Principles of Chemistry I and Laboratory
Title: Principles
of Chemistry I and Laboratory
SCI123_32
Spring Semester 2019
Meeting Day and Times Lab: 10:30 AM-1:15 PM Wednesday 3-513
Lecture: 10:30 AM-1:15 PM Fridays 3-448
Instructor: Dr. Kimberly Stieglitz
Required Course Readings
Chemistry 2e: https://openstax.org/details/books/chemistry
Paul Flowers, University of North Carolina at Pembroke
Klaus Theopold, University of Delaware
Richard Langley, Stephen F. Austin State University
PRINT BOOK ISBN-10 1-938168-39-9 PRINT BOOK ISBN-13 978-1-938168-39-0
PDF VERSION ISBN-10 1-947172-09-3 PDF VERSION ISBN-13 978-1-947172-09-8 ENHANCED TEXTBOOK ISBN-10 1-938168-12-7 ENHANCED TEXTBOOK ISBN-13 978-1-938168-12-3
and selected problems from: Chang and Goldsby, McGraw Hill Education 12th Edition ISBN-13: 978-0078021510
Principles of Chemistry I Laboratory Manual 2nd Edition ISBN13: 978-1-60036-794-6
Required Materials:
Electronic Calculator capable of displaying scientific notation and performing logarithmic and exponential functions (ln x, log x, ex, 10x)
LAB COATS ARE REQUIRED FOR ALL LABORATORY SESSIONS
Supporting Materials:
Internet support including copies of the syllabus, homework assignments and lecture notes are available at the Course website on MyRCC.
Reserve Materials in Library:
Chemistry / Twelve or eleventh Edition, Raymond Chang, McGraw-Hill
(The text also available in electronic format from McGraw-Hill http://textbooks.zinio.com which should be cheaper)
General Course Description
Principles of Chemistry is a study of fundamental chemical concepts: scientific measurements, matter and energy, stoichiometry, atomic structure, the periodic table, chemical bonding, gases and liquids. The course is designed primarily for students with a concentration in biological or physical sciences and for students interested in transfer to a four-year program in engineering. A three-hour lab session is required each week.
Prerequisites: English Composition I (ENG101) Eligible; Pre-Calculus (MAT103) Corequisite; General Science (SCI 099) or Placement.
PREMED/NURSING STUDENTS PLEASE NOTE: This course is intended for students planning to transfer as science majors. This includes students who are considering being PREMED when transferring to four year colleges and universities. Nursing/Health Careers students planning on applying to Nursing School or other allied health programs should take SCI121 not this course.
Principles of Chemistry I and II and Lab (SCI123 and SCI124), fulfills the chemistry requirement of biology, pharmacy, premed, prevet, engineering, or chemistry majors. It is expected that the student will go on to the second semester of this sequence Principles of Chemistry II (SCI124) or equivalent; SCI123 is not designed to be a one semester introductory course. This course is generally viewed as a science major introductory chemistry class. If your intended program of study is a physical science, pharmacy, pre-med/pre-vet, or engineering major this course is required. Laboratory work serves to reinforce concepts as well as introduce students to the scientific method, basic laboratory techniques, and the importance of safety in the laboratory environment.
Students in most allied health programs and non-science majors filling a science elective should enroll in General Chemistry I (SCI121). The SCI123 course is not designed to be a one-semester overview of general and inorganic chemistry but is the first semester of a two -semester sequence for science and engineering majors. If there are questions regarding whether you need SCI121 or SCI123 for your program of study, discuss this matter with the instructor or your academic advisor.
Student Commitment and Tips
The study of general chemistry for science, pharmacy, engineering and pre-med/pre-vet majors is challenging but not impossible. In order to be successful in this course you will need to be aware of the following:
The course material is defined by the course content of previous SCI123 courses and the content of the science major general chemistry courses at other institutions. As a result there is a lot of material to be covered in one semester (15 weeks) and in general the material builds on concepts developed earlier in the semester. As a result it is your responsibility to keep up with reading, lectures and homework. Especially in a course which relies on earlier concepts to explain newer, more complex ideas it is imperative that you pace yourself accordingly. You will find a good way to perform poorly in this course is to wait until just before the next quiz or exam and “cram” your studying into a short (sometimes caffeine enhanced) burst of intensive effort.
