Chemistry 123 A Course Syllabus / Fall 2012

Transcription

1 Chemistry 123 A Course Syllabus / Fall 2012 Instructor: Dr. Caleb A. Arrington Course Number and Title: Chem 123 General Chemistry I Meeting Place: RMSC-325 Instructor Office Hours(RMSC 306-A): M 10:00 am 11:00 am W 10:00 am 11:00 am F 2:00 pm 3:00 pm Meeting Time: T, Th: 9:30 am 10:50 am Instructor Caleb.Arrington@Wofford.edu Instructor Campus Phone: (864) Course Description: Chemistry 123 the first course in a two-part sequence that introduces students to the foundational principles of chemistry. Students will be exposed to the theoretical and experimental bases of the molecular structure of matter, measurement systems, theory of gases, thermochemisty, and theories of atomic structure and molecular structure. The course includes three one-hour lectures and one three-hour laboratory each week. Goals of Course: Chemistry 123 provides an introductory discovery of the qualitative and quantitative nature of mater and the changes that it undergoes. Detailed student learning objectives are provided at the course web site. Course Website: Details of the course including: current assignments, lecture handouts, old course exams and a course calendar are found on our course web site: Course Evaluation: The work in Chem 123 is given course credit through the following assessments: Assessment (# of assign.) Total Points Electronic Homework ( 33) 100 ChemActivities (20) 100 Weekly Homework (10) 100 Laboratory Reports (6) 90 Exams (4) 400 Final Exam 200 TOTAL 990

2 Electronic Review Questions: Daily work in college courses is the single most effective study habit for academic success. Cramming for an exam is stressful and does not lead to long-term subject mastery. After most class meetings an on-line assignment using the Moodle program will be made to help you develop a mastery of the course material for that day. Each set of exercises will be worth three points. The three points will be assigned based on the percentage of the assignment successfully completed as follows: (100 % - 85% = 3 pts., 84% - 60% = 2 pts., 59% - 40 % = 1 pt., below 40% 0 pts.). Moodle assignments are due at the start of the next class after they are assigned. Late assignments receive no course credit. These on-line quizzes are individual work. Having another person complete your Moodle assignment is in violation of the Wofford College Honor Code. You may receive help on these problems, but you must be the one entering the answers into the computer. You may attempt the assignment until you have a the score that you want. ChemActivities: As course material is covered in a group activity, work will be collected and graded. Each assignment will be graded out of 5 points. Missed group work cannot be made up. If you have a university excused absence, please see me about performing the assignment at an alternate time. Weekly Homework: Homework problems from the text will be assigned and collected each week. Homework is due each Monday at 2:00 pm. Assigned problems will be given for each set of course material. Homework problems are to be completed in a composition book (not a spiral notebook). Five of the typically twenty problems will be selected for grading. Graded problems are worth two points. Ungraded material has not been evaluated and may in fact be incorrect. Be neat. Messy work may appear incorrect to the grader. A correct response must communicate to the reader the process by which the solution is obtained. Reporting isolated values will not be given full credit. Late homework receives a penalty of three points per day. Working together on homework is encouraged. Laboratory Reports: See the laboratory syllabus for the requirements of a laboratory report. Late laboratory reports receive a penalty of three points per day. Exams: Closed book exams will be given in-class on the following tentative dates: Only approved calculator (ex. TI-30XS) will be permitted. Thursday, September 27 th (Chapters 1-3) Thursday, October 18 th (Chapters 1-5) Tuesday, November 15 th (Chapters 1-8) Thursday, December 6 th (Chapters 1-10) Thursday, December 13 th 9:00 a.m. (Cumulative Final Exam) In the event of a University activity or a significant illness, arrangements for taking an exam at an alternate time may be made by scheduling with me prior to the exam. Missed exams without prior arrangements may not be retaken. Calculators are not to be used as information storage devices. Using calculators as such is considered cheating and will result in an Honor Code violation. Technology Skills: A student completing this course will be proficient in the use of scientific calculators. Students will use document preparation software to produce written laboratory reports. Additionally, course participants will be introduced to molecular modeling software on a personal computer.

3 Absence Policy: Success in the course will rely heavily upon class attendance. In the event of a University activity or a significant illness, arrangements for taking an exam at an alternate time may be made by scheduling with me prior to the exam. Missed exams without prior arrangements may not be retaken. Statement for Academic Integrity: All work in the laboratory and course is conducted under the Honor Code of Wofford College. Any case of academic dishonesty will be dealt with to the fullest extent of the honor code. Required Course Materials: Lecture Texts: (1.) R. Chang, Chemistry, 11 th Ed., McGraw-Hill, Inc., (2.) Moog and Garoutte, An Inquiry into Chemistry, John Wiley and Sons, Inc ISBN. Laboratory Safety Glasses: These safety classes are available in the bookstore and are required for all laboratory work. Calculator: A scientific calculator is a requirement for this course. However, programmable calculators with alpha-numeric functionality (ex. TI-83) are not permitted during exams. The suggested calculator for this course is the TI-30XS. If you are using another brand of calculator you must have it approved by the instructor prior to the exam. Unapproved calculators will not be allowed during any exam. Late work: All work in this course receives a three point per day late penalty. Unless

4 Final Grade: Final grades will be based on the total number of course points accumulated throughout the semester. Skipping a 3-point homework assignment is the same as skipping a 3-point problem on an exam. Based on a percentage of the total course points the grade distribution below will constitute the final letter grade. (A ) (C ) (A ) (C ) (B+) (D+) (B ) (D ) (B ) (D ) (C+) (F ) below 50 Tentative Schedule for Course: If you believe that you possess a disability that requires accommodation, see me by the end of the first week of class. I am happy to work with anyone desiring accommodation. The instructor reserves the right to change any part of this syllabus during the semester if deemed necessary. When made, these changes will be announced in class.

