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Organic Chemistry for Hydrocarbon

Organic Chemistry for Hydrocarbon . Alkanes. Hydrocarbon chains where all the bonds between carbons are single bonds Name uses the ending – ane Examples: Meth ane , Prop ane , But ane , Oct ane , 2-methylpent ane. Prefixes for Carbons. Physical & Chemical Properties Alkanes Alkenes

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Organic Chemistry for Hydrocarbon

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  1. Organic Chemistry for Hydrocarbon

  2. Alkanes • Hydrocarbon chains where all the bonds between carbons are single bonds • Name uses the ending –ane • Examples: Methane, Propane, Butane, Octane, 2-methylpentane

  3. Prefixes for Carbons

  4. Physical & Chemical Properties • Alkanes • Alkenes • Alkynes • Aromatics

  5. Physical & Chemical Properties • Alkanes & Cycloalkanes

  6. Physical Properties of Alkanes and Cycloalkanes • Boiling points of unbranched alkanes increase smoothly with number of carbons • Melting points increase in an alternating pattern according to whether the number of carbon atoms in the chain is even or odd

  7. Physical Properties of Alkanes and Cycloalkanes • Branched chain has higher boiling point than strength chain (in case of number of carbon is equal) • Alkanes are non-polar molecules, this indicates that alkanes are water-insoluble compounds. • Alkanes are non-conductive compounds.

  8. 1. Chemical Properties of Alkanes and Cycloalkanes • Alkanes & cycloalkanes • are well flammable. • no soot from combustion.

  9. Chemical Properties of Alkanes and Cycloalkanes Alkanes & cycloalkanes are saturated compounds. (having only single bonds) Chemical reactions: Substitution reactions

  10. Chemical Properties of Alkanes and Cycloalkanes 2. Halogenation is a chemical reaction that incorporates a halogen atom into a molecule. More specific descriptions exist that specify the type of halogen:fluorination, chlorination, bromination, and iodination light CH4 + Cl2 CH3Cl + HCl chlorination light C7H10 + Br2 C7H9Br + HBr bromination *light is a necessary factor to make a reaction*

  11. Chemical Properties of Alkanes and Cycloalkanes • Alkanes & Cycloalkanes cannot be reacted and reduced color of KMnO4. Note! light + Br2 Br-CH2-CH2-CH2-Br Addition reaction light + Cl2 Cl-CH2-CH2-CH2-CH2-Cl Unstables alicyclic alkanes: more reacitivity

  12. Physical & Chemical Properties • Alkenes & Cycloalkenes

  13. Physical Properties of Alkenes and Cycloalkenes • Boiling points and melting point of alkenes increase with number of carbons. If no. of carbon is same, alkenes have less boiling point and melting point than alkanes, i.e., b.p. of C4H10 >C4H8 • Alkenes are non-water soluble compounds, but can soluble in non-polar solvent i.e. ether, hexane • Alkenes are non-conductive compounds.

  14. Chemical Properties of Alkenes and Cycloalkenes 1. Combustion reaction 2C5H10 +15O2 10CO2 + 10H2O +heat 2. Addition reaction addition at double bond of carbon atom 2.1 Halogenation – halide addition, not required light CH2=CH2 + Cl2  Cl-CH2-CH2-Cl

  15. Chemical Properties of Alkenes and Cycloalkenes 2.2 Hydrogenation – hydrogen addition with Ni or Pt acted as catalyst, alkanes will be obtained. Ni CH3-CH=CH2 + H2 CH3-CH-CH2 H H 2.3 Hydrohalogenation – acid halide addition and alkyl halide will be obtained CH2=CH2 + HCl  H-CH2-CH2-Cl

  16. Chemical Properties of Alkenes and Cycloalkenes 2.4 Hydration – water addition with H2SO4 acted as catalyst, alcohols will be obtained. H2SO4 CH2=CH2 +H2O  HO-CH2-CH2-OH 3. Oxidation reaction react with KMnO4 (Oxidizing agent) in water, glycol will be obtained. 2KMnO4 + 4H2O + CH3-CH=CH-CH3  3CH3-CH-CH-CH3 + 2MnO2 + 2KOH OH OH

  17. Physical & Chemical Properties • Alkynes

  18. Physical Properties of Alkynes • Boiling points and melting point of alkenes increase with number of carbons. If no. of carbon is same: boiling point of alkynes > alkanes > alkenes • Alkynes are non-water soluble compounds, but can soluble in non-polar solvent i.e. ether, hexane

  19. Chemical Properties of Alkynes 1. Combustion reaction 2C2H2 +5O2 4CO2 + 2H2O +heat 2. Addition reaction addition at triple bond of carbon atom 2.1 Halogenation – halide addition, not required light CHCH + Cl2  Cl-CH=CH-Cl Cl-CH=CH-Cl + Cl2 Cl-CH-CH-Cl Cl Cl

  20. Chemical Properties of Alkynes 2.2 Hydrogenation – hydrogen addition with Ni or Pt acted as catalyst. Ni HCCH + 2H2 CH3-CH3 2.3 Hydrohalogenation – acid halide addition and alkyl halide will be obtained CHCH + HCl  H-CH=CH-Cl H-CH=CH-Cl + HClH-CH-CH-Cl H Cl

  21. Chemical Properties of Alkynes • 2.4 Hydration – water addition with H2SO4 acted as catalyst, • alcohols will be obtained if reactant is ethyne. • H2SO4O • CHCH +H2O  H-CH2-C-H • Normally, ketones will be obtained. • H2SO4O • CH3-CCH +H2O  CH3-C-CH3

  22. Chemical Properties of Alkynes • 3. Oxidation reaction • react with KMnO4 (Oxidizing agent) in water • Carboxylic acid and CO2 will be obtained for alkyne with primary carbon • 3CHCH + 8KMnO4 + 4H2O  3HCOOH + 3CO2 + 8MnO2 + 8KOH • Ketone will be obtained for alkyne with secondary carbon • O O • 3RCCR + 4KMnO4 +2H2O  3R-C-C-R + 4MnO2 + 4KOH

  23. Physical & Chemical Properties • Aromatic compounds

  24. Physical Properties of Aromatics • Non-water soluble compounds • Soluble in non-polar organic solvent i.e. ether • Low boiling point and melting point • Individual odor compounds

  25. 15 2 Chemical Properties of Aromatics 1. Combustion reaction + O2 6CO2 + 3H2O 2. Substitution reaction 2.1 Halogenation – halide substitute with FeCl3 as catalyst FeCl3 Cl + Cl2  + HCl

  26. Chemical Properties of Aromatics 2.2 Hydrogenation Under high pressure and temperature with Ni as catalyst + 3H2 2.3 Alkylation Alkyl group substitute by alkyl halide to hydrogen with AlCl3 as catalyst CH3 AlCl3 + CH3Br + HBr

  27. Naming of Aromatic compounds CH3 H3C CH3 CH3 C2H5 CH3

  28. Naming of Aromatic compounds

  29. Hexane CH3 CH2 CH2 CH CH3 CH3 Isohexane CH3 CH2 CH2 CH2 CH2CH3 Isomers Compounds that have the same molecularformula, but different molecular structures, are called structural isomers C6H14 straight chain C6H14 Branched chain alkanes

  30. Structural Isomers of Butane, C4H10

  31. CH3 Isomers Differences compounds Same compounds

  32. Isomers C5H12 C4H8 C3H8O Dichlorocyclomethane Trichlorocyclomethane

  33. Functional compounds

  34. Functional compounds Identify the functional group of following compounds CH3CH2CH2COOH C3H7OH HCOH CH3COOCH2CH3

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