1. Organic Chemistry: Study of carbon based molecules
Bonding: Covalent (share valence e-)
All Nonmetals
Made of carbon, hydrogen and other
nonmetals like sulfur, oxygen, nitrogen etc.

3. Carbon Atoms Form the “Backbone” Carbon has 4 valence and needs 4 more
ALWAYS forms 4 bonds
Bonds can be single, double or triple
Due to variety and number of bonds carbon can form you can have an
enormous number of combinations!

4. Properties of Organic Compounds
Relatively Low MP (compared to ionic, metallic)
MP depends on polarity of molecule & strength of IMF
Many are Non-polar molecules: (Lowest MP)
Weak attractions (VanDerWaals /dispersion forces)
Larger NP molecules have higher MP than smaller
Some are Polar molecules: (Slightly Higher MP)
Can have Dipole-dipole attractions or H-bonding
Molecules held together more
Stronger IMF

5. For nonpolars
the more atoms in chain the higher the Boiling Point

6. Properties of Organic Compounds
SOLUBILITY: Depends on polarity of molecule
(Many org. compounds are nonpolar, like oils & lipids.)
Polar molecules: Assymmetry = polar
soluble in polar solvents like water
Nonpolar molecules: Symmetry = nonpolar
soluble in nonpolar solvents like hexane
Polar compound will dissolve in water
Nonpolar compound

7. Properties of Organic Compounds
Conductivity in Solution
Organic Molecules DO NOT ionize in solution
Therefore, they don’t conduct in solution
and are NONELECTROLYTES
Important Exception: ORGANIC ACIDS
Ex: CH3COOH

8. Properties of Organic Compounds
Undergo combustion or burn readily
Complete and balance this combustion reaction
C3H O2 → ____ + ______

9. Properties of Organic Compounds
Have slow rates of reaction
Due to complexity of bonds
Often catalyst is needed to speed up reactions
React more slowly than ionics
Tend to breakdown or decompose at low
temperatures
Compared to other compounds

10. Formula Writing & Drawing Molecules
Types of Formulas
Molecular Ex:
Empirical Ex:
Structural Ex:
Condensed Structural Ex

12. Organic Prefixes (Table P)
Indicate how many carbon atoms
are in the entire molecule. You
will only see molecules with a
max of 10 carbons.

13. Homologous Series of Hydrocarbons (Table Q)
Each member of the series differs by one carbon and a certain # of hydrogen

14. Alkanes General Formula: CnH2n+2 Single bonds between carbon atoms
Name ends in “ane”
SATURATED hydrocarbons
(holding as many hydrogen atoms as possible)

16. Alkenes General Formula: CnH2n One double carbon to carbon bond
*Address needed for bond location
Name ends in “ene”
UNSATURATED hydrocarbons
(not totally filled with hydrogen)

17. Unsaturated = it isn’t “saturated” with hydrogen

18. Alkynes General Formula: CnH2n-2 One triple carbon to carbon bond
*Address needed for bond location
Name ends in “yne”
UNSATURATED hydrocarbons
(not totally filled with hydrogen)

20. What is molecular formula for these compounds?
_____________
Note how it matches general formula CnH2n-2

21. dienes, diynes etc… Have multiple double or triple bonds.
Give the address for each multiple bond.
End of name becomes “-diene…or –triene”
Use prefix “di/tri/tetra/penta” etc…if more than one of the same thing on the chain.
Name of Diene: ___________________

22. Branching Hydrocarbons
Have hydrocarbon “branches” off the main carbon chain.
Called “alkyl” groups
Name of Branched Hydrocarbon: ______________________

23. Naming Branched Hydrocarbons
Find longest continuous carbon chain and name it (parent chain)
Find address of each branch
Count carbons in each branch
Name branches using prefix ending in “yl”
Ex: 2 carbon branch would be an “ethyl” branch.
Note:
If more than one of the same type of branch use
“di”, “tri”, “tetra” etc…instead of repeating the name

24. Remember: First find the longest carbon chain and name it!!
Name of compound:
___________________
Name : ___________________ Name: ______________________
Remember: First find the longest carbon chain and name it!!

25. What are the names of these compounds?
Hint: find the longest continuous chain of carbon atoms and name it.

27. Isomers Same molecular formulas, but different structural formulas.
Same molecular formulas, but different structural formulas.
Atoms in molecule have a different arrangement.
The more atoms the larger # possible isomers
The more carbon atoms, the more possible arrangements of atoms!

28. 2 isomers with same molecular formula.
Can you draw another isomer below with the same molecular formula?

