Chemical Principles: The Quest for Insight. 4th ed PDF

Chemical Principles: The Quest for Insight. 4th ed. New York

Course Description

This course provides an introduction to the chemistry of biological, inorganic, and organic molecules. The emphasis is on basic principles of atomic and molecular electronic structure, thermodynamics, acid-base and redox equilibria, chemical kinetics, and catalysis.

In an effort to illuminate connections between chemistry and biology, a list of the biology-, medicine-, and MIT research-related examples used in 5.111 is provided in Biology-Related Examples

Lecture Notes

Lecture notes (with blanks) are provided for each lecture. Students are expected to follow along during the lecture in order to fill in the blanks in the notes.

Required Textbook:

Atkins, Peter, and Loretta Jones. Chemical Principles: The Quest for Insight. 4th ed. New York, NY: W.H. Freeman and Company, 2007. ISBN: 9781429209656.

The reading assignment listed for the first session is a review of information you are expected to know before you begin the class. This information is not discussed during lecture.

In addition, no lecture notes were provided for the first session. The handout associated with that lecture is an overview of the class format and expectations.

SES #	TOPICS	READINGS	LECTURE NOTES
L1	The importance of chemical principles	Section A.1 Sections B.3-B.4 Sections C-H Sections L-M	(PDF)
L2	Discovery of electron and nucleus, need for quantum mechanics	Sections A.2-A.3 Sections B.1-B.2 Section 1.1	(PDF)
L3	Wave-particle duality of light	Sections 1.2 and 1.4	(PDF)
L4	Wave-particle duality of matter, Schrödinger equation	Sections 1.5-1.6	(PDF)
L5	Hydrogen atom energy levels	Sections 1.3, 1.7 up to equation 9b, and 1.8	(PDF)
L6	Hydrogen atom wavefunctions (orbitals)	Section 1.9	(PDF - 1.2 MB)
L7	p-orbitals	Sections 1.10-1.11	(PDF)
L8	Multelectron atoms and electron configurations	Sections 1.12-1.13	(PDF)
L9	Periodic trends	Sections 1.14-1.18, and 1.20	(PDF - 1.6 MB)
L10	Periodic trends continued; Covalent bonds	Sections 2.5-2.6, and 2.14-2.16	(PDF - 1.6 MB)
L11	Lewis structures	Sections 2.7-2.8	(PDF)
L12	Exceptions to Lewis structure rules; Ionic bonds	Sections 2.3 and 2.9-2.12	(PDF - 1.1 MB)
L13	Polar covalent bonds; VSEPR theory	Sections 3.1-3.2	(PDF - 5.1 MB)
L14	Molecular orbital theory	Sections 3.8-3.11	(PDF)
L15	Valence bond theory and hybridization	Sections 3.4-3.7	(PDF - 1.0 MB)
L16	Determining hybridization in complex molecules; Termochemistry and bond energies/bond enthalpies	Sections 6.13, 6.15-6.18, and 6.20	(PDF)
L17	Entropy and disorder	Sections 7.1-7.2, 7.8, 7.12-7.13, and 7.15	(PDF)
L18	Free energy and control of spontaneity	Section 7.16	(PDF)
L19	Chemical equilibrium	Sections 9.0-9.9	(PDF)
L20	Le Chatelier's principle and applications to blood-oxygen levels	Sections 9.10-9.13	(PDF)
L21	Acid-base equilibrium: Is MIT water safe to drink?	Chapter 10	(PDF)
L22	Chemical and biological buffers	Chapters 10 and 11	(PDF)
L23	Acid-base titrations	Chapter 11	(PDF)
L24	Balancing oxidation/reduction equations	Section K Chapter 12	(PDF)
L25	Electrochemical cells	Chapter 12	(PDF)
L26	Chemical and biological oxidation/reduction reactions	Chapter 12	(PDF)
L27	Transition metals and the treatment of lead poisoning	pp. 669-681	(PDF)
L28	Crystal field theory	pp. 681-683	(PDF - 1.4 MB)
L29	Metals in biology	pp. 631-637	(PDF - 1.2 MB)
L30	Magnetism and spectrochemical theory	Chapter 16	(PDF)
L31	Rate laws	Sections 13.1-13.5	(PDF)
L32	Nuclear chemistry and elementary reactions	pp. 498-501 and 660-664	(PDF)
L33	Reaction mechanism	pp. 549-552	(PDF)
L34	Temperature and kinetics	Sections 13.11-13.13	(PDF)
L35	Enzyme catalysis	Sections 13.14-13.15	(PDF)
L36	Biochemistry		(PDF)