Organic Compounds | Jamb Chemistry

Tetravalency of Carbon

1. Carbon has 4 valence electrons in its outermost shell.
2. To achieve stability, carbon forms 4 covalent bonds.
3. This property is known as tetravalency.
4. Tetravalency makes carbon highly versatile in forming compounds.
5. Carbon bonds with elements like hydrogen, oxygen, and nitrogen.
6. Carbon also bonds strongly with itself, forming chains and rings.
7. The carbon-carbon (C-C) bond is strong and stable.
8. Carbon compounds are diverse, forming millions of organic compounds.
9. Single bonds involve sharing 1 pair of electrons (C-C).
10. Double bonds involve 2 shared pairs of electrons (C=C).
11. Triple bonds involve 3 shared pairs of electrons (C≡C).
12. Carbon compounds can be straight-chained, branched, or cyclic.
13. Tetravalency allows carbon to bond with 4 different atoms simultaneously.
14. The ability to form stable compounds is the basis of organic chemistry.
15. Tetravalency enables the formation of isomers with the same formula.
16. Carbon’s unique bonding properties lead to functional groups.
17. Carbon bonds are directional, giving rise to specific geometries.
18. Examples of geometries include tetrahedral (CH4), planar (C=C), and linear (C≡C).
19. Tetravalency allows carbon to form long hydrocarbon chains.
20. Carbon is the foundation of all living organisms due to its bonding ability.
    
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Naming Organic Compounds

21. Organic compounds are named using IUPAC rules.
22. The name has 3 parts: prefix, root, and suffix.
23. The root name indicates the number of carbon atoms in the main chain.
24. Meth- (1C), eth- (2C), prop- (3C), but- (4C), etc., are common roots.
25. Suffixes indicate bond types: -ane for single, -ene for double, -yne for triple.
26. Example: CH4 is methane; C2H4 is ethene; C2H2 is ethyne.
27. Substituents (like CH3, Cl) are named with prefixes such as methyl, chloro, etc.
28. The position of bonds or substituents is shown by numbers.
29. Example: But-2-ene indicates a double bond on the 2nd carbon.
30. For cyclic compounds, the prefix cyclo- is added (e.g., cyclohexane).
31. Alcohols have the suffix -ol (e.g., ethanol: CH3CH2OH).
32. Aldehydes use the suffix -al (e.g., formaldehyde: HCHO).
33. Carboxylic acids have -oic acid (e.g., ethanoic acid: CH3COOH).
34. Ketones use -one (e.g., propanone: CH3COCH3).
35. Naming helps relate the structure to the compound systematically.
36. Example: C3H8O can be propanol (alcohol) or propanone (ketone).
37. Halogenated hydrocarbons are named using prefixes like fluoro-, chloro-, bromo-.
38. Alkenes and alkynes are named by indicating the position of multiple bonds.
39. Example: Pent-1-ene has a double bond at carbon 1.
40. Proper naming ensures clarity in chemical communication.
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Catenation

41. Catenation is the ability of carbon to form long chains.
42. Carbon forms C-C bonds, which are strong and stable.
43. Catenation leads to the formation of straight chains, branched chains, and rings.
44. It occurs due to carbon's tetravalency and strong bonds.
45. Hydrocarbons are primary examples of catenation.
46. Saturated compounds have single bonds only (e.g., alkanes).
47. Unsaturated compounds have double or triple bonds (e.g., alkenes, alkynes).
48. Catenation allows the formation of large molecules like polymers.
49. Examples include methane (CH4), ethane (C2H6), and benzene (C6H6).
50. Without catenation, organic chemistry would not exist.
    
