This document discusses several topics related to chemical bonding: Covalent bonding occurs when atoms share valence electrons to form stable molecular structures. Lewis structures use dots to represent these shared and unshared electron pairs, following the octet rule which states that atoms seek a full outer shell of 8 electrons. Exceptions exist for some atoms. Polar covalent bonds form when electrons are unequally shared between atoms, resulting in a partial positive and negative charge.

1. TOPICS
Covalent Bonding
Lewis Structure
Octet Rule
Polar Covalent Bond

2. Chemical bonding
Atoms combines with one another to
form compounds,which properties
different from that of atoms.
The attractive force exist between
the atoms in the compound is called
Chemical bond

3. Covalent bond
Covalent or shared electron pair of
bonding was explained by G.N.Lewis
(greatest American chemist) in 1916. He
proposed that, "Sharing of two electrons
by two hydrogen atoms permits each one
to have a stable closed shell electronic
configuration analogous to helium".

4. There are two types of electrons-
Core electrons and Valance electrons.
Sharing of electrons will takes place in the
valance shell.

5. Example for Single Covalent Bond

6. Example for double and triple
covalent bond

8. Lewis Structure
Structural formulas in which the
electrons are represented as dots are
called lewis Structure

9. The electron pairs which are not
involved in bond formation is
unshared pairs or lone pairs.Thus
the fluorine has three unshared pairs
of electrons.

10. Atoms in the same coloumn of the
periodic table have similar valence
electrons.Thus they are called
Isoelectronic atoms

11. Examples for lewis structure

13. Octet rule

15. Octet rule exceptions

16. Polar covalent bond

17. Electron polarization in the
compound can be explained by
Electrostatic potential map,which
uses the colour of the rainbow
shades. Blue colour is to dominate
the polarized positive charge and
Red is for polarized negative
charge.