MEDGAR EVERS COLLEGE OF CUNY
DEPARTMENT OF PHYSICAL, ENVIRONMENTAL,
AND COMPUTER SCIENCES
SYLLABUS FOR CHM 201–001 GENERAL CHEMISTRY I
INSTRUCTOR:
TEXTBOOK:CHEMISTRY by John McMurry and Robert C. Fay, Fourth Edition, Published by
Prentice-Hall Inc., 20xx
LABORATORY
MANUAL:
LABORATORY EXPERIMENTS by John H. Nelson and Kenneth C. Kemp for Chemistry The Central Science, 9th or 10th Edition, Published by Prentice-Hall Inc.
COURSE DESCRIPTION
CHM 201, General Chemistry I is a the first course of a year-long study of general chemistry. The purpose of the general chemistry sequence, CHM 201 and CHM 202, is to provide students who are science and pre-engineering majors with a solid foundation in the principles of chemistry. The principles studied in this sequence will be necessary in more advanced courses in chemistry such as organic chemistry, biochemistry, and analytical chemistry. These principles also the foundation for all biological processes and hence are necessary for both basic and advanced study of the biological sciences.
PREREQUISITES AND COREQUISITES
The prerequisite for CHM 201 is CHM 112 or the equivalent knowledge of chemistry presented in CHM 112. A grade of C or better must be attained in CHM 112 to proceed to CHM 201. If a student receives a grade of C- or lower in CHM 112, CHM 112 must be repeated. CHM 201 is a prerequisite for CHM 202, General Chemistry II. The General Chemistry sequence, CHM 201 and CHM 202 are prerequisites for the Organic Chemistry sequence, CHM 303 and CHM 304. A corequisite for this course is MTH 151, Precalculus
LECTURE OUTLINE FOR CHM 201
Lecture 1.Begin Chapter 1. Chemistry: Matter and Measurement
Approaching Chemistry: Experimentation
Chemistry and the Elements
Elements and the Periodic Table
Some Chemical Properties of the Elements
Experimentation and Measurement
Measuring Mass
Measuring Length
Measuring Temperature
Derived Units: Measuring Volume
Lecture 2.Finish Chapter 1Derived Units: Measuring Density
Accuracy, Precision, and Significant Figures in Measurement
Rounding Numbers
Calculations: Converting from One Unit to Another
Interlude: Chemicals, Toxicity, and Risk
Lecture 3.Begin Chapter 2.Atoms, Molecules , and Ions
Conservation of Mass and the Law of Definite Proportions
Dalton’s Atomic Theory and The Law of Multiple Proportions
The Structure of Atoms: Electrons
The Structure of Atoms: Protons and Neutrons
Atomic Number
Atomic Mass
Lecture 4.Finish Chapter 2.Compounds and Mixtures
Molecules, Ions, and Chemical Bonds
Acids and Bases
Naming Chemical Compounds
Interlude: Are Atoms Real?
Lecture 5.Begin Chapter 3.Formulas, Equations, and Moles
Balancing Chemical Equations
Chemical Symbols on Different Levels
Avogadro’s Number and the Mole
Stoichiometry: Chemical Arithmetic
Yields of Chemical Reactions
Lecture 6.Continue Chapter 3.Reactions with Limiting Amounts of Reactants
Concentrations of Reactants in Solution: Molarity
Diluting Concentrated Solutions
Solution Stoichiometry
Lecture 7.Finish Chapter 3.Titration
Percent Composition and Empirical Formulas
Determining Empirical Formulas: Elemental Analysis
Determining Molecular Weights: Mass Spectrometry
Interlude: Did Ben Franklin Have Avogadro’s Number? A Ballpark Calculation
Lecture 8.Begin Chapter 4.Reactions in Aqueous Solutions
Some Ways That Chemical Reactions Occur
Electrolytes in Aqueous Solutions
Aqueous Reactions and Net Ionic Equations
Lecture 9.TEST on Chapters 1–3
Lecture 10.Continue Chapter 4.Precipitation Reactions and Solubility Rules
Acids, Bases, and Neutralization Reactions
Oxidation–Reduction (Redox) Reactions
Identifying Redox Reactions
The Activity Series of the Elements
Lecture 11.Finish Chapter 4.Balancing Redox Reactions: The
Oxidation–Number Method
Balancing Redox Reactions: The
Half–Reaction Method
Redox Titrations
Some Applications of Redox Titrations
Interlude: Photography: A Series of Redox Reactions
Lecture 12.Begin Chapter 5.Periodicity and Atomic Structure
Development of the Periodic Table
Light and the Electromagnetic Spectrum
Electromagnetic Radiation and Atomic Spectra
Particlelike Properties of Electromagnetic Radiation: The Planck Equation
Wavelike Properties of Matter: The de Broglie Equation
