Organic Chemistry Week 1 Notes
Organic Chemistry Week 1 Notes CHEM 333 001
Popular in Organic Chemistry I
Popular in Chemistry
CHEM 321 001
verified elite notetaker
This 7 page Class Notes was uploaded by Hayley on Friday August 28, 2015. The Class Notes belongs to CHEM 333 001 at University of South Carolina taught by John Lavigne in Summer 2015. Since its upload, it has received 112 views. For similar materials see Organic Chemistry I in Chemistry at University of South Carolina.
Reviews for Organic Chemistry Week 1 Notes
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
Date Created: 08/28/15
Chem 333 Dr Lavigne Week 1 824828 Basic Review Monday 824 Atoms Protons P 0 Neutrons Electronse39 Electrons have di ferent Quantum levels 0 Different shells o 1234 Orbitals o s p d f When doing this remember 1 Afban fill the bottom lowest energy first 2 Hunds 1e39 in each orbital of the same energy before filling it with a second e39 3 Pauli Match spin Example Carbon Atomic Number6 so 6e T T 2p H 25 H ls For Carbon there are 4 valence e39 the 2s and 2p are the valence orbitals Use the valence orbitals to create the Lewis structure Make sure to follow the octet rule when writing out the Lewis structure Chem 333 Dr Lavigne Week 1 824 828 You can also find the of valence e39 for an element by looking at the Roman numeral above its column Example Lewis Structure for Carbon C Bonding 6 sharing Ionic Bonds gives e39 awaycation accepts e39anion39 strong bonds codependent with a high melting point 0 but can dissociate easily in a polar solvent Na Cl39 together form an ionic bond because they are oppositely charged opposites attract Covalent Bonds Share e39 0 Not all sharing may be equal because of a difference in electronegativity Electronegativity o A Eneg lt 5 9 nonpolar o A Eneg lt 19 and gt 5 9 polar covalent o A E neg gt 19 9 ionic Trends Electronegativity Increases going to the right if you are looking at it 0 Increasing going up the rows Periodic Table Chem 333 Dr LaVigne Week 1 824 828 ionic compounds are usually on opposite sides of periodic table Nonpolar Same atom CC Same Column CSi Polar Same side Same row but not same atom Organic Chemistry Tips 6070 reactions but 34 mechanisms 0 If there is an X present it stands for a halogen Heteroatoms N O F Cl Br I P S Se Wednesday 826 Trends continued The smaller the atom the more Electronegativity it has 0 CH is non polar covalent o CBr is polar covalent H How do you write HCF H H3CF because is the right way because in the Lewis structure the carbon is bonded to Flourine I I gt this arrow denotes bond dipole if bond is polar 639 and 6 denotes a partial charge Chem 333 Dr Lavigne Week 1 824 828 Naming Prefixes Number of Carbons 1meth 2 eth 3 prop 4 but 5 pent 6heX 7hept 8 oct 9dec Bond line diagrams Bends and ends are Carbons 0 must write out heteroatoms EX Br This bond line diagram has 4 carbons and 1 Br 0 If C has no full charge then add H until 4 Bonds with C 0 NaC5Sink Electrophile Lewis Acids e39 acceptor OHBr539SourceNucleophileLewis Base e39 donor Bonding Rules 1 Only Valence e39 2 Connectivity neutral species only a H X 1 Bond 3 lone pairs b C 4 Bonds no lone pairs Chem 333 Dr Lavigne Week 1 824 828 C N 3 Bonds 1 lone pair d O 2 bonds 2 lone pairs EX OH39 is neg charged so above doesn t apply C3H8 is fully saturated alkane Use eX C4H10 is fully saturated M or H branched Using we see that C3H6 is unsaturated Need to know degreed of saturation ie how many H pairs are missing from being fully saturated To do this use Index of Hydrogen Deficiency IHD I D 0 formula 2n2H in formula 2 where n of C 0 for each degree IHD there are multiple bonds or cycles eX cng IHD 25282 which 42 2 which looks lik7 This is just one way to do it There are other ways Bond line drawing isn t very good sorry For heteroatoms remember to 1 Write in H also for alkane and aldehydes 2 Remember lone pairs Formal Charge of owned valence e39 of unshared 12 shared e39 eX Carbon valence electrons Chem 333 Dr Lavigne Week 1 824 828 So 4 062 1 so the charge is 1H3C Friday 82815 Recap of Bonding 1 Only Valence Electrons Formal Charge Bond angles Bond lengths Bond strength Connectivity ofbonds oflone pairs Bond line diagrams when to write in H 0 Index of Hydrogen deficiency Resonance Isomers o Conformational o Constitutional 991999 Isomers Conformational Same molecular form but different orientation in space same connectivity but diff orientation in space ex Pentane Isomer Constitutional Isomer Same molecular form but different connectivity EX Use pentane as original from above Y Branched both pentane but different connectivity Chem 333 Dr Lavigne Week 1 824828 Remember the 3 CS of OChem 1 Common Sense 2 Count 3 Chemistry magic number4 Resonance 0 Way molecules become more stable 0 more e39 in multiple bonds 1t bonds never move a single bond Molecular Geometry Methane CH4 is a tetrahedron VESPR e39 repel Geometrye39 pairs repel get max distance from each other 0 Bond angle HCH1095 degrees 0 When drawing the 3D structure I Wedges come out I Lines go back Ex NH3 nitrogen has a lone pair and has full possession of it looks bigger Tetrahedral linear planar are common in organic chemistry 0 Electron density 0 3 areas of electron density 0 trig planar
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'