1. What is meant by the term Organic?

2. Page 2

3. Characteristics of organic compounds
Formed as a result almost exclusively of covalent bonding
Generally nonpolar  Generally insoluble in water
usually soluble in nonpolar solvents (other organic compounds)
Non-electrolytes except organic acids which are weak electrolytes
Have low melting points (due to weak intermolecular forces that hold them together)
The great number of carbons leads to a higher melting point.

4. Characteristics of organic compounds, (continued)
Have slower reaction rates than inorganic compounds
covalent bonds within organic molecules are strong
activation energies are high
catalysts are often used to increase reaction rates

5. How can we describe Hydrocarbons?

6. Hydrocarbons
Definition - compounds composed of only hydrogen and carbon
There are so many hydrocarbons found in nature; nearly impossible to study all! They are grouped in Homologous series.
Homologous series - group of organic compounds with similar properties and related structures (differ from each other by CH3)

7. 3 Important Homologous Series of Hydrocarbons:
Alkanes
Alkenes
Alkynes

8. Aliphatic - hydrocarbon chains
Saturated
Definition - has no bonds that can be broken to add extra hydrogen
called Alkanes
family of hydrocarbons with all single bonds
general formula CnH2n+2
named with suffix "ANE“
Table P – Organic Prefixes
As the number of carbons increases, the boiling point increases.

9. TAKE OUT PAPER AND DRAW PLEASE
Name and draw the first ten Alkanes
Go to table P and look at the prefix for the number of carbons
1 carbon is Meth
All alkanes end in ‘ane’
‘meth’ and ‘ane’
Methane
2 carbons is Eth
‘eth’ and ‘ane’
Ethane

10. The First Ten Straight-Chain Hydrocarbons

11. The First Ten Straight-Chain Hydrocarbons

12. Page 3

13. What are the Unsaturated Hydrocarbons?

14. Unsaturated - has double or triple bonds that can be broken to add more hydrogen
Alkenes
family of hydrocarbons with at least one double bond
general formula CnH2n
named with suffix "ENE“
Starts with Ethene.

15. Alkenes TAKE OUT PAPER AND DRAW PLEASE
Draw the first nine Alkenes
Go to table P and look at the prefix for the number of carbons
2 carbons is Eth
All alkenes end in ‘ene’
‘eth’ and ‘ene’
Ethene
3 carbons is Prop
‘prop’ and ‘ene’
Propene

16. Alkenes TAKE OUT PAPER AND DRAW PLEASE
Draw the first nine Alkenes
Go to table P and look at the prefix for the number of carbons
4 carbons is But
All alkenes end in ‘ene’
‘but’ and ‘ene’
Butene

17. Alkenes

18. Alkynes Alkynes family of hydrocarbons with one triple bond
general formula CnH2n-2
named with suffix "YNE“
Starts with Ethyne.

19. Alkynes Draw the first nine Alkynes
Go to table P and look at the prefix for the number of carbons
2 carbons is Eth
All alkenes end in ‘yne’
‘eth’ and ‘yne’
Ethyne
3 carbons is Prop
‘prop’ and ‘yne’
Propyne

20. Packet Page 4

21. With this ring I, get confused?

22. The Benzene Series (Aromatic hydrocarbons)
The benzene series consists of molecules which are cyclic in nature.
The general formula is CnH2n-6.
Benzene H C
H C C H
C6H6 H

23. Although it appears that the structure has alternating double and single
bonds, the bonding involves six identical bonds. A resonance
structure is used to show structural formula of benzene.
H H
C C
H C C H H C C H
An abbreviated structural formula can be used in place of the above: OR

24. Toluene or Methylbenzene C7H8
H C C CH3
H C C H C
An abbreviated structural formula can be used in place of the above:
CH CH3

25. Alkylderivatives of Benzene

26. Page 5 Practice

27. Aim: How can we name organic compounds?
We have rules!!!!
YAY!!!!!!!!!!!

28. Rule 1: Find the longest continuous chain

29. Rule 2: Assign numbers to each C atom in the longest chain, starting at the end with the attached group.

30. Rule 3: If more than one of the same types of group is attached to the main chain prefixes are used to identify the attached groups.

31. Rule 4: When naming alkenes or alkynes the carbon with the double/triple bond, the carbon number with the double/triple bond must be identified in the name.

