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Organic chem 1 Week 2 Notes

by: Jasmine Nord

Organic chem 1 Week 2 Notes CHEM 3010

Marketplace > University of Tennessee - Chattanooga > CHEM > CHEM 3010 > Organic chem 1 Week 2 Notes
Jasmine Nord

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These are all the notes from this past week. It's a continuation of chapter 1 notes. There are tons of pictures and examples. Play close attention to the practice problems, there are some that Meba...
Organic Chemistry I
Class Notes
Organic Chemistry, Chemistry, Mebane, week2
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This 4 page Class Notes was uploaded by Jasmine Nord on Sunday September 4, 2016. The Class Notes belongs to CHEM 3010 at University of Tennessee - Chattanooga taught by Dr.Mebane in Summer 2016. Since its upload, it has received 11 views. For similar materials see Organic Chemistry I in CHEM at University of Tennessee - Chattanooga.


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Date Created: 09/04/16
Organic Chem Chap 1 Notes (continued…) Week 8/29­9/2 1. How to draw Lewis Structures a. Determine the total number of valence electrons supplied by all atoms in the structure. i. for a negative ion, increase the total # by the charge ii. for a positive ion, decrease the total # by the charge b. Write a skeleton of the compound and give all atoms an octet of electrons (an exception is H which gets two). c. Double bonds decrease the total # of electrons in the structure by 2.  Triple bonds decrease the total # of electrons in the structure by 4. d. Calculate the formal charge of your dot structure. e. In a neutral molecule, the sum of the formal charges is zero.  In an ion, the formal charges must add up to the charge of the ion. 2. Examples of what was done in class   3. Other forms of structures a. Dash formula  (Kekule structures) Google “Kekule structures” for more examples i. b. Condensed structure Example; CH Br or CH OCH i. 3 3 3 ii. Google “condensed structural formula” 4. Molecular Orbital theory a. The tendency of atoms to fill their octet by sharing & assigning electrons to certain orbital b. molecular orbital (which overlap of atomic orbital) i. where the electrons are in the molecule the electrons that surround the molecule ii. 5. atomic orbital (1s, 2s, 2p , 2p ,x2p )y z a. the volume of space around an atom’s nucleus where atoms are likely to be found 6. bonding molecular orbital (σ) a. The constructive combination of 2 atomic orbital. A bond is formed b. Google “Sigma bonds” for more example 7. anti­bonding molecular orbital (σ*) a. The deconstructive combination of 2 orbital. b. The 2 orbital essentially cancel each other out. So two sounds waves colliding. No bond is formed 8. There are two ways to form molecular orbital a. Sigma Bonds (σ) i. Symmetrically distributed ii. 2 orbital sharing “S” orbital electrons b. Pi Bonds (π) i. Side by side overlap of two in­phase “P” orbital electrons ii. Side by side of two out­phase orbital are anti­pi orbital c. Google “Sigma and Pi bonds” for examples  9. VSEPR (Valance Shell Electron Pair Repulsion) a. Putting electron pairs as far apart as possible b. Sort of have to think back to gen chem. 1 c. You can Google each geometry name for examples # of electron pairs Geometry 2 Linear (180º apart) 3 Trigonal planer (120º apart) 4 Teterhedral (109.5º apart)  10. Hybridization a. He talked a lot about hybridization. I don’t really understand it enough so  you may need to do your own research but he talked about it in length.  Pages 40­ 45 in the textbook are all about it.   11. Practice problems ( LOOK PROBLEMS 43 & 44. He WILL put similar  problems like them ON THE TEST) a. Pg 15  i. #16  b. Pg 16 i. #17 c. Pg 17 i. #18 d. Pg 18 i. #19 e. Pg 19 #22 i. f. Pg 43 i. #43 g. Pg 44 i. #44 12. Important Pages in the book a. Pg 17  i. For Kekule structure examples ii.For condensed structures examples b. Pg 22 i. Fig. 1.1 c. Pg 23 i. Fig. 1.3 d. Pg 25  i. Fig. 1.4 e. Pg 32 i. Fig 1.13 ii. Fig 1.14 f. Pg 40­45 (This is just review of hybridization)  i. 1.15 g. Pages 46­49 i. All concepts and more practice problems


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