Credits: 4 Lecture Hours: 3 Lab/Studio Hours: 3

Transcription

1 Code: CHEM-100 Title: Principles of Chemistry Institute: STEM Department: Chemistry Course Description: The student will be able to identify and interpret the basic concepts of inorganic chemistry including electronic structure of atoms, periodic behavior, compound information, quantitative relationships between elements, compounds and equations, states of matter, acids and bases. The course is for students who have never had chemistry and who wish to continue into CHEM 101. Prerequisites: MATH-025 or satisfactory completion of College's foundational studies requirement in algebra Credits: 4 Lecture Hours: 3 Lab/Studio Hours: 3 REQUIRED TEXTBOOK/MATERIALS: Textbook: Introductory Chemistry, Steven Zumdahl, 7 th Edition See WebAdvisor and the College Bookstore for textbook information. Laboratory Manual: Foundations of College Chemistry, Hein, Peisen, Best, Miner 14 th Edition, 2013 John Wiley and Sons Inc Safety Goggles: New Jersey state law requires that all students wear appropriate splash and impact proof safety goggles while performing laboratory experiments. They are available at the College Store. Laboratory Coat ADDITIONAL TIME REQUIREMENTS: Students must attend their regularly scheduled weekly laboratory class. COURSE LEARNING OUTCOMES: Upon completion of this course, students will be able to: Utilize critical thinking skills to learn fundamental concepts from basic inorganic, chemistry Use the scientific method to perform chemistry-based problem solving. Reinforcement of chemical concepts will be made as hands-on skills are developed in the laboratory program Solve quantitative problems dealing with conversions Analyze the structure of the atom Differentiate between the various types of chemical reactions

2 GRADING STANDARD: A = % A- = 89-91% B+ = 86-88% B = 82-85% B- = 79-81% C+ = 76-78% C = 70-75% D = 65-69% F = <65% Unit examination results will be reported as the grade assigned by the faculty calculated to the first decimal place. These grades will be weighed according to course grading policy. In calculating the course grade, 0.5 will round up to the next numerical grade and 0.4 will round down to the next lower numerical grade. COURSE CONTENT: Unit 1: Introduction; Mathematical review, Dimensional analysis, Conversions, Introduction to the periodic table Unit 2: Nomenclature of chemical compounds,chemical equations Unit 3: Stoichiometry Unit 4: Energy,atomic theory,chemical bonding Unit 5: Gases, Solutions, Acids and Bases DEPARTMENT POLICIES: 1. Students must attend their regularly scheduled weekly laboratory section. Students are not allowed to attend any other lab section for any reason. 2. Students must pass (65% or better) both the lecture and the laboratory portion of the course in the same semester or they will fail the course. COLLEGE POLICIES: For information regarding: Brookdale s Academic Integrity Code Student Conduct Code Student Grade Appeal Process Please refer to the BCC STUDENT HANDBOOK AND BCC CATALOG. NOTIFICATION FOR STUDENTS WITH DISABILITIES: Brookdale Community College offers reasonable accommodations and/or services to persons with disabilities. Students with disabilities who wish to self-identify must contact the Disabilities Services Office at (voice) or (TTY) to provide appropriate documentation of the disability, and request specific accommodations or services. If a student qualifies, reasonable accommodations and/or services, which are appropriate for the college level and are recommended in the documentation, can be approved. ADDITIONAL SUPPORT/LABS: Lab/instructional assistants are available for help both for lab and lecture. The times of availability are posted in MAS 025.

3 UNIT I: Chapters 1-4 Learning Outcomes Recommended Learning Materials 1. Investigate the importance of chemistry Read , 1.5 and how to succeed in a chemistry course 2. Examine the scientific method Read Questions Perform operations using scientific Read 2.1 notation Questions Use the metric system to convert Read between powers of 10. Identify common Memorize table 2.2 units of measurement. Questions Express measurement uncertainties and perform calculations with significant figures. 6. Use dimensional analysis to convert between units 7. Perform calculations between the three temperature scales 8. Perform calculations using density and specific gravity 9. Compare and contrast the three different states of matter 10. Distinguish between physical and chemical properties and changes 11. Distinguish between elements and compounds 12. Categorize substances as either mixtures or pure compounds. Categorize mixtures as either homogenous and heterogenous. 13. Explore techniques to separate components of a mixture 14. Examine the elements and identify names and symbols for the common elements 15. Examine Dalton s atomic theory and the law of constant composition 16. Explore the information provided by a chemical formula 17. Examine the subatomic parts that make up an atom 18. Examine isotopes and solve basic isotope problems 19. Categorize elements on the periodic table with respect to groups, periods, metals, nonmetals, and metalloids 20. Explore the natural states of some elements Read Questions 31-37, Read 2.6 Questions Read 2.7 Questions Read 2.8 Questions Read 3.1 Questions 1-8 Read 3.2 Questions Read 3.3 Questions Read 3.4 Questions Read 3.5 Questions Read Memorize names and symbols for elements 1-54 Questions7-13 Read 4.3 Questions Read 4.4 Questions Read Questions Read 4.7 Questions Read 4.8 Questions Read 4.9

