2. Organic Chemistry Is the study of the chemistry of carbon compounds containing hydrogen:hydrocarbons

3. Origin Originally defined as the chemistry of living materials or originating from living sources. Wohler synthesized urea from non organic sources (1800 – 1882) Now generally defined as the chemistry of carbon and its compounds.

4. Organic foods are foods that are produced using methods that do not involve modern synthetic inputs such as synthetic pesticides and chemical fertilizers.pesticides chemical fertilizers This is different from the scientific use of the term "organic," to refer to a class of molecules that contain carbon, especially those involved in the chemistry of life.a class of molecules that contain carbon

5. HOW DO ORGANIC COMPOUNDS LOOK LIKE? Ethanol Caffeine Aspirin

6. CHOCOLATE Theobromine is the primary alkaloid found in cocoa and chocolatecocoa chocolate Its presence is one of the causes for chocolate's mood- elevating effects.

7. Vitamin C Natural Ascorbic Acid Unlike most mammals and other animals, humans do not have the ability to make their own vitamin C. Therefore, we must obtain vitamin C through our diet Synthetic Synthetic vitamins are made in a laboratory setting from coal tar derivatives.

8. Uses of hydrocarbons

9. Gasoline is a mixture of hydrocarbons (C 8 H 18 for example) that contain no atoms of oxygen. Gasohol contains ethyl alcohol, C 2 H 5 OH, which does contain oxygen. The addition of alcohol to gasoline, therefore, adds oxygen to the fuel.

10. Petroleum: http://science.howstuffworks.com/environmental/energy/oil- refining2.htmhttp://science.howstuffworks.com/environmental/energy/oil- refining2.htm

11. Libra Oil Field Xvsdzc

12. Why is carbon so special?

13. Carbon can form single, double and triple bonds with itself The bond length is defined as the distance between the nuclei of the atoms involved in the bond. The strength of the C-C bond indicates it is quite thermally stable in comparison to other elements in the same group. Si-Si 226 Ge-Ge 188

14. Carbon can catenate One of the remarkable property of carbon atom is its unique capacity to link with other carbon atoms. It can form chains and rings.

15. Carbon cannot expand its octet of valence electrons CCl 4 is immiscible in water and does not react. SiCl 4 reacts vigorously in water to produce HCl because a njon bonding pair of electrons in water is able to expand the octet of silicon.

17. The silicon atom is bigger, and so there is more room around it for the water molecule to attack. But silicon has the additional advantage that there are empty 3d orbitals available to accept a lone pair from the water molecule. Carbon doesn't have 2d orbitals.

18. Hydrocarbons Saturated : CONTAIN ONLY SINGLE BONDS Alkanes Unsaturated : CAN CONTAIN A DOUBLE OR A TRIPLE BOND Alkenes, Alkynes & Aromatics C - C C = CC

19. Homologous Series One in which all the members have the same general formula. The neighbouring members differ by CH 2, show similar chemical properties and a gradation in their physical properties.

20. Alkanes a homologous series Alkanes are saturated hydrocarbons that contain only single carbon-carbon bonds.

22. The simplest alkane is CH 4 The general formula of an alkane is C n H 2n+2 The first 4 members are gases at standard conditions, and are good fuels

23. Prefixes for # of Carbons 1Meth6Hex 2Eth7Hept 3Prop8Oct 4But9Non 5Pent10Dec

24. Homologous Series: A homologous series of alkanes CH 4 Methane C2H6C2H6 Ethane C3H8C3H8 Propane C 4 H 10 Butane C 5 H 12 Pentane Each compound in this series differs from the previous compound by a –CH 2 –

25. Propane Butane

26. Structural Isomers Structural isomers are compounds with the same molecular formula but different structural formula. As the number of carbon atoms in an alkane molecule increases, so do the possibilities for isomerism of this kind.

28. General Properties of Alkanes The boiling points of alkanes are very low for their molecular mass. This is because the molecule is completely nonpolar( inertness) It increases with an increase in mass.

29. Boiling Points of Alkanes http://wiki.chemeddl.org/index.php/8.2_Organic_Compounds:_Hydrocarbons The more spherical the isomer, the lower boiling point( less dispersion forces) due to less surface area to form intermolecular bonds.

