Chapter 2 chemistry form 5

1. Carbon compound
•Compound that contain carbon, hydrogen and elements
Such as sulphur, nitrogen, oxygen
Organic compounds Inorganic compounds
•Carbon containing compound
Example:
-Protein
-Carbohydrates
-Alcohol
•Non-carbon containing compounds
Example
-Silica
-Marble
Bauxite
-Oxides of carbon
-carbonates
-hydrogen carbonates
-cyanides
-metallic carbonates
Exceptions

2. HYDROCARBON
Saturated hydrocarbon Unsaturated hydrocarbon
•Carbon-carbon single bond
•Single covalent bond
C C
H H
H H
H H
C C
H H
H H
H H
•Hydrocarbons are pertroleum,natural gas,coal and
rubber tree
•Non-hydrocarbon contain other elements such as nitrogen
oxygen

3. ALKANES
•General formulae : CnH2n+2
n= 1,2,3,4,…………
•Saturated hydrocarbon
C

4. NAMING ALKANES
•IUPAC ( International Union of Pure and Applied Chemistry)
ROOT END
Denotes the longest chain Denotes the family of
(number of carbon atoms) organic compound
Ends with -ene
Molecular Formula CnH2n+2

5. Carbon atom Root name
1 Meth-
2 Eth-
3 Prop-
4 But-
5 Pent-
6 Hex-
7 Hept-
8 Oct-
9 Non-
10 Dec-

6. Molecular formula
Shows the actual number of atoms of each type of
elements in the compounds
Structural formula
Shows the order in which atoms are bonded
together in a molecule and by what
types of bonds

9. Physical properties
Electrical conductivity
Melting and boiling point
Solubility Density

10. CHEMICAL PROPERTIES
Combustion Substitution
Reaction

11. Substitution Reaction

12. Number of Isomers of Alkanes
Number of C Atoms Possible Isomers
1-3 1
4 2
5 3
6 5
7 9
8 18
9 35
10 75
15 4,347
20 366,319

13. ALKENE
unsaturated chemical compound
carbon–carbon double bond =
general formula CnH2n
functional groups

14. Naming Alkene

15. Physical properties same as ALKANE

16. CHEMICAL PROPERTIES
Combustion Addition
Halogenation
Hydration Hydrogenation Formation of
Diol
Addition of
Hydrogen Halide

17. HYDROGENATION
CH2=CH2 + H2 → CH3-CH3
Catalyst = platinum, nickel or palladium
Temperature : 180°C

20. Isomers of Alkenes

21. Naming Branched Alkanes Practice
1. C
C
C—C—C—C
C
C
2. C
C—C—C—C—C—C—C
C C
C
C C
C
3. C—C—C—C—C—C—C
C C
C
C
C C 5.
4. C—C—C—C—C—C
C
C
C
C
6. C
C
C C C
C C C
C
C
C—C—C—C—C—C—C
C C C
C
7. C
C C C C C C
C C
C

22. DRAW THE FOLLOWING…
8. 2-methylbutane: 9. 4-ethyl-3-methylheptane:
10. 4-ethyl-3,5-dimethylheptane: 11. 3,4-dimethylhexane:
12. 2,3,4,5-tetramethylnonane:

23. ALCOHOL
• organic compound
• hydroxyl functional group -
OH
• general formula
CnH2n+1OH
• Elements in Alcohol
-Carbon
- Hydrogen
- Oxygen

24. Ethanol

25. ISOMERISM
Propanol

26. BUTANOL

27. Preparation of Alcohol
1. FERMENTATION
Yeast produce an enzyme called zymase.
Zymase enzyme breaks down the glucose molecules to simpler molecule,
namely ethanol and carbon dioxide.
Yeast is killed by ethanol concentrations in excess of about 15%, and that
limits the purity of the ethanol that can be produced.

29. 2. HYDRATION

30. Chemical Properties of Alcohol
1.Combustion
C2H5OH + 3O2 → 2CO2 + 3H2O

31. 2.Dehydration of Alcohol
• Decompose to form alkene and water.

33. 3. Oxidation
Alcohols can be oxidized to produce carboxylic acid
by oxidizing agent
a.Acidified potassium dichromate(VI)
b.Acidified potassium manganate (VII)
Oxidising Agent

34. Oxidation of Alcohol
Alcohol is heated under reflux with excess oxidising agent.
The reflux technique used to prevent the alcohol vapour escape to the surrounding.
When the reaction is complete, the carboxylic acid is distilled off.

35. acidified potassium dichromate(VI)
• orange solution containing the dichromate(VI) ions is
reduced to a green solution containing chromium(III) ions.
acidified potassium manganate (VII)
• purple colour of potassium manganate (VII) decolourised.

36. Uses of Alcohol

38. CARBOXYLIC ACID
General Formula: CnH2n+1COOH, n = 0, 1, 2, .....
Functional Group:
Carboxyl

39. Number of Carbon Name of Alkane
Name of Carboxylic
Acid
1 methane methanoic acid
2 ethane ethanoic acid
3 propane propanoic acid
4 butane butanoic acid
5 pentane pentanoic acid
6 hexane hexanoic acid

40. Preparing Carboxylic Acid
= Oxidation of ALCOHOL

41. • Base
Carboxylic Acid + Base Oxide/Alkali → Salt + Water
• metal carbonate
Carboxylic Acid + Metal Carbonate → Salt + Carbon Dioxide + Water
• Metal
Carboxylic Acid + Reactive Metal → Salt + H2
Chemical Properties
Just like other acids, carboxylic acid can react with:

42. Carboxylic acid reacts with alcohol to produce ESTER in the
Presence of CONCENTRATED SULPHURIC ACID
• Esterification
Carboxylic Acids + Alcohol → Ester + Water

43. Preparing Ester

47. OIL AND FATS
Natural ESTER
Fats –Solid at RT
Oil – Liquid at RT

48. Fatty acid + glycerol Fat /oil + water
Carboxylic acid alcohol ester

49. ESTERIFFICATION TO PRODUCE FAT

54. Converting Unsaturated fat to Saturated fat
HYDROGENATION

55. Industrial Extraction of Palm Oil

57. CROSS SECTION OF AN OIL PALM FRUIT

58. Extraction Process of Palm Oil

61. Polymer is a long chain made of single units that are
linked together.
The single units that link together to form a polymer are
called monomers
POLYMER
Polymerization process of joining monomer to form polymer

62. Natural polymer Synthetic Polymer
Obtained from Man made polymer
Plants of animals
Exp; starch, natural rubber Exp: plastic, synthetic
Cotton, protein, silk rubber, nylon, PVC
POLYMER

63. NATURAL POLYMER

64. Synthetic polymer
Nylon
plastic
PVC
Synthetic rubber

65. Natural polymers
Protein
Amino acid

67. CARBOHYDRATES
Monomer
Carbohydrates
Polymer

68. NATURAL RUBBER
Made from monomer called isoprene
Obtained from rubber tree
isoprene

70. Properties of natural rubber
• Elastic and soft
• Not stable towards heat
Becomes warm at 50 degree celcius and melt/decompose
at 200 degree celcius
• Does not conduct electricity
• Hard and brittle and cold
• Insoluble in water but soluble in organic solvent such
as chloroform, benzene

73. Coagulation of Latex

79. Vulcanized Rubber