4 21. Explore how ions are formed and use the periodic table to predict charges of the ions and formulas of organic ionic compounds. Read Questions 70-73, 76-78, 81-84

5 UNIT II: Chapters Apply nomenclature rules to binary ionic Read 5.2 compounds Questions Apply nomenclature rules to covalent Read 5.3 compounds Memorize table 5.3 Questions Review nomenclature rules for binary Read 5.4 compounds Questions Apply nomenclature rules to naming Read 5.5 compounds that contain polyatomic ions Memorize table 5.4 Questions Apply nomenclature rules to write Read 5.7 chemical formulas from names Questions Examine the evidence that indicates a Read 6.1 chemical reaction has taken place Questions Examine the parts of a chemical Read 6.2 equation Questions 7-12, Balance a chemical equation and Read 6.3 understand the information provided in a Questions chemical equation. 9. Predict whether a chemical reaction will Read 7.1 occur Question Use solubility rules to predict if a Read 7.2 precipitation reaction will occur Questions Write balanced equations (molecular, Read 7.3 ionic, net ionic) for double displacement Questions reactions. 12. Analyze acids and bases as well as Read 7.4 their reactions Questions Examine oxidation reduction reactions Read 7.5 Questions Classify various types of reactions Read such as precipitation, double displacement, Questions acid-base, oxidation-reduction, combustion, synthesis, decomposition

6 UNIT III: Chapters Demonstrate how large numbers can Read 8.1 be counted by weighing Question 1 2. Perform calculations relating numbers, Read grams, and moles Questions 5,6, Use molar mass to convert between Read mass and moles Questions Calculate the percent composition of a Read 8.6 compound from its formula Questions Distinguish between empirical and Read molecular formulas. Determine empirical Questions 55-62, and molecular formulas from appropriate data 6. Use a balanced chemical equation to Read 9.1 relate amounts Questions Perform mole-mole stoichiometric Read 9.2 calculations Questions Perform mass calculations Read 9.3 Questions Perform limiting reagent calculations Read Questions Perform percent yield calculations Read 9.6 Questions60-64

7 UNIT IV: Chapters Use the law of conservation of energy Read 10.1 Questions Differentiate between temperature and Read 10.2 heat Question 7 3. Use the terms system, surroundings, Read 10.3 exothermic and endothermic to discuss Questions heat flow. 4. Perform basic specific heat calculations Read 10.5 Questions Review Rutherford s model of the atom Read Examine the properties of electromagnetic radiation. Distinguish between different types of electromagnetic radiation. 7. Describe how energy is absorbed and emitted by atoms using the Bohr model 8. Use the guidelines of placing electrons in orbitals to write electron configurations for atoms 9. Differentiate between ionic, covalent, and polar covalent bonding 10. Use electronegativity to predict the type of bonding present in a compound 11. Use bond polarities to describe dipole moments 12. Use electron configurations to explain the charges on ions 13. Use the Duet and Octet rules to draw Lewis Structures. Use resonance to explain why one individual lewis structure is sometimes insufficient to describe a molecule Questions 1-2 Read 11.2 Review figure 11.4 Questions 4,6,8 Read Questions 9, 11-16, 19, Read Questions 29-34, 37, 43, Read 12.1 Questions 3-6 Read 12.2 Questions 9-18 Read 12.3 Questions Read 12.4 Questions Read Questions 54-66

8 Unit V: Chapter Identify common pressure units and Read 13.1 describe how pressure is measured Questions 4,8 2. Examine Boyle s, Charles, and Read Avogodro s Laws qualitatively. No Questions 13-15, 25-27, 39 calculations 3. Use the Ideal gas law to calculate Read 13.5 properties of gases Questions Use Dalton s Law of partial Pressures Read 13.6 to explain and calculate the properties of a Questions collection of gases 5. Use the kinetic Molecular theory of Read gases to explain the properties of gases at Questions a molecular and a macroscopic scale 6. Use the ideal gas equation to solve gas Read stoichiometry problems Questions Examine the phase changes for water Read 14.1 Questions 1,6 8. Distinguish between intermolecular and Read 14.2 intramolecular forces. (no calculations) Questions Identify the different intermolecular Read 14.3 forces Questions Identify the different types of solids and Read describe the bonding in each Questions Examine how various compounds Read 15.1 dissolve Questions Use the terms saturated, unsaturated, Read 15.2 concentrated, and dilute to describe Questions 9-12 solutions 13. Calculate mass % and molarity of a Read solution Questions 21-25, 33-36, Perform dilution calculations Read Review the properties of an acid and a base. Apply both the Arrhenius and Bronsted-Lowry definitions of an acid and a base. 16. Categorize electrolytes, acids, and bases as strong or weak and write their ionization in water 17. Review water as an amphoteric substance, 18. Examine the ph scale and perform basic calculations Questions Read 16.1 Questions 3-10 Read 16.2 Questions 17-20,25-26 Read 16.3 Questions 27-28, Read Questions 37-43