The document provides a comprehensive overview of carbon, its chemical structure, properties, and the types of covalent bonds formed, including examples with hydrogen, oxygen, and nitrogen. It also covers concepts in organic chemistry, such as hydrocarbons, isomerism, and functional groups, alongside their significance and differentiation between soaps and detergents. Additionally, it discusses carbon allotropes like graphite and diamond, and emphasizes the importance of understanding carbon compounds in various scientific applications.

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2. • CARBON is the chemical element with
symbol C and atomic number 6. As a
member of group IV on the periodic
table, it is nonmetallic and tetravalent—
making four electrons available to
• form covalent chemical bonds.
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3. Some Physical Properties of
Carbon
 Atomic number: 6
 Atomic mass: 12.0107 amu
 Melting Point: 3,823 K
 Boiling Point: 4,098 K
 Density: 2.2670 g/cm3
 Phase (room temp.): Solid
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4. Types of Covalent Bond
•Single Covalent Bond :mutual sharing of one pair of electrons.
•Double Covalent Bond :mutual sharing of two pair of electrons.
•Triple Covalent Bond :mutual sharing of three pair of electrons.
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5. Eg. :- Formation of single covalent bond in Hydrogen
molecule - H2
The atomic number of hydrogen is 1, its electronic
arrangement is 1, it has 1 valence electron. It needs 1
electron more to attain stability. So two hydrogen
atoms share 1 pair of electrons resulting in the
formation of a single covalent bond in hydrogen
molecule H2.
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6. Formation of double covalent bond in oxygen molecule - O2
The atomic number of oxygen is 8, its EC is 2,6, it
has 6 VE, it needs 2 electrons more to attain
stability. So two oxygen atoms share two pairs of
electrons resulting in the formation of a double
covalent bond in oxygen molecule O2.
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7. Formation of triple covalent bond in Nitrogen molecule - N2
The atomic number of nitrogen is 7, its EC is 2,5,
it has 5 VE, it needs 3 electrons more to attain
stability. So two nitrogen atoms share three pairs
of electrons resulting in the formation of a triple
covalent bond in nitrogen molecule N2.
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8. • Low Melting and boiling point.
• Physical State (liquid or gas)
• Low Density.
• Solubility.
• Bad Conductor of Electricity.
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9. Covalent Compounds
• Insoluble in water.
• Gaseous, liquids or soft
solids.
• Low boiling and melting
point.
• Soluble in organic solvents.
Ionic Compounds
• Soluble in water.
• Crystalline solids.
• High boiling and melting
point.
• Insoluble in organic
solvents.
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10. Allotropes of Carbon
 Two or more forms of
the same element that
differ significantly
in chemical & physical
properties are known
as allotropes.
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11. Graphite
Graphite is derived from the Greek word
“graphein” which means to write. It was
named by the German Geologist Abraham
Werner in 1789.
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12. Diamond
In diamond, each carbon atom
is tetra headedly attached to four other
carbon atoms forming a rigid three
dimensional structure.
Thus it is the hardest substance known.
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13. Fullerenes
• Fullerene research is expected to lead to new
materials, lubricants, coatings, catalysts, electro-optical
devices, and medical applications.
• First identified in 1985 by R. F. Curl, Jr., R. E.
Smally, and H. W. Kroto (who shared the 1996
Nobel Prize in Chemistry)
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14.  Organic Chemistry: The branch of chemistry dealing
with carbon compounds, other than CO , CO2 and
carbonates, is called Organic Chemistry.
 Organic compounds: The compounds of carbon, other
than CO , CO2 and carbonates, are called Organic
Compounds
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15. Isomerism
Compounds having the same molecular formulae but
different structural arrangement of atoms in them
are known as isomers, and the phenomenon is known as
isomerism.
Examples of Isomerism:
Butane – C4H10 has 2 isomers.
They are Normal butane and
Iso butane.