34. Naming Alkanes a)Attached carbon groups (substituents) end in –yl –Methyl CH 3 - –Ethyl CH 3 CH 2 - –Propyl CH 3 CH 2 CH 2 – 3-ethylpentane

35. Types of Formulas 1. Chemical Formula (Sum) C 3 H 8 2. Structural Formula 3. Condensed Formula CH 3 CH 2 CH 3 4. Line Formula

36. Naming Alkanes

37. b) Other substituents -chloro Cl -bromo Br -iodo I -ol -ol OH

38. STEP 1 Longest chain is ______________. STEP 2 Number chain from end nearest substituent. Cl CH 3  CH 3 ─CH 2 ─CH─CH─CH 3 STEP 3 Locate substituents and name alphabetically. Cl CH 3  CH 3 ─CH 2 ─CH─CH─CH 3

39. Line Formula : http://elchem.kaist.ac.kr/jhkwak/OkanaganPdb97/nomenclature/ane-100.htm http://elchem.kaist.ac.kr/jhkwak/OkanaganPdb97/nomenclature/ane-100.htm

40. Types of Formulas STRUCTURALCHEMICALCONDENSEDLINENAMING

41. Aspirin: ASA

42. Alkenes “Unsaturated” hydrocarbons, contain one double bond between carbon atoms. General Formula: C n H 2n

43. Alkynes “Unsaturated” hydrocarbons, contain one triple bond between carbon atoms. General Formula: C n H 2n-2

44. Alkene names change the end to –ene

46. CH 2 = CH ─ CH 2 ─ CH 3 1-butene CH 3 ─ CH=CH─ CH 3 2-butene CH 3 | CH 3 ─ CH=C─CH 3 2-methyl-2-butene CH 3 ─ C  C ─ CH 3 2-butyne Naming Alkenes & Alkynes 1 2 3 4 1 2 3 4 4 3 21 1 2 3 4

47. Alkynes “Unsaturated” hydrocarbons, contain one triple bond between carbon atoms. General Formula: C n H 2n-2

49. Functional Groups functional groups are certain atoms or groups of atoms that give compounds characteristic properties. CH 3 CH 2 OH alcohol

50. Class of Compound Functional Group ExampleNameUses 1. Alcohol 2. Carboxylic Acid 3. Aldehyde 4. Ketone 5. Ester 6. Ether 7. Amine

52. Problems http://seacoast.sunderland.ac.uk/~hs0dad/ qm/ctinew/v2bprops.htmhttp://seacoast.sunderland.ac.uk/~hs0dad/ qm/ctinew/v2bprops.htm

53. Sites:http://www.pkwy.k12.mo.us/west/tea chers/anderson/pack10/pack10.html Assignments: http://www.pkwy.k12.mo.us/west/teachers/ anderson/pack10/pack10.htmlhttp://www.pkwy.k12.mo.us/west/teachers/ anderson/pack10/pack10.html Chemistry of petroleum: http://www.sciencenetlinks.com/Esheet.php?DocID=181 http://www.sciencenetlinks.com/Esheet.php?DocID=181

54. Aspirin The origins of the aspirin date back to about 400 BC, when Hippocrates prescribed an extract from the bark of the willow tree as a remedy for fever and pain.. Felix Hoffmann, a young chemist working for the German pharmaceutical giant Bayer AG, was looking for a new painkiller to treat his father's rheumatism. He prepared acetylsalicylic acid in 1897, and according to the literature, Henrich Dreser, head of Bayer laboratories, started its clinical use shortly thereafter. Bayer registered Aspirin trademark and began selling it in 1899. In the name of "aspirin" (as suggested by Hoffmann) "a" stand for "acetyl" and "spir" for spireic acid (a different name of salicylic acid). Some prefer to believe that the compound was named after Saint Aspirinius, patron saint of headaches.

55. Aspirin, ASA a)How much ASA will be produced when 15g of salycilic acid is being used ? b) What will be the percent yield if you were able to produce 17g of ASA?

57. Conclusion and Evaluation 1. What is the percent yield? 2. List at least thgree sources of errors 3. What realistic suggestions in terms of materials and procedure can you make in order to get better results?