32. Packet Pages 10-11

33. Aim: How can we represent organic compounds?

34. What are we showing in the following pictures?
Different symbols or signs to represent one thing- women! The bottom is written in braille.

35. Different ways to represent one compound
Molecular Formula
Structural Formula
Condensed Structural Formula
Ball-and-Stick Model
Space-Filling Model

36. Molecular Formula Shows the kind and number of atoms in a compound.
Example: CH4 or C2H6
Tells us that there are carbon and hydrogen atoms. For methane, there are 4 hydrogens for 1 carbon atom.

37. Structural Formula
In addition, shows the bonding patterns and two-dimensional view.
For example:

38. Condensed Structural Formula
Written structural formula
For example: Methane: CH4
Ethane: CH3CH3

39. Ball-and-Stick Model
Shows a 3D structure of the compound
Example:

40. Space-Filling Model Shows the actual structure of the compound
Example:

41. Molecules Models of Organic Hydrocarbons
Fig 8.4

42. Isomers
Isomers: When a molecular formula can be represented by more than one structural arrangement
Isomers have the same molecular formula, but different physical and chemical properties.
As the # of carbon atoms increases, so does the # of possible isomers

43. Isomers
How would you draw the structural formula for a 4 carbon hydrocarbon?

44. Structural Isomers of Butane
Fig 8.5

45. Isomer Practice Draw 3 Isomers for 5 and 6 carbon Alkanes.
Be sure you have the correct number of hydrogens.

46. What are the various Functional Groups?

47. Functional Groups
Atoms or groups of atoms that replace hydrogen atoms in a hydrocarbon.
This will form new compounds?
They have distinct physical and chemical properties.
There are 9 functional groups
All found on Table R!

48. C, H and O Alcohols (R-OH)
ethanol, isopropyl alcohol, (rubbing alcohol)
Ethers (R-O-R)
dimethyl ether (old anaesthetic)
Ketones
acetone (nail polish remover)
Aldehydes (a ketone with at least one R = H)
formaldehyde
Esters
many fine odours
Carboxylic acids
acetic acid
Carbohydrates
(CH2O)n, glucose, starch, cellulose

49. 1. Halides 2-fluoropropane
A Halogen (F, Cl, Br, or I) replaces a hydrogen on a hydrocarbon.
Used as organic solvents
General Formula: R-X (X= Halogen & R= Alkyl group)
Add fluoro for F Designate the location of
Chloro for Cl the halide with 1,2 etc
Bromo for Br
Iodo for I
2-fluoropropane

50. 2. Alcohols
Organic compounds in which one or more hydrogen atoms are replaced by an –OH group.
-OH group is called a hydroxyl group.
NOT A BASE!
They are nonelectrolytes (Do not form ions in solution).
Polar substances
General Formula: R-OH
Naming: Position of OH group must be assigned & -ANE ending changes to –OL.

51. Classification of Alcohols
There are primary, secondary, and tertiary carbon atoms:
Primary Carbon: Attached to one carbon only
Secondary: Attached to two carbon atoms
Tertiary: Attached to three carbon atoms.

52. Alcohols
“ol” ending

53. 3. Aldehydes
Organic compounds in which a carbonyl group (C=O) is found on the end carbon (a primary carbon):
Naming: Substitute –AL in place of final –E of alkane name.
General Formula
Propanal
propanal

54. 4. Ketones C=O group is on the inside of a hydrocarbon:
Naming: Substitute –ONE in place of final –E of alkane name.
General Formula:
Propanone
propanone

55. 5. Ethers Two carbon chains are joined together by an oxygen atom:
Naming: name the alkyl groups and add ether at the end.
General Formula: R-O-R
Methyl ethyl Ether
Methoxyethane

56. 6. Organic Acids Organic compounds that have a Carboxyl group (-COOH):
Naming: Substitute –OIC ACID in place of final –E in alkane name.
Ethanoic acid= Acetic acid
General Formula:
Ethanoic Acid

57. Carboxylic Acids

58. 3-methyl-2-hexanoic acid armpit in a jar

59. Isovaleric acid “locker room concentrate”

60. 4-ethyloctanoic acid “wet male goat”

61. 7. Esters General Formula:
Have strong aromas; for example, flavorings in bananas, wintergreen, oranges.

