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U of M CHEM 2301 - Course Introduction and Lewis Structures

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CHEM 2301 1st Edition Lecture 1Outline of Current Lecture I. Course introductionII. Drawing Lewis structuresIII. Lewis structures of common moleculesCurrent Lecture- Course introductiono Instructors: Professor Tolman and co-instructor Dr. Alex Johno Lecture behavior Be on time and fill seats in the middle of the rows first No sitting in the aisles  No cell phones or texting during class No laptops No sleeping Take notes and practice drawing molecules Ask questions and participateo How to do well in organic chemistry Keep up and learn the material like learning a new language Come to class and participate Keep up and do a little every day Do lots of problems effectively  Read the material in the book that will be covered in class before the lecture After class, download lecture slides and work on the in-chapter problems in the booko Getting help Bring questions to office hours TA tutor room  Study advice on the Moodle site ChemFoundations sessionso Setting up your clicker Turn on the clicker Hold down the power button until the frequency begins to flash, then press ACo Goals of the course By the end of the course, you should have a basic understanding of: - Geometric and electronic structure of basic organic molecules- How structure relates to reactivity for certain types of systemsThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.- How to solve organic chemistry problems- Know how organic molecules react and how to make them- The bottom line: Almost all reactions involve a molecule willing to give up electrons interacting with a molecule that wants them.- Drawing Lewis Structureso Draw a molecular skeletono Count valence electronso Adjust for chargeo Arrange electrons to fill most shellso Assign formal charges- Counting electronso For octet: court all the electrons around the atomo For formal charge: count all electrons in lone pairs and count one electron for each bond- Possible carbon bonding patterns- Lewis structures of common molecules- CH3 group = methyl group- Names ending in “ene” mean there is a double bond- Names ending in “onium” mean there is a positive charge - Isoelectronic: Two molecules with the same number of electrons but different atoms o CH4 and NH4+Carbonium ionCarbide ionCH4 (Methane)NH4+ (Ammonium ion)CH3OH (Methanol)C2H4


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