Course Syllabus Course Description Introduction of core chemical concepts to help the student acquire a long-term, meaningful understanding of the basic principles and relevant connections to those principles operating in everyday life. Course Textbook Brown, T. L., LeMay, H. E. Jr., Bursten, B. E., Murphy, C. J., & Woodward, P. M. (2012). Chemistry: The central science, Volume I (12th ed.). Upper Saddle River, NJ: Prentice Hall. Course Learning Objectives Upon completion of this course, students should be able to: 1. Describe the states of matter, their properties, and the effect of chemical measurements on chemical calculations. 2. Utilize the correct units of measurement in calculations to represent mass, length, temperature, volume, density, and energy. 3. Analyze Dalton's atomic theory with respect to the structure of the atom. 4. Describe the organization of the periodic table, and compare and contrast properties of the main group elements. 5. Relate the properties of the transition elements to the formation of coordination compounds. 6. Solve chemical problems relating to stoichiometry, and differentiate between various types of chemical reactions. 7. Summarize the applications of various gas laws and the kinetic molecular theory. 8. Analyze the various theories of chemical bonding, and compare and contrast ionic and covalent bonds. 9. Determine the orbital configuration for each element and describe the use of electron configurations to explain the internal energy of an element. 10. Name chemical compounds, write chemical formulas, and balance chemical equations. 11. Define and determine the implications of the first law of thermodynamics and the law of conservation of energy. 12. Calculate the concentration of a solution using molarity, mole fraction, and mass percent. 13. Apply the laws of thermodynamics to evaluate reaction heat changes qualitatively and quantitatively. 14. Derive and discuss the three-dimensional structure of simple molecules. Credits Upon completion of this course, the students will earn three (3) hours of college credit. Course Structure 1. Unit Learning Objectives: Each unit contains Unit Learning Objectives that specify the measurable skills and knowledge students should gain upon completion of the unit. 2. Written Lectures: Each unit contains a Written Lecture, which discusses lesson material. 3. Reading Assignments: Each unit contains Reading Assignments from one or more chapters from the textbook. 4. Learning Activities (Non-Graded): These non-graded Learning Activities are provided to aid students in their course of study. 5. Key Terms: Key Terms are intended to guide students in their course of study. Students should pay particular attention to Key Terms as they represent important concepts within the unit material and reading. 6. Discussion Boards: Discussion Boards are a part of all CSU term courses. Information and specifications regarding these assignments are provided in the Academic Policies listed in the Course Menu bar. CHM 1030, General Chemistry I 1
7. Unit Assessments: This course contains seven Unit Assessments, one to be completed at the end of Unit I-VII. Assessments are composed of multiple-choice questions and written response questions. 8. Unit Assignments: Students are required to submit for grading Unit Assignments in Units I, V, and VIII. Specific information and instructions regarding these assignments are provided below. 9. Final Exam (Proctored): Students are to complete a Final Exam in Unit VIII. All Final Exams are proctored see below for additional information. You are permitted four (4) hours to complete this exam, in the presence of your approved proctor. This is an open book exam. Only course textbooks and a calculator, if necessary, are allowed when taking proctored exams. 10. Ask the Professor: This communication forum provides you with an opportunity to ask your professor general or course content related questions. 11. Student Break Room: This communication forum allows for casual conversation with your classmates. Unit Assignments When responding to a problem statement, include an in-depth analysis and references. When solving problems, please show your FULL solution steps. Show what is given, then the formula that you are about to use, then the data entered into the formula, followed by your final answer with proper units. Use proper APA format for citing sources and references. Unit I Problem Solving Find the answers to the following problem statements: 1. Mercury, the only metal that exists as a liquid at room temperature, melts at 234.3 K. Convert this melting point to degrees Celsius. 2. Mercury has a boiling point of 356.58 C. Convert this temperature to degrees Fahrenheit. 3. Mercury metal is poured into a graduated cylinder that holds exactly 22.5 ml. The mercury used to fill the cylinder weighs 306.0 g. From this information, calculate the density of mercury, in grams per cubic centimeter. 4. What is the density of mercury in pounds per cubic inch (lb/in 3 )? 1 lb = 454g, 1 in= 2.54 cm. 5. What are some of the physical and chemical properties of Mercury? Mention at least two of each. Unit V Problem Solving In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation anion distances are 2.01 Å (Li F), 2.82 Å (Na Cl), 3.30 Å (K Br), and 3.67 Å (Rb I), respectively. 1. Predict the cation anion distance using the values of ionic radii given in Figure 7.7, on page 257 in the textbook. 2. Calculate the difference between the experimentally measured ion ion distances and the ones predicted from Figure 7.7. Assuming we have an accuracy of 0.04 Å in the measurement, would you say that the two sets of ion ion distances are the same or not? Why, or why not? 3. What estimates of the cation anion distance would you obtain for these four compounds using bonding atomic radii? Are these estimates as accurate as the estimates using ionic radii? Explain your answer. Unit VIII Problem Solving 1. Place the following 5 gases in order of increasing average molecular speed at 300 K: CO, SF6, H2S, Cl2, HBr. Explain your answer. 