometry to find the concentration of an absorbing species in solution. 8. Measure colligative properties. 9. Observe factors affecting reaction rates. 10. Graph and interpret measured data. NOTE: The Principles of Chemistry course sequence (CHEM 1211 / 1212) is designed for students majoring in science, mathematics, and engineering. Many institutions in the University System of Georgia have other general chemistry courses designed for non-science majors, or for students interested in certain health sciences. The Chemistry Academic Advisor Committee asserts that the most significant difference between the 'majors' course and other, lower-level courses is not in content-based or process-based learning outcomes but in the depth of the material covered and in the level of the mathematics used. Therefore, the learning outcomes presented in this document may also be considered a reasonable guide for lower-level chemistry courses as well, recognizing that certain learning outcomes may not be included in those courses and other outcomes (such as chemistry principles relating to the study of organic chemistry) may be added as important outcomes.

7 For specific information about other general chemistry courses or a particular Principles of Chemistry course, please contact the chemistry department as the appropriate University System institution.. Grading: The course grade is determined according to the following point distribution: Major Exams (Best 3 of 4) 201 pts Quizzes (Best 9 /10) 135 pts Homework 64 pts Lab 200 pts* Final Exam 200 pts Total 800 pts * You must attend your laboratory section at the end of the semester your laboratory instructor will give me a list of students in their section and their laboratory grades Letter grades are assigned based on the following scale (which may be varied slightly): = A = A = A = B = B = B = C = C = C- Grades: There will be four major examinations, chapter homework assignments and chapter quizzes. All of these together make up 2/3 of the lecture grade. No make-up examinations or quizzes will be given. Missed examinations will be recorded as a zero. The remaining 1/3 of the lecture grade will be based on the final examination, a standardized, multiple choice examination covering all the material from CH1211K.. This test is provided by the American Chemical Society (ACS) and is nationally normalized. To receive a passing grade in this course, the student MUST 1) take the final examination, and 2) and meet certain minimum requirements in the laboratory portion of the course.

8 Examinations: The best 3 of the 4 examination grades will be counted toward the student s grade. Each student is allowed to drop one exam grade. There will be no make-up exams. I reserve the right to assign seats for exams or move a student with or without cause during the exams. Quizzes: These quizzes will test mostly algorithmic problem solving, in other words, the student s ability to set up and solve a numerical problem. The best 10 quiz grades out of 11 will be counted toward the final grade. There will be no make-up quizzes. The purpose of these quizzes is 3 fold. 1. The quiz should primarily be used for the student to self-assess their learning and for the instructor to provide feedback to the student. 2. A weekly quiz reinforces the need for students to continually keep on top of the material covered in lecture. 3. It gives the instructor the ability to go back over material that a large number of students are having difficulty with thus tailoring the class toward the students. In grading in-class quizzes and examinations, partial credit will be given for correct setup of numerical problems, but answers are expected in the proper units and expressed to the proper number of significant figures. Use of electronic calculators on examinations is not required, but is strongly encouraged. A scientific calculator with capabilities for square roots, logarithms (base-10 and natural is best), exponent capabilities, and memory registries is recommended. Homework: Homework is through Mastering General Chemistry: You are responsible for knowing all due dates. Our class number is number is MCBARROW You will need to go into the website The instructions are fairly easy. Class Attendance and Preparation: Attendance in class is not recorded (with some few exceptions). However, students are responsible for class preparation and for any material presented in the course of the lectures whether or not it is contained in the textbook. Chemistry is a highly structured course, with each new topic based on others previously developed. Thus it is critical for students to keep consistently up-to-date in their readings and assignments. To fall even one class period behind is to risk considerable difficulty in mastery of future material. Therefore students should 1) review previous material, especially if it was not perfectly understood 2) complete reading assignments before the lecture in which the topics are covered, or at least immediately after the lecture 3) Complete assigned problems and exercises on time, with an emphasis on mastery of concepts and principles involved rather than looking for a formula that will give the expected answer (remember that the question can be asked in a different way and not just with different numbers!) Students are expected to attend all classes and laboratories (even when attendance is

9 not recorded) and are responsible for all assignments and materials presented. In the event of unavoidable absences, it is the responsibility of the student to find out what materials were covered or what assignments made in his or her absence. The University requires that faculty members must, on a date after the midpoint of the course to be set by the Provost (or her designee) 1. give a WF to all those students who are on their rolls but no longer taking the class and 2. report the last day the student attended or turned in an assignment. Your constructive assessment of this course plays an indispensable role in shaping education at Georgia State. Upon completing the course, please take time to fill out the online course evaluation. Students who wish to request accommodation for a disability may do so by registering with the Office of Disability Services. Students may only be accommodated upon issuance by the Office of Disability Services of a signed Accommodation Plan and are responsible for providing a copy of that plan to instructors of all classes in which accommodations are sought. Cell Phones and Beepers: In consideration of your classmates, turn off all sound alerts during every lecture and examinations. There will be no exceptions Chemistry Department Policy on Student Conduct and Integrity: The Georgia State University Policy on Academic Honesty is in force in this course. This includes but is not necessarily limited to infractions in the area of plagiarism, cheating on examinations, unauthorized collaborations, falsification, and multiple submissions. This policy is published in On Campus: the Student Handbook, which is available to all members of the university community. All examinations must represent your individual effort, with no unauthorized aid. To either give or receive unauthorized information during an examination is cheating, as is the use of any unauthorized supplementary material. In addition all laboratory work performed in conjunction with this course must represent your individual effort. Only original data obtained by your own in-laboratory experimentation are permitted to be used, except when expressly authorized by your laboratory instructor. Data from supplementary sources, handbooks, reference literature, etc. must be clearly referenced (title, author, volume, pages(s), etc.). Falsification or destruction of data constitutes cheating as well. Conduct disruptive of class, examinations, or laboratories or falsification or destruction of information related to chemistry courses will be taken as a

10 violation of the policies of the Board of Regents of the University System of Georgia and the Georgia State University Student Code of Conduct, Section 6.0. Any suspected offenses may be referred to the Chairman of the Department or the Dean of Students for appropriate disciplinary action. Syllabus and Assignments: The foregoing provides a general plan for the course, deviations from which may be necessary. The instructor will announce any such changes in class. One of the best ways to prepare for examinations in general chemistry is to work as many problems as possible. This includes problems from the end of chapter problem sets as well as the Mastering Gen Chem problem sets

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