1 / 52

Organic Chemistry

Chapter 22-23. Organic Chemistry. Organic Chemistry. Study of carbon-based compounds Carbon has 4 valence electrons Carbon always forms 4 covalent bonds N (3), O (2), H (1) Carbon compounds form chains and/or rings. Hydrocarbons. Molecule or compound composed of carbon and hydrogen only

Download Presentation

Organic Chemistry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Chapter 22-23 Organic Chemistry

  2. Organic Chemistry • Study of carbon-based compounds • Carbon has 4 valence electrons • Carbon always forms 4 covalent bonds • N (3), O (2), H (1) • Carbon compounds form chains and/or rings

  3. Hydrocarbons • Molecule or compound composed of carbon and hydrogen only • Three Main Types • Alkanes, Alkenes, Alkynes

  4. Alkanes • All single C─C bonds H H H │ │ │ H─ C─ C─ C─ H │ │ │ H H H H H H H │ │ │ │ H─ C─ C─ C─ C─ H │ │ │ │ H H H H H H H H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H C3H8 C4H10 C5H12 General Formula CnH2n+2

  5. Alkenes • At least one double C=C bond H H H │ │ │ H─ C─ C= C─ H │ H H H H H │ │ │ │ H─ C─ C─ C= C─ H │ │ H H H H H H H │ │ │ │ │ H ─ C─ C─ C─ C= C─ H │ │ │ H H H C3H6 C4H8 C5H10 General Formula CnH2n

  6. Alkynes • At least one triple C≡C bonds H │ H─ C─ C≡ C─ H │ H H H │ │ H─ C─ C─ C≡ C─ H │ │ H H H H H │ │ │ H ─ C─ C─ C─ C≡ C─ H │ │ │ H H H C3H4 C4H6 C5H8 General Formula CnH2n-2

  7. Homologous Series • Group of compounds with similar structure and function • Table Q • Members increase by one carbon and two hydrogens

  8. H │ H─ C─ H │ H H H │ │ H─ C─ C─ H │ │ H H H H H │ │ │ H─ C─ C─ C─ H │ │ │ H H H H H H H │ │ │ │ H─ C─ C─ C─ C─ H │ │ │ │ H H H H CH4 C2H6 C3H8 C4H10 H H H H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H H H H H H H │ │ │ │ │ │ H ─ C─ C─ C─ C─ C─ C─ H │ │ │ │ │ │ H H H H H H C5H12 C6H14 Alkane Homologous Series

  9. H H │ │ H─ C= C─ H H H H │ │ │ H─ C─ C= C─ H │ H H H H H │ │ │ │ H─ C─ C─ C= C─ H │ │ H H C2H4 C3H6 C4H8 H H H H H │ │ │ │ │ H ─ C─ C─ C─ C= C─ H │ │ │ H H H H H H H H H │ │ │ │ │ │ H ─ C─ C─ C─ C─ C= C─ H │ │ │ │ H H H H C5H10 C6H12 Alkene Homologous Series

  10. H─ C≡ C─ H H │ H─ C─ C≡ C─ H │ H H H │ │ H─ C─ C─ C≡ C─ H │ │ H H C2H2 C3H4 C4H6 H H H │ │ │ H ─ C─ C─ C─ C≡ C─ H │ │ │ H H H H H H H │ │ │ │ H ─ C─ C─ C─ C─ C≡ C─ H │ │ │ │ H H H H C5H8 C6H10 Alkyne Homologous Series

  11. Saturated vs. Unsaturated • Saturated Hydrocarbons • Contain only single Carbon to Carbon bonds (Alkanes) • Unsaturated Hydrocarbons • Contains at least one multiple (double, triple) Carbon to Carbon bond • Alkenes and Alkynes

  12. Naming Simple Hydrocarbons • Name is based on two parts • Number of carbons in longest continuous chain (Table P) • Type of bonds between carbons • Single –ane • Double –ene • Triple –yne

  13. Examples H H H H │ │ │ │ H─ C─ C─ C─ C─ H │ │ │ │ H H H H • Butane • Pentane H H H H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H

