Sample Syllabus

CHE 201

College Chemistry I

Spring, 2012

BOROUGH OF MANHATTAN COMMUNITY COLLEGE The City University of New York Department of Science

Title of Course Course Code

College Chemistry 1 CHE 201

___ Class Hours_4______

Laboratory Hours per Week_____3_______

Semester _____Spring, 2012____________________________ Credits________4_________________________ Instructor Information Name: Telephone: Office: Email: Course Description This is a two-semester course sequence that involves the study of chemical principles including atomic and molecular theories, molecular structure, and reactivity. The laboratory will include experiments illustrating the chemical principles. CHE 201-202 two terms required. Required in A.S. (Science), A.S. (Engineering Science), A.S. (Science for Forensics), and A.S. (Biotechnology Science). Fulfills science requirement for A.A. (Liberal Arts). Prerequisite for CHE 202 is CHE 201. Basic Skills Prerequisites ACR 094, ENG 088 or ESL 062, and MAT 056. Prerequisites____________________________________________________________ Corequisites_____________________________________________________________ Student Learning Outcomes Course Student Learning Outcomes (Students will be able to…) 1. learn the concepts and principles of chemistry.

1

Measurements (means of assessment for student learning outcomes listed in first column) 1. Examinations, Homework Assignments and Laboratory Experiments

CHE 201

College Chemistry I

2. recognize the importance of and develop a skill in problem solving. 3. relate chemistry to other areas of science. 4. unify the diverse topics of chemistry.

Spring, 2012 2. Examinations, Homework Assignments and Laboratory Experiment 3. Examinations, Homework Assignments and Laboratory Experiments 4. Homework Assignments and Laboratory Experiments

Below are the college’s general education learning outcomes, the outcomes that are checked in the left-hand column indicate goals that will be covered and assessed in this course. (Check at least one.) General Education Learning Outcomes

Measurements (means of assessment for general education goals listed in first column) Students will submit written lab reports and answer critical questions in pre-lab and post-lab assignments.

x

Communication Skills- Students will be able to write, read, listen and speak critically and effectively.

x

Quantitative Reasoning- Students will be able to use quantitative skills and the concepts and methods of mathematics to solve problems.

Students will solve problems requiring algebraic manipulation, proportional reasoning, exponential notation and to analyze graphically conceptual and experimental data.

x

Scientific Reasoning- Students will be able to apply the concepts and methods of the natural sciences. Social and Behavioral Sciences- Students will be able to apply the concepts and methods of the social sciences. Arts & Humanities- Students will be able to develop knowledge and understanding of the arts and literature through critiques of works of art, music, theatre or literature. Information & Technology Literacy- Students will be able to collect, evaluate and interpret information and effectively use information technologies. Values- Students will be able to make informed choices based on an understanding of personal values, human diversity, multicultural awareness and social responsibility.

Homework assignments, examinations, and experimental observations.

2

CHE 201

College Chemistry I

Spring, 2012

Required Text & Readings 1. Moore, John W., Stanitiski, Conrad L., and Jurs, Peter C., Chemistry The Molecular Science 4td Edition, Brooks/Cole Cengage Learning (2011) ISBN 978-14390-4930-3 2. Wentworth, R. A. D., Experiments in General Chemistry 9th Ed, Brooks/Cole Cengage Learning (2009), ISBN 978-0-618-94988-5 Other Resources Use of Technology (if applicable) Evaluation & Requirements of Students Examinations 5@10% Final Examination (Comprehensive) Laboratory

50% 20%. 30%

College Attendance Policy At BMCC, the maximum number of absences is limited to one more hour than the number of hours a class meets in one week. For example, you may be enrolled in a threehour class. In that class, you would be allowed 4 hours of absence (not 4 days). In the case of excessive absences, the instructor has the option to lower the grade or assign an F or WU grade. Academic Adjustments for Students with Disabilities Students with disabilities who require reasonable accommodations or academic adjustments for this course must contact the Office of Services for Students with Disabilities. BMCC is committed to providing equal access to all programs and curricula to all students. BMCC Policy on Plagiarism and Academic Integrity Statement Plagiarism is the presentation of someone else’s ideas, words or artistic, scientific, or technical work as one’s own creation. Using the idea or work of another is permissible only when the original author is identified. Paraphrasing and summarizing, as well as direct quotations, require citations to the original source. Plagiarism may be intentional or unintentional. Lack of dishonest intent does not necessarily absolve a student of responsibility for plagiarism. Students who are unsure how and when to provide documentation are advised to consult with their instructors. The library has guides designed to help students to appropriately identify a cited work. The full policy can be found on BMCC’s web side, www.bmcc.cuny.edu. For further information on integrity and behavior, please consult the college bulletin (also available online).

3

CHE 201

College Chemistry I

Outline of Topics Week Ch/ Sec

Topic

Spring, 2012

Pages

The Nature of Chemistry 1

1.1 1.2 1.3 1.4 1.5 1.6 1.7 1.8 1.9 1.10 1.11 1.12

Why Care About Chemistry Molecular Medicine How Science is Done Identifying Matter: Physical Properties Chemical Changes and Chemical Properties Classifying Matter: Substances and Mixtures Classifying Matter: Elements and Compounds Nanoscale Theories and Models Atomic Theory Chemical Elements Communicating Chemistry: Symbolism Modern Chemical Sciences

2–3 3–5 6–6 7 - 11 11 - 13 13 - 15 15 - 17 17 - 20 21 - 23 23 - 26 27 - 28 29 - 30

