1. Chemical
bonding
By A y u s h D e w a n g a n
G u i d e d b y i s h a m a m
P r i n c i p a l M r s . D a l j e e t K o r a d a
2. Introduction
Chemical bonding provides the energy
necessary to hold two different atoms
together as part of a chemical compound.
Strength of the bond depends on the
molecules or atoms involved in the process
of bond formation.
3. Types of Chemical Bonding
Ionic Bonds
Covalent Bonds
Hydrogen Bonds
Metallic Bonds
4. Ionic Bonds
An Ionic bond is when an electron leaves
one atom and exothermically enters into
orbit around another. These to oppositely
charged ions now attract each other.
Ionic bonds are generally formed between
metals and nonmetals
5. Example of Ionic Bond
A classic example of ionic bonding is between Na and Cl. Na is a
silvery metal. It has 1 valence electron. Cl is a yellow-green gas, and
it needs 1 electron to fill its valence shell. If you put the gas and
the metal together, then they will burn as electrons are exchanged.
The metal dissolves and the gas disappears. The ions now have
opposite charges and are attracted to each other by electrostatic
forces. They form a crystal with the rock salt structure.
6. Covalent Bonds
A type of chemical bond in which there is
mutual sharing of electrons between two
atoms is called covalent bond. It is
further classified into single, double, and
triple covalent bond with respect to
mutual sharing of one, two, and three
bonds respectively.
7. Example of Covalent Bond
when two hydrogen atoms get close enough together, the attraction
is balanced in both directions and they share the electrons
between them. A covalent bond is made and hydrogen gas (H2) is
formed.
In the hydrogen molecule (H2) the darker area between the two
nuclei shows where the two electrons, which are now shared, are
most likely to be.
8. Hydrogen Bonds
A hydrogen bond is the attractive force
between the hydrogen attached to an
electronegative atom of one molecule and
an electronegative atom of a different
molecule.
Usually the electronegative atom is
oxygen, nitrogen, or fluorine, which has a
partial negative charge.
9. Example of Hydrogen Bond
Each hydrogen atom is covalently bonded to the oxygen via a
shared pair of electrons. Oxygen also has two unshared pairs of
electrons. Thus there are 4 pairs of electrons surrounding the
oxygen atom, two pairs involved in covalent bonds with hydrogen,
and two unshared pairs on the opposite side of the oxygen atom.
Oxygen is an "electronegative“ atom compared with hydrogen.
10. Metallic Bonds
Metallic bonding is the type of bonding
found in metallic elements. This is the
electrostatic force of attraction between
positively charged ions and delocalized
outer electrons.
Metallic bonding refers to the interaction
between the delocalized electrons and the
metal nuclei.
11. Example of Metallic Bond
As the metal cations and the electrons are oppositely charged,
they will be attracted to each other, and also to other metal
cations. These electrostatic forces are called metallic bonds, and
these are what hold the particles together in metals.
