S20-Lectures-Week1

S20-Lectures-Week1 - Chemistry S-20ab Chemistry E-2a:...

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Chemistry S-20 : Introduction Course Content This course introduces students to the chemistry of carbon-containing compounds. Organic chemistry is at the heart of biology and medicine: proteins, carbohydrates, fats, and DNA are all organic compounds. Plastics, detergents, cosmetics, and pharmaceuticals are also organic compounds. Course Organization Lectures give overview of each topic, conceptual background, and demonstrations Textbook provides much more detail and explains how to solve problems Laboratory gives hands-on experience and reinforces chemical concepts Discussion Sections show how to solve problems and give you practice Review Lectures ( Fri . at 3:00 pm) give extra help in problem solving P ractice problems give you practice in problem-solving Practice examinations give you more practice in solving problems Examinations evaluate your ability to solve organic chemistry problems Course Philosophy The Chemistry Team: Our Coaching Staff: Background We expect that you have taken a one-year course in General Chemistry and that you remember (or can quickly review) most of what you learned in that course. Chemistry S-20ab Week 1 1
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The Organic Chemist’s Periodic Table As of Tuesday, June 16 : chemists have identified 47,923,347 organic and inorganic substances ; 35,000,716 are available commercially! (www.cas.org/cgi-bin/cas/regreport.pl) “Learning organic chemistry is hard work. The amount of information out there is as close to infinite as makes no difference. .. The best solution is to make sure that we understand what we learn. .. develop a feel for the way molecules behave .” —A.J. Kirby, Cambridge UK Chemistry S-20ab Week 1 2
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The Hydrogen Atom The hydrogen atom is the simplest atom. What is the structure of the hydrogen atom? It turns out that, contrary to our expectations, the electron in a hydrogen atom can have only certain allowed energies, and it can make transitions between these energy levels only in discrete amounts. We say that the energy levels of an electron in a hydrogen atom are quantized . Erwin Schrödinger realized that an electron confined to an atom might behave like a wave confined to a string. He was able to derive the wavefunction that describes the behavior of an electron in an atom. Each possible solution of his famous equation corresponds to a standing wave , and is referred to as an orbital . An orbital is a three- dimensional region of space which defines where an electron can be found. The Schrödinger Equation requires three quantum numbers. What are these quantum numbers, what are the valid integer values they can take, and what do they represent? n Name: Possible Values: Represents: l Name: Possible Values: "The Chemist's Code": Represents: m l Name: Possible Values: Represents: Reading : Section 1.6 Chemistry S-20ab Week 1 3
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The s orbitals and Radial Nodes The s orbitals are spherical in shape. ( s = spherical) How can we imagine the distribution of electrons in an s orbital?
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S20-Lectures-Week1 - Chemistry S-20ab Chemistry E-2a:...

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