You will need some math skills in order to be successful in this course. Intermediate Algebra (MAT 099) or its equivalent is a prerequisite for this course. You will be expected to understand scientific notation and the use of logarithms and exponents. You should have a calculator which can display in scientific notation and perform logarithm functions. How you approach a problem logically and set-up the solution is more important than the numerical answer. When you approach problems, try to think and execute the solutions clearly. Use common sense in your problem solving -- is the number on your calculator display one that makes sense? There should be no shortage of paper for this class so set out your answers so both you and I can follow them.
Expect to read the chapter several times as well as review your lecture notes before attempting the homework problems. In general a high level of effort expended on solving homework problems will lead to a greater probability of success in examinations and quizzes. It is very easy to deceive yourself into a false sense of confidence regarding homework problems if you look at the problem and then follow a written solution or flip constantly into the chapter to refresh yourself on the important points. You will be much better off to reread the chapter and attempt the homework problems without looking at the text or answer solutions. Failure to discipline yourself in this activity will lead to poor performance on exams and quizzes as well as the laboratory sessions.
More Study Tips:
It is your responsibility to keep up with the class pace, to understand the reading and the lectures and especially to do the homework. Do not hesitate to ask questions during the lecture and laboratory sessions in order to be sure you understand the material. The chances are that if something is not clear to you, it is also not clear to many of the other students. To be successful in this course you will need to plan to spend at least 10-15 hours per week working on your assignments NOT including class and laboratory time. If you are not willing or unable to meet this commitment, it is recommended that you not take this course at this time. Due to the rigid scheduling there will be no opportunity to make up missed work.
Academic Requirements
You are responsible for:
1. All material covered in class
2. All material assigned in the text
3. Mastering the concepts developed in lecture and text
4. Performing all homework assignments
5. Completing all laboratory assignments
6. Reading and understanding all handout materials
7. Demonstrating proficiency by passing in assigned homework assignments, taking in-class quizzes and examinations, and passing in required laboratory assignments.
Student Learning Outcomes
| As a result of home, classroom and laboratory study, the students at the end of this course will demonstrate the following knowledge and skills: | ||
| OUTCOMES | ACTIVITIES | ASSESSMENT |
| Perform unit conversions of quantities associated with physical and chemical properties | 1. Express numbers in scientific notation. 2. Convert to and from various units using the factor label method and SI unit conversion tables. 3. Apply the distinction between precision and accuracy of data. 4. Express experimental data to the correct number of significant figures |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests. |
| Explain classification of matter based on its composition and physical state. Describe matter on the basis of its atomic makeup. Describe the structure of the atom in terms of protons, electrons, and neutrons and its relationship to the periodic table. | 1. Explore the notion of conservation of matter and energy. 2. Identify the properties of gases, liquids and solids. 3. Examine the difference between physical and chemical processes. 4. Examine the structure of the atom, identify the number of protons, electrons and neutrons for each of the elements. |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems 4. In-class tests |
| Identify basic concepts related to the periodic table. Understand the concept of the mole and its relationship to mass, volume and number of particles. | 1. Identify the basic concept of the mole relative to the number of atoms, molecules, etc. 2. Use the factor/label method of converting mass, volume and number of particles to moles. 3. Use the periodic table to explain some of the properties of the elements. |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests. |
| Explain how atoms form compounds. Name and write chemical formulas for compounds. | 1. Solve problems related to chemical nomenclature. 2. Write balanced chemical equations from a written description of a reaction. |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests. |
| Use symbols and formulas to write chemical equations to represent chemical reactions. Identify different types of reactions. Predict amounts of products resulting from a chemical reaction. | 1. Mass balance calculations.. 2. Identify limiting reactants. 3. Identify reduced and oxidized species in redox reactions. 4. Calculate concentrations from data obtained in acid-base and redox titrations. |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests. |
| Describe the detailed structure of atoms. Describe the arrangement of electrons around the nucleus of the atom. Contrast the Bohr and Quantum theories. Discuss the energies associated with the spectrum of excited atoms. | 1. Calculate the energy associated with the excitation and subsequent return of an electron to its orbital. 2. Write the detailed structure of atoms with atomic orbital diagrams. 3. Relate how the structure of the atom influences the formation of molecules. |
1. Hands-on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests. |
| Discuss the gas laws and the kinetic molecular theory of gases. | 1. Calculate density and molecular mass using the ideal gas law. 2. Calculate diffusion rates of gases and relate these to the molecular mass. |
1. Hands on Lab work. 2. Graded assignments. 3. In-class problems. 4. In-class tests |
Teaching Procedure
The lecture portion of the course will be an informal discussion of the course topics. Questions are encouraged during the discussion and the solution to selected problems is presented and analyzed. In additionl group exercises will be assigned modeled after research in teaching and learning to help everyone with a deeper understanding of fundamental concepts of the course. For details on these in class exercises please go to www.pogil.org. Homework assignments will be issued with a due date normally one week after being assigned. Quizzes will be administered throughout the semester normally on the next class session after a chapter has been completed. The laboratory portion of the course will generally consist of a short discussion by the instructor followed by hands-on experimentation by the student and the generation of a written report after the experiment.