2. Calculate and compare the rms speeds of CO and Cl2 molecules at 300 K. 3. Calculate and compare the most probable speeds of CO and Cl2 molecules at 300 K. APA Guidelines CSU requires that students use the APA style for papers and projects. Therefore, the APA rules for formatting, quoting, paraphrasing, citing, and listing of sources are to be followed. A document titled APA Guidelines Summary is available for you to download from the APA Guide Link, found in the Learning Resources area of the mycsu Student Portal. It may also be accessed from the Student Resources link on the Course Menu. This document provides links to several internet sites that provide comprehensive information on APA formatting, including examples and sample papers. CHM 1030, General Chemistry I 2
CSU Grading Rubric for Papers/Projects The course papers will be graded based on the CSU Grading Rubric for all types of papers. In addition, all papers will be submitted for electronic evaluation to rule out plagiarism. Course projects will contain project specific grading criteria defined in the project directions. To view the rubric, click the Academic Policies link on the Course Menu, or by accessing the CSU Grading Rubric link, found in the Learning Resources area of the mycsu Student Portal. Final Examination Guidelines Final Examinations are to be administered to students by an approved proctor on a date that is mutually convenient. The student is responsible for selecting a qualified proctor that must be approved by the university. A list of acceptable proctors is provided in the Examination Proctor Policy. To review the complete Examination Proctor Policy including a list of acceptable proctors, proctor responsibilities, proctor approval procedures and the Proctor Agreement Form, go to the mycsu Student Portal from the link below. http://mycsu.columbiasouthern.edu You are permitted four (4) hours to complete this exam, in the presence of your approved proctor. This is an open book exam. Only course textbooks and a calculator, if necessary, are allowed when taking proctored exams. Communication Forums These are non-graded discussion forums that allow you to communicate with your professor and other students. Participation in these discussion forums is encouraged, but not required. You can access these forums with the buttons in the Course Menu. Instructions for subscribing/unsubscribing to these forums are provided below. Click here for instructions on how to subscribe/unsubscribe and post to the Communication Forums. Ask the Professor This communication forum provides you with an opportunity to ask your professor general or course content questions. Questions may focus on Blackboard locations of online course components, textbook or course content elaboration, additional guidance on assessment requirements, or general advice from other students. Questions that are specific in nature, such as inquiries regarding assessment/assignment grades or personal accommodation requests, are NOT to be posted on this forum. If you have questions, comments, or concerns of a nonpublic nature, please feel free to email your professor. Responses to your post will be addressed or emailed by the professor within 48 hours. Before posting, please ensure that you have read all relevant course documentation, including the syllabus, assessment/assignment instructions, faculty feedback, and other important information. Student Break Room This communication forum allows for casual conversation with your classmates. Communication on this forum should always maintain a standard of appropriateness and respect for your fellow classmates. This forum should NOT be used to share assessment answers. Grading Discussion Boards (8 @ 3.5%) = 28.0% Unit Assessments (7 @ 5.5%) = 38.5% Assignments (3 @ 4%) = 12.0% Final Exam = 21.5% Total = 100.0% CHM 1030, General Chemistry I 3
Course Schedule/Checklist (PLEASE PRINT) The following pages contain a printable Course Schedule to assist you through this course. By following this schedule, you will be assured that you will complete the course within the time allotted. CHM 1030, General Chemistry I 4
Course Schedule By following this schedule, you will be assured that you will complete the course within the time allotted. Please keep this schedule for reference as you progress through your course. Unit I Introduction: Matter and Measurement Chapter 1: Introduction: Matter and Measurement Assessment by Problem Solving by Unit II Atoms, Molecules, and Ions Chapter 2: Atoms, Molecules, and Ions Assessment by Proctor Approval Form Unit III Stoichiometry and Calculations Chapter 3: Stoichiometry: Calculations with Chemical Formulas and Equations Assessment by CHM 1030, General Chemistry I 5
Course Schedule Unit IV Reactions in Aqueous Solutions and Thermochemistry Chapter 4: Reactions in Aqueous Solution Chapter 5: Thermochemistry Assessment by Unit V Structure of Atoms and Periodic Properties of the Elements Chapter 6: Electronic Structure of Atoms Chapter 7: Periodic Properties of the Elements Assessment by Problem Solving by Unit VI Basic Concepts of Chemical Bonding Chapter 8: Basic Concepts of Chemical Bonding Assessment by CHM 1030, General Chemistry I 6
Course Schedule Unit VII Molecular Geometry and Bonding Theories Chapter 9: Molecular Geometry and Bonding Theories Assessment by Request to take Final Exam Unit VIII Gases Chapter 10: Gases Problem Solving by Final Exam by CHM 1030, General Chemistry I 7