Lecture 13.Continue Chapter 5.Quantum Mechanics and the Heisenberg Uncertainty
Principle
Wave Functions and Quantum Numbers
The Shapes of Orbitals
Quantum Mechanics and Atomic Spectra
Electron Spin and the Pauli Exclusion Principle
Orbital Energy Levels in Multielectron Atoms
Lecture 14.Finish Chapter 5.Electron Configuration of Multielectron Atoms
Electron Configurations and the Periodic Table
Some Anomalous Electron Configurations
Electron Configurations and Periodic Properties: Atomic Radii
Interlude: The Aurora Borealis: Atomic Spectra on a Grand Scale
Lecture 15.Begin Chapter 6.Ionic Bonds and Some Main–Group Chemistry
Ions and Their Electron Configurations Ionic Radii
Ionization Energy
Higher Ionization Energies
Electron Affinity
Ionic Bonds and the Formation of Ionic Solids
Lecture 16.Finish Chapter 6.The Alkali Metals (Group 1A)
The Alkaline Earth Metals (Group 2A)
The Group 3A Elements: Aluminum
The Halogens (Group 7A)
The Noble Gases (Group 8A)
The Octet Rule
Interlude: Salt
Lecture 17.Begin Chapter 7.Covalent Bonds and Molecular Structure
The Covalent Bond
Strengths of Covalent Bonds
A Comparison of Ionic and Covalent Bonds
Polar Covalent Bonds: Electronegativity
Electron–Dot Structures
Electron–Dot Structures of Polyatomic Molecules
Electron–Dot Structures and Resonance
Lecture 18.TEST on Chapters 4–6
Lecture 19.Continue Chapter 7Formal Charges
Molecular Shapes: The VSEPR Model
Valence Bond Theory
Lecture 20.Finish Chapter 7Hybridization and sp3 Hybrid Orbitals
Other Kinds of Hybrid Orbitals
Molecular Orbital Theory of Bonding: The Hydrogen Molecule
Molecular Orbital Theory of Other Diatomic Molecules
Combining Valence Bond Theory and Molecular Orbital Theory
Interlude: Molecular Shape, Handedness, and Drugs
Lecture 21.Begin Chapter 8.Thermochemistry: Chemical Energy
Energy
Energy Changes and Energy Conservation
Internal Energy and State Functions
Expansion Work
Lecture 22.Continue Chapter 8.Energy and Enthalpy
The Thermodynamic Standard State
Enthalpies of Chemical and Physical Change
Calorimetry and Heat Capacity
Hess’s Law
Standard Heats of Formation
Lecture 23.Finish Chapter 8.Bond Dissociation Energies
Fossil Fuels, Fuel Efficiency and Heats of Combustion
An Introduction to Entropy
An Introduction to Free Energy
Interlude: The Evolution of Enthalpy
Lecture 24.Begin Chapter 9.Gases: Their Properties and Behavior
Gases and Gas Pressure
The Gas Laws
The Ideal Gas Law
Lecture 25.Continue Chapter 9.Stoichiometric Relationships with Gases
Partial Pressure and Dalton’s Law
The Kinetic–Molecular Theory of Gases
Lecture 26.Finish Chapter 9.Graham’s Law: Diffusion and Effusion of Gases
The Behavior of Real Gases
The Earth’s Atmosphere
Interlude: Inhaled Anaesthetics
Lecture 27.TEST on Chapters 7–9
Lecture 28.Review for the Final Examination.
The Final Examination is scheduled for Monday, May 22, 2006, from
1:00 – 3:00 p.m. The Final Examination will cover Chapters 1-9.
The Final Average for the course will be determined as follows:
3 Tests35 %
Best 3 of 5 Quizzes15 %
Laboratory25 %
Homework, Classroom and
Workshop Attendance
and Participation 5 %
Final Examination20 %
Some quizzes and tests may be given during the laboratory period. There will be no make-up quizzes or make-up tests given.
The Laboratory is a very important part of this course. You may have only two absences (excused or unexcused) in the laboratory without penalty.
Students enrolled in CHM 201 must be enrolled in CHML 201 A student must receive a passing grade in CHM 201 in order to receive a passing grade in CHML 201.
PRACTICE SAFE LAB
EYE PROTECTION MUST BE WORN AT ALL TIMES IN THE CHEMISTRY LABORATORY
You must wear safety glasses or other approved eye protection at any time during the laboratory period that anyone in the laboratory is working with chemicals. Therefore, it is the student’s responsibility to bring approved eye protection to the laboratory each week. This eye protection is not supplied by the department. It is available in the bookstore. Students who do not have approved eye protection or who do not wear approved eye protection will be dismissed from the laboratory for the day and will receive a 0 for that day’s work.