Course Topics/Assignments/Required Course Reading
and Tentative Test Schedule:
Laboratory: 10:30 AM-1:15 PM Wednesdays
Lecture : 10:30 AM-1:15 PM Fridays
| Section 1 | Chapters (Chang/ Openstax): 1, 2, 3. Hour Exam I February 15, 2019 Conversions, Structure of the Atom, Chemical Nomenclature, Mass relationships, The mole and Stoichiometry. |
| Section 2 | Chapters (Chang/Openstax): 4, 5, and 6 Hour Exam II March 29, 2019 Chemical Reactions in Aqueous Solution, Molarity, Titrations, Gas Laws, Enthalpy. |
| Section 3 | Chapters (Chang/Openstax): 7, 8, 9, and 10.1-10.5 (Tentative) Hour Exam III April 26, 2019 Electronic Structure of the Atom, Periodicity, Lewis/Dot Structures, Chemical Bonding |
Final Exam cumulative chapters 1 through 10 Wednesday May 15th 10:30 am - 1:15 pm.
Homework Assignments will be assigned in class including the due date of assignments to be passed in for grading. Note that attempting additional problems can only help you to succeed in this class. The last day to withdraw from the course is April 8, 2019. It is your responsibility to determine if you need to withdraw from the class. Requests for incompletes (IP) grades are honored only under extreme circumstances. Failure to understand the withdrawal process is not sufficient to obtain an IP grade.
Instructional Objectives (Summary)
1. Recognize basic principles involved in the study of chemistry including the importance of measurements used. Use basic scientific units and recognize their relationship to each other, unit conversions and handling large and small numbers.
2. Explain classification of matter based on its composition and physical state. Define physical and chemical properties and recognize physical and chemical changes in matter.
3. Describe matter on the basis of its atomic make-up. Describe the structure of the atom in terms of protons, neutrons, and electrons and its relationship to the periodic table and periodic properties.
4. After learning about atomic properties, explain how atoms form compounds. Recognize the nature of bonds in compounds. Name and write chemical formulas for compounds.
5. Using symbols and formulas, write chemical equations to represent chemical reaction, identify different types of chemical reactions.
6. Do calculations using chemical equations and predict amounts of substances produced in chemical reactions.
7. Discuss theories behind bonding using molecular orbital and related concepts. Show how different types of bonds form. Describe bond properties and how they affect molecular shapes and how molecular shapes are related to chemical activity.
8. Discuss the gas laws and the kinetic molecular theory of gases. Solve problems related to the gas laws.
9. Define properties of liquids and solids. Explain how inter-and intra-molecular forces are responsible for the physical properties of matter. Describe phase changes in matter.
10. Describe different types of solutions and how they form. Distinguish between electrolytes and non-electrolytes and describe factors that affect solubility. Do calculations involving reactions in aqueous solutions.
Specific Educational Course Objectives
1. Students will categorize matter into elements, compounds and mixtures.
2. Students will describe both Dalton and quantum atomic theory including representations of atomic orbitals in terms of fundamental quantum numbers.
