1 / 40

Hydrocarbon Derivatives:

Hydrocarbon Derivatives:. Halocarbons, Alcohols, & Ethers. Hydrocarbons. Contain only carbon & hydrogen But carbon can form strong covalent bonds to other elements, incl. O, N, F, Cl, Br, I, S, & P. Functional Group.

carney
Download Presentation

Hydrocarbon Derivatives:

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. Hydrocarbon Derivatives: Halocarbons, Alcohols, & Ethers

  2. Hydrocarbons • Contain only carbon & hydrogen • But carbon can form strong covalent bonds to other elements, incl. O, N, F, Cl, Br, I, S, & P

  3. Functional Group • One or more H’s in a hydrocarbon can be replaced by an atom or group of atoms. • An atom or group of atoms in an organic molecule that always behaves in the same way is called a functional group. • Adding a functional group changes the chemical & physical properties in specific ways, depending on the functional group.

  4. Intermolecular Forces • Determine Boiling Point & Solubility • Van der Waals or dispersion – nonpolar – weakest. • Dipole-dipole – intermediate. Molecule must have atoms with different electronegativities & not arranged symmetrically. • Hydrogen bonding – strongest. Molecules must contain H bonded to F, O, or N. Memory Jogger

  5. Halocarbons Alcohols Ethers Amines Aldehydes Ketones Carboxylic Acid Ester Amide Amino Acid Functional Groups

  6. Functional Group #1 Halocarbons

  7. Organic Halides • One or more of the hydrogen atoms in an alkane is replaced with a halogen (F, Cl, Br, or I). • Not hydrocarbons! Often called halocarbons or alkyl halides.

  8. Naming Halides • Figure out the base name. • Use prefixes to specify substituent: fluoro, chloro, bromo, iodo • If more than one, use di, tri, etc. to specify # of substituents. • If necessary, give locations of halogens by numbering C-atoms in backbone.

  9. CH3Cl CH3CHFCH3 H H H H–C–C–C–H H F H H H–C–Cl H         2-fluoropropane chloromethane C3H7F

  10. Naming Halides CH3CCl2CHClCH3 H Cl H H H – C – C – C – C– H H Cl Cl H 2,2,3-trichlorobutane C4H7Cl3

  11. Ranking Halogens • If more than 1 kind of halogen atom, list them alphabetically. • Chain is numbered to give lowest number to halogen that comes first in alphabet.

  12. Different Halogens 4 3 2 1 Chlorine is 1st alphabetically, so it determines numbering. 2-chloro-4-fluoro-3-iodobutane

  13. Name: Br CH3CH2CHCHCH3 I 3-bromo 2-iodo pentane F Cl HCCH F Cl 1,1-dichloro-2,2-difluoroethane

  14. Properties of Halocarbons • For an alkane & an alkyl halide of similar size & shape, the alkyl halide has the higher boiling point & higher density. Why? • CH4: bp = -162C & density = 0.423 g/ml • CH3Cl: bp = -24C & density = 0.911 g/ml Stronger intermolecular forces. What intermolecular forces for CCl4?

  15. Inc Inc

  16. Uses of Alkyl Halides • Cleaners & solvents • Teflon & PVC’s are alkyl halides. • Refrigerants. (used to be chlorofluorocarbons. Now hydrofluorocarbons.) • Starting materials in many reactions.

  17. Halogen Derivatives • CH3Cl = local anesthetic • CHCl3 = solvent, general anesthetic • CHI3 = antiseptic • CCl4 = dry cleaning solvent • CF2Cl2 = refrigerant • Fluorocarbons = teflon, lubricants, synthetic blood • Chlorofluorocarbons = aerosol propellants, refrigerants

  18. Table R • General Formula for halocarbons: R-X • R represents the entire hydrocarbon part of the molecule. (The alkyl part.) • X represents the halogen (F, Cl, Br, or I).

  19. Functional Group #2 Alcohols

  20. Alcohols • An –OH group replaces a H in a hydrocarbon. • The –OH group is called the hydroxyl group. -OH H HCOH H H HCH H    

  21. Alcohols are nonelectrolytes! • The hydroxyl group resembles the hydroxide ion of inorganic bases, but it does not form ions in water! • The hydroxyl group is polar. So alcohols are soluble in water.

  22. Naming AlcohOLs • Based on alkane name. • Name the parent chain. • Drop the –e and add –OL. • If the parent chain has 3 or more C atoms, number the C’s & give the location of the –OH group.

  23. Naming H H H H HCCCCH OH H H H H H H H HCCCCH H OH H H 1-Butanol bp = 100C 2-Butanol Bp = 115C Note: Never more than 1 –OH group per C

  24. More than 1 hydroxyl group • Prefixes di-, tri-, tetra- used before the –ol ending to tell the # of hydroxyl groups. • So don’t drop the -e from the alkane name. • These hydroxyls are on different C atoms!

  25. Classifying Alcohols • By # of hydroxyl groups • Monohydroxy: 1 hydroxyl group • Dihydroxy: 2 “ “ • Trihydroxy: 3 “ “ • By position of each hydroxyl group on main carbon chain.

  26. Monohydroxy Alcohols • Primary: hydroxyl group attached to end C of chain or branch. • Secondary: hydroxyl group attached to C in a chain – C is bonded to 2 other C’s. • Tertiary: hydroxyl group attached to C at a branch point – C is bonded to 3 other C’s.

  27. H H H H H-C-C-C-C-O-H H H H H 1-butanol primary H H H H H-C-C-C-C-H H H O H H 2-butanol secondary Monohydroxy

  28. H H-C-H H H H-C-C-C-H H O H H 2-methyl 2-propanol Tertiary Monohydroxy

  29. H H H-C-C-H O O H H H H H H-C-C-C-H O O O H H H Dihydroxy Trihydroxy

  30. Properties of Alcohols • Contain a H bonded to an O atom. • Therefore Hydrogen Bonding occurs. • Alcohols have a higher boiling point than the corresponding alkane. • Like dissolves Like. Alcohols tend to be very soluble in water.

  31. R - O R - H O + H +

  32. Which compound has the highest boiling point? • CH4 • C2H6 • C3H8 • C3H7OH Correct response = D.

  33. Table R • General Formula for Alcohols: ROH. • R represents the entire hydrocarbon part of the molecule. • OH is the hydroxyl group.

  34. Functional Group #3 Ethers

  35. Ethers • General formula is ROR where R may or may not be the same as R. • R and R are hydrocarbon branches. • O is an oxygen bridge. • Ethers are not linear. They are bent, like water.

  36. Properties of Ethers • In a pure ether, no hydrogen bonding – no H bonded to O. Do have weak dipole-dipole interactions – bent, like H2O. • Dipole-dipole interactions are between dispersion forces & hydrogen bonding. • Ethyl ether once used as anesthesia

  37. Properties of Ethers • Compared to alkanes: • Higher boiling pts than similar alkanes. • More soluble in water than alkanes. • Compared to alcohols: • Lower boiling pts than similar alcohols. • Much less soluble in water than alcohols.

  38. Naming Ethers • If the 2 hydrocarbon branches are identical, name the branch (once) & add the word ether. • If the 2 branches are different, list them in alphabetical order followed by the word ether.

  39. H H HCOCH H H Methyl Ether H H H H H H HCCCOCCCH H H H H H H Propyl Ether

  40. H H H H HCOCCCH H H H H Methylpropyl Ether

More Related