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Classification by Functional Groups

51. Functional groups are specific atoms or bonds determining a compound’s reactivity.
52. Alcohols (-OH) are organic compounds containing hydroxyl groups.
53. Aldehydes (-CHO) have a terminal carbonyl group.
54. Ketones (C=O) have a carbonyl group within the carbon chain.
55. Carboxylic acids (-COOH) contain the carboxyl group.
56. Amines (-NH2) contain the amino group.
57. Halogens (F, Cl, Br, I) create haloalkanes.
58. Functional groups influence physical and chemical properties.
59. Classifying compounds by groups simplifies their study.
60. Examples: CH3OH (methanol, alcohol), HCOOH (formic acid, carboxylic acid).
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Petroleum: Fractional Distillation and Cracking

61. Petroleum is a mixture of hydrocarbons.
62. It is separated by fractional distillation.
63. The column works based on boiling points of hydrocarbons.
64. Lighter hydrocarbons condense at the top.
65. Heavier hydrocarbons condense at the bottom.
66. Major products include:
    • LPG (C1-C4): Cooking gas.
    • Petrol (C5-C10): Vehicle fuel.
    • Diesel (C15-C20): Heavy engines.
67. Cracking breaks long hydrocarbons into smaller alkanes and alkenes.
68. Cracking can be thermal or catalytic.
69. Reforming rearranges molecules to improve fuel quality.
70. Petroleum products are vital for energy and chemical industries.
    
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Alkanes, Alkenes, Alkynes

71. Alkanes are saturated hydrocarbons (CnH2n+2).
72. They only contain single bonds.
73. Examples: Methane (CH4), Ethane (C2H6).
74. Alkenes are unsaturated hydrocarbons with double bonds (CnH2n).
75. Example: Ethene (C2H4).
76. Alkynes have triple bonds (CnH2n-2).
77. Example: Ethyne (C2H2).
78. Alkenes and alkynes are more reactive than alkanes.
79. Addition reactions occur in unsaturated hydrocarbons.
80. Combustion of alkanes produces CO2 and water.
    
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Isomerism

81. Isomers have the same molecular formula but different structures.
82. Structural isomerism includes chain, position, and functional group isomerism.
83. Geometrical isomerism occurs in alkenes (cis/trans forms).
84. Example: Butane (C4H10) has chain isomers.
85. Isomerism explains the diversity of organic compounds.
86. Different isomers have different properties.
87. Example: C2H6O can be ethanol or dimethyl ether.
88. Isomers are crucial in pharmaceuticals.
89. Geometrical isomers differ in physical properties.
90. Isomerism increases the number of compounds possible.
    
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Ethyne (Acetylene)

91. Ethyne is the simplest alkyne with formula C2H2.
92. It is a colorless gas.
93. It burns with a sooty flame.
94. Ethyne is used in welding (oxyacetylene flame).
95. It is prepared by reacting calcium carbide with water.
96. Ethyne is a starting material for polymers.
97. It undergoes addition reactions to form saturated compounds.
98. Ethyne can polymerize to form benzene.
99. Its high energy makes it suitable for cutting metals.
100. Ethyne is used in the production of organic solvents.
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Final Summary Points

101. Carbon’s tetravalency enables diverse compound formation.
102. Organic compounds are systematically named.
103. Catenation leads to long carbon chains.
104. Functional groups define properties of compounds.
105. Petroleum is separated through fractional distillation.
106. Cracking and reforming improve fuel production.
107. Alkanes, alkenes, and alkynes differ in bonding.
108. Isomerism explains the structural diversity of compounds.
109. Ethyne is a key industrial alkyne.
110. Organic compounds are the basis of life.
111. Alkanes are stable and less reactive.
112. Alkenes and alkynes are unsaturated and more reactive.
113. Petroleum provides essential fuels.
114. Cracking produces valuable hydrocarbons.
115. Isomerism impacts the chemical and physical properties.
116. Carbon’s tetravalency and catenation lead to millions of compounds.
117. Functional groups enable compound classification.
118. Organic chemistry governs industrial processes.
119. Understanding carbon compounds has practical significance.
120. Organic compounds are vital to modern life.

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