  14. Alkenes and Alkynes • Name includes location of multiple bond • Carbons numbered to give multiple bond the lowest possible number • 1-butyne 2-butyne H H │ │ H─ C─ C─ C≡ C─ H │ │ H H H H │ │ H─ C─ C≡ C ─ C─ H │ │ H H

  15. Chemical Formula • Shows only number of each type of element • C2H6 • C6H12O6

  16. Structural Formula • Shows how each atom is bonded to each other H H H H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H H H │ │ H─ C─ C─ C≡ C─ H │ │ H H

  17. Condensed Structural Formula • Shows who is bonded to who, without the actual bonds H H H │ │ │ H─ C─ C─ C─ H │ │ │ H H H H H H │ │ │ H─ C─ C= C─ H │ H

  18. Branched Hydrocarbons • Alkyl Group • Hydrocarbon branch • Branch name ends with -yl • Location of branch is indicated by number • Number carbons to give lowest possible number • Multiple bond still takes priority in numbering

  19. Examples H H CH3 H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H • 3-Methyl Pentane • 2-Methyl 1-Butene H │ H─ C─ H │ H CH2 H │ │ │ H─ C─ C= C─ H │ H

  20. Isomers • Two or more compounds with the same chemical formulas, but different structural formulas and properties • Different Names

  21. Isomer Example C5H12 H H H H H │ │ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ │ H H H H H H H CH3 H │ │ │ │ H─ C─ C─ C─ C─ H │ │ │ │ H H H H Pentane Methyl Butane H CH3 H │ │ │ H─ C─ C─ C─ H │ │ │ H CH3 H Dimethyl Propane

  22. Functional Groups • Specific arrangement of atoms that give compounds a unique property • Table R • Examples • Hydroxyl Group, -OH O • Carbonyl Group, ─ C ─ ǁ

  23. Halogen attached to a carbon Prefix indicates which halogen Table R # for which carbon halogen is attached Multiple bonds still take priority in numbering Halides

  24. Halides H H Cl H │ │ │ │ H─ C─ C─ C─ C─ H │ │ │ │ H H H H Br H H │ │ │ H─ C─ C= C─ H │ H 2-Chlorobutane 3-Bromopropene CH3CH2CHClCH3 CH2BrCHCH2

  25. Hydroxyl group (-OH) attached to a carbon # for which alcohol group is attached Name ends in –ol Multiple bonds still take priority in numbering Alcohol

  26. Alcohol H H H H │ │ │ │ HO─ C─ C─ C─ C─ H │ │ │ │ H H H H H H H H H H │ │ │ │ │ │ H ─ C─ C─ C─ C─ C─ C─ H │ │ │ │ │ │ H H H OH H H 3-Hexanol 1-Butanol CH3CH2CH2CH2OH CH3CH2CH2CHOHCH2CH3

  27. Carbonyl group at end of chain Name ends with –al Condensed structural formula ends with -CHO Aldehyde O ǁ ─ C ─ H

  28. Aldehyde H H H H O │ │ │ │ ǁ H ─ C─ C─ C─ C─ C─ H │ │ │ │ H H H H H H O │ │ ǁ H─ C─ C─ C─ H │ │ H H Propanal Pentanal CH3CH2CHO CH3CH2CH2CH2CHO

  29. Ketones • Carbonyl group not on end of chain • Number indicates which carbon the oxygen is attached to • Name ends with –one • Condensed structural formula has -CO- in it O ǁ ─ C ─

  30. Ketones H O H H H │ ǁ │ │ │ H ─ C─ C─ C─ C─ C─ H │ │ │ │ H H H H H O H │ ǁ │ H─ C─ C─ C─ H │ │ H H Propanone 2-Pentanone CH3COCH3 CH3COCH2CH2CH3

  31. Amine • Nitrogen attached to a carbon • Number indicates which carbon the nitrogen is attached to • Name ends in –amine • Multiple bonds still take priority in numbering