3. Students will categorize reactions as acid-base, precipitation or oxidation-reduction reactions.
4. Students will write correct molecular formulas and balance chemical equations.
5. Students will assign oxidation numbers and identify what is being oxidized and reduced in an oxidation-reduction reaction.
6. Students will convert between grams, moles and numbers of atoms or molecules.
7. Students will predict the theoretical quantity in grams and moles produced in a chemical reaction including the identification of a limiting reagent.
8. Students will calculate quantities associated with matter in the gas phase by the algebraic rearrangement of the ideal gas law and related concepts.
9. Students will write appropriate thermochemical equations and calculate enthalpy changes using standard tables and Hess’s Law of summation.
10. Students will predict the electronic configuration of atoms and ions from their position in the periodic table.
11. Students will differentiate between ionic and covalent bonding and be able to describe each of these types of bonding for representative elements using the octet rule.
12. Students will describe electronegativity and interpret how electronegativity differences between atoms affect chemical bonding patterns including ionic vs. covalent bonding as well as polar vs. non-polar bonds.
13. Students will generate acceptable Lewis structures from a molecular formula and predict molecular geometry using the VSEPR model.
14. Students will predict the direction and magnitude of dipole moments based on bonding patterns and molecular geometry.
15. Students will explain covalent bonding using valence bond and molecular orbital models.
16. Students will predict the hybridization of atoms (valence bond model) in structures and chemical formulas.
Laboratory Educational Objectives
1. The student will measure and record experimental data including the proper way to delete incorrect data.
2. The student will record raw data and present experimental results and observations in a scientifically accepted format and using the scientific method.
3. The student will communicate results clearly and neatly and submit a written report of the laboratory results.
4. The student will set up apparatus and generate data from a written procedure.
5. The student will dispose safely and responsibly all chemical wastes generated during the experiment.
6. The student will respond responsibly to potential or real laboratory accidents
7. The student will work with a laboratory partner or in a group to generate experimental data.
8. The student will independently draw conclusions about the experimental system and to report these finding in written form.
9. The student will calculate an enthalpy change from calorimeter data.
10. The student will measure some property of matter in the gas phase.
11. The student will represent and interpret some physical properties by generating and analyzing graphical data.
Laboratory Schedule
SPRING SEMESTER 2019
| Lab # * | Title of Laboratory | Week of |
| Magic Bottle | Lab Safety Orientation/Magic Bottle Experiment | Jan 28th |
| 1 | Introduction to Experimental Measurement | Feb 4th |
| 2 | Density Measurements | Feb 11th |
| 4 | Determination of an Empirical Formula for Magnesium Oxide | Feb 18th |
| 8 | Solution Preparation and Dilution and Beer’s Law Spectrophotometry (2 weeks) | Feb 25th |
| 8 | Solution Preparation and Dilution and Beer’s Law Spectrophotometry (cont.) | Mar 4th |
| 5 | Introduction to Chemical Reactions and Unknown Identification of Precipitant Product | Mar 11th |
| 6 | Quantitative Analysis of Calcium Ion in Solution Variation on Titrations | Mar 25th |
| 7 | Acid-Base Chemistry: Standardization of NaOH Solution and Acetic Acid Content in Vinegar | Apr 1st |
| 10 | Determination of the Ideal Gas Constant R, MW of a Butane, PV Measurements | Apr 8th |
| 9 | Experimental Determination MgO Heat of Formation (ΔHMgO) | Apr 15th |
| 3 | Spectroscopy---Viewing Atomic Emissions of Pure Diatomic Molecules and Measuring Absorbance of a Pure Solution | Apr 22nd |
| 11** | Introduction to Bonding Theory Part I (Ch7) (PC Desktop computers in lab) | Apr 29th |
*Refers to Laboratory Manual, Principles of Chemistry I
Laboratory Manual 2nd Edition ISBN13: 978-1-60036-794-6.
* Week of March 18th is the spring break, so no lab is scheduled for this week.
**SOFTWARE FOR THIS LAB HAS BEEN INSTALLED ON COMPUTERS IN THE LAB IN 513 AND INSTALLED ON LAPTOPS THAT ARE AVAILABLE FOR USE THIS SEMESTER STORED IN PREP ROOM.