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16. Compounds of carbon in which their molecules are composed
of only carbon and hydrogen atoms are called hydrocarbons.
 SATURATED
HYDROCARBON
 UNSATURATED
HYDROCARBON
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17. •A Hydrocarbon is an organic compound that
contains only the elements hydrogen and carbon.
•In a saturated hydrocarbon, all the bonds are
single bonds.
•Alkane is another name for a
saturated hydrocarbon.
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18. Examples of Saturated
Hydrocarbons
Examples of Saturated
Ethane C2H6
Propane C3H8
Butane C4H10
Hydrocarbons
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19.  A hydrocarbon that contains one or
more double or triple bonds is an
unsaturated hydrocarbon.
 There are three types of unsaturated
hydrocarbons : Alkenes , Alkynes &
Aromatic hydrocarbons .
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20. Examples of Unsaturated
Hydrocarbons
Ethene C2H4
Propane C3H6
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21. Systematic Nomenclature of Carbon
Compounds
Number of carbon atoms
in the parent chain
Root word
1 Meth
2 Eth
3 Prop
4 But
5 Pent
6 Hex
7 Hept
8 Oct
9 Non
10 Dec
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22. Homologous series
A homologous series is a group of organic
compounds having similar structures and
similar chemical properties in which the
successive compounds differ by CH2 group
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23. Characteristics
-) All members of homologous series can be
represented by the same general formula .
-) All compound show similar chemical properties .
-) The members of homologous series show a
gradual change in their physical properties with
increase in molecular mass .
-) Any two adjacent homologues differ by 1 carbon
atom and 2 hydrogen atom in their molecular
formulae ...
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24. Alkanes
The general formula of alkanes is CnH2n+2 where n is
no. of carbon atoms in 1 molecule of alkanes.
Single Bond……
ALKANE MOLECULAR
FORMULA
Methane CH4
Ethane C2H6
Propane C3H8
Butane C4H10
pentane C5H 24 12

25. The general formula of alkenes is CnH2n where n is no.
of carbon atoms in 1 molecule of alkenes.
At least 1 Double Bond……
Alkenes Molecular formula
ALKENES
Ethene C2H4
Propene C3H6
Butene C4H8
Pentene C5H10
Hexene C6H12
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26. ALKYNES
The general formula of alkyne is CnH2n-2
where n is no. of carbon atoms in 1
molecule of alkyne.
At least 1 Triple Bond……
ALKYNE MOLECULAR
FORMULA
Ethyne C2H2
Propyne C3H4
Butyne C4H6
Pentyne C5H8
Hexyne C6H10
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27. FUNCTIONAL GROUPS
In organic chemistry, functional groups are specific groups of atoms
within molecules that are responsible for the characteristic chemical
reactions of those molecules.
FUNCTIONAL GROUPS SUFFIX / PREFIX
& SYMBOLS
ALDEHYDE Suff – ‘al’
ALCOHOL Suff – ‘ol’
KETONE Suff–‘one’
CARBOXYLIC ACID Suff – ‘oic acid’
HALOGEN Pref – chloro , bromo, floro, iodo
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28. Soaps
Soaps :-
Soaps are long chain sodium or potassium salts of carboxylic acids.
Eg:- Sodium stearate – C17H35COONa
Structure of soap molecule :-
A soap molecule has two parts. A long hydrocarbon part which is
hydrophobic (water repelling) and soluble in oil and grease and a
short ionic part which is hydrophyllic (water attracting) and
insoluble in oil and grease.
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29. Cleansing Action of Soap
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30. Differences between soaps and detergents
Soaps Detergents
Soaps are sodium salts of fatty
acids.
Detergents are sodium salts of
sulphonic acids.
Soaps clean well in soft water but do
not clean well in hard water.
Detergents clean well with both hard
and soft water.
Soaps do not clean as much as
detergents.
Detergents clean better than
soaps.
Soaps are biodegradable and do not
cause pollution.
Some detergents are non
biodegradable and cause pollution.
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