62. The fine smell of esters

63. 8. Amines
Formed when one or more of the hydrogen’s in ammonia is replaced by an alkyl group:
Naming: Substitute –AMINE in place of final –E of alkane name.
General Formula:

64. 9. Amides Formed by the combination of 2 amino acids: General Formula:
Form proteins
Naming: Replace final –E with -AMIDE
propanamide

65. Functional Groups

66. Packet Pages 13-15

67. Aim: How do organic compounds react?
Do Now: Name the Functional Group:
1. CH3COOH
2. CH3COOCH3
3. CH3CHO

68. Which one is faster?
Making Wine or Dissolving Alka Seltzer in water?

69. Organic Reactions
Occur more slowly than inorganic reactions because of the covalent bonds.
There are 7 types of Organic Reactions.

70. Substitution
Involves the replacement of 1 or more of the hydrogen atoms in a saturated hydrocarbon with another atom or group:
C2H6 + Cl C2H5Cl + HCl +

71. Addition Involves adding 1 or more atoms at a double or triple bond:
Ethene + Chlorine ,2 dichloroethane

72. Fermentation
A chemical process in which yeast cells secrete the enzyme zymase and break down glucose into carbon dioxide and ethanol:

73. Esterification
Reaction between an organic acid and an alcohol to produce an ester plus water:
Ethanoic acid + Ethanol Water + Ethyl ethanoate

74. Saponification
When an ester reacts with an inorganic base to produce an alcohol and a soap:
Fat Base Glycerol + Soap

75. Combustion Almost all organic compounds will combust , or burn:
Compound + Oxygen Carbon Dioxide + Water

76. Polymerization
Polymers: Organic compounds made up of chains of smaller units (monomers) covalently bonded together.
Polymerization: Formation of these large polymer molecules.
Examples of Natural Polymers: Cellulose, Proteins, & Starch
Synthetic Polymers: Nylon & Rayon

77. Addition Polymerization
Joining of monomers of unsaturated compounds:

78. Condensation Polymerization
Bonding of monomers by removing water from hydroxyl groups and joining monomers by an ether or ester linkage:

79. Summary: Identify the Reaction
C2H6 + Cl C2H5Cl + HCl
C6H12O C2H5OH + 2CO2
CH3COOH + CH3OH CH3COOCH3 + H2O
nC2H (C2H4)n

80. Packet Pages 29-32

81. Aim: How can we review Organic Chemistry for our test?

82. Carbon Carbon forms four bonds always!
Carbon can form single, double, or triple bonds.
Single = Saturated
Double or Triple = Unsaturated
Carbon can covalently bond to other carbon atoms.

83. Hydrocarbons Have hydrogen and carbon atoms only!
Homologous Series: Members that have similar properties.
3 Types: Alkanes, Alkenes, and Alkynes

84. Alkane All single bonds All end in –ane
Each member differs by 1 carbon and 2 hydrogen atoms.
General Formula: Cn H2n + 2

85. Alkene Has at least one double bond All end in –ene.
General Formula: CnH2n

86. Alkyne Has at least one triple bond All end in –yne.
General Formula: CnH2n-2

87. Formulas Molecular: Shows the kind and number of atoms in a compound.
Example: CH4 or C2H6
Structural:
In addition, shows the bonding patterns and two-dimensional view.

88. Isomers
Isomers: When a molecular formula can be represented by more than one structural arrangement
Isomers have the same molecular formula, but different physical and chemical properties.
As the # of carbon atoms increases, so does the # of possible isomers

89. Functional Groups Found on Table R!
Alcohols: Can be classified in two ways:
Primary, Secondary, or Tertiary (with ONE -OH group only)!
1 –OH: Monohydroxy
2 -OH: Dihydroxy
3 –OH: Trihydroxy

90. Organic Reactions 7 Types: Need to know reactants & products.
Combustion
Substitution
Addition
Esterification
Saponification
Fermentation
Polymerization: Addition & Condensation

91. Organic Reactions Occur more slower than inorganic reactions. Why?
Review: Covalent bonds have low melting and boiling points, are poor conductors, and are nonpolar substances.

92. Number of Possible Isomers for Selected Alkanes

93. Some Common Alkyl Groups

94. Naming Alkanes

95. Cis-Trans Isomerism Does the term “trans” have anything to do with
the topic of “trans-fats” we have been hearing
a lot about recently?

96. Different Ways of Representing the Alkane Ethyne