1. ORGANIC CHEMISTRY
Basic Concepts
Janardhan Acharyulu
PGT(Chemistry)
K V KANCHANBAGH

2. General introduction
Organic compounds are vital for life like genetic
bearing DNA and protein essential in our blood ,
muscles and skin

Organic chemicals like clothing,fuels,polymers,dyes
and medicines

First F Wholer synthesized an organic compound
UREA from an inorganic compound ammonium
cyanate
NH₄CNO
NH2 CONH2


3. Synthesis of acetic acid by Kolbe and methane by
Berthelot showed that organic compounds could be
preapred from inorganic synthesis

Carbon has the unique property called catanation
which forms covalent bonds with other carbons and
atoms like H,O,N,S, halogens etc


4. Shapes of organic compounds
Tetra valence of Carbon and the formation
of covalent bonds by it are explained in
terms of electronic configuration and
hybridizationof s and p orbitals

Formation and shapes of molecules Methane, Ethene and
Ethyne are exlpained in terms of sp³ , sp² and sp hybrid
orbitals by carbon in respective molecules


5. 

A molecule of
methane contains
four C-H ᓂ bonds
On the basis of sp³
hybridization of carbon atom
the structure of methane
molecule is predicted to be
Tetrahedral

6. 

Structure of ethane
Ethane contains six
C-H ᓂ bonds and
one C-C ᓂ bond

7. 
Structure of ethene
explained to be planar on
the basis of sp²
hybridization one C-C ᓂ
bond and one c-c Ꙥ
bond


8. 
Structure of ethyne to
be linear on the basis of
sp hybridization, the
carbon carbon triple
bond of ethyne
consists of one C-C ᓂ
bond and two C-C Ꙥ
bonds, the Ꙥ bonds
are formed by
sideways overlap of
the p-orbitals

9. Hybridization influences bond length and enthalpy

The sp hybrid orbital contains more s- character and

closer to its nucleus and forms shorter and stronger
bonds than sp₃ hybrid orbital

The sp² hybrid orbital is inter mediate between sp and
sp³ , hence the length and enthalpy values are also
intermediate

The change in hybridization affects the elecro-vity of
carbon,the greater the s – character the greater is the -vity,

Thus a carbon atom having an sp hybrid orbital with 50%
of s-character is more electro-vity than the other hybrid
orbitals

10. Characteristic Features of Ꙥ-
bonds
For Ꙥ bond formation it is essential that the porbitals on the adjacent carbon atoms must be
parallel for a parallel sideways overlap

Some of characters are

(i) All the atoms directly attached to the carbon atoms of the
double bond lie in the same plane

(ii) The p-orbitals of a Ꙥ-bond are mutually parallel

and are perpendicular to the plane of the molecule

The electron charge cloud of the Ꙥ-bond lies above
and below the plane of the bonding atoms