MASTER SYLLABUS

2020-2021

A.	Academic Division: Health Sciences

B.	Discipline: Science

C.	Course Number and Title: CHEM 1220 Chemistry II

D.	Course Coordinator:

Assistant Dean: Melinda S. Roepke, MSN, RN

Instructor Information:

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Office Location:	Click here to enter text.

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E.	Credit Hours: 5

Lecture: 4 hours

Laboratory: 3 hours

F.	Prerequisites: CHEM1210

G.	Syllabus Effective Date: Fall, 2020

H.	Textbook(s) Title:

Chemistry: The Central Science (plus Mastering Chemistry)

Author(s): Brown, LeMay, Bursten, Murphy

Copyright Year: 2018

Edition: 14th

ISBN: 9780134557328

Optional Textbooks: Student’s Guide to Accompany Chemistry: The Central Science

Author(s): Hill

Copyright Year: 2018

Edition: 14th

IBSN: 9780134554075

Workbook(s) and/or Lab Manual:

Chemistry 1220 General Chemistry Laboratory Manual, Hayden‐McNeil Publishing, Inc.

Author(s): Hill

Copyright Year: Produced for Ohio State University

Edition:

ISBN: 9780738091105

J.	Course Description: This is the second semester of chemistry for science majors or pre-professional students. A quantitative introduction to intermolecular forces, phase changes, colligative properties, chemical kinetics, chemical equilibrium, acid-base equilibria, thermodynamic, electrochemistry, organic chemistry and nuclear chemistry. Student will be exposed to applications of chemistry in society. (TAG # OSC009; If combined with CHEM1210 TAG # OSC023)

K.	College-Wide Learning Outcomes

College-Wide Learning Outcomes	Assessments - - How it is met & When it is met
Communication – Written
Communication – Speech
Intercultural Knowledge and Competence
Critical Thinking
Information Literacy
Quantitative Literacy

L.	Course Outcomes and Assessment Methods:

Upon successful completion of this course, the student shall:

Outcomes	Assessments – How it is met & When it is met
Demonstrate intermolecular forces and phase diagrams.	Quiz - 2nd week Written lab report Midterm Exam – 4th week Final – 15th week
Describe the solution process and demonstrate colligative properties.	Quiz – 3rd week Written Lab Report Mid-Term Exam – 4th week Final – 15th week
Explain chemical kinetics	Written Lab Report Mid-Term Exam – 4th week Final – 15th week
Demonstrate chemical equilibrium	Quiz – 5th week Written Lab Report Mid-Term Exam-8th week Final Exam – 15th week
Explain and demonstrate acid-base equilibria and buffers.	Quiz-6th, 7th week Written Lab Reports Mid-Term Exam-8th week Final Exam – 15th week m – 8th week
Describe chemical thermodynamics, entropy and free energy.	Quiz-9th week Mid-Term Exam- 12th week Final Exam – 15th week
Explain and demonstrate electrochemistry.	Quiz- 10th & 11th week Written Lab Report Mid-Term Exam-12thweek
Define organic chemistry.	Quiz- 13th week Formal Written Lab Report Mid-Term Exam- 12th week
Explain transition metals & coordination chemistry.	Quiz – 14th week Final Exam – 15th week
Describe nuclear chemistry.	Quiz- 14th week Final Exam 15th week
Discuss social and philosophical implications of scientific discoveries and describe the potential of science and technology to address problems of the contemporary world.	Formal Written Lab Reports - weekly Midterm Exam – 12th week Final Exam – 15th week

M.	Topical Timeline (Subject to Change):

Lecture Topics

Liquids and Intermolecular Forces: A molecular comparison of gases, liquids and solids, Intermolecular forces Select properties of liquids ,Phase changes, Vapor pressure, Phase diagrams.

Properties of solutions: The solution process, Solubility and saturated solutions, Factors affecting solubility

Properties of solutions : Expressing solution concentration, Colligative properties, Colloids

Chemical Kinetics: Reaction rates, Concentration and rate laws, Concentration vs. time, Temperature and rate, Reaction mechanisms

Chemical Equilibrium: The concept of equilibrium, Equilibrium constants, Heterogeneous equilibria, Calculating equilibrium constants (ICE tables), Applications of equilibrium constants, Le Châtelier’s principle

Acid Base Equilibria: Acid‐Base Equilibria, Bronsted‐Lowry acids and bases, the pH Scale, Strong acids and bases, Weak acids and bases, Relationship between Ka and Kb, pH of salt solutions, Chemical structure and acidity/basicity, Lewis acids and bases

Additional Aspects of Aqueous Equilibria : Common ion effect, Buffered solutions, Acid‐Base titrations, Solubility equilibria and Ksp, Factors that affect solubility, Selective precipitation of ions

Chemical thermodynamics: Spontaneous processes, Entropy and the 2nd law of thermodynamics, Molecular interpretation of energy, Gibbs Free Energy, Free Energy Equilibrium

Electrochemistry: Oxidation states and balancing redox reactions, Voltaic cells, Cell potentials, Free energy, redox reactions, the Nernst equation, Batteries and fuel cells, Corrosion, Electrolysis

Organic Chemistry: organic compounds, nomenclature, elementary reactions

Transition metals and coordination chemistry: The transition metals, coordination complexes, Ligands, Nomenclature, Isomerism, Color and magnetism of transition metal compounds, Crystal field theory

Nuclear Chemistry: Radioactivity, Patterns of nuclear stability, Nuclear transmutations, Rates of radioactive delay, Energy changes in nuclear reactions, Nuclear fission and fusion, Radiation in the environment and living systems

Laboratory exercises

Check-in/Intermolecular Forces

Freezing Point Depression

Rate of an Iodine Clock Reaction

Volumetric Analysis: Standardization of NaOH and HCl

Equilibrium

Investigation of Buffer Systems

Some Nonmetals and their Compounds; Hydrolysis of Salts

Qualitative Analysis Group I

Redox Titration

Electrochemistry

Spectrophotometric Analysis of Commercial Aspirin

Research Experience

Synthesis of Acetanilide/Recitation Review/Checkout

N.	Course Assignments:

Homework

Formal Lab Reports

Quizzes, Mid-Term, Final

O.	Recommended Grading Scale:

NUMERIC	GRADE	POINTS	DEFINITION
93–100	A	4.00	Superior
90–92	A-	3.67	Superior
87–89	B+	3.33	Above Average
83–86	B	3.00	Above Average
80–82	B-	2.67	Above Average
77–79	C+	2.33	Average
73–76	C	2.00	Average
70-72	C-	1.67	Below Average
67–69	D+	1.33	Below Average
63-66	D	1.00	Below Average
60-62	D-	0.67	Poor
00-59	F	0.00	Failure

P.	Grading and Testing Guidelines:

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Q.	Examination Policy:

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R.	Class Attendance and Homework Make-Up Policy:

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S.	Classroom Expectations:

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T.	College Procedures/Policies:

Important information regarding College Procedures and Policies can be found on the syllabus supplement located at

http://catalog.ncstatecollege.edu/mime/download.pdf?catoid=5&ftype=2&foid=3