  32. Amine H H H H │ │ │ │ H2N─ C─ C─ C─ C─ H │ │ │ │ H H H H H H H H H H │ │ │ │ │ │ H ─ C─ C─ C─ C─ C─ C─ H │ │ │ │ │ │ H H H NH2 H H 3-Hexanamine 1-Butanamine CH3CH2CH2CH2NH2 CH3CH2CH2CHNH2CH2CH3

  33. Amide • Carbonyl group with an amine group attached to it • Must be on an end • Name ends in -amide O H ǁ ǀ ─ C ─ N ─ H

  34. Amide H H H H O │ │ │ │ ǁ H ─ C─ C─ C─ C─ C─ NH2 │ │ │ │ H H H H H H O │ │ ǁ H─ C─ C─ C─ NH2 │ │ H H Propanamide Pentanamide CH3CH2CONH2 CH3CH2CH2CH2CONH2

  35. Organic Acid O ǁ ─ C ─ O ─ H • Carbonyl group with a hydroxyl group attached to it • Must be on an end • Name ends in –oic acid • Condensed structural formula ends with -COOH • Hydroxyl H is the acidic H

  36. Organic Acid H H H O │ │ │ ǁ H ─ C─ C─ C─ C─ OH │ │ │ H H H H O │ ǁ H ─ C─ C─ OH │ H Ethanoic Acid Butanoic Acid CH3COOH CH3CH2CH2COOH

  37. Ether • Single oxygen between 2 carbon chains • Name each carbon chain H H H H │ │ │ │ H─ C─ C─O ─ C─ C─ H │ │ │ │ H H H H H H H H H H │ │ │ │ │ │ H ─ C─ C─ C─ C─ O─ C─ C─ H │ │ │ │ │ │ H H H H H H Diethyl Ether Butyl Ethyl Ether CH3CH2OCH2CH3 CH3CH2CH2CH2OCH2CH3

  38. O ǁ ─ C ─ O ─ Ester • Carbonyl group with single oxygen between carbon chains • Name in two parts • 1st – Branch off oxygen as alkyl group • 2nd – Chain containing Carbonyl group • Ending in –oate

  39. Ester H O H │ ǁ │ H ─ C─ O ─ C─ C─ H │ │ H H H H H O H H │ │ │ ǁ │ │ H ─ C─ C─ C─ C─ O─ C─ C─ H │ │ │ │ │ H H H H H Methyl Ethanoate Ethyl Butanoate CH3COOCH3 CH3CH2CH2COOCH2CH3

  40. Organic Reactions • Saponification • Fermentation • Combustion • Addition • Substitution • Polymerization (2 types) • Esterification

  41. Organic Reactions • Saponification • Production of Soap • Fermentation • Production of ethanol and CO2 from sugar • C6H12O6 2C2H5OH + 2CO2

  42. Combustion • Complete Combustion of a Hydrocarbon • CxHy + O2 CO2 + H2O • Example: • C3H8 + 5O2 3CO2 + 4H2O

  43. Addition • Addition of a halogen onto an alkene or alkyne Br Br │ │ H─ C≡ C─ H + Br─Br  H─ C= C─ H Br Br Br Br │ │ │ │ H─ C= C─ H + Cl─Cl  H─ C─ C─ H │ │ Cl Cl

  44. Substitution • Substitution of one halogen in place of a hydrogen on an alkane H H H H │ │ │ │ H─ C─ C─ H + Cl─Cl  H─ C─ C─ H + H ─ Cl │ ││ │ H H H Cl H H Br H │ │ │ │ H─ C─ C─ H + Br─Br  H─ C─ C─ H + H ─ Br │ ││ │ H Cl H Cl

  45. Polymerization • Connecting of smaller pieces into a long repeating chain • Plastics, starches, nylon • Two types: • Addition • Condensation -(C2H4)n-

  46. Addition Polymerization • Double or triple bonds break to connect pieces together H H H H H H H H │ │ │ │ │ │ │ │ C═C + C═C  ─ C─C─C─ C ─ │ │ │ │ │ │ │ │ H H H H H H H H n

More Related