Atoms and Elements 2

2.1 2.2 2.3 2.4 2.5 2.6 2.7 2.8 2.9

Atomic Structure and Subatomic Particles Nuclear Atom Atom Size Uncertainty and Significant Figures Atomic Numbers and Mass Numbers Isotopes and Atomic Weight The Mole Molar Mass Periodic Table

41 - 43 43 - 44 45 - 50 50 - 53 53 - 56 56 - 59 59 - 60 61 - 62 62 - 66

Chemical Compounds 3

4

3.1 3.2 3.3 3.4 3.5 3.6 3.7 3.8 3.9 3.10 3.11

Molecular Compounds Naming Binary Inorganic Compounds Hydrocarbons Alkanes Ions and Ionic Compounds Naming Ions and Ionic Compounds Properties of Ionic Compounds Moles of Compounds Percent Composition Determining Empirical and Molecular Formulas Biological Periodic Table

Quantities of Reactants and Products

4

76 - 78 79 - 80 80 –83 83 - 85 85 - 90 91 - 93 94 - 98 98 - 102 103 - 104 104 - 107 107 - 109

CHE 201

5

College Chemistry I

4.1 4.2 4.3 4.4 4.5 4.6 4.7

Spring, 2012

Chemical Equations Chemical Reactions Balancing Chemical Equations Mole and Chemical Reactions Limiting Reactants Percent Yield Percent Composition and Empirical Formulas

121 - 122 122 - 128 122 - 131 131 - 136 137 - 142 142 - 145 145 - 149

Chemical Reactions 6

5.1 5.2 5.3 5.4 5.5 5.6 5.7 5.8

Precipitation Reactions Acid Base Reactions Oxidation Reduction Reactions Oxidation Numbers and Redox Reactions Displacement Reactions, Redox and the Activity Series Solution Concentration Molarity and Reactions in Aqueous Solutions Aqueous Solution Titrations

162 - 168 168 - 176 179 - 183 183 - 186 186 - 189 189 - 195 195 - 198 198 - 199

Energy and Chemical Reactions 7

8

6.1 6.2 6.3 6.4 6.5 6.6 6.7 6.8 6.9 6.10 6.11 6.12

The Nature of Energy Conservation of Energy Heat Capacity Energy and Enthalpy Thermochemical Equations Enthalpy Changes for Chemical Reactions Where Does Energy Come From? Calorimetry Hess’s Law Standard Molar Enthalpies of Formation Chemical Fuels Energy from Foods

212 - 215 215 - 220 220 - 224 224 - 230 230 - 232 232 - 236 236 - 238 238 - 242 243 - 244 244 - 249 249 - 254 254 - 257

Electron Configuration and the Periodic Table 9

9

7.1 7.2 7.3 7.4 7.5 7.6 7.7 7.8 7.9

Electromagnetic Radiation and Matter Plank’s Quantum Theory Bohr Model of the Hydrogen Atom Quantum Mechanical Model of the Atom Quantum Numbers, Energy Levels and Orbitals Atomic Orbital Shapes Atom Electron Configurations Ion Electron Configurations Atomic Radii

5

272 – 274 274 – 279 279 – 285 285 – 288 288 - 294 294 - 295 296 – 302 302 – 306 306 – 309

CHE 201

College Chemistry I 7.10 7.11 7.12 7.13

Ionic Radii Ionization Energies Electron Affinities Ionic Compound Formation

Spring, 2012 309 – 311 311 – 314 314 – 314 315 – 317

Covalent Bonding 10

11

8.1 8.2 8.3 8.4 8.5 8.6 8.7 8.8 8.9 8.10 8.11 8.12

Covalent Bonding Lewis Structures Hydrocarbon Structures Multiple Covalent Bonds Multiple Covalent Bonds in Hydrocarbons Bond Length and Bond Energy Bond Polarity and Electronegativity Formal Charge Lewis Structures and Resonance Exceptions to the Octet Rule Aromatic Compounds Molecular Orbital Theory

328 – 329 329 – 334 334 – 336 337 – 339 339 – 342 342 – 347 347 – 350 350 – 352 352 – 355 355 – 358 359 – 360 360 –366

Molecular Structures

13

9.1 9.2 9.3 9.4 9.5 9.6 9.7

Molecular Models VSEPR Hybridization Hybridization in Molecules with Multiple Bonds Molecular Polarity Intermolecular Forces DNA

376 –377 377 – 389 390 – 395 395 –397 397 – 401 402 – 410 410 – 414

Gases and the Atmosphere 14

15

10.1 10.2 10.3 10.4 10.5 10.6 10.7 10.8

The Atmosphere Gas Pressure Kinetic Molecular Theory Ideal Gases Quantities of Gases in Chemical Reactions Gas Density and Molar Mass Gas Mixtures and Partial Pressures Real Gases Examination Week

6

425 - 427 427 - 429 429 - 433 433 - 441 442 - 443 444 - 446 447 - 451 451 - 453

CHE 201 Expt

College Chemistry I Title

Spring, 2012 Page

Laboratory Safety, Laboratory Rules and Check In 1C

Measurements of Mass and Volume

33

1A

Identification of Unknown Compound

15

1B

Paper Chromatography

23

2

Isotopes and Mass Spectroscopy

43

3A

Empirical Formula of an Oxide

59

3B

Hydrates and Their Thermal Decomposition

67

4B

Ionic Reactions in Aqueous Solutions

89

4C

How Much Acetic Acid in Vinegar?

99

6

Thermochemistry and Hess’s Law

125

7

Absorption Spectrum of Cobalt (II) Chloride

141

8

Solubilities Within A Family

155

9A

Identity of an Insoluble Precipitate

163

10A

Geometric Isomers

181

5B

Decomposition of Potassium Chlorate

115

7