29. Cyclical Hydrocarbons
Form rings
Start with “cyclo-”
Shows skeleton of molecule only as a type of shorthand

30. Benzene Series Benzene Series: CnH2n-6 alternating double bonds.
6 carbon ring with
alternating double bonds.
Electrons in double bonds “resonate” between bond sites giving more strength to all the bonds
Branches and functional groups are often attached to the ring

31. Ortho/Meta/Para locations

33. Organic Functional Groups Reference Table R

34. Halides Contain one or more halogen atoms.
Fluoro / chloro / bromo / iodo prefix
Use address
Use di, tri, tetra if more than one of same

35. Name of this compound:
________________________

36. Alcohols Have one or more “Hydroxyl” groups (-OH) Use address
Name ends in “-ol”
If more than one (–OH), name ends in “diol”, or “triol”
Important Example: Glycerol or 1, 2, 3 propantriol
Draw a Picture of Glycerol:

37. Examples of Alcohols

38. Types of Alcohols Primary Secondary Tertiary

39. Aldehydes Carbon double bonded to oxygen at end
of a carbon chain (“carbonyl” group)
ADDRESS NOT NEEDED (always at end!)
End in “–al”
Note: no address needed for functional group!

40. Ketones
Carbon double bonded to oxygen in middle of a carbon chain (“carbonyl” group)
Use address
End in “-one”

41. Name this ketone: ____________________________
Note the basic difference between ketone and aldehydes
Name this ketone: ____________________________

42. Ethers Oxygen atom within carbon chain
Count carbon atoms on either side of oxygen and name them like “alkyl” branches.
“Butterflies” with belly buttons

43. Name of Ether: ___________________

45. Organic Acids
At the end of the carbon chain is a “carboxyl” group containing two oxygen atoms.
ADDRESS NOT NEEDED (always at end!)
End in “-oic acid”
Has an acidic hydrogen that ionizes so these are ELECTROLYTES

46. Name of Organic Acid:
_______________________
Name of Organic Acid:
_______________________
Name of Organic Acid:
_______________________

47. Esters
Within the chain, there is an oxygen atom that is next to a carbon double bonded to oxygen
Name both sides around the oxygen atom
Side with carbon “Alkyl” branch, ends in “yl”
Side with the double bonded oxygen ends in “oate”

48. Name of Ester:
_________________

49. Amines Have an “amine” group containing nitrogen. Use address
Ends in “-amine”
Important Example:
Amino Acid
Draw basic Amino Acid
Name of Amine: ______________________

51. Or can have 2 or 3 branches named like alkyl groups
Name of Amine:
______________________________

52. Amides
Also have a nitrogen atom, but it is next to a carbon double bonded to oxygen.
End in “amide”.
Name of Amide: _____________________________

53. The nitrogen can also be central instead of at the end, with alkyl branches.
Name of Amide:
__________________________
Name of Amide:
_____________________________

54. Organic Reactions Combustion Fermentation Substitution & Addition
Polymerization
Esterification
Saponification
Fractional Distillation
Cracking

55. Combustion Burning or oxidation of a hydrocarbon. Needs O2
Produces CO2 and H2O
Always EXOTHERMIC
If not enough O2 present, you can get “incomplete” combustion resulting in carbon monoxide (CO) and soot (C).

57. Fermentation Makes ALCOHOL!!!
Sugar is metabolized by yeast enzymes to make ethanol and CO2
How stuff works: (2:10)

58. Substitution Happens with ALKANES
One hydrogen atom comes off and is “substituted” for another atom.
Results in TWO products
Ex: Halogen Substitution

60. Addition ALKENES and ALKYNES. Add atoms without removing hydrogen
Double or triple bond “opens up”
Two atoms “add on” for
each broken bond
Results in ONE product.

61. Ex:
Halogen Addition
Hydrogenation

62. Polymerization Joining together of many individual “monomers” to
make a “polymer”.
Ex: Synthetic Polymers
Nylon
Rayon
Polyethelene
Polystyrene (styrofoam)
Polyester
Ex: Natural Polymers
DNA/RNA
Starch, Cellulose
Proteins

63. Types of Polymerization
Condensation Polymerization
Remove water to join monomers
Ex: Amino Acids joining to make “peptide” bonds
Addition Polymerization
Open up double/triple bonds to join monomers
Happens to alkenes/alkynes

64. Addition Polymerization

65. Joining Amino Acid Monomers
H2O is also a product!
CONDENSATION
POLYMERIZATION

66. ***Esterification***
Dehydration synthesis (water is removed to join molecules)
Alcohol + Organic Acid Ester + Water
Ester molecules often have nice odors
Fats are a type of ester made of glycerol and 3 fatty acid chains
Esterification Demo:

67. Name of Alcohol: ___________________
Name of Org. Acid __________________
Name of Ester: ____________________
Other product is always water!!

68. Saponification (Making Soap)
Soap molecules are long molecules that are nonpolar at one end & polar at the other end.
Can bring oil and water together
Ester + Base Glycerol + Soap
Saponification Process: (3:30)
Cleansing action of soap (2:00):

70. Petroleum Processing

71. Fractional Distillation
Separation of a petroleum mixture by differences in Boiling Point temperature.
Most compounds in petroleum are non-polar hydrocarbons.
Larger chains = stronger VDW = higher BP
Smaller chains = weaker VDW = lower BP
Fractional Distillation: (4 min)

72. Cracking Breaking of long hydrocarbon chains into smaller ones.
Often used on long chain hydrocarbons found in petroleum to make them into more usable fuels.
Usually involves a catalyst
Catalytic Cracking and Why it is done: (3:50)

73. Examples of Cracking