5 Student Learner Outcomes: Carry out calculations involving density and specific gravity. Perform unit conversion using the factor label technique. Know the names and symbols of all the common chemical elements. Use the rules for significant digits to most accurately express numerical results. Describe Rutherford's scattering experiment and the information it revealed about the structure of the atom. Define atomic number, mass number, neutron number; show how these are related and can be found from standard nuclide notation. Describe the atomic weight scale, and show how the dimensionless units of this scale relate to the actual masses of atoms. Sketch a diagram of a mass spectrometer, and describe its use. Find the average atomic weight of a mixture of isotopes, or find the composition of a mixture of two isotopes from the average atomic weight. Define the mole; explain the physical significance of Avogadro's number. Relate the mass of a substance to the number of molecules or formula units it contains. Be able to name and write formulas for the commonly-encountered ions. Compare the meaning of a formula of a substance such as CH 4 with that of an ionic solid such as KCl. Calculate the fractional or percent composition of a compound from its formula. Find the simplest formula given the masses of the elements contained in a sample of a compound. Write balanced net ionic chemical equations. Calculate the mass or moles of a substance produced or consumed in a chemical reaction. Identify the "limiting reactant" in a reaction in which the initial masses of two or more substances are given, and calculate the quantity of all substances present when the reaction is complete. Express the percent yield of the products in a chemical reaction. Carry out calculations relating solution molarity, mass composition, and dilution. Calculate the molality of a solution. Define an electrolyte, and select examples of electrolytes and non-electrolytes from a list of formulas. Assign oxidation numbers to an element in a compound. Identify the oxidant, reductant, conjugate oxidant, and conjugate reductant. Identify disproportionation reactions. Use solubility guideline to determine if a chemical reaction will form a precipitate. Give the measurements necessary to quantitatively describe a gas. Explain how a pressure-measuring device operates. Use the gas law relations to predict the state of a gas after some change has occurred. Employ the ideal gas equation in stoichiometry calculations. Explain the kinetic molecular theory of gases. Describe the effects experienced by real gas molecules and how this effect ideal behavior. Calculate the amount of heat given off or absorbed in a reaction, given the mass of any one substance and the heat (enthalpy) of the reaction. Define the standard enthalpy of formation of a substance. Use a table of standard enthalpies of formation or combustion to calculate H for a chemical reaction or a phase change. Use Hess' Law to evaluate the H of a chemical change by combining the H's of two or more processes. Use a table of bond enthalpies to estimate the heat of formation of a substance. Explain how a calorimeter works, and how a calorimeter constant is determined and used. Construct or interpret a graph showing how the enthalpy of a substance might vary with temperature, over a range of temperatures encompassing solid, liquid, and gas phases. Define the heat capacity of a substance. State the relationships between the frequency, wavelength and speed of a wave.

6 Give a qualitative description of the electromagnetic spectrum. i.e., the names of the various spectral regions (X-rays, infrared, etc.)and the approximate wavelength limits of visible light. Describe the photoelectric effect: the experimental method and the information obtained from it. Use the Planck constant to relate the energy of a photon to its wavelength. Describe the significance of absorption and emission spectra, and the methods of observing them. Describe the physical significance of the uncertainty principle, with respect to both positionmomentum and energy-time. Describe Bohr's model of the hydrogen atom, and the experimental evidence that led to it. State the main postulates of this model, as well as its principle defects. Sketch a schematic energy level diagram for a hydrogen-like atom, showing the ground state and the onset of the continuum. Explain the significance of the latter. Describe the effect that quantum mechanics has had on our view of the atom since Bohr's model was introduced; how does quantum theory explain the inability of the electron to fall into the nucleus? Describe the physical significance of the quantum numbers n, l, m, and s, and the rules that govern the values they can have. Use the "Aufbau principle" to work out a plausible electron configuration for any element, given the atomic number. Identify the principal groups of elements in the periodic table (alkaline earths, actinides, halogens, etc.) and describe the electron configurations common to all elements of a given group. Describe and explain periodic trends in atomic radius, ionization energy and electron affinity. Recognize an isoelectronic series of species, and order them according to atomic radius. Use a activity series to predict if a chemical reaction will occur. Describe the principal measurable properties of chemical bonds, and comment on their significance. Write a chemical reaction whose energy change would correspond to a given bond energy. Describe the fundamental requirements for the formation of a chemical bond in terms of both energetics and electron distribution. Describe Lewis' theory of the covalent bond; explain the physical origin of the Octet Rule. Write Lewis "electron-dot" formulas for simple molecules and ions composed of elements in the first two rows of the periodic table. Explain the meaning of electronegativity, and predict the relative electric charge distribution in a bond on the basis of the locations of the two elements in the periodic table. Write appropriate "resonance structures" for a molecule such as NO 3 or HCOO, and explain their physical meaning. Predict the shape of a molecule on the basis of the numbers of bonding and nonbonding electrons around the central atom. Discuss how the concept of hybrid orbitals serves as a useful model to explain bonding in many simple molecules. Give examples of sp, sp 2, sp3 hybridization in simple molecules based on firstrow atoms. Show how hybrid orbitals involving d electrons can be used to explain the bonding in molecules having square-planar and octahedral coordinations. Show how pi- and sigma bonds arise in molecules such as HCCH, H 2 CCH 2, HCN, and H 3 CCH 3. Describe the basic concepts involved in the molecular orbital model, and the physical nature of bonding and antibonding orbitals. Use simple molecular orbital theory to predict the bond order and paramagnetism in small diatomic molecules. Identify the three common states of matter. Explain three types of internuclear forces and how their strength effects their physical properties. Name the